Post on 18-Dec-2015
Solution• a homogeneous mixture
of two or more components. The components of a solution are atoms, ions, or molecules, which makes them 10-9 m or smaller in diameter.
• Ex. Salt water
Suspensions• The particles in
suspensions are larger than those found in solutions. Components of a suspension can be evenly distributed by a mechanical means, like by shaking the contents, but the components will settle out.
• Ex: Oil and Water
Colloids• Particles intermediate size can be
mixed such that they remain evenly distributed without settling out. These particles range in size from 10-8 to 10-6 m in size.
• The mixture they form is called a colloidal dispersion.
• A colloidal dispersion consists of colloids in a dispersing medium.• Ex: Milk
Parts of a solution:
1. Solute: substance being dissolved (NaCl)
2. Solvent: dissolving medium (H
2O)
Solvation: the process of solvent particles surrounding solute particles to form a solution
“Like dissolves Like”This is the general rule to determine
whether solvation occurs.
“Like” refers to the solvent and solute being either polar or nonpolar.
Polarity of a molecule is a result of how the electrons are shared and arranged.
Water is a polar molecule.
“Universal solvent”
Telling Them Apart• You can tell suspensions from colloids
and solutions because the components of suspensions will eventually separate.
• Colloids can be distinguished from solutions using the Tyndall effect. – A beam of light passing through a true
solution, such as air, is not visible. – Light passing through a colloidal
dispersion will be reflected by the larger particles and the light beam will be visible. (Ex. smoky or foggy air)
When Substances Combine:
1.Soluble: a substance that dissolves in a solvent
2.Insoluble: a substance that does not dissolve in a solvent
3.Immiscible: two liquids that are immiscible, they separate after mixing (water & oil)
4.Miscible: two liquids that are soluble in each other.
Rate of SolvationFactors affecting the rate of solvation:
1. Agitation: stirring, shaking; allows particles to dissolve faster
2. Temperature: heat adds energy which allows particles to move faster and disassociate from each other faster.
3. Particle size: smaller particles increase surface area for the solvent to act on.
Affect of Temperature on Solubility
Solubility : maximum amount of solute that will dissolve in a given amount of solvent, 100g usually
Solubility Terminology:1.Saturated solution: contains the
maximum amount (g) of dissolved solute
2.Unsaturated solution: contains LESSLESS than the maximum amount (g) of dissolved solute
3.Supersaturated solution: contains MOREMORE that the maximum amount of dissolved solute.
What type of a solution is a solution that contains 70g PbNO
3 at
40ºC in 100g H
2O?
SATURATEDSATURATED
What type of a solution is a solution that contains 35g NaCl at 80ºC in 100g H
2O?
UNSATURATEDUNSATURATED
What type of a solution is a solution that contains 120g K
2NO
3
at 60ºC in 100g H
2O?
SUPER-SUPER-SATURATEDSATURATED
Factors Affecting Solubility:
1.Temperature: many substances are more soluble at high temperature. But, gases will dissolve better at colder temperatures.
Factors Affecting Solubility:
2. Pressure: Gases will dissolve best under pressure.
Henry’s Law: solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid.
“The BENDS”Deep sea divers may experience a condition called
the "bends" if they do not readjust slowly to the lower pressure at the surface. As a result of
breathing compressed air and being subjected to high pressures caused by water depth, the amount
of nitrogen dissolved in blood and other tissues increases. If the diver returns to the surface too
rapidly, the nitrogen forms bubbles in the blood as it becomes less soluble due to a decrease in
pressure. The nitrogen bubbles can cause great pain and possibly death.
To alleviate this problem somewhat, artificial breathing mixtures of oxygen and helium are used. Helium is only one-fifth as soluble in blood as nitrogen. As a result, there is less dissolved gas to form bubbles.
Solution Concentrations
Concentration: the amount (g) of solute dissolved in a specific amount of solvent
1. Concentrated: large amount of solute for the amount of solute.
2. Dilute: small amount of solute for the amount of solution.
Methods of Determining Concentration of Solution:
Concentration RatiosConcentration
descriptionRatios
Percent by mass mass of solute
mass of solution x 100
Percent by volume volume of solute
volume of solution x 100
Molaritymoles of solute liter of solution
Using Percent to Describe Concentration
• Percent by mass usually describes solutions in which a solid is dissolved in a liquid.
• Represents the ratio of the solute’s mass to the solution’s mass expressed as a percent.
• The mass of solution equals the sum of the masses of the solute and solvent.
Using Percent to Describe Concentration
Calculating Percent by MassIn order to maintain a sodium chloride
concentration similar to ocean water, an aquarium must contain 3.6 g NaCl per 100g of water. What is the percent by mass of NaCl in the solution?
Find mass of the solution.Mass of solution = g solute + g solvent
= 3.6g + 100g= 103.6 g
Using Percent to Describe Concentration
Calculating Percent by MassIn order to maintain a sodium chloride concentration similar to
ocean water, an aquarium must contain 3.6 g NaCl per 100g of water. What is the percent by mass of NaCl in the solution?
Substitute values into equation Percent by mass = mass of solute
mass of solution x100
= 3.6g ÷ 103.6g x 100
=3.5%
Using Percent to Describe Concentration
Calculating Percent by Volume• describes solutions in which both the
solute and solvent are liquids• Volume of the solution is the sum of the
volumes of the solute and solventExample: 70% isopropyl alcohol means that
70 volumes of alcohol are dissolved in 100 volumes of water, thus 30 volumes of water are in every 100 volumes of the isopropyl alcohol solution.
Using Percent to Describe Concentration
Calculating Percent by VolumeWhat is the percent by volume of ethanol in a
solution that contains 35mL of ethanol dissolved in 155mL of water?
Volume of solution = vol. solute + vol. solvent = 35mL + 155mL =
190mL = 35mL x 100
190mL
=18.4%
Calculating Molarity• Molarity (M) is the number of moles of
solute dissolved per liter of solution.• Also known as molar concentration.• A liter of solution containing one mole
of solute is a 1M solution.• Formula:
Molarity(M) = moles of solute liters of solution
Calculating MolarityExample: A 100.5 mL intravenous (IV) solution
contains 5.10g of glucose (C6H12O6). What is the molarity of this solution? [molar mass of glucose is 180.16 g/mol]
Use molar mass to calculate the number of moles of C6H12O6. Round to 4 places after decimal.
5.10 g C6H12O6 1 mol C6H12O6
180.16 g C6H12O6
= .0283 mol C6H12O6
Calculating Molarity2. Convert mL to L. 100.5mL x 1L = 0.1005 L solution
1000mL3. Substitue the known values into the
equation.Molarity = moles solute
liters of solution
M = 0.0283 mol C6H12O6 = 0.282 mol/L soln.0.1005 L soln.
= 0.28M
Diluting Solutions
Often stock solutions must be diluted from one concentration to another. How is the volume of the stock solution to be diluted determined?
Rearrange the molarity equation and the number of moles solute does not change and we get the equation:
M1V1 = M2V2
Diluting does
Not add solute,Only
solvent.
Diluting Stock Solutions
What volume, in milliliters of 2.00M calcium chloride solution would you use to make 0.50 L of 0.30M calcium chloride solution?
Analyze the problem: what do you have and what are you looking for.
Given Unknown
M1 = 2.00M CaCl2 V1 = ? L
M2 = 0.300M
V2 = 0.50L
Diluting Stock Solutions
What volume, in milliliters of 2.00M calcium chloride solution would you use to make 0.50 L if 0.30M calcium chloride solution?
Solve for the Unknown: rearrange the equation to solve for the unknown
M1V1 = M2V2
V1 = M2 V2
M1
Diluting Stock SolutionsWhat volume, in milliliters of 2.00M
calcium chloride solution would you use to make 0.50 L if 0.30M calcium chloride solution?
Substitute known values and solve.
V1 = 0.50L x 0.300M2.00M
V1 = 0.075L x 1000mL ( the question asked for mL!!!)
1L
V1 = 75mL
Colligative Properties
Physical properties of a solution that are affected by the number of particles in the solution.
• Lowers vapor pressure: less gas escapes from the liquid because of the solute
Colligative Properties• Raises boiling point: it takes more
energy to overcome the attraction between the solute and solvent
• Lowers freezing point: solute disrupts the solvent particles from forming a solid
example: Antifreeze (ethylene glycol)