Lab #3 – A Microscale Study of Chemical...

Lab 1 ndash Scientific Observation and Description

In order to become a good scientist you must learn how to become a good observer An observation is the process of using your senses to gather information There are five senses that a good scientist must use These senses are sight hearing smell taste and touch In this lab you will learn how to use your senses in order to observe a variety of science ldquoexperimentsrdquo

We tend to think of ourselves as good observers Yet there is much more to observation than meets the eye It takes concentration alertness to detail ingenuity and patience It also takes practice Try it yourself See how complete a description you can write about a familiar object ndash a burning candle Be ldquoscientificrdquo about this and start with an experiment This means you will observe a burning candle in a laboratory because the laboratory is a place where conditions can be controlled

Most of our observations tend to be qualitative like color texture sound etc In science while these observations are very important we need to realize that quantitative observations those that can be measured or quantified are often even more important After all these can be measured

How can we know what conditions in an experiment should be controlled Sometimes the important conditions are difficult to discover but an experiment can be meaningless unless the conditions that matter are controlled Here are some conditions that might be important but are not important in this one1 The experiment is done on the second floor2 The experiment is done in the daytime3 The room lights are on

Here are some conditions that might be important in your experiment1 The lab bench is near the door2 The windows are open3 You are standing close enough to the candle to breathe on it

Why is the second set of conditions important It is important because all three conditions relate to a common factor a candle does not burn well in a draft

Important conditions are often not as easily recognized as these A good experimentalist pays much attention to the discovery and control of conditions that are important

PurposeWhat is your reason for doing this lab What are you trying to discover learn

(2-3 sentences)

Pre-lab1 What is an observation2 What is the difference between a qualitative and quantitative observation3 Why are controls important in experiments

1

Procedure1 Obtain a candle beaker piece of foil and match2 Place candle on foil and begin observations3 Record your observations4 After you have observed your candle unlit light your candle5 Observe your lit candle record data 6 Cover candle with beaker and observe 7 Record your observations

Post-lab analysis1 How many observations did you make total2 Label your observations as either qualitative or quantitative3 Which type of observation did you make most often Why4 What are some things that you could do to improve your observational skills

ConclusionWhat did you learn from doing this lab activity What would you have changed

to make this a better experience Do you have any questions (2-3 sentences)

2

Lab 2 ndash Laboratory Techniques

Read lab 1A pp 702-705 in your textbook Holt Chemistry Visualizing Matter


(2-3 sentences)

Pre-lab1 What tools will you be using in this lab2 Where are the following items and how is each item used Eyewash station fire blanket fire extinguisher3 Copy the data tables below into your notebook (note that there are columns for finding masses with a triple or quad beam balance as well as with a digital balance)

Data Table 1Material Mass (g) on triple-beam Mass (g) on digital

balanceWeighing paperWeighing paper + NaCl

Data Table 2Material Mass (g) [tb]

Step 11Mass (g) [tb]Step 12

Mass (g) [dig]Step 11


Empty beakerBeaker + 50 mL water50 mL of waterBeaker + 100 mL of water100 mL of waterBeaker + 150 mL of water150 mL of water

ProcedureFollow the procedure as written in your book with one exception when you are asked to find the mass of water in steps 11 and 12 you will not only find the mass on a triple or quad beam balance but on a digital balance as well

Post-lab

3

1 Based on your observations which type of flame is hotter the flame formed when the air ports are open or the flame formed when they are closed What is the hottest part of the flame2 Which of the following measurements could have been made by your balance 342 g of glass 566672 g of aspirin or 0000017 g of paper Why3 Make a graph of mass versus volume for data from steps 11 and 12 The mass of water (g) should be graphed along the y-axis as the depended variable and the volume of water (mL) should be graphed along the x-axis as the independent variable Use as much of your graph paper as possible and use a separate color for the best-fit line for each of the sets of data4 When methane (natural gas) is burned it usually produces carbon dioxide and water If there is a shortage of oxygen the flame is not as hot and black carbon is formed Which steps in the lab demonstrate these flames5 Which is the most accurate method for measuring volumes of liquids a beaker or a graduated cylinder Explain why6 The density of water is equal to its mass divided by its volume Calculate the density of water using your data from step 11 (use your data from the triple-beam balance) Then calculate the density of water using your data from step 12 How do they compare



4

Lab 3 ndash Accuracy and Precision

Read lab 2A pp 708-711 of your textbook Holt Chemistry Visualizing Matter


(2-3 sentences)

Pre-lab1 Define accuracy and precision2 How is the uncertainty of a measurement expressed3 Copy data tables 1 and 2 from p 709 into your lab notebook

ProcedureFollow the procedure as written in the textbook

Post-lab 1 What is the uncertainty in a measurement made by each of these devices the ruler the 100 mL graduated cylinder the 24 mL graduated cylinder and the balance2 Calculate the volume of the 100 mL graduated cylinder up to its 50 mL mark (Hint V = r2h for a cylinder)3 Assume the accepted value for the volume of a graduated cylinder up to the 50 mL mark is 5000 mL Calculate the percentage error in your calculations from question 24 Subtract the volume of the water from the combined volume of the metal and the water to calculate the volume of the metal alone Subtract the mass of the water and cylinder from the mass of the metal water and cylinder to determine the mass for the metal then calculate its density Show all your work5 Record the metal-density calculations made by the other teams and calculate the average density of the unknown metal6 Compare your value and the class average of the unknown metalrsquos density with the densities for metals given in the handbook Determine the identity of the metal7 A store has a balance with a scale marked in gram units and each unit is divided in half by a smaller mark A student working in the store after school measured a sample mass as 5367 g using this balance What is wrong with this measurement



5

Lab 4 ndash Separation of a Mixture (percent composition) from Flinn Scientific ChemTopic Labs

6

7

8

9

10

Lab 5 ndash Using the Scientific Method with a ldquoBlack Boxrdquo (adapted from Lab-aids 100 Ob-scertainer kit)

One of the first topics one focuses on in any science class is that of the scientific method There is not just ldquoone formulardquo for the scientific method but there are general guidelines In many ways the scientific method is a cycle as pictured in the diagram below

For our purposes in chemistry class we will focus on the following steps1 Question ndash ldquowhat do I want to learn more aboutrdquo2 Hypothesize ndash research to help you make an educated guess and then answer your question3 Experiment ndash test your hypothesis4 Observe and record ndash make careful observations (both direct and indirect) and write down what happens5 Analyze ndash use your information to draw conclusions about your experiment Was your hypothesis correct6 Share results ndash explain your results by presenting your experiment observations and conclusions

In our ldquoblack boxrdquo activity we will be using careful observations to check the accuracy of our hypotheses These observations will be indirect meaning that we will use senses other than sight to determine the configuration of the black box In science many things cannot be seen directly therefore learning how to make indirect observations is very important

Our hypothesis will be an intelligent guess as to what is ldquogoing onrdquo inside the container and how it relates to the inside partitions There is a steel ball rolling around in the container and our goal is to determine what the partitions inside look like without actually seeing them


(2-3 sentences)

11

Pre-lab1 What is the scientific method (general description)2 What are the steps to the scientific method as described in the lab3 What is the difference between direct and indirect observations 4 Which type of observation will you be using in this lab and why

5 Set up your data collection as shown below Make sure there are enough spaces for 5 different ob-scertainers

Ob-scertainer ______

Hypothesis Re-test (final hypothesis) Actual model

Procedure1 Obtain an ob-scertainer and record the in your data section2 Carefully shake and tilt your ob-scertainer3 From the sound and path of the steel ball determine a hypothesis for the shape and location of the partitions within the ob-scertainer and record this in your first data blank4 Test this hypothesis by moving the ball along the partitions according to your hypothesis If you wish to make changes do so in the second circle This will be your final hypothesis5 Save the third circle to fill in after your teacher has revealed the actual configuration6 Continue testing at least four more ob-scertainers Some of them may be more difficult than others but do not spend more than 5 minutes on each DO NOT OPEN THE OB-SCERTAINERS

Post-lab questions analysis1 Were any of your hypotheses correct2 Which one(s) were not correct3 Why do you think some were harder to guess than others4 How did you use the scientific method in this experiment

Conclusion (should be at least 2-3 sentences)What did you learn from doing this lab activity What would you have changed

to make this a better experience Do you have any questions

12

Lab 6 - A Microscale Study of Chemical Changes (Adapted from Addison-Wesleyrsquos Microscale Chemistry)

Chemistry is a science that investigates changes in matter Chemical reactions are the changes chemicals undergo The changes you observe are called ldquomacroscopic changesrdquo Often these changes such as color change the formation of a solid or the formation of gas bubbles are visible Thus though we cannot see the atoms and molecules reacting we can see indications that chemical changes have taken place

Different atoms and molecules often react in different ways Chemistry attempts to explain macroscopic changes in terms of the behavior of atoms and molecules that is on the submicroscopic level You can use these different reactions to detect the presence of specific kinds of chemicals in mixtures

In this lab you will study some reactions of common chemicals contained in consumer products You will observe the notable macroscopic changes these chemicals undergo In later labs you will interpret these macroscopic changes in terms of submicroscopic changes the behavior of atoms and molecules As the name implies submicroscopic changes are changes we cannot see even with a microscope The essence of understanding chemistry is to infer from macroscopic changes the submicroscopic behavior of atoms and molecules

Pre-lab1 What is a macroscopic change2 What are three macroscopic changes that can indicate a chemical reaction is taking place3 What is a submicroscopic change4 Create a data table in your notebook in which you can record any macroscopic changes you might view when mixing chemicals as outlined on the experimental page

ProcedureSee experimental page for the actual procedure

Clean-upAvoid contamination by cleaning up in a way that protects you and your

environment Carefully clean the small-scale reaction surface by absorbing the contents onto a paper towel wipe it with a damp paper towel and dry it Dispose of the paper towels in the waste bin Wash your hands thoroughly with soap and water

13

Experimental pageUse small-scale pipets to put 2 drops of each chemical on the Xrsquos in the indicated

spaces below For the background contrast view the drops on the black and white backgrounds provided by the Xrsquos Stir each mixture by blowing air through an empty pipet Record what you see in your data table

a

XNaHCO3

+HCl

h

XNaHSO4

+Na2CO3

b

XHCl+Blue dye

i

XNa2CO3

+Phen

c

XBlue dye+NaOCl

Now add 1 drop of HCl

j

XPhen +NaOH

d

XNaOCl+KI

Now add 1 drop of starch

k

XNaOH+AgNO3

e

XKI+Pb(NO3)2

l

XAgNO3

+NH3

Place a drop of this in your lab NB

f

XPb(NO3)2

+CaCl2

m

XNH3

+CuSO4

g

XCaCl2

+NaHSO4

Be patient

n

XCuSO4

+NaHCO3

14

Post-lab1 Sodium hydrogen carbonate (NaHCO3) is baking soda When HCl is added to NaHCO3 carbon dioxide bubbles are formed What is the chemical formula for carbon dioxide and in what consumer product is this gas commonly found2 Which of the other mixings gave a similar result3 What gas do you think results from the mixing in Question 24 Sodium hypochlorite NaOCl is a common ingredient in household bleaches and cleansers What happens to the color of blue dye when both HCl and NaOCl are added5 A precipitate is a solid that separates upon mixing solutions Which reaction produced a very bright yellow precipitate6 Observe the scrap of paper you used to absorb the AgNO3 + NH3 mixture

What evidence do you see that indicates that silver compounds are light-sensitive

ConclusionTwo ndash three complete sentences to ldquowrap-uprdquo your lab

15

Lab 7 - Penny Density

IntroductionTodayrsquos penny is quite different from pennies minted 3 decades ago Before

1982 pennies were made of an alloy of copper An alloy is a solid solution consisting of atoms of different metals After 1983 pennies have been made with copper coating a core composed of another metal These differences in the composition of older and more recently minted pennies have resulted in differences in the pennyrsquos characteristics including its density or mass per unit volume In this experiment you will determine and compare the densities of pennies minted before 1982 and after 1983 We will use density data to try to identify the metal used in the core of pennies minted after 1983

Pre-lab1 Define the terms meniscus alloy and density2 What are some possible reasons for using a metal other than copper as the core of the penny now3 Copy the data tables below into your lab notebook Make sure to leave enough room to enter the correct informationTable 1 (pre-1982 pennies)

of pennies Mass (g) Total volume (mL) Net vol of pennies (mL)

5

1015

2025

Table 2 (post-1983 pennies) of pennies Mass (g) Total volume (mL) Net vol of pennies

(mL)510152025

Procedure1 Work with one set of pennies at a time Find the mass of 5 pennies from one set Record the mass in your data table

16

2 Add 5 more pennies to the first group Obtain the mass of these 10 pennies and record their mass in the appropriate space in your data table Repeat this procedure for the remaining pennies (5 at a time)3 Fill a 50 mL graduated cylinder to the 20 mL mark with tap water Be sure to use the bottom of the meniscus (the curve of water in a container due to surface tension) to measure the water level4 Still working with the same set of 25 pennies gently drop 5 of the pennies into the graduated cylinder Record the new water level in the appropriate space of your data table5 Add 5 more pennies to the graduated cylinder making a total of 10 pennies Record the water level in your data table Repeat this procedure for the remaining pennies (5 at a time)6 Discard the water Dry the pennies with a paper towel and either pass them to another group to use or return them to the teacher7 Repeat steps 1-6 using the 25 pennies in the other set of coins Record your data in the other data table8 Complete your data tables Find the net volume of each group of pennies by subtracting 20 mL (your starting volume) from the total volume recorded for each group Enter the net volume in the appropriate column

Post-lab1 Construct a graph of your results Let the y-axis reflect the mass of the pennies and the x-axis represent the net volume Plot the data for the pre-1982 pennies first Then draw the best-fitting straight line (the straight line that connects as many points as possible)2 On the same graph plot the data for the pennies minted after 1983 Draw the best-fitting straight line Use a different color for this graph3 Find the slope of each line Recall that slope = yx (also recall that you should use points on the line not necessarily data points)4 Find the density of copper from a resource book5 Is the density of copper similar to the slope of the line you determined for the pre-1982 pennies6 What is the density of the pennies minted since 1983 (this is the slope from your post-1983 graph)7 Compare the slope of the line for these pennies with the density listed for each metal in your resource Which element(s) have a density similar to your results (name at least two)8 Be sure to attach your graph to your notebook

Conclusion Write a conclusion statement in your notebook summarizing what you learned in this lab

17

Lab 8 ndash Rutherford Experiment

Pre-lab (you may need your textbook for some of this - pp 84-85)1 Describe the Rutherford gold-foil experiment2 What is an alpha particle3 Which atomic model did Rutherford disprove with his experiment4 What piece of the atom did Rutherford discover and how did he describe it5 The fact that the vast majority of alpha particles passed undeflected through the gold foil indicates what about atoms

IntroductionIn Rutherfordrsquos day Thomsonrsquos ldquoplum-puddingrdquo model of the atom was used to

describe the atom In this model Thomson proposed that the electrons of an atom were embedded in a positively charged ball of matter One of Thomsonrsquos students Ernest Rutherford quickly disproved this model

In Rutherfordrsquos experiment he shot alpha particles or positively charged helium ions at a thin piece of gold foil Had Thomsonrsquos model been correct many of the alpha particles would have been deflected What Rutherford found however was that most of the alpha particles shot at the foil passed straight through undeflected A very small number of particles were deflected some even backward He reasoned that only a very concentrated positive charge localized somewhere within the gold atom could possibly repel the fast-moving positively charged alpha particles sufficiently to reverse their direction of travel

Rutherford hypothesized that this localized region called the nucleus must have a large mass compared with the alpha particle or else the incoming particle would have knocked the positive charge out of the way He concluded that most of the gold foil was ldquoempty spacerdquo

Rutherford was able to determine the diameter of the nucleus using indirect methods After all the nucleus is a very small piece of an atom and an atom itself is too small to be measured with ordinary devices

In this activity you will also be using indirect methods to determine the diameter of a ldquonucleusrdquo In our case the ldquonucleusrdquo will be a marble You will be rolling ldquoalpha particlesrdquo (other marbles) at the ldquonucleusrdquo (target marble) From the ratio of collisions to trials you will determine the size of your nuclear marble Itrsquos a little bit like throwing snowballs at a car while yoursquore blindfolded If you have very few hits per number of trials the car will ldquofeelrdquo small

Wersquore going to develop two expressions for the probability of a hit between the rolling marble (RM) and the nuclear marble (NM) One expression of the probability (P) of a hit would be the ratio of the path width within which RM could roll and collide with the NM and the overall width (w) of the target area

P = path width overall widthP = 2(R+r)w (where R is the radius of the RM

NM r is the radius of the RM and R + r NMis the distance between the centers of RM

the RM and the NM)

18

If the number of target marbles is increased to N the probability of a hit is increased by a factor of N thus P = 2(R + r)Nw

The probability of a hit can also be determined experimentally by counting the number of trials and the number of hits such that

P = HTYou now have two expressions for the probability of a hit Assume that both of

the expressions are equivalent Also if the radius of the RM and NM are equal then R + r = d where d is the diameter of either one of the marbles

Procedure1 Place anywhere from 1-5 marbles in a 60 cm square target area (this is approximately an area of 3 tiles by 3 tiles)2 Roll marbles randomly toward the whole target area (Donrsquot look at the NM since you ldquocanrsquot really see it anywayrdquo) If a RM hits more than one NM it counts as just one hit If a RM goes outside the target area it does not count as a trial3 Continue rolling marbles randomly until your group has completed at least 200 trials Make sure you keep a record of trials hits in your lab notebook

Post-lab1 Determine the radius of your NM using equations from the introduction2 Actually measure the diameter of your NM (If you used more than one marble measure the diameter of the whole ldquonucleusrdquo)3 Calculate your percent variation (actual-calculated) x 100

actual

ConclusionDonrsquot forget a conclusion

19

Lab 9 - Conservation of Mass Lab Reaction in a Bag

IntroductionldquoPlop plop fizz fizz oh what a relief it isrdquo claims an old television ad for a

popular antacid Just what is in the tablet that is relieving the upset stomach What reaction is causing the fizzing Can you write a chemical equation for this process With a bit of investigating you will be able to discover answers to all these questions

As you learned in this chapter Antoine Lavoisier in the 18th century formulated the ldquoLAW OF CONSERVATIONrdquo of mass which states that matter can neither be created nor destroyed During a chemical reaction the bonds of the reactants are broken and rearranged to form new substances Because matter must be conserved these new substances or products must contain the same number and type of atoms as the reactants

In this investigation you will first verify the law of conservation of mass Then in the second part you will be given some known compounds to react

Pre-Lab 1 Define reactants2 Define products3 What are 6 indicators a chemical reaction has happened (see pp 18-19)4 Why is it necessary to use a zip-lock bag5 If the density of water is 100 gml and you measure a volume of 2500 mL What is the mass6 What is the common name for sodium bicarbonate7 What is the Law of Conservation of Mass8 Copy the data tables in your lab notebook

Materials1048736 Goggles 1048736 Apron1048736 Graduated Cylinder 1048736 Zip ndash lock plastic bag1048736 Electronic Balance 1048736 Antacid tablet1048736 Scoopula or spoon 1048736 Calcium Chloride1048736 Sodium Carbonate 1048736 Bromthymol blue indicator

ProcedurePART A~ Antacid tablet1 Put your goggles and apron on Measure 25 mL of tap water into a re-sealable plastic bag Flatten the air out of the bag and seal it Record its mass in data table 12 Record the mass of the antacid tablet in data table 13 Tip the bag sideways and while holding the bag pour 25 ml of water into one corner4 Place the antacid tablet in the bag but DO NOT LET IT TOUCH THE WATER5 Seal the plastic bag while still holding onto the tablet and the water in the corner of one of the bags6 Let the tablet drop into the water

20

7 Observe the reaction until it comes to a complete stop You will know this when the bubbling and fizzing stop8 Mass the bag and all the reactants and products and record the mass in data table 1

PART B ndash CaCl2 NaHCO3 and water1 Calculate the total mass of the bag and reactants in each reaction and record these values in the appropriate data table2 Using the formula for the density of water calculate the mass of the water Record the results in data table 23 Add 1 scoop of calcium chloride CaCl2 to the second plastic bag4 Add 1 scoop of sodium bicarbonate NaHCO3 to the bag and shake gently to mix5 Determine the mass of the bag and its contents Record this value in data table 26 Measure 25 mL of water into the graduated cylinder Add 5 drops of bromthymol blue indicator to the water7 Tip the bag sideways and while holding the solids in the bottom corner pour the liquids in the other corner Twist the bag if you like so the solids will not get wet from the waterbromthymol blue8 Keeping the trapped air to a minimum reseal the bag Hold the bag and let the liquid move from one end of the bag to the other until the content are mixed9 Observe the reaction until it comes to a complete stop Record your observations10 Record the mass of the unopened bag in data table 2 Clean up your work area and wash your hands before leaving the labObservationsData Table 1 - Do not forget unitsMass of bag and waterMass of antacid tabletMass of all reactants (mass of bag and water + mass of antacid tablet)Mass of bag and productsWrite observations here

Data Table 2 ndash Do not forget unitsMass of bag and dry reactantsVolume of waterMass of water(hint D = MV ~ pre-lab question)Mass of all reactants (mass of bag + mass of water + dry reactants)Mass of bag and productsWrite observations here

21

Table 3 ndash Physical properties of reactantsSubstance Property 1 Property 2 Property 3antacid tabletcalcium chloridebaking soda

Post-lab1 How do the values for total mass before and after each reaction demonstrate the law of conservation of mass

- If your values do not match what is a possibility for this discrepancy2 In part A did you observe a physical or chemical change to the antacid tablet What is your evidence for this observation3 In part B did you observe a physical or chemical change to the reactants (Calcium chloride and sodium bicarbonate) What is your evidence for this observation7 Bromthymol blue is an indicator that turns yellow when present in an acidic solution Was your bag acidic or basic and how do you know

Conclusion Donrsquot forget to write at least 2-3 sentences to conclude your lab

22

Lab 10 ndash Flame Tests (see p 720-723 of textbook)

Pre-lab1 Explain how and why different chemicals emit different colors of light2 How will you determine the identity of the salts in your unknown solution3 What might be a reason for using cobalt blue glass4 Set up an appropriate data table (see p 721)

ProcedureFollow procedure from the textbook except sketch the line spectrum you see rather than writing a wavelength in nm

Post-lab1 For 3 of your samples explain how the color of the flame and the line spectrum relate2 What ions were in your unknown solution and how did you make that decision3 How can a spectroscope help you to identify the components of a solution having several different metal ions4 A student observes three unknowns all of which are some shade of red How could he correctly identify the metal ions present in each

ConclusionDonrsquot forget to write at least 2-3 sentences to conclude your lab

23

Lab 11 ndash The Mendeleev Lab of 1869 ndash p 726 of textbook

Pre-lab1 Who is credited with creating the periodic table2 How was his arrangement of elements unique3 Copy the data table from p 727 into your lab notebook Be sure to leave enough space for all nine unknown elements

ProcedureFollow the procedure from the textbook

Post-lab1 Summarize your reasoning for the identity you assigned each unknown2 Describe any trends you saw in two of the families of elements


24

Lab 12 ndash Periodic Table Trends

In this lab you will investigate the properties of several elements on the periodic table and classify them as metals non-metals or metalloids

The periodic table can be divided into three rather distinct groups of elements Metals are to the left side of the periodic table They tend to be good conductors of heat and electricity They tend to have a high luster (are very shiny) are malleable (able to be bent or hammered into sheets) and ductile (able to be pulled into thin wires) Not all metals are malleable and ductile but most are Nonmetals are to the right side of the periodic table and tend to have properties opposite those of metals Nonmetals tend to be dull brittle (break easily when hit) and non-conductive Metalloids fall somewhere between metals and non-metals in spatial relation on the periodic table and in their properties

Pre-lab Questions1 In your lab notebook draw the following table Write each of the following properties under the appropriate heading Write the whole property not just the letter of the property

METALS NON-METALS METALLOIDS

a good conductor of heatb poor conductor of heat (insulator)c semi conductord shiny high lustere solids tend to be dullf malleableg brittleh ductilei good conductor of electricityj poor conductor of electricity

25

Procedure 1 In your lab notebook draw a table like the one shown below 2 Observe the appearance of each of the elements Record physical state color

luster and other observable characteristics3 Using the micro-conductivity tester determine whether the elements conduct

electricity If you observe carefully you might see that some are semi-conductors

4 To determine which elements are malleable place a single piece of the element on a paper towel and gently tap it with a hammer An element is brittle if it shatters when it is hit An element is malleable if it flattens when it is tapped

5 To test the reactivity with 1 M HCl label 9 wells with the symbols for each element Add 5 drops of the acid to each well Then add a small sample (approx 01 gram) of each element to the labeled wells Formation of bubbles of hydrogen is evidence that a reaction is occurring (Note not all reactions are vigorous so watch closely)

Element Appearance Conductivity Malleability Reactivity with HCl

Non-metal Metal or Metalloid

Copper

Silicon

Magnesium

Carbon

Nickel

Aluminum

Zinc

Sulfur

Tin

26

6 For the following elements try to decide if they are a metal non-metal or metalloid based on their appearanceElement Appearance Non-metal

Metal or Metalloid

Oxygen

Lead

Bismuth

Silver

Nitrogen

Antimony

Hydrogen

7 On the blank periodic table label the elements that we tested in lab From your observations label them as metal non-metal or metalloid Color each group (metals non-metals and metalloids) a different color

Post-labAnswer the following questions in your lab notebook Use complete sentences

1 Which elements displayed characteristics of metals2 Where are the metals located on the periodic table3 Which elements displayed characteristics of non-metals4 Where are the non-metals located on the periodic table5 Which elements displayed some characteristics of metals and some of non-

metals6 Do metallic characteristics of elements seem to increase from left to right or right

to left7 Do metallic characteristics seem to increase from top to bottom or bottom to top


27

Lab 13 - Creating ionic compounds

Ionic compounds are created when positively charged ions (cations) and negatively charged ions (anions) are attracted to each other While the ions themselves are charged particles compounds composed of ions are electrically neutral The ionic compounds are electrically neutral because the total number of positive charges in the compound are equal to the total number of negative charges Every ionic compound is composed of both cations and anions You will notice that most cations are metal atoms which have lost at least one electron while most anions are non-metals which have gained at least one electron

Ions from which these compounds can be composed are either monatomic containing only one atom or polyatomic containing more than one atom The charge of an ion is the charge on the whole ion regardless of whether the ion is monatomic or polyatomic In this activity we will be using models of ions to create and name ionic compounds

Writing formulas for ionic compounds is not difficult but it does require practice The number of cations needed to make the compound neutral is written as a subscript after the symbol for that cation (for example if you need 2 sodium ions you would write Na2) The number of anions needed to make the compound neutral is written as a subscript after the symbol for that anion (2 sulfur = S2 or 2 phosphate = (PO4)2)

Naming ionic compounds is fairly simple The cation is always written first in the formula and is therefore always named first The cation name is the same as the name of the element (if itrsquos monatomic) or the name of the polyatomic ion (if itrsquos a polyatomic ion) If the cation can have more than one charge as with iron a roman numeral is written after the cation name to show the charge of the cation For example Fe2+ would be written iron (II) and Fe3+ would be written iron (III)

The anion is named by dropping the end of the element name and changing it to ldquo-iderdquo For example when lithium is combined with fluorine you get the compound LiF The name for this compound would be lithium fluoride (Li has a +1 charge and F has a -1 charge)

Pre-lab1 What is an ion2 What is a cation3 What is an anion4 How do monatomic and polyatomic ions differ5 How do you change the name of an element to make it an anion name6 Copy the data table from the procedure into your lab notebook7 List the names of the polyatomic ions found in the table below (you may use

your book)

28

ProcedureUse the ion models to determine the formulas and names for compounds composed of the ions listed in the table below

Cation Anion Formula Compound Name1 Mg2+ Cl-

2 Na+ O2-

3 Fe2+ Br-

4 Al3+ PO43-

5 NH4+ NO3

-

6 Fe3+ SO42-

7 K+ S2-

Post-lab1 Which of the ions above have more than one possible charge2 Using your knowledge from the lab what would the formula of a compound

composed of copper (I) and sulfur look like What would the name of this compound be

3 Combine iron (II) and phosphate Write the formula and name4 Why do we use a roman numeral in some names of ionic compounds


29

Lab 14 ndash Formula of an Ionic Compound (Flinn lab)

30

Lab 15 ndash Molecular structure and VSEPR model

Pre-lab1 What is a Lewis structure and how is one determined2 What is the VSEPR model3 What is meant by polarity and how do polar and nonpolar bonds differ4 What are the basic shapes which a molecule can have5 Set up a table for your observations in your lab notebook (see the one in the

lab procedure for a guide)

IntroductionA single covalent bond is formed when tow atoms share a pair of electrons Each

atom provides one of the electrons of the pair If the two atoms are alike the bond is said to be nonpolar covalent If the atoms are not alike one exerts a greater attractive force on the electrons and the bond is polar covalent More than one pair of electrons may be shared resulting in a multiple bond

A group of atoms held together by covalent bonds is called a molecule Molecules can be either polar or nonpolar If the bonds are nonpolar the molecule is nonpolar If bonds are polar molecules can still be nonpolar if the charge distribution throughout the molecule is symmetrical A moleculersquos symmetry depends on its shape that is the positions in space of the atoms making up the molecule Some possible shapes are linear angular (bent) pyramidal and tetrahedral Other possible shapes can be found in chapter 6

Although we represent molecules on paper as being two-dimensional for convenience they are actually three-dimensional By building molecular models chemists come to understand the bonding shapes and polarity of even the most complex molecules

Procedure1 Obtain a molecular model building set Study the color code identifying the

different kinds of atoms2 Observe that the following atoms have one hole (bonding site) hydrogen

fluorine chlorine bromine and iodine The atoms with two holes are oxygen and sulfur A nitrogen atom has three holes and a carbon atom has four holes The shorter ldquobondsrdquo are for single bonds while the longer more flexible ldquobondsrdquo are for multiple bonds

3 Construct models of the molecules listed in your data table checking with your teacher along the way

4 Record your observations

31

Post-lab1 Which molecules were non-polar because all bonds were non-polar2 Which molecules had polar covalent bonds but were non-polar because of

symmetry3 Which two shapes appeared to produce polar molecules4 Name two types of substances that do not contain molecules with covalent

bonds

Conclusion

Data table exampleName Formula Structure Shape PolarityHydrogenWaterMethaneChlorineAmmoniaHydrogen fluorideEthyneDichloro-methaneNitrogenCarbon dioxideMethanolHydrogen peroxideOxygenHydrogen sulfide

Ethanol

32

Lab 16 - Paper Chromatography

IntroductionChromatography is used to separate mixtures of substances into their components

All forms of chromatography work on the same principle They all have a stationary phase (a solid or a liquid supported on a solid) and a mobile phase (a liquid or a gas)

The mobile phase flows through the stationary phase and carries the components of the mixture with it Different components travel at different rates Well look at the reasons for this further down the page

In paper chromatography the stationary phase is a very uniform absorbent paper The mobile phase is a suitable liquid solvent or mixture of solvents

Rf values Some compounds in a mixture travel almost as far as the solvent does some stay much closer to the base line The distance traveled relative to the solvent is a constant for a particular compound as long as you keep everything else constant - the type of paper and the exact composition of the solvent for example

The distance traveled relative to the solvent is called the Rf value For each compound it can be worked out using the formula

Rf = distance traveled by compound distance traveled by solvent

For example if one component of a mixture traveled 96 cm from the base line while the solvent had traveled 120 cm then the Rf value for that component is 96 12 = 080

Pre-lab1 What is chromatography2 What is a stationary phase (define and give an example)3 What is a mobile phase (define and give an example)4 What is meant by an Rf value and how is it calculated5 When drawing lines on your coffee filter to show where your dyes began why should you use pencil rather than ink

Procedure1 Coffee filters usually are round but its easier to compare your results if the paper is square So your first task is to cut the coffee filter into a square Measure and cut an 8x8 cm square from a coffee filter 2 Using a pencil (ink from a pen would run so pencil is better) draw a line 1 cm from the edge of one side of the paper 3 Make six pencil dots (or however many colors of candymarkers you have) along this line about 05 cm apart 4 Underneath each dot label the color of the candy marker you will test on that spot You wont have space to write the whole color name Try BMM for blue m amp m GS for green skittle or something equally easy 5 Space 6 drops of water (or however many colors you are testing) equally distant on a plate or piece of foil

33

6 Position one candy of each color on the drops Give the color about a minute to come off into the water Pick up the candy and throw it away 7 Dip a toothpick into a color and dab the color onto the pencil dot for that color Use a clean toothpick for each color Try to keep each dot as small as possible 8 Allow the filter paper to dry then go back and add more color to each dot a total of three times so you have lots of pigment in each sample 9 When the paper is dry fold it in half with the color sample dots on the bottom Ultimately you are going to stand this paper up in a salt solution (with the liquid level lower than the dots) and capillary action is going to draw the liquid up the paper through the dots and toward the upper edge of the paper The pigments will become separated as the liquid moves 10 Pour salt solution into a clean tall glass so that the liquid level is 05 cm (You want the level to be below the sample dots) Check this by holding the paper up against the outside of the glass Pour out a little salt solution if the level is too high 11 Once the level is correct stand the filter paper inside the glass with the dot side down and the edge of the paper wetted by the salt solution [Capillary action will draw the salt solution up the paper As it passes through the dots it will begin to separate the dyes You will notice some candy colors contain more than one dye The dyes separate because some dyes are more likely to stick to the paper while other dyes have a higher affinity for the salt water In paper chromatography the paper is called the stationary phase and the liquid (salt water) is called the mobile phase]12 When the salt water is 05 cm from the top edge of the paper remove it from the glass and place it on a clean flat surface to dry (before it dries record the distance that both the dye and the solvent moved for at least one of your candies markers so that you can complete post-lab question number 6)13 Prepare a second filter using food dyes Follow the procedure steps 1-414 Place one drop of each food dye on the corresponding dot and allow the filter paper to dry before following steps 9-12

Post-lab1 When the coffee filters are dry compare the results of chromatography for the different colors

a Which candies markers contained the same dyes (These are the candies that have corresponding bands of color)

b Which candies contained multiple dyes (These are the candies that had more than one band of color) 2 Can you match any of the colors with the names of the dyes listed on the ingredients for the candies (compare your first chromatogram with that of the food dyes)3 Were you surprised at any of the separations you saw Explain4 Do you think this same procedure would work for permanent markers Why or why not5 Tape the chromatograms into your notebook6 Determine the Rf value for one of the dyes Show your work

Conclusion

34

Lab 17 ndash Mole Relationships in a Decomposition Reaction

IntroductionOne of the most important applications of the mole concept is for expressing mole

relationships between substances in a chemical reaction To illustrate this let us consider the reaction between hydrogen and oxygen forming water

2H2(g) + O2(g) 2H2O(l)In this equation the formulas of all participants represent molecules The coefficients represent the relative numbers of each kind of molecule involved in the reaction The number of molecules is directly proportional to the number of moles Therefore we can say that 2 moles of hydrogen molecules react with 1 mole of oxygen molecules to form 2 moles of water molecules Each mole may be expressed in terms of a gram-molecular mass Converting the mole ratio into gram ratios shows that 40 g of hydrogen react with 320 g of oxygen and form 360 g of water This discussion is summarized in the equations below

Equation 2H2(g) + O2(g) 2H2O(l)Moles 2 1 2Molecules 2(602 x 1023) 1(602 x 1023) 2(602 x 1023)Grams 40 320 360Atoms 4(602 x 1023) 2(602 x 1023) 6(602 x 1023)

It can be seen that the total mass of product is the same as the sum of the mass of the reactants Also the total number of all reactant atoms is equal to the total number of product atoms in agreement with the Law of Conservation of Matter Note that the total number of moles or total number of molecules of product do not necessarily equal those of the reactants This is because atoms rearrange themselves into different combinations during a reaction

This experiment is designed to illustrate mole relationships in chemical reactions You will thermally decompose sodium bicarbonate (baking soda) The products are sodium carbonate water and carbon dioxide Decomposition refers to the breaking down of a compound into smaller compounds or even individual elements Thermal decomposition refers to the breaking down of a compound by using heat From the experimentally determined masses of the sodium bicarbonate you will (or should) be able to determine the mole ratio and the coefficients for a balanced equation

Pre-lab1 What is a mole2 What is a coefficient3 Write formulas for the following compounds sodium bicarbonate sodium

carbonate water and carbon dioxide4 Calculate the molar masses of each of the above compounds5 Define thermal decomposition6 Set up an appropriate data table (hint anywhere in the procedure where you

see the word ldquorecordrdquo will need a spot in a data table)

35

Procedure1 Weigh a clean dry crucible to the nearest 001 g and record2 Place 2 to 3 g of sodium bicarbonate in the crucible and weigh the crucible

and contents to the nearest 001 g Record3 Pace the crucible on a clay triangle which rests on an iron ring (see figure A)

Heat gently for 5 to 6 minutes Increase the intensity of the flame and heat strongly for another 3 to 4 minutes

4 Cool Crucible to room temperature and weigh Record5 Reheat the sample strongly for another 5 minutes 6 Cool reweigh and record If this mass is within +- 003 g the sample has

completely decomposed and you may begin your calculations If not repeat step 4 until the masses are precise

Follow-upCarbonates bicarbonates sulfites and bisulfites are examples of thermally

unstable compounds Carbonates decompose to yield carbon dioxide and a simpler compound as seen in the equation below

(heat)CaCO3(s) CaO(s) + CO2(g)

Post-lab1 Write an unbalanced equation to represent the decomposition of sodium

bicarbonate to sodium carbonate carbon dioxide and water vapor2 Determine the number of moles of sodium bicarbonate that were used in your

experiment 3 a Calculate the number of moles of sodium carbonate formed in your

experiment (hint yoursquoll first need to determine the mass of sodium carbonate formed)b Calculate the mole ratio of sodium bicarbonate to sodium carbonate (you will need to use your answers from 2 and 3a to determine this ratio)

36

c Write an equation for the decomposition reaction which is balanced according to your experiment (remember that the coefficients represent the mole ratio) It is okay if your equation is not ldquocorrectrdquo

4 a Write the correctly balanced decomposition equation for sodium bicarbonateb Use the correctly balanced equation to calculate the mass of sodium carbonate that should have been obtained by decomposing the original sodium bicarbonate c Calculate the percent error between the experimental and calculated values ( |calculated ndash experimental| calculated = percent error)

5 List the sources of error and indicate how the error affects your results6 Write an equation for the thermal decomposition of BaCO3


37

Lab 18 ndash Isotopic Pennies Relative abundance of ldquopenniumrdquo isotopes

Isotopes are atoms of the same element which differ in their numbers of neutrons The neutrons are contained in the nucleus of the atom along with protons Because the two isotopes are the same element by definition their nuclei must contain the same number of protons Only the neutrons differ Protons and neutrons each with a mass of approximately 1 amu are much more massive than electrons The mass number of the atom is defined as the number of protons + the number of neutrons Electrons are not accounted for because they have so little mass

mass number = number of protons + number of neutrons

Because each proton or neutron has a mass of 1 amu the mass of the atom in amu is approximately equal to the mass number Isotopes must have different mass numbers and therefore also different masses because of the different numbers of neutrons For example there are three different isotopes of carbon atoms carbon-12 carbon-13 and carbon-14 Each type has 6 protons but the numbers of neutrons are 6 7 and 8 respectively Their masses also differ and are approximately 12 amu 13 amu and 14 amu Pennies from before 1982 and after 1982 are like isotopes they are both worth 1 cent but they have different masses (do you know why)

It is important to understand that despite the difference in mass all isotopes of a single element are chemically alike The number of protons and electrons are the same and it is the number of electrons that primarily determine the chemical behavior of the elements

When the atomic mass of an element is reported it is actually an average of all the isotopes which exist for that element Similarly a mixture of pre-1982 and post-1982 pennies must have an average mass in between the mass of either type of penny Exactly what the mass is will depend on the relative amounts of the isotopes Some isotopes are more common in nature and are said to have a higher ldquonatural abundancerdquo When the amount of one isotope is expressed as a percent of the total atoms of that type it is known as a ldquopercent abundancerdquo In this lab you will work ldquobackwardsrdquo You will measure the mass of a sample of a mixture of ten of the pennies but you will not be able to look at them From this mass you will estimate andor calculate the abundance (how many) of each penny is in your sample

You will use this lab to become familiar with the ideas of isotopes and relative abundance and to understand how an average atomic mass can be used to determine relative abundance

Pre-lab Read the sections in your text on these topics and use them to help you in the lab

1 Isotopes of the same element have the same what They have different what

2 The atomic mass of an isotope is measured in amu and is nearly equal to the mass number Look up the three isotopes of hydrogen and sketch each of them in your lab notebook Also fill in the isotope symbol name the ldquowordrdquo name and the approximate mass (with units) of each of these isotopes

3 The atomic mass of an element can be found in the periodic table under the letter symbol for each element Look at some atomic masses Record the atomic mass of Boron Carbon and Nitrogen

38

Notice that these are not whole numbers as mass numbers are The atomic mass of an element is the weighted average of the masses of the isotopes of that element A weighted average reflects both the mass and the abundance of the isotopes For example the atomic mass of H is 10079 AMU This means that on average the mass of each H atom is 10079

4 Note that the average mass of hydrogen (10079 amu) is not close to 2 amu even though the three isotopes hve masses of about 12 and 3 amu respectively Based on this information which isotope must be most abundant (plentiful) Explain

5 Set up an appropriate data table

Procedure Begin by massing individual samples of both pre-1982 and post-1982 pennies as directed Return used pennies to the bin and randomly choose new pennies for each trial or measurement

1 Find the mass of one pre-1982 penny2 Find the mass of one post-1982 penny3 Find the mass of six (6) pre-1982 _______ divide this by six (6)________________4 Find the mass of six (6) post-1982 _______ divide this by six (6)________________5 Using the model that pennies are atoms of the element pennium which isotope must have more neutrons (pre- or post-1982) Explain6 Which isotope must have more protons Explain7 Obtain an empty container Find its mass

Bring the container to your teacher to get a 10 atom sample of the element pennium Pennium is of course a mixture of two different isotopes of pennies Without looking you will

- determine which isotope is more abundant in questions 8-10 (Do not answer those questions here)- calculate the exact percent abundance of each isotope in questions 11-15

8 Do not open the container Find its mass with the pennies inside ______________ Return the unopened container to your teacher9 Find the mass of the 10 pennies by difference and record

Post-lab1 What is the average mass of a penny in your ten-penny sample (show your calculation) This represents the ldquoatomic massrdquo of pennium2 Looking at your ldquoatomic massrdquo do you have more pre-1982 isotopes more post-1982 or about

the same Make a guess at the number of post-1982 pennies in your sample Explain fully

The exact percent abundance of each isotope can be calculated using the following equation (Note that in this equation the percent must be expressed as a decimal or fraction not a percent and is therefore sometimes called a fraction abundance ex 65 (percent) = 065 (decimal equivalent of fraction))

Equation for processing (use in step 13) [(Mass isotope 1)bull(fraction abundance isotope 1) + (mass isotope 2)bull (fraction abundance isotope 2) = Atomic Mass]

39

3 If the abundance is unknown (as it is here) ldquoxrdquo may be substituted for the fraction of one isotope We can also substitute (1 - x) for the fraction of the second isotope Do NOT substitute here Explain (a) why we can use (1 - x) for the second isotope and (b) can you use x-1 instead of 1 - x

4 Based on the masses of pennies you took in steps 1-4 what would be the best value to plug in for the mass of each isotope Explain and give a specific number to use in 5 for each isotope

5 (a) Now substitute into the equation above to algebraically calculate the percent abundances of the two isotopes of pennium You may not use trial and error

6 This question is NOT about YOUR sample (a) Noting that the various samples I handed out in class contained exactly 10 pennies what percent abundances are the only ones possible (b) What allows real samples of matter to have much more specific abundances such as 6917

7 (a) Now what is your best guess for the real percent and number of post-1982 pennies in your sample Explain briefly (b) Why is it unlikely that your calculated answer in step 13 came out ldquoexactrdquo to sig figs (Hint is there a difference between pennies and atoms)

Conclusion

Extra credit (No trial and error allowed show algebra) Chromium exists in the following isotopes 49941 amu (441 abundant) 519405 amu (8346 abundant) 529407 amu and 539389 amu What are the abundances of the last two isotopes

40

Lab 19 - Jelly Bean EquationsThe Law of Conservation of Matter states that matter cannot be created nor destroyed This applies to chemical equations The number of atoms of each type of element must be equal on both sides of an equation

Materials NeededReaction Grid4 different colors of jelly beans (16128amp 4 of the respective colors)

Pre-lab1 What is the law of conservation of matter and how does it apply to balancing chemical equations2 What is the difference between a coefficient and a subscript

DirectionshellipBalance the equations on your lab sheet by doing the following1 Write down a color of jelly bean to represent an atom of each

element in the equation Use the color that you have the most of to represent oxygen

2 Create the molecules in the equation using the jelly beans for each element in the compound

Be sure to put the correct number of atoms of each element on For example Ca(OH)2 equals 1 Ca 2 Orsquos and 2 Hrsquos

3 Place each molecule in the correct box on the ldquoReaction Gridrdquo You may not have to use all four boxes on the grid Once you have the original equation laid out on the grid you can only add more molecules like you have with the original Adding single jelly beans or taking them away is the same as changing a subscript and you CANNOT EVER change a subscript

4 Balance each equation by adding additional molecules until all types of atoms are equal For example of orange reactants must equal of orange products etc

5 Write down the balanced equation in your lab notebook Use the table provided as an example The number of molecules in each box (number of toothpicks of each molecule) is equal to the coefficient for that compound

41

EQUATIONS1 Al + O2 Al2O3 Balanced Equation______________________________

Al ____________O ____________

2 HgO Hg + O2 Balanced Equation______________________________

Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________

6 Fe + CuCl2 FeCl2 + Cu_________________________________Fe____________Cu____________Cl_____________

7 Mg + HCl H2 + MgCl2_________________________________Mg_____________H ______________Cl______________

8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________

9 HgO + Cl2 HgCl + O2_________________________________Hg____________O_____________Cl_____________

10 Ca(OH)2 + HNO3 Ca(NO3)2 + H20____________________________Ca_____________ H_______________O_____________ N_______________

42

Write in the color of the jelly bean here

Post-lab

1 What is meant by a balanced equation

2 How does the Law of Conservation of matter apply to chemical equations

3 How do you know that the equations you balanced are truly balanced

4 Why werenrsquot you allowed to just add or remove single jelly beans

5 On your reaction grid you had jelly bean ldquomoleculesrdquo to represent your reactants and separate jelly bean ldquomoleculesrdquo to represent your products In a real chemical reaction would the atoms (jelly beans) be different on each side or would they be the same Explain

6 The number of ldquomoleculesrdquo in each box of your reaction grid was equal to the _______________________ for that compound

Conclusion 2-3 sentences explaining what you learned through this activity

43

Lab 20 ndash Precipitation Reactions and Net ionic Equations

The majority of ionic solids like salts (KCl and NaCl) are soluble in water because the polar water molecules surround the individual ions of the salt Those that do not dissolve and go into solution form solid products called precipitates These precipitates have many colors and often help scientists identify what the precipitate is present In meteorology the term precipitation refers to meteorological phenomena such as rain or snow Precipitation in chemical solutions occurs when two chemicals react to form a product that is insoluble in water and falls out of solution like rain or snow A precipitate is a solid substance that separates from solution during a chemical reaction A precipitate can be identified by the cloudy milky gelatinous or grainy appearance it gives to the mixture

A barium sulfate precipitate can be produced by the reaction of barium chloride and sodium sulfate A chemical equation to describe the reaction is written and balanced like this

BaCl2 (aq) + Na2SO4 (aq) 2 NaCl (aq) + BaSO4(s)

Barium sulfate BaSO4 (s) is a common precipitate used as an X-ray contrast medium because it is insoluble in water an opaque to x-rays Typically a patient drinks an aqueous slurry of barium sulfate just before he is x-rayed The precipitate coats his stomach and intestines These organs then show up on the x-ray film in vivid contrast aiding the doctorrsquos diagnosis Notice the reaction that forms BaSO4 is a double-replacement reaction in which the cations and anions of the reactants trade partners to form the products

To write a total ionic equation rewrite all aqueous substances as their component ions and keep all solid substances unchanged

Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2

(aq) 2Na+(aq) + 2Cl-

(aq) + BaSO4(s)

Cancel all components of the reaction that are identical on both the reactant and product side of the reaction These are called spectator ions Write the net ionic equation by rewriting the reaction equation including only those reactants and products that change in the reaction

Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44

Always check to see that your net ionic equation is balanced

When doing these reactions involving ionic compounds remember that they are made of positive and negative ions held together by the attractive electrostatic forces that occur between oppositely charged particles In water soluble ionic compounds break apart completely into their respective ions Example NaCl (s) when put into water yields Na+ (aq)

and Cl- (aq) and AgNO3 also dissociates in water to form these respective ions Ag+

(aq) and N03

-(aq) It turns out that when these two solutions of sodium chloride and silver nitrate are

mixed a solid falls out and precipitation occurs The new mixture still contains Na+(aq) and

N03- (aq) and the newly formed precipitate is AgCl (s) How do we know that AgCl forms a

solid precipitate Remember to reference the solubility pyramid I use that helps you decide what will and wonrsquot go into solution (fig 1)

Fig 1 In this experiment you will mix 7 different ionic solutions in all possible combinations to determine which combinations result in precipitate formation Based on your results you will write complete ionic equations and net ionic equations for each reaction that has takes place Use your solubility chart to determine which compounds yield precipitates While the lab focuses on the solubility of different compounds my purpose in having you do this activity is to give you more practice looking at chemical reactions writing formulas naming inorganic compounds and describing chemical changes with equations

Pre-lab

1 In chemistry how is precipitate defined2 What characteristics can help you identify a precipitate

3 What is a spectator ion

4 What is a net ionic equation How does it differ from a complete ionic equation

45

5 Set up an appropriate data table (see figure 2 below)

Procedure In this experiment you will mix 7 different ionic solutions in a well plate in all 49 possible combinations to determine which combinations result in precipitate formation Based on your results you will write complete and net ionic equations for each reaction that creates a precipitate Use the solubility chart that is represented by Fig 1 above to compare your lab results with the expected results You will be combining solutions containing the dissolved ionic substances below In each test you will need to add 2 drops (Donrsquot make a Mess) of the first solution to a well plate Then add 2 drops (Donrsquot make a Mess) of the second solution a drop at a time Whenif you see the formation of a precipitate you have witnessed a reaction and will need to write a balanced chemical equation for that reaction You will be required to (a) describe the precipitate (b) find the correct formula for the ionic products (c) write and balance the entire equation for each reaction you witness and (d) write and balance the net ionic equation Chart out your chemical tests in an organized table similar to the fig 2 and then write the reactions underneath Solutions you will have available sodium sulfate Na2SO4

sodium chloride NaClsilver nitrate AgNO3

sodium iodide NaIlead nitrate Pb(NO3)2

ammonium carbonate (NH4)2CO3

calcium chloride CaCl2

Presenting your data Make a table which has columns and rows headed by the formulas of each of the solutions to be tested As you mix chemicals you will report the results from each of those combinations in the ldquoboxrdquo on the table which lies at the intersection of the column and row labeled with those two substances If a precipitate forms describe its physical characteristics in the box If no precipitate forms mark NR in the box

Na2SO4 NaCl AgNO3 NaI Pb(NO3)2 (NH4)2CO3 CaCl2

Na2SO4 xNaCl xAgNO3 xNaI xPb(NO3)2 x(NH4)2CO3 x

46

CaCl2 xFig 2

Make sure you include in your lab a description of any precipitates and the chemical compounds that make up the reactants products the full ionic equation and the net ionic equation with (aq) and (s) designations

Post-lab1 For each of the wells in which a precipitate occurred

a Write the complete balanced equation for the reaction being sure to include (aq) or (s)

b Write the complete ionic equation for the reactionc Write the net ionic equation for the reaction

2 What conclusions can be drawn from your observations List any similarities and differences in the physical behavior (ie color texture) of the precipitates as compared to their formula

3 Some heavy ions that precipitate out of solutions are used for specific purposes because of this insolubility Barium sulfate is an example It is used as a darkening compound for x-rays since it shows as a dark outlined area that might help locate abnormalities in the upper and lower gastrointestinal tracts Explain how silverrsquos ability to make a precipitate when activated by light is used in our every day life

Conclusion

47

Lab 21 - Stoichiometry and Gravimetric Analysis ndash lab 10B on p 744

Read your textbook (pp 744-747) for an introduction to stoichiometry and gravimetric analysis

Pre-lab1 Explain gravimetric analysis2 What are the reactants being used in this lab3 What are the formulas for these reactants4 Write a balanced double-displacement reaction for these substances5 How is percentage error calculated6 Copy the data table from p 745 into your lab notebook

ProcedureFollow the procedure as outlined on pages 746-747 of the text Instead of using a

drying oven we will be leaving our samples on the lab table to dry overnight

Post-lab1 From pre-lab question 4 determine the precipitate from the reaction2 Calculate the mass of the dry precipitate3 Calculate the moles of the dry precipitate4 How many moles of sodium carbonate were present in your original 15 mL

sample (hint use the mole-ratio from the equation)5 There was 030 mol of strontium chloride in every liter of solution Calculate the

number of moles of strontium chloride that were added Determine whether the strontium chloride or sodium carbonate was the limiting reactant

6 How many grams of sodium carbonate were present in the 15 mL sample (use question 4)

7 Assuming you were given a 05 M solution of sodium carbonate the theoretical yield would equal 0795 g for every 15 mL Calculate your percentage error

Conclusion Donrsquot forget a 2-3 sentence conclusion

48

Lab 22 - Heat of Fusion of Ice

Introduction When a physical or a chemical change takes place energy is either given off or

absorbed This energy is usually in the form of heat When heat is given off the change is exothermic If heat is absorbed the change is endothermic It is important for chemists to be able to measure these changes in heat Most measurements are made with a device called a calorimeter The technique used in measuring heat changes is called calorimetry A simple calorimeter can be constructed by placing a styrofoam cup in a beaker Styrofoam is an excellent insulator that absorbs heat very slowly More sophisticated calorimeters have been developed where very precise measurements are required When two bodies at different temperatures come in contact with each other heat flows from the warmer body to the colder body This exchange of heat will continue until the two bodies are at the same temperature In the calorimeter heat is exchanged between the substance to be measured and water By making direct measurements of the temperature of the water it is possible to compute the heat gained by the water and therefore the heat lost by the body being measured The specific heat capacity of water the amount of energy required to raise the temperature of 1 g of water by 1oC is equal to 418 JgoC and is represented by the letter ldquocrdquo in the equation q = mcT In this experiment you will measure the amount of heat required to melt ice The amount of heat required to melt 1 gram of ice is called the heat of fusion In this experiment the heat lost by the hot water will be equal to the heat gained by the ice in the process of melting The following relationships will be used in this experiment

Heat lost by hot water = heat gained by ice

Materials Styrofoam Cup Ice Bunsen Burner and StrikerRing Stand Ring Wire GauzeThermometer Crucible Tongs 400ml Beaker

Pre-lab1 What is the difference between an endothermic and an exothermic reaction2 What device is used to measure changes in heat3 Of what will our simple calorimeter be composed and why4 What is heat of fusion5 What is specific heat capacity and what is that value for water6 Copy the data table into your lab notebook

49

Procedure1 Heat 300ml of water to a temperature of 50˚C Note This is below boiling2 Transfer 150ml of this heated water to the Styrofoam cup Record this volume

(V1) on your data table 3 Measure and record the temperature (T1) of the heated water that is in the

Styrofoam cup Immediately add 2 to 3 ice cubes to the heated water 4 Gently stir the ice water mixture with the thermometer The cup should

contain ice at all times Therefore if the last of the ice is about to melt add another ice cube

5 Monitor the temperature of the ice water mixture as you stir Continue stirring (and adding ice if necessary) until the temperature evens off (no longer drops) Record this final temperature (T2)

6 Using tongs slowly remove the un-melted ice Allow any water from the tongs and ice to drip back into the cup Measure and record the final volume of water in the Styrofoam cup (V2)

Data Table Remember UnitsVolume Temperature

Initial V1 T1

Final V2 T2

Post-lab SHOW WORK1 Using the known density of water (1gml) find the mass in grams (m1) of the

original volume of water (V1)2 Find the volume in milliliters of the water resulting from the melted ice

(Vice = V2 - V1) 3 Find the mass in grams (m2) of the volume of water resulting from the melted ice4 Find the change in temperature of the water (ΔT = T1 - T2 )5 Calculate the heat lost by the original mass of water using q = mcΔT Note The

specific heat of water is 418 Jg˚C6 Find the heat of fusion of the ice used in this experiment (ΔHfus = qm2)7 Convert the ΔHfus from Jg into kJmol using the molar mass of H2O8 Find your percent error by comparing your ΔHfus in kJmol to the true value of

601kJmol error = (true value ndash experimental value) true value X 1009 List a minimum of three possible sources of error in this experiment10 How might the use of a ldquorealrdquo calorimeter reduce your percent error11 One source of error is the flow of heat between the water in the cup and the

surrounding Explain how this error is reduced by starting with the water at about 50˚C

12 In what way does a calorimeter make use of the law of conservation of energy13 Is the process of fusion exothermic or endothermic Explain using evidence from

your experiment14 What is the difference between heat and temperature

50

Lab 23 - Graphing a Heating Curve for Water

Materials

safety glasses lab coat or apronstopwatch or timer hot platesmall beaker icethermometer plastic thermometer clampgraph paper

IntroductionThe first law of thermodynamics basically states that energy can be transformed (changed from one form to another) but cannot be created or destroyed This leads into the concept of how different substances can change from one phase to another by absorbing or releasing energy When the system is heated energy is transferred into it In response to the energy it receives the system changes for example by increasing its temperature A plot of the temperature versus time is called the heating curve

Water is a common substance Ice is the stable phase below 0oC Both solids and liquids coexist at 0oC When heat is put into the system more solid will melt Thus the temperature does not change The normal boiling point is 100oC As heat is absorbed some water will boil off but the temperature is kept at 100oC This change in temperature may be observed and measured against time in an effort to visualize the heat curve for water

Pre-lab1 What is a heating curve2 Explain the first law of thermodynamics3 Copy the data table into your notebook4 Why do you think you should keep the thermometer bulb from touching the

bottom of the beaker

Procedure1 Put on safety goggles and lab coat or apron2 Use the data chart provided to record time and temperature The time column

starts with 0 The temperature column is blank You will record the temperatures in the temperature column during the investigation

3 Fill the small beaker with ice Insert the thermometer Wait 2 minutes Observe and record the starting temperature (0 time) in the data table

4 Place the beaker of ice on the hot plate Position the thermometer in the clamp so that the bulb of the thermometer does not touch the bottom of the beaker

5 Turn the hot plate on high and start the timer After 30 seconds record the thermometer reading without removing the thermometer from the beaker (DO NOT TOUCH THE HOT PLATE )

6 Continue to record the temperature on the chart every 30 seconds7 Make a note when the ice has melted and when the water begins boiling

51

AnalysisWrite your data in the following table

Time Temperature

Post-lab1 Prepare a graph from your data that includes the following information

a Label the x-axis with the time (in minutes) This is your independent variable Label the y-axis as temperature (in degrees Celsius) This is your dependent variableb Plot your points using your recorded datac Label the 5 areas on your graph solid (S) liquid (L) gas (G) freezing pointmelting point FPMP and condensationboiling point (CPBP)d Trace with colored pencils the following parts of the line on your graph slowest molecular motion (in red) fastest molecular motion (in green)e DONrsquoT FORGET TO TITLE YOUR GRAPHf Your graph should look like stair steps not a straight line

2 Explain what is happening to the water molecules in the flat areas of the line on your graph during the phase changes from solid to liquid and liquid to gas3 When the ice is melting is it releasing heat or absorbing heat Explain your answer4 If you put the liquid water into the freezer and recorded its temperature as it refroze would it be absorbing heat or releasing heat Explain your answer

Explore Further (for extra credit)

Research what is occurring when you have a fever What part does water play in regulating your body temperature What happens to the chemical bonds of enzymes when exposed to too much heat

52

Lab 24 ndash Hessrsquos Law and Enthalpy of Formation

Introduction

Most chemical reactions either use heat from the environment or release heat into the environment The amount of heat released or absorbed when 1 mole of compound is made from its elements under standard conditions is known as standard enthalpy of formation and is symbolized Hf When heat is released the reaction is said to be exothermic The heat produced in an exothermic reaction appears as one of the products and the standard enthalpy is negative When heat is absorbed the reaction is said to be endothermic The heat absorbed in an endothermic reaction appears as one of the reactants and the standard enthalpy is positive

In this experiment you will measure and compare the quantity of heat involved in three chemical reactions You will be using this information to prove Hessrsquos law which states that the overall enthalpy change in a reaction is equal to the sum of the enthalpy changes of the individual steps in the process Essentially two of the reactions when added together should equal the other reaction The hope is that the sum of the heats of formation of the first two reactions will be equal to the heat of formation of the third reaction

In this experiment a coffee cup will again serve as our calorimeter We will assume that the enthalpy of formation is used to change the temperature of the aqueous solution only Any small heat losses to the surroundings will be neglected We will also assume that the aqueous solution has the same heat capacity as water 1 calgoC or 418 JgoC

The reactions we will be comparing in this lab are as follows

1 Solid sodium hydroxide dissolving in water to form an aqueous solution of ions

NaOH(s) Na+(aq) + OH-(aq) + x1cal

2 An aqueous solution of sodium hydroxide reacts with an aqueous solution of hydrogen chloride to form water and an aqueous solution of sodium chloride

Na+(aq) + OH-(aq) + H+(aq) + Cl-(aq) H2O(l) + Na+(aq) + Cl-(aq) + x2cal

3 Solid sodium hydroxide reacts with an aqueous solution of hydrogen chloride to form water and an aqueous solution of sodium chloride

NaOH(s) + H+(aq) + Cl-(aq) H2O(l) + Na+(aq) + Cl- (aq) + x3cal

53

Pre-lab1 Define enthalpy of formation2 Define Hessrsquos law3 What are the differences between an exothermic and an endothermic reaction4 What specific heat capacity c will be used to calculate the enthalpy of formations for the aqueous solutions5 Set up a data table You will need room for three reactions Mass volume of NaOH volume of HCl T1 and T2 for each of the three reactions (you will not fill in all spaces for all reactions)

ProcedureCAUTION SODIUM HYDROXIDE IS EXTREMELY CORROSIVE TO THE SKIN AND MAY CAUSE BLINDNESS IF IT GETS INTO YOUR EYES

Part I1 Put 200 mL of cool tap water into a coffee cup Stir CAREFULLY with a thermometer until a constant temperature is reached (about room temperature) Measure this temperature as accurately as possible and record it as T1

2 Obtain a sample of about 4 g of sodium hydroxide and determine its mass to the nearest 001 g Record this mass Do not handle the sodium hydroxide with your fingers Since sodium hydroxide becomes moist when it is in contact with the open air be sure to keep the lid closed when you are not using it

3 Pour the solid sodium hydroxide into the water in the coffee cup Place the thermometer into the solution and stir gently but continuously until the sodium hydroxide is dissolved Record the extreme temperature reached as T2 Before proceeding to part II discard the solution and rinse the cup thoroughly with water

Part II1 Measure 100 mL of 10 M HCl into the coffee cup Record the exact volume Measure 100 m of 10 M NaOH into a 250 mL beaker and record its exact volume Both of these solutions should be at or slightly below room temperature Check this with the thermometer and record their temperatures as T1

2 Add the sodium hydroxide solution to the hydrochloric acid solution in the coffee cup Mix quickly and record the extreme temperature reached as T2

3 Discard the solution and rinse the cup before proceeding to Part III

54

Part III1 Repeat steps 1 2 and 3 of part I but substitute 100 mL of 1 M HCl and 100 mL of tap water for the 200 mL of tap water in step 1

2 Discard the solution and rinse the cup thoroughly

Calculations and post-lab questions1 For each part calculate the following

a the change in temperature of the water or water solutionb the amount of heat absorbed by the solution in joulesc the number of moles of NaOH used (realize that 1M NaOH has 1 mol of

NaOH per 1 L of solution)d the amount of heat evolved (part b) per mole of NaOH used (part c)

2 Express the above results as enthalpy of formation Hf (recall that enthalpy of formation should be expressed as Jmol with a sign designating whether the reaction is endothermic or exothermic)

3 Write net ionic equations for reactions 2 and 3

4 In part I H represents the heat evolved as solid NaOH dissolves Look at the net ionic equations for parts II and III and make similar statements as to what the enthalpy of formation for parts II and III represent

5 a Compare H3 with (H1 + H2) and explain in terms of your answer to question 4

b Calculate the percentage difference between H3 with (H1 + H2) assuming H3 is the accepted value

6 Suppose you had used 8 g of NaOH(s) in part Ia how would this have affected the change in temperatureb what would have been the number of joules evolved in your experimentc what effect would this have had on your calculations of H1 the heat evolved per mole

Conclusion

55

Lab 22 - Virtual chemistry lab for acid-base titration ( Modified from httplrseduiucedustudentsmihyewonchemlab_instructionhtml)

Have you seen an acid or base solution If your answer is no you must be an alien because we earth people encounter acids and bases in everyday life Orange juice which we drink everyday is a citric acid solution Vinegar Acetic acid Commercial antacid Magnesium hydroxide (base) Household cleaning products Ammonia (base)Hmmm

What is the common property of orange juice and vinegar Sour taste right Acids have a sour taste and acid solutions are capable of dissolving certain metals such as iron and zinc In contrast bases have a bitter taste and slippery feel

What is acid-base exactlyAcids were defined by the Swedish chemist Arrhenius as substances that when dissolved in water produce hydrogen ions (H+) For example gaseous hydrogen chloride reacts with water to give hydrochloric acid and increases the amount of hydrogen ion in the water

Bases are also defined as substances that when dissolved in water yield hydroxide ions (OH-) For example sodium hydroxide (NaOH) dissolves in water and increases of the amount of hydroxide ions in the water

cf The symbol (g) is used to designate the gaseous state (s) for the solid and (aq) for the aqueous state

56

How can we know its an acid or baseTasting a lab chemical is very dangerous and you dont want to taste a liquid to determine whether it is an acid or not Then what would you do

One easy way is using indicators One familiar example is a litmus indicator Litmus indicators change the color from blue to red when added to acid solutions In contrast base solutions change litmus indicators in color from red to blue Many natural dyes found in fruits vegetables and flowers act as indicators too For example red cabbage extract is red in acidic solution and blue in base solution

However the indicators cannot show which acid solution is more acidic than the other acid solutions or which base solution is more basic than the other base solutions Then what would you do to measure the acidity of solutions

Scientists use the pH scale to determine how acidic or basic a solution is pH is a measure of the hydrogen ion concentration of a solution and is defined as the equation

Usually the pH scale goes from 0 to 14 and acids are found between 0 to 7 and bases are from 7 to 14 The middle point of the pH scale is 7 and distilled water is exactly 7 In other words water is neither acidic nor basic but neutral The lower pH value an acid solution has the more acidic it is In contrast the higher pH value a base solution has the more basic it is According to the pH values some common acids and bases are arranged in the following figure Now can you tell which one is more acidic lemon juice or vinegar

57

What would happen if an acid and a base were mixed upLets think about it this way What would happen if a hydrogen ion (H+) from an acid reacted with a hydroxide ion (OH-) from a base Thats right Water would be produced

If the spectator ions (other than H+ and OH- ions) from the acid and the base are put back into the equation it would read for example

showing that an acid reacts with a base to yield water plus an ionic compound called a salt This acid-base reaction is called a neutralization reaction

58

What is titrationUsing the neutralization reaction you can determine the concentration of an acid or a base solution As shown in the previous equation one hydrogen ion from an acid reacts with exactly one hydroxide ion from a base to produce a water molecule If adding 100 hydroxide ions to an acid solution makes it a neutral solution (only water and salt) there must be 100 hydrogen ions in the original acid solution and you can calculate the concentration of the acid solution

To titrate an unknown acidbase solution take a certain amount of the unknown solution and add a standard reagent of the known concentration carefully until the neutralization reaction is completed This point where the number (or mole) of hydrogen ions and hydroxide ions are equal is defined as the equivalence point To determine the equivalence point scientists use an indicator or a pH meter With the data of volume of the standard reagent used the concentration of the unknown solution can be calculated This whole process is called titration

Titration procedure First you need to choose volume of an unknown acid or base solution and put it in an Erlenmeyer flask

Second fill a burette with a standard reagent of known concentration and read the initial volume of the solution Of course if you put an acid in the Erlenmeyer flask you need to put a base in the burette and vice versa A burette is a good apparatus for the determination of an equivalence point in acid-base titration because you can accurately read the volume of solution used

Third add a couple of drops of an indicator in the flask for titration An indicator is a soluble dye that changes its color noticeably over a fairly short range of pH Different indicators show color changes at different pH values and it is important to determine an indicator to be used according to the expected equivalence point

If a pH meter is available put a pH electrode in the flask

Fourth slightly open the cork of the burette and add the standard reagent into the unknown solution Around the

59

expected equivalence point of the titration you need to drop the solution very slowly and mix the solutions very well because around the equivalence point just one drop of solution from the burette can make a radical pH change in the mixed solution If the color of the solution in the Erlenmeyer flask changes record the volume of the solution in the burette and add a few drops of the solution to make sure the equivalence point you found is correct

Finally using the data from your acid-base titration you can calculate the concentration of the unknown solution The equation for this procedure is as follows (Here M means molarity (concentration) of solution and V means volume of solution)

For example if you choose 100 mL hydrochloric acid solution as a concentration-unknown solution and it takes 100 mL of 0100 M sodium hydroxide solution to titrate the concentration of the hydrochloric acid is 0100 M

If you want to use a polyprotic acid or base (which can donate two or more hydrogen or hydroxide ions per molecule) for titration you need to multiply the molarity of the solution by the number of hydrogen or hydroxide ions it can donate per molecule

Pre-lab1 Define the following terms equivalence point titration and standard reagent2 What is a burette A pipette3 How can the concentration of an unknown acid or base be determined if you know the volume of standard base or acid with which the unknown is titrated4 Write equations for the reactions of solutions of hydrochloric acid with sodium hydroxide and vinegar (acetic acid ndash CH3COOH) with sodium hydroxide

60

ProcedureGo to httplrseduiucedustudentsmihyewonchemlab_experimenthtml and read through the procedurePart A You will choose a strong acid (either HCl or HNO3) and titrate it with a strong base (NaOH)Part B You will choose a weak acid (acetic acid) and titrate it with a strong base (NaOH)

Post-lab1 At what point in the titration did your mixture experience the greatest pH change in the shortest time2 If you titrate 30 mL of an unknown concentration of hydrochloric acid with 33 mL of 05 M NaOH what is the concentration of your unknown acid3 Why is phenolphthalein such a good choice for acid-base titrations

Conclusion

61

Lab 26 ndash Elasticity of Gases Boylersquos Law

Robert Boyle (1627-1691) an Irish chemist made several contributions to physics and chemistry the most notable of which is Boylersquos Law which details the relationship between the pressure of a gas and the volume it inhabits

Pressure is defined as an applied force per unit area and is given by the formula P = FA The SI unit for pressure is the pascal (Pa) although you may be more familiar with pounds per square inch (psi) torr or millimeters of mercury (mm Hg) There are several different devices which can be used for measuring pressure For example when measuring tire pressure you would use a pressure gauge A barometer is a special form of pressure gauge used to measure atmospheric pressure

In the experiment we will be doing a given quantity of gas will be trapped in a syringe The pressure on this gas will then be increased by placing weights (books) on top of the plunger of the syringe The total pressure acting on the gas consists of the weight of the books plus the weight of the atmosphere Ptotal = Pbooks + Patm

Pre-lab1 Who was Robert Boyle2 Boyle determined the relationship between what two aspects of gas at the same temperature3 What is pressure4 What types of devices are used to measure pressure5 What are several units used for measuring pressure6 Leave space for Part I observations and create a data table similar to the one below for Part II

Pressure ( books)

Vol 1 (mL) Vol 2 (mL) Vol 3 (mL) Avg vol (mL)

123456

ProcedurePart I ndash Qualitative ObservationsRecord all observations under Part I1 Take the barrel of the syringe in one hand and the plunger in the other Place the plunger in the syringe and push down on the plunger (be sure the cap is on and make sure you donrsquot press too hard) Record your observations2 Place a piece of string alongside the plunger and push the plunger to the bottom of the syringe again making sure the cap is on the syringe Remove the string and then attempt to remove the plunger from the syringe Record your observations

62

Part II ndash Quantitative Observations

1 Set the plunger at the highest mark of a dry syringe by inserting the piece of string as before Remove the string and place the sealed tip of the syringe into the block of wood which is cut out for it Clamp the syringe stopper arrangement in an upright position as shown in the diagram 2 Record the mass of one textbook3 Carefully center a textbook on top of the plunger Read as precisely as possible the volume of gas trapped in the syringe when a load of one book is on the plunger Be sure to record the uncertainty that you estimate is associated with each reading Record the pressure in books and the volume of gas in milliliters Repeat the procedure twice by removing the book and replacing it Read and record the volume each time the book is replaced4 Repeat step 3 for each of the 5 remaining books Do not worry if the syringe does not return to the original volume when the books are removed This is not due to air loss but to friction between the plunger and the syringe Do not attempt to correct for it

Post-lab

63

Lab 22 -Virtual chemistry lab for acid-base titration (Modified from httplrseduiucedustudentsmihyewonchemlab_instructionhtml)

Have you seen an acid or base solution

What is acid-base exactly

What would happen if an acid and a base were mixed up

What is titration

Titration procedure

Procedure1 Obtain a candle beaker piece of foil and match2 Place candle on foil and begin observations3 Record your observations4 After you have observed your candle unlit light your candle5 Observe your lit candle record data 6 Cover candle with beaker and observe 7 Record your observations

Post-lab analysis1 How many observations did you make total2 Label your observations as either qualitative or quantitative3 Which type of observation did you make most often Why4 What are some things that you could do to improve your observational skills



2




(2-3 sentences)










Post-lab

3




4




(2-3 sentences)






5


6

7

8

9

10







(2-3 sentences)

11









12









13



a

XNaHCO3

+HCl

h

XNaHSO4

+Na2CO3

b

XHCl+Blue dye

i

XNa2CO3

+Phen

c

XBlue dye+NaOCl


j

XPhen +NaOH

d

XNaOCl+KI


k

XNaOH+AgNO3

e

XKI+Pb(NO3)2

l

XAgNO3

+NH3


f

XPb(NO3)2

+CaCl2

m

XNH3

+CuSO4

g

XCaCl2

+NaHSO4

Be patient

n

XCuSO4

+NaHCO3

14




15






5

1015

2025


(mL)510152025


16




17












the RM and the NM)

18







actual


19









20




21





22






23






24







25








Copper

Silicon

Magnesium

Carbon

Nickel

Aluminum

Zinc

Sulfur

Tin

26


Metal or Metalloid

Oxygen

Lead

Bismuth

Silver

Nitrogen

Antimony

Hydrogen







27








your book)

28



2 Na+ O2-

3 Fe2+ Br-

4 Al3+ PO43-

5 NH4+ NO3

-

6 Fe3+ SO42-

7 K+ S2-





29


30













31



bonds

Conclusion


Ethanol

32












33





Conclusion

34











35













36





37












38













39






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure




(2-3 sentences)










Post-lab

3




4




(2-3 sentences)






5


6

7

8

9

10







(2-3 sentences)

11









12









13



a

XNaHCO3

+HCl

h

XNaHSO4

+Na2CO3

b

XHCl+Blue dye

i

XNa2CO3

+Phen

c

XBlue dye+NaOCl


j

XPhen +NaOH

d

XNaOCl+KI


k

XNaOH+AgNO3

e

XKI+Pb(NO3)2

l

XAgNO3

+NH3


f

XPb(NO3)2

+CaCl2

m

XNH3

+CuSO4

g

XCaCl2

+NaHSO4

Be patient

n

XCuSO4

+NaHCO3

14




15






5

1015

2025


(mL)510152025


16




17












the RM and the NM)

18







actual


19









20




21





22






23






24







25








Copper

Silicon

Magnesium

Carbon

Nickel

Aluminum

Zinc

Sulfur

Tin

26


Metal or Metalloid

Oxygen

Lead

Bismuth

Silver

Nitrogen

Antimony

Hydrogen







27








your book)

28



2 Na+ O2-

3 Fe2+ Br-

4 Al3+ PO43-

5 NH4+ NO3

-

6 Fe3+ SO42-

7 K+ S2-





29


30













31



bonds

Conclusion


Ethanol

32












33





Conclusion

34











35













36





37












38













39






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure




4




(2-3 sentences)






5


6

7

8

9

10







(2-3 sentences)

11









12









13



a

XNaHCO3

+HCl

h

XNaHSO4

+Na2CO3

b

XHCl+Blue dye

i

XNa2CO3

+Phen

c

XBlue dye+NaOCl


j

XPhen +NaOH

d

XNaOCl+KI


k

XNaOH+AgNO3

e

XKI+Pb(NO3)2

l

XAgNO3

+NH3


f

XPb(NO3)2

+CaCl2

m

XNH3

+CuSO4

g

XCaCl2

+NaHSO4

Be patient

n

XCuSO4

+NaHCO3

14




15






5

1015

2025


(mL)510152025


16




17












the RM and the NM)

18







actual


19









20




21





22






23






24







25








Copper

Silicon

Magnesium

Carbon

Nickel

Aluminum

Zinc

Sulfur

Tin

26


Metal or Metalloid

Oxygen

Lead

Bismuth

Silver

Nitrogen

Antimony

Hydrogen







27








your book)

28



2 Na+ O2-

3 Fe2+ Br-

4 Al3+ PO43-

5 NH4+ NO3

-

6 Fe3+ SO42-

7 K+ S2-





29


30













31



bonds

Conclusion


Ethanol

32












33





Conclusion

34











35













36





37












38













39






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure




(2-3 sentences)






5


6

7

8

9

10







(2-3 sentences)

11









12









13



a

XNaHCO3

+HCl

h

XNaHSO4

+Na2CO3

b

XHCl+Blue dye

i

XNa2CO3

+Phen

c

XBlue dye+NaOCl


j

XPhen +NaOH

d

XNaOCl+KI


k

XNaOH+AgNO3

e

XKI+Pb(NO3)2

l

XAgNO3

+NH3


f

XPb(NO3)2

+CaCl2

m

XNH3

+CuSO4

g

XCaCl2

+NaHSO4

Be patient

n

XCuSO4

+NaHCO3

14




15






5

1015

2025


(mL)510152025


16




17












the RM and the NM)

18







actual


19









20




21





22






23






24







25








Copper

Silicon

Magnesium

Carbon

Nickel

Aluminum

Zinc

Sulfur

Tin

26


Metal or Metalloid

Oxygen

Lead

Bismuth

Silver

Nitrogen

Antimony

Hydrogen







27








your book)

28



2 Na+ O2-

3 Fe2+ Br-

4 Al3+ PO43-

5 NH4+ NO3

-

6 Fe3+ SO42-

7 K+ S2-





29


30













31



bonds

Conclusion


Ethanol

32












33





Conclusion

34











35













36





37












38













39






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure


6

7

8

9

10







(2-3 sentences)

11









12









13



a

XNaHCO3

+HCl

h

XNaHSO4

+Na2CO3

b

XHCl+Blue dye

i

XNa2CO3

+Phen

c

XBlue dye+NaOCl


j

XPhen +NaOH

d

XNaOCl+KI


k

XNaOH+AgNO3

e

XKI+Pb(NO3)2

l

XAgNO3

+NH3


f

XPb(NO3)2

+CaCl2

m

XNH3

+CuSO4

g

XCaCl2

+NaHSO4

Be patient

n

XCuSO4

+NaHCO3

14




15






5

1015

2025


(mL)510152025


16




17












the RM and the NM)

18







actual


19









20




21





22






23






24







25








Copper

Silicon

Magnesium

Carbon

Nickel

Aluminum

Zinc

Sulfur

Tin

26


Metal or Metalloid

Oxygen

Lead

Bismuth

Silver

Nitrogen

Antimony

Hydrogen







27








your book)

28



2 Na+ O2-

3 Fe2+ Br-

4 Al3+ PO43-

5 NH4+ NO3

-

6 Fe3+ SO42-

7 K+ S2-





29


30













31



bonds

Conclusion


Ethanol

32












33





Conclusion

34











35













36





37












38













39






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure

7

8

9

10







(2-3 sentences)

11









12









13



a

XNaHCO3

+HCl

h

XNaHSO4

+Na2CO3

b

XHCl+Blue dye

i

XNa2CO3

+Phen

c

XBlue dye+NaOCl


j

XPhen +NaOH

d

XNaOCl+KI


k

XNaOH+AgNO3

e

XKI+Pb(NO3)2

l

XAgNO3

+NH3


f

XPb(NO3)2

+CaCl2

m

XNH3

+CuSO4

g

XCaCl2

+NaHSO4

Be patient

n

XCuSO4

+NaHCO3

14




15






5

1015

2025


(mL)510152025


16




17












the RM and the NM)

18







actual


19









20




21





22






23






24







25








Copper

Silicon

Magnesium

Carbon

Nickel

Aluminum

Zinc

Sulfur

Tin

26


Metal or Metalloid

Oxygen

Lead

Bismuth

Silver

Nitrogen

Antimony

Hydrogen







27








your book)

28



2 Na+ O2-

3 Fe2+ Br-

4 Al3+ PO43-

5 NH4+ NO3

-

6 Fe3+ SO42-

7 K+ S2-





29


30













31



bonds

Conclusion


Ethanol

32












33





Conclusion

34











35













36





37












38













39






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure

8

9

10







(2-3 sentences)

11









12









13



a

XNaHCO3

+HCl

h

XNaHSO4

+Na2CO3

b

XHCl+Blue dye

i

XNa2CO3

+Phen

c

XBlue dye+NaOCl


j

XPhen +NaOH

d

XNaOCl+KI


k

XNaOH+AgNO3

e

XKI+Pb(NO3)2

l

XAgNO3

+NH3


f

XPb(NO3)2

+CaCl2

m

XNH3

+CuSO4

g

XCaCl2

+NaHSO4

Be patient

n

XCuSO4

+NaHCO3

14




15






5

1015

2025


(mL)510152025


16




17












the RM and the NM)

18







actual


19









20




21





22






23






24







25








Copper

Silicon

Magnesium

Carbon

Nickel

Aluminum

Zinc

Sulfur

Tin

26


Metal or Metalloid

Oxygen

Lead

Bismuth

Silver

Nitrogen

Antimony

Hydrogen







27








your book)

28



2 Na+ O2-

3 Fe2+ Br-

4 Al3+ PO43-

5 NH4+ NO3

-

6 Fe3+ SO42-

7 K+ S2-





29


30













31



bonds

Conclusion


Ethanol

32












33





Conclusion

34











35













36





37












38













39






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure

9

10







(2-3 sentences)

11









12









13



a

XNaHCO3

+HCl

h

XNaHSO4

+Na2CO3

b

XHCl+Blue dye

i

XNa2CO3

+Phen

c

XBlue dye+NaOCl


j

XPhen +NaOH

d

XNaOCl+KI


k

XNaOH+AgNO3

e

XKI+Pb(NO3)2

l

XAgNO3

+NH3


f

XPb(NO3)2

+CaCl2

m

XNH3

+CuSO4

g

XCaCl2

+NaHSO4

Be patient

n

XCuSO4

+NaHCO3

14




15






5

1015

2025


(mL)510152025


16




17












the RM and the NM)

18







actual


19









20




21





22






23






24







25








Copper

Silicon

Magnesium

Carbon

Nickel

Aluminum

Zinc

Sulfur

Tin

26


Metal or Metalloid

Oxygen

Lead

Bismuth

Silver

Nitrogen

Antimony

Hydrogen







27








your book)

28



2 Na+ O2-

3 Fe2+ Br-

4 Al3+ PO43-

5 NH4+ NO3

-

6 Fe3+ SO42-

7 K+ S2-





29


30













31



bonds

Conclusion


Ethanol

32












33





Conclusion

34











35













36





37












38













39






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure

10







(2-3 sentences)

11









12









13



a

XNaHCO3

+HCl

h

XNaHSO4

+Na2CO3

b

XHCl+Blue dye

i

XNa2CO3

+Phen

c

XBlue dye+NaOCl


j

XPhen +NaOH

d

XNaOCl+KI


k

XNaOH+AgNO3

e

XKI+Pb(NO3)2

l

XAgNO3

+NH3


f

XPb(NO3)2

+CaCl2

m

XNH3

+CuSO4

g

XCaCl2

+NaHSO4

Be patient

n

XCuSO4

+NaHCO3

14




15






5

1015

2025


(mL)510152025


16




17












the RM and the NM)

18







actual


19









20




21





22






23






24







25








Copper

Silicon

Magnesium

Carbon

Nickel

Aluminum

Zinc

Sulfur

Tin

26


Metal or Metalloid

Oxygen

Lead

Bismuth

Silver

Nitrogen

Antimony

Hydrogen







27








your book)

28



2 Na+ O2-

3 Fe2+ Br-

4 Al3+ PO43-

5 NH4+ NO3

-

6 Fe3+ SO42-

7 K+ S2-





29


30













31



bonds

Conclusion


Ethanol

32












33





Conclusion

34











35













36





37












38













39






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure







(2-3 sentences)

11









12









13



a

XNaHCO3

+HCl

h

XNaHSO4

+Na2CO3

b

XHCl+Blue dye

i

XNa2CO3

+Phen

c

XBlue dye+NaOCl


j

XPhen +NaOH

d

XNaOCl+KI


k

XNaOH+AgNO3

e

XKI+Pb(NO3)2

l

XAgNO3

+NH3


f

XPb(NO3)2

+CaCl2

m

XNH3

+CuSO4

g

XCaCl2

+NaHSO4

Be patient

n

XCuSO4

+NaHCO3

14




15






5

1015

2025


(mL)510152025


16




17












the RM and the NM)

18







actual


19









20




21





22






23






24







25








Copper

Silicon

Magnesium

Carbon

Nickel

Aluminum

Zinc

Sulfur

Tin

26


Metal or Metalloid

Oxygen

Lead

Bismuth

Silver

Nitrogen

Antimony

Hydrogen







27








your book)

28



2 Na+ O2-

3 Fe2+ Br-

4 Al3+ PO43-

5 NH4+ NO3

-

6 Fe3+ SO42-

7 K+ S2-





29


30













31



bonds

Conclusion


Ethanol

32












33





Conclusion

34











35













36





37












38













39






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure









12









13



a

XNaHCO3

+HCl

h

XNaHSO4

+Na2CO3

b

XHCl+Blue dye

i

XNa2CO3

+Phen

c

XBlue dye+NaOCl


j

XPhen +NaOH

d

XNaOCl+KI


k

XNaOH+AgNO3

e

XKI+Pb(NO3)2

l

XAgNO3

+NH3


f

XPb(NO3)2

+CaCl2

m

XNH3

+CuSO4

g

XCaCl2

+NaHSO4

Be patient

n

XCuSO4

+NaHCO3

14




15






5

1015

2025


(mL)510152025


16




17












the RM and the NM)

18







actual


19









20




21





22






23






24







25








Copper

Silicon

Magnesium

Carbon

Nickel

Aluminum

Zinc

Sulfur

Tin

26


Metal or Metalloid

Oxygen

Lead

Bismuth

Silver

Nitrogen

Antimony

Hydrogen







27








your book)

28



2 Na+ O2-

3 Fe2+ Br-

4 Al3+ PO43-

5 NH4+ NO3

-

6 Fe3+ SO42-

7 K+ S2-





29


30













31



bonds

Conclusion


Ethanol

32












33





Conclusion

34











35













36





37












38













39






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure









13



a

XNaHCO3

+HCl

h

XNaHSO4

+Na2CO3

b

XHCl+Blue dye

i

XNa2CO3

+Phen

c

XBlue dye+NaOCl


j

XPhen +NaOH

d

XNaOCl+KI


k

XNaOH+AgNO3

e

XKI+Pb(NO3)2

l

XAgNO3

+NH3


f

XPb(NO3)2

+CaCl2

m

XNH3

+CuSO4

g

XCaCl2

+NaHSO4

Be patient

n

XCuSO4

+NaHCO3

14




15






5

1015

2025


(mL)510152025


16




17












the RM and the NM)

18







actual


19









20




21





22






23






24







25








Copper

Silicon

Magnesium

Carbon

Nickel

Aluminum

Zinc

Sulfur

Tin

26


Metal or Metalloid

Oxygen

Lead

Bismuth

Silver

Nitrogen

Antimony

Hydrogen







27








your book)

28



2 Na+ O2-

3 Fe2+ Br-

4 Al3+ PO43-

5 NH4+ NO3

-

6 Fe3+ SO42-

7 K+ S2-





29


30













31



bonds

Conclusion


Ethanol

32












33





Conclusion

34











35













36





37












38













39






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure



a

XNaHCO3

+HCl

h

XNaHSO4

+Na2CO3

b

XHCl+Blue dye

i

XNa2CO3

+Phen

c

XBlue dye+NaOCl


j

XPhen +NaOH

d

XNaOCl+KI


k

XNaOH+AgNO3

e

XKI+Pb(NO3)2

l

XAgNO3

+NH3


f

XPb(NO3)2

+CaCl2

m

XNH3

+CuSO4

g

XCaCl2

+NaHSO4

Be patient

n

XCuSO4

+NaHCO3

14




15






5

1015

2025


(mL)510152025


16




17












the RM and the NM)

18







actual


19









20




21





22






23






24







25








Copper

Silicon

Magnesium

Carbon

Nickel

Aluminum

Zinc

Sulfur

Tin

26


Metal or Metalloid

Oxygen

Lead

Bismuth

Silver

Nitrogen

Antimony

Hydrogen







27








your book)

28



2 Na+ O2-

3 Fe2+ Br-

4 Al3+ PO43-

5 NH4+ NO3

-

6 Fe3+ SO42-

7 K+ S2-





29


30













31



bonds

Conclusion


Ethanol

32












33





Conclusion

34











35













36





37












38













39






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure




15






5

1015

2025


(mL)510152025


16




17












the RM and the NM)

18







actual


19









20




21





22






23






24







25








Copper

Silicon

Magnesium

Carbon

Nickel

Aluminum

Zinc

Sulfur

Tin

26


Metal or Metalloid

Oxygen

Lead

Bismuth

Silver

Nitrogen

Antimony

Hydrogen







27








your book)

28



2 Na+ O2-

3 Fe2+ Br-

4 Al3+ PO43-

5 NH4+ NO3

-

6 Fe3+ SO42-

7 K+ S2-





29


30













31



bonds

Conclusion


Ethanol

32












33





Conclusion

34











35













36





37












38













39






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure






5

1015

2025


(mL)510152025


16




17












the RM and the NM)

18







actual


19









20




21





22






23






24







25








Copper

Silicon

Magnesium

Carbon

Nickel

Aluminum

Zinc

Sulfur

Tin

26


Metal or Metalloid

Oxygen

Lead

Bismuth

Silver

Nitrogen

Antimony

Hydrogen







27








your book)

28



2 Na+ O2-

3 Fe2+ Br-

4 Al3+ PO43-

5 NH4+ NO3

-

6 Fe3+ SO42-

7 K+ S2-





29


30













31



bonds

Conclusion


Ethanol

32












33





Conclusion

34











35













36





37












38













39






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure




17












the RM and the NM)

18







actual


19









20




21





22






23






24







25








Copper

Silicon

Magnesium

Carbon

Nickel

Aluminum

Zinc

Sulfur

Tin

26


Metal or Metalloid

Oxygen

Lead

Bismuth

Silver

Nitrogen

Antimony

Hydrogen







27








your book)

28



2 Na+ O2-

3 Fe2+ Br-

4 Al3+ PO43-

5 NH4+ NO3

-

6 Fe3+ SO42-

7 K+ S2-





29


30













31



bonds

Conclusion


Ethanol

32












33





Conclusion

34











35













36





37












38













39






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure












the RM and the NM)

18







actual


19









20




21





22






23






24







25








Copper

Silicon

Magnesium

Carbon

Nickel

Aluminum

Zinc

Sulfur

Tin

26


Metal or Metalloid

Oxygen

Lead

Bismuth

Silver

Nitrogen

Antimony

Hydrogen







27








your book)

28



2 Na+ O2-

3 Fe2+ Br-

4 Al3+ PO43-

5 NH4+ NO3

-

6 Fe3+ SO42-

7 K+ S2-





29


30













31



bonds

Conclusion


Ethanol

32












33





Conclusion

34











35













36





37












38













39






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure







actual


19









20




21





22






23






24







25








Copper

Silicon

Magnesium

Carbon

Nickel

Aluminum

Zinc

Sulfur

Tin

26


Metal or Metalloid

Oxygen

Lead

Bismuth

Silver

Nitrogen

Antimony

Hydrogen







27








your book)

28



2 Na+ O2-

3 Fe2+ Br-

4 Al3+ PO43-

5 NH4+ NO3

-

6 Fe3+ SO42-

7 K+ S2-





29


30













31



bonds

Conclusion


Ethanol

32












33





Conclusion

34











35













36





37












38













39






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure









20




21





22






23






24







25








Copper

Silicon

Magnesium

Carbon

Nickel

Aluminum

Zinc

Sulfur

Tin

26


Metal or Metalloid

Oxygen

Lead

Bismuth

Silver

Nitrogen

Antimony

Hydrogen







27








your book)

28



2 Na+ O2-

3 Fe2+ Br-

4 Al3+ PO43-

5 NH4+ NO3

-

6 Fe3+ SO42-

7 K+ S2-





29


30













31



bonds

Conclusion


Ethanol

32












33





Conclusion

34











35













36





37












38













39






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure




21





22






23






24







25








Copper

Silicon

Magnesium

Carbon

Nickel

Aluminum

Zinc

Sulfur

Tin

26


Metal or Metalloid

Oxygen

Lead

Bismuth

Silver

Nitrogen

Antimony

Hydrogen







27








your book)

28



2 Na+ O2-

3 Fe2+ Br-

4 Al3+ PO43-

5 NH4+ NO3

-

6 Fe3+ SO42-

7 K+ S2-





29


30













31



bonds

Conclusion


Ethanol

32












33





Conclusion

34











35













36





37












38













39






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure





22






23






24







25








Copper

Silicon

Magnesium

Carbon

Nickel

Aluminum

Zinc

Sulfur

Tin

26


Metal or Metalloid

Oxygen

Lead

Bismuth

Silver

Nitrogen

Antimony

Hydrogen







27








your book)

28



2 Na+ O2-

3 Fe2+ Br-

4 Al3+ PO43-

5 NH4+ NO3

-

6 Fe3+ SO42-

7 K+ S2-





29


30













31



bonds

Conclusion


Ethanol

32












33





Conclusion

34











35













36





37












38













39






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure






23






24







25








Copper

Silicon

Magnesium

Carbon

Nickel

Aluminum

Zinc

Sulfur

Tin

26


Metal or Metalloid

Oxygen

Lead

Bismuth

Silver

Nitrogen

Antimony

Hydrogen







27








your book)

28



2 Na+ O2-

3 Fe2+ Br-

4 Al3+ PO43-

5 NH4+ NO3

-

6 Fe3+ SO42-

7 K+ S2-





29


30













31



bonds

Conclusion


Ethanol

32












33





Conclusion

34











35













36





37












38













39






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure






24







25








Copper

Silicon

Magnesium

Carbon

Nickel

Aluminum

Zinc

Sulfur

Tin

26


Metal or Metalloid

Oxygen

Lead

Bismuth

Silver

Nitrogen

Antimony

Hydrogen







27








your book)

28



2 Na+ O2-

3 Fe2+ Br-

4 Al3+ PO43-

5 NH4+ NO3

-

6 Fe3+ SO42-

7 K+ S2-





29


30













31



bonds

Conclusion


Ethanol

32












33





Conclusion

34











35













36





37












38













39






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure







25








Copper

Silicon

Magnesium

Carbon

Nickel

Aluminum

Zinc

Sulfur

Tin

26


Metal or Metalloid

Oxygen

Lead

Bismuth

Silver

Nitrogen

Antimony

Hydrogen







27








your book)

28



2 Na+ O2-

3 Fe2+ Br-

4 Al3+ PO43-

5 NH4+ NO3

-

6 Fe3+ SO42-

7 K+ S2-





29


30













31



bonds

Conclusion


Ethanol

32












33





Conclusion

34











35













36





37












38













39






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure








Copper

Silicon

Magnesium

Carbon

Nickel

Aluminum

Zinc

Sulfur

Tin

26


Metal or Metalloid

Oxygen

Lead

Bismuth

Silver

Nitrogen

Antimony

Hydrogen







27








your book)

28



2 Na+ O2-

3 Fe2+ Br-

4 Al3+ PO43-

5 NH4+ NO3

-

6 Fe3+ SO42-

7 K+ S2-





29


30













31



bonds

Conclusion


Ethanol

32












33





Conclusion

34











35













36





37












38













39






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure


Metal or Metalloid

Oxygen

Lead

Bismuth

Silver

Nitrogen

Antimony

Hydrogen







27








your book)

28



2 Na+ O2-

3 Fe2+ Br-

4 Al3+ PO43-

5 NH4+ NO3

-

6 Fe3+ SO42-

7 K+ S2-





29


30













31



bonds

Conclusion


Ethanol

32












33





Conclusion

34











35













36





37












38













39






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure








your book)

28



2 Na+ O2-

3 Fe2+ Br-

4 Al3+ PO43-

5 NH4+ NO3

-

6 Fe3+ SO42-

7 K+ S2-





29


30













31



bonds

Conclusion


Ethanol

32












33





Conclusion

34











35













36





37












38













39






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure



2 Na+ O2-

3 Fe2+ Br-

4 Al3+ PO43-

5 NH4+ NO3

-

6 Fe3+ SO42-

7 K+ S2-





29


30













31



bonds

Conclusion


Ethanol

32












33





Conclusion

34











35













36





37












38













39






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure


30













31



bonds

Conclusion


Ethanol

32












33





Conclusion

34











35













36





37












38













39






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure













31



bonds

Conclusion


Ethanol

32












33





Conclusion

34











35













36





37












38













39






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure



bonds

Conclusion


Ethanol

32












33





Conclusion

34











35













36





37












38













39






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure












33





Conclusion

34











35













36





37












38













39






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure





Conclusion

34











35













36





37












38













39






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure











35













36





37












38













39






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure













36





37












38













39






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure





37












38













39






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure












38













39






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure













39






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure






Conclusion


40











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure











41


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure


Al ____________O ____________


Hg____________O_____________

3 NaOH + H2SO4 Na2SO4 + H2O ______________________________

Na__________ H_____________O___________ S ____________

4 Fe + O2 Fe2O3______________________________________Fe_____________O _____________

5 H2 + O2 H2O ______________________________________H____________O____________



8 H2O + Fe Fe2O3 + H2_________________________________H____________O____________Fe____________



42


Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure

Post-lab








43







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure







Ba+2(aq) + 2Cl- (aq) + 2Na+

(aq) + SO4-2


(aq) + BaSO4(s)


Ba+2(aq) + SO4

-2(aq) BaSO4(s)

44




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure




(aq) and N03






Pre-lab




45










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure










46

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure

CaCl2 xFig 2







Conclusion

47












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure












48







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure







49








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure








Initial V1 T1

Final V2 T2









50


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure


Materials












51


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure


Time Temperature






52


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure


Introduction











53









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure









54












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure












Conclusion

55







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure







56






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure






57




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure




58








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure








59






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure






60



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure



Conclusion

61






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure






Pressure ( books)


123456


62



Post-lab

63





What is titration

Titration procedure



Post-lab

63





What is titration

Titration procedure

Lab #3 – A Microscale Study of Chemical...

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Transcript of Lab #3 – A Microscale Study of Chemical...