a cenote
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Transcript of a cenote
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a cenote
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INTRODUCTIONWATER IN LIFE ON EARTH
Water covers almost two thirds of our planet
Water has been the key to much of Earth’s evolutionary
history
Life itself is almost certainly originated from water
Our body is about 60% water by mass
Water possesses many unusual properties essential to
supporting life on Earth
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INTRODUCTIONWATER AS A MEDIUM Water has an exceptional ability to dissolve a wide variety
of substances
Water on Earth invariably contains a variety of dissolved
substances
Water is the medium for most of the chemical reactions
that take place within us and around us
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INTRODUCTIONWATER AS A MEDIUM
http://imnews.imbc.com/replay/nwdesk/article/3243453_5780.html
Figure 4.1 Cenote formation
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4.1 GENERAL PROPERTIES OF AQUEOUS SOLUTIONS
ELECTROLYTIC PROPERTIES Consider two aqueous solutions: NaCl (aq) & C6H12O6 (aq)
Electrolyte & nonelectrolyte
Solution, solvent, and solute
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4.1 GENERAL PROPERTIES OF AQUEOUS SOLUTIONS IONIC & MOLECULAR COMPOUNDS IN
WATER Dissolution (solvation) process in water We can predict the nature of ionic compounds (Na2SO4) in
water from the chemical formula Most molecular compounds are nonelectrolytes Glucose, CH3OH, and HCl (ionic)
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4.1 GENERAL PROPERTIES OF AQUEOUS SOLUTIONSSTRONG AND WEAK
ELECTROLYTES Strong electrolytes exist in solution (nearly) completely as ions; NaCl, HCl
Weak electrolytes exist in solution mostly in the form of molecules with only a small fraction in the form of ions; CH3COOH (about 1% ionized)
Dissolution & ionization (CH3COOH & Ba(OH)2 ) (weak) (strong)
Soluble ionic compounds are strong electrolytes: metal+nonmetal compounds & ammonium containing compounds (NaCl, FeSO4, Al(NO3)3, NH4Br, (NH4)2CO3)
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4.2 PRECIPITATION REACTIONSPRECIPITATION REACTION
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4.2 PRECIPITATION REACTIONSSOLUBILITY GUIDELINES FOR IONIC
COMPOUNDS Solubility: the amount of a substance dissolved in a given
quantity of solvent at a given temperature Some ionic substances are insoluble in water because the
attraction between the opposite charges is too great for the water molecules to separate the ions
No general rules to predict solubility of a substance
All ionic compounds containing NO3-, or CH3COO-
All ionic compounds containing the alkali metal ions or,
NH4+
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4.2 PRECIPITATION REACTIONSSOLUBILITY GUIDELINES FOR IONIC COMPOUNDS
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4.2 PRECIPITATION REACTIONS
EXCHANGE (METATHESIS) REACTIONS
IONIC EQUATIONS Molecular equations
Ionic equations (complete ionic equations)
Net ionic equations
Spectator ions
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4.3 ACID-BASE REACTIONS Many acids and bases are industrial and household
substances Hydrochloric acid: important industrial chemical & main
component of gastric juice in our stomach.
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4.3 ACID-BASE REACTIONS
ACIDS Substances that ionize in water to form H+,
thereby increasing the concentration of H+
Proton donors
Monoprotic acids: HCl and HNO3
Diprotic acids: H2SO4
CH3COOH (acetic acid)
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4.3 ACID-BASE REACTIONS
BASES Substances that accept (react with) H+ Bases produce hydroxide ions (OH-) when they dissolve in
water
NaOH, KOH and Ca(OH)2 are common bases
NH3 is also a common base although it does not have OH-
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4.3 ACID-BASE REACTIONS
STRONG AND WEAK ACIDS AND BASES Strong acids and bases
•Acids and bases that are completely ionized in solution Weak acids and bases
•Acids and bases that are partly ionized in solution
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4.3 ACID-BASE REACTIONS IDENTIFYING STRONG AND WEAK
ELECTROLYTES
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4.3 ACID-BASE REACTIONSNEUTRALIZATION REACTIONS AND
SALTS Differences in the properties of acids and bases
•Sour and bitter taste
•Color changes with certain dyes Neutralization reaction occurs when a solution of an acid
and a solution of a base are mixed
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4.3 ACID-BASE REACTIONSNEUTRALIZATION REACTIONS AND SALTS
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4.3 ACID-BASE REACTIONSNEUTRALIZATION REACTIONS AND
SALTSSample Exercise 4.7 Writing Chemical Equations for a
Neutralization ReactionFor the reaction between aqueous solutions of acetic acid (CH3COOH) and barium hydroxide, Ba(OH)2, write (a) the balanced molecular equation, (b) the complete ionic equation, (c) the net ionic equation.
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4.3 ACID-BA SE REACTIONSACID-BASE REACTIONS WITH GAS
FORMATION Consider a acid-base reaction:
Carbonic acid is unstable
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Heartburn, reflux, indigestion, and sour stomach
Histamine-2 (H2) blockers including cimetidine (Tagamet), famotidine (Pepcid), and ranitidine (Zantac), and the proton pump inhibitor (PPI) omeprazole (Prilosec)
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4.4 OXIDATION-REDUCTION REACTIONS
OXIDATION AND REDUCTION
Oxidation – loss of electrons by a substance
Reduction – gain of electrons by a substance
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4.4 OXIDATION-REDUCTION REACTIONS
OXIDATION AND REDUCTION
Ca(s) is oxidized and O2(g) is reduced
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4.4 OXIDATION-REDUCTION REACTIONS
OXIDATION NUMBERS The degree of oxidation of an atom in a chemical compound Assigning oxidation number
• Elements in their elemental form have an oxidation number of 0.
• The oxidation number of a monatomic ion is the same as its charge.
• Nonmetals tend to have negative oxidation numbers, although some are positive in certain compounds or ions
- O: -2 (-1 in O2-2), H: +1 (-1 when bonded to metals),
F: -1, other halogens: -1 (+N when bonded to oxygen)• The sum of the oxidation numbers in a neutral compound is 0.• The sum of the oxidation numbers in a polyatomic ion is the
charge on the ion.
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4.4 OXIDATION-REDUCTION REACTIONS
OXIDATION NUMBERS
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4.4 OXIDATION-REDUCTION REACTIONSOXIDATION OF METALS BY ACIDS AND
SALTS By acids
By salts
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4.4 OXIDATION-REDUCTION REACTIONSOXIDATION OF METALS BY ACIDS AND
SALTS
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4.4 OXIDATION-REDUCTION REACTIONS
ACTIVITY SERIES Can we predict whether a certain metal will be oxidized either
by an acid or by a particular salt? It would be unwise to store a solution of nickel nitrate,
Ni(NO3)2, in an iron container.
Different metals vary in the ease with which they are oxidized Zn is oxidized by aqueous solution of Cu2+, but Ag is not. Activity series of metals in aqueous solution
•A list of metals arranged in order of decreasing ease of oxidation
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4.4 OXIDATION-REDUCTION REACTIONSACTIVITY SERIES
Any metal on the listcan be oxidizedby the ions of elements below it
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4.4 OXIDATION-REDUCTION REACTIONSACTIVITY SERIES
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4.4 OXIDATION-REDUCTION REACTIONSACTIVITY SERIES
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• Why is gold a special metal? - intrinsic beauty and rarity - soft and easy to be formed - the least active metal• Gold can be found in nature as a
pure element rather than combined with oxygen or other elements, which account for its early discovery.
• Used in jewelry (73%), coins (10%), and electronics (9%).
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4.5 CONCENTRATIONS OF SOLUTIONSMOLARITY
The concentration of a solution as the number of moles of solute in a liter of solution
Figure 4.16 Preparing 0.250 L of a 1.00M solution of CuSO4.
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4.5 CONCENTRATIONS OF SOLUTIONS
FW 142 g/mol
MOLARITY
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4.5 CONCENTRATIONS OF SOLUTIONSTHE CONCENTRATION OF AN
ELECTROLYTE Some substances produce multiple cations and/or anions
(Na2SO4, MgCl2)
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4.5 CONCENTRATIONS OF SOLUTIONS
INTERCONVERTING M, mol, AND VOLUME
FW 142 g/mol
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DILUTION How would you prepare 250.0 mL of 0.100 M cupric sulfate
solution from 1.00 M solution?
4.5 CONCENTRATIONS OF SOLUTIONS
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DILUTION – PREPARATION OF SOLUTIONS
4.5 CONCENTRATIONS OF SOLUTIONS
Figure 4.17
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4.6 SOLUTION STOICHIOMETRY AND CHEMICAL ANALYSIS Let’s consider a question:
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4.6 SOLUTION STOICHIOMETRY AND CHEMICAL ANALYSIS
FW 74.1 g/mol
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4.6 SOLUTION STOICHIOMETRY AND CHEMICAL ANALYSIS
NaOH, FW 40.0 g/mol
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4.6 SOLUTION STOICHIOMETRY AND CHEMICAL ANALYSIS
TITRATIONS Titration is an analytical technique in which one can
determine the concentration of a solute in a solution. Standard solution Equivalence point Indicators
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4.6 SOLUTION STOICHIOMETRY AND CHEMICAL ANALYSIS
TITRATIONS
Figure 4.19
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4.6 SOLUTION STOICHIOMETRY AND CHEMICAL ANALYSIS
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4.6 SOLUTION STOICHIOMETRY AND CHEMICAL ANALYSIS
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FW 212.3 g/mol
Ag3PO4, FW 212.3 g/mol
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1.
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2.
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3.