Solutions
Chap. 15
I. What is a solution?
I. What is a solution?
A. Terms
I. What is a solution?
A. Terms
1. Solute/solvent
The solute is the substance that gets
The solvent does the
.
.
I. What is a solution?
A. Terms
1. Solute/solvent
solute
solvent
The solute is the substance that gets dissolved.
The solvent does the dissolving.
I. What is a solution?
A. Terms
1. Solute/solvent
2. Soluble/insoluble
A substance that is
can be dissolved.
I. What is a solution?
A. Terms
1. Solute/solvent
2. Soluble/insoluble
A substance that is soluble can be dissolved.
I. What is a solution?
A. Terms
1. Solute/solvent
2. Soluble/insoluble
3. Miscible/
immiscible
Miscible substances are
will dissolve in each other.
that
I. What is a solution?
A. Terms
1. Solute/solvent
2. Soluble/insoluble
3. Miscible/
immiscible
Miscible substances are liquids that
will dissolve in each other.
I. What is a solution?
A. Terms
1. Solute/solvent
2. Soluble/insoluble
3. Miscible/ immiscible
4. Electrolytes/nonelectrolytes
Electrolytes are liquids that are
capable of conducting electricity.
I. What is a solution?
B. Types of solutions
I. What is a solution?
B. Types of solutions
1. Gaseous solutions
Air and other mixtures of gases
I. What is a solution?
B. Types of solutions
1. Gaseous solutions
2. Liquid solutions
In some cases water is the solvent. These are
called (
).
I. What is a solution?
B. Types of solutions
1. Gaseous solutions
2. Liquid solutions
In some cases water is the solvent. These are
called (aqueous).
I. What is a solution?
B. Types of solutions
1. Gaseous solutions
2. Liquid solutions
3. Solid solutions
Combinations of solids. Some are
homogenous mixtures of metals (
)
I. What is a solution?
B. Types of solutions
1. Gaseous solutions
2. Liquid solutions
3. Solid solutions
Combinations of solids. Some are
homogenous mixtures of metals (alloys)
I. What is a solution?
C. Making a solution
I. What is a solution?
C. Making a solution
1. Solute/solvent particles
are separated.
I. What is a solution?
C. Making a solution
1. Solute/solvent particles
are separated.
2. Solvent particles are
attracted to solute
particles.
This is called solvation.
With the solvent
this is called hydration
I. What is a solution?
C. Making a solution
1. Solute/solvent particles
are separated.
2. Solvent particles are
attracted to solute
particles.
This is called solvation.
With the solvent water this is called hydration
I. What is a solution?
C. Making a solution
1. Solute/solvent particles
are separated.
2. Solvent particles are
attracted to solute
particles.
3. ‘Like dissolves like’
Polar/Non-polar Substances
Polar
Non-polar
Water
Carbon tetrachloride
Methanol
Toluene (paint thinner)
Ethanol
Hexane, heptane, octane
Acetic acid
Benzene
Acetone
Oil
Ionic compounds
I. What is a solution?
D. Dissolving Ionic Compounds
in H2O
1. Water is polar because it has
two oppositely
ends
I. What is a solution?
D. Dissolving Ionic Compounds
in H2O
1. Water is polar because it has
two oppositely charged ends
I. What is a solution?
D. Dissolving Ionic Compounds
in H2O
1. Water is polar because it has
two oppositely charged ends
2. The
end of water is
attracted to the anion
Anion = negative ion
I. What is a solution?
D. Dissolving Ionic Compounds
in H2O
1. Water is polar because it has
two oppositely charged ends
2. The positive end of water is
attracted to the anion
Anion = negative ion
I. What is a solution?
D. Dissolving Ionic Compounds
in H2O
3. The combined
of water
molecules overcomes the
attractive force of solute.
I. What is a solution?
D. Dissolving Ionic Compounds
in H2O
3. The combined pull of water
molecules overcomes the
attractive force of solute.
I. What is a solution?
D. Dissolving Ionic Compounds
in H2O
3. The combined pull of water
molecules overcomes the
attractive force of solute.
4. The ionic compound is
dissociated into individual
ions.
Ex.
NaCl (s)
Na+ + Cl-
I. What is a solution?
E. Dissolving Molecular
Compounds in H2O.
I. What is a solution?
E. Dissolving Molecular
Compounds in H2O.
1. Water’s charged ends are
attracted to charged
portions of solute.
I. What is a solution?
E. Dissolving Molecular
Compounds in H2O.
1. Water’s charged ends are
attracted to charged
portions of solute.
2. The solute is surrounded by
water molecules.
I. What is a solution?
E. Dissolving Molecular
Compounds in H2O.
1. Water’s charged ends are
attracted to charged
portions of solute.
2. The solute is surrounded by
water molecules.
3. The solute remains intact.
I. What is a solution?
F. Rate of Solvation
To speed up solvation. . .
I. What is a solution?
F. Rate of Solvation
To speed up solvation. . .
1. Stir/shake
I. What is a solution?
F. Rate of Solvation
To speed up solvation. . .
1. Stir/shake
2. Break apart solute
I. What is a solution?
F. Rate of Solvation
To speed up solvation. . .
1. Stir/shake
2. Break apart solute
3. Heat the solvent
II. Is it soluble?
II. Is it soluble?
A. Not all ionic compounds
dissolve in water.
II. Is it soluble?
A. Not all ionic compounds
dissolve in water.
1. Solubility Table
II. Is it soluble?
A. Not all ionic compounds
dissolve in water.
1. Solubility Table
2. Writing physical states
(in equations)
Insoluble = (s) for solid
Soluble = ______________
II. Is it soluble?
A. Not all ionic compounds
dissolve in water.
1. Solubility Table
2. Writing physical states
(in equations)
Insoluble = (s) for solid
Soluble = (aq) for aqueous
II. Is it soluble?
A. Not all ionic compounds
dissolve in water.
1. Solubility Table
2. Writing physical states
(in equations)
3. Solubility Rules
Self Check – Ex. 1
Is copper (II) chloride
soluble?
Self Check – Ex. 2
Is zinc carbonate soluble?
Self Check – Ex. 3
Is calcium hydroxide
soluble?
II. Is it soluble?
A. Not all ionic compounds
dissolve in water.
B. In reality, ionic compounds
all dissolve in varying degrees.
Some compounds are very soluble while
others are slightly soluble
II. Is it soluble?
A. Not all ionic compounds
dissolve in water.
B. In reality, ionic compounds
all dissolve in varying degrees.
1. Solubility depends on
___________
Solubility
Curve
II. Is it soluble?
A. Not all ionic compounds
dissolve in water.
B. In reality, ionic compounds
all dissolve in varying degrees.
1. Solubility depends on
temperature
2. Solubility depends on
physical state
II. Is it soluble?
A. Not all ionic compounds
dissolve in water.
B. In reality, ionic compounds
all dissolve in varying degrees.
1. Solubility depends on
temperature
2. Solubility depends on
physical state
3. Solubility of gas depends
on pressure
Henry’s Law
The solubility (S) of a gas
in a liquid is directly
proportional to the
pressure (P) of the gas
S1
P1
=
S2
P2
Self Check – Ex. 4
The solubility of O2 in
water is 1.2 g/L when the
pressure 2.0 atm. What is
the solubility when the
pressure is 6.0 atm?
III. Heat of solution
III. Heat of solution
A. Many reactions warm up
when you mix substances
Exothermic – heat given off
III. Heat of solution
A. Many reactions warm up
when you mix substances
B. Some reactions get colder
when you mix substances
Endothermic – heat absorbed
IV. Concentration
IV. Concentration
A. Terms
IV. Concentration
A. Terms
1. Concentrated
A solution that has a lot of
per solvent
IV. Concentration
A. Terms
1. Concentrated
A solution that has a lot of solute per solvent
IV. Concentration
A. Terms
1. Concentrated
2. Dilute
A solution that has a lot of
.
IV. Concentration
A. Terms
1. Concentrated
2. Dilute
A solution that has a lot of solvent.
IV. Concentration
A. Terms
1. Concentrated
2. Dilute
3. Saturated
A solution with
solute.
IV. Concentration
A. Terms
1. Concentrated
2. Dilute
3. Saturated
A solution with the maximum amount of solute.
IV. Concentration
A. Terms
1. Concentrated
2. Dilute
3. Saturated
4. Supersaturated
A solution with
.
IV. Concentration
A. Terms
1. Concentrated
2. Dilute
3. Saturated
4. Supersaturated
A solution with more solute than it can hold.
IV. Concentration
A. Terms
B. Measurements
Quantifying concentrations
IV. Concentration
A. Terms
B. Measurements
1. Percentage
IV. Concentration
A. Terms
B. Measurements
1. Percentage
a. By mass
Percent by mass =
mass solute
mass solution
Solution = solute & solvent
x 100
Self Check – Ex. 5
What is the percent by
mass when 40 g of salt is
added to 200 g of water.
IV. Concentration
A. Terms
B. Measurements
1. Percentage
a. By mass
b. By volume
Percent by volume =
x 100
IV. Concentration
A. Terms
B. Measurements
1. Percentage
a. By mass
b. By volume
Percent by volume =
volume solute
volume solution
x 100
Self Check – Ex. 6
What is the percent by
volume when 50 mL of
methanol is added to 450
mL of water.
IV. Concentration
A. Terms
B. Measurements
1. Percentage
2. Molarity
Molarity =
moles solute
volume solution
x 100
Self Check – Ex. 7
A solution is formed by
adding 7.4 g of Ca(OH)2 to
500 mL of solution. What is
the molarity?
Self Check – Ex. 8
How many grams of
potassium nitrate, KNO3
are required to make 250
mL solution with a
molarity of 0.40 M?
IV. Concentration
A. Terms
B. Measurements
1. Percentage
2. Molarity
3. Molality
Molality =
moles solute
volume solution
x 100
Self Check – Ex. 9
What is the molality of a
solution of 60 g of NaOH
and 2000 g of water?
IV. Concentration
A. Terms
B. Measurements
1. Percentage
2. Molarity
3. Molality
4. Mole fraction
Mole fraction =
moles solute
moles solution
IV. Concentration
A. Terms
B. Measurements
C. Diluting solutions
M1V1 = M2V2
V. Solution Stoichiometry
V. Solution Stoichiometry
A. Concentrations are ratios,
used like conversion factors
V. Solution Stoichiometry
A. Concentrations are ratios,
used like conversion factors
B. Remember the rules
Stoich. Rules
1. Balance Equation
Stoich. Rules
1. Balance Equation
2. ID units of Unknown
Stoich. Rules
1. Balance Equation
2. ID units of Unknown
3. Write given
Stoich. Rules
1.
2.
3.
4.
Balance Equation
ID units of Unknown
Write given
Insert ‘conversion factors’
Self Check – Ex. 10
How many grams of AgCl
are formed when a 35.5 mL
sample 0.12 M AgNO3 is
added to excess NaCl
solution?
Self Check – Ex. 11
How many milliliters of
0.25 M HCl is required to
react with 4.0 g of NaOH?
VI. Colligative Properties
Properties affected by the number of solute
particles, but not the identify of those particles
VI. Colligative Properties
A. Vapor Pressure: it’s lowered
A measure of liquid water’s ability to become a
vapor
VI. Colligative Properties
A. Vapor Pressure: it’s lowered
B. Boiling Point: it’s elevated
VI. Colligative Properties
A. Vapor Pressure: it’s lowered
B. Boiling Point: it’s elevated
C. Freezing Point: it’s lowered
VI. Colligative Properties
A.
B.
C.
D.
Vapor Pressure: it’s lowered
Boiling Point: it’s elevated
Freezing Point: it’s lowered
Osmotic Pressure: it’s lowered
Osmosis is movement of water through a semipermeable membrane
VII. Heterogeneous Mixtures
VII. Heterogeneous Mixtures
A. Suspensions
VII. Heterogeneous Mixtures
A. Suspensions
B. Colloids
The end