Solution-
homogenous mixture
Solutesubstance being dissolved
Solventthe dissolving medium
Solubilitythe amount of solute that will dissolve in a
given amount of solvent at a given
temperature
Can you filter a solution?
No
 What is a suspension? Can you filter a
suspension?
Yes
Saturated solution-
contains the maximum amount of solute
Unsaturated solutioncontains less than the maximum amount of
solute, can dissolve more solute
Supersaturated solutioncontains more than the maximum amount
of solute, prepared by heating
SUPERSATURATED SOLUTIONS
Videohttps://www.youtube.com/watch?v=0wif
FbGDv4I
https://www.youtube.com/watch?v=mxO9rtVj
oR4
Electrolyte-
solution that will conduct electricity
Nonelectrolytesolution that will not conduct
electricity
What type of compounds are electrolytes?
ionic compounds, acids, bases
What type of compounds are
nonelectrolytes?
covalent compounds
What happens to ionic compounds when
they are dissolved in water?
break apart into ions
Write the dissociation reaction for:
NaCl(s) →
NaCl(s) → Na+(aq) + Cl-(aq)
KNO3(s) →
KNO3(s) → K+(aq) + NO3-(aq)
Al(NO3)3(s) →
Al(NO3)3(s) → Al+3(aq) + 3 NO3-(aq)
EXAMPLES OF SOLUTIONS
 Solid dissolved in a liquid
Kool-Aid/sweet tea
 Gas dissolved in a liquid
Coke
 Liquid dissolved in a liquid
Vinegar
 Gas dissolved in a gas
Air
 Solid dissolved in a solid
Jewelry; metal alloys
EFFECTS OF TEMPERATURE ON
SOLUBILITY
Solids dissolved in liquids – (Ex: sweet tea)
solubility increases as the temperature
increases
Gases dissolved in liquids – (Ex: soda)
solubility decreases as the temperature
increases
EFFECTS OF PRESSURE ON
SOLUBILITY
Gases only (Ex: soda)
solubility increases as pressure increases
SOLUBILITY CURVE
LIKE DISSOLVES LIKE
Polar compounds will dissolve polar compounds (and
ionic)
Nonpolar compounds will dissolve nonpolar compounds
Alcohols will dissolve polar and nonpolar but NOT
ionic.
SALT DISSOLVING IN WATER
Polar Solvents
Nonpolar Solvents
H2O
 CCl4
NH3
Oil
Benzene (C6H6)
Miscible –
will mix (dissolve)
Immiscible –
will not mix
VIDEO
 https://www.youtube.com/watch?v=JE4pwRD8t9Q
ARE THE FOLLOWING MISCIBLE OR
IMMISCIBLE?
Oil and water?
immiscible
Oil and CCl4?
miscible
Water and CCl4?
immiscible
Oil and benzene?
miscible
UNITS OF CONCENTRATION
Explain the difference between a concentrated and
a dilute solution.
Molarity (M) =
What does 0.100 M HCl tell you?
PRACTICE
1. Calculate the molarity of a solution if 3.00 moles
of sugar are dissolved in 1.0 L of solution.
3.0 M
PRACTICE
2. Calculate the molarity of a solution made by
dissolving 125 g of C12H22O11 in 1.50 L of solution.
0.243 M
PRACTICE
3. How many g of NaOH are contained in
1500. ml of a 0.330 M solution?
19.8 g
DILUTION
Adding water to a solution will dilute the solution and the
molarity _____________but the # of moles of solute
________
M1V1 = M2V2
PRACTICE
1. What volume of 10.0 M NaOH is needed
to prepare 1000. ml of a 0.100 M NaOH
solution?
10.0 ml
PRACTICE
2. What is the molarity of an acid solution if
12.5 ml of a 6.00 M solution is diluted to a
final volume of 500. ml?
0.15 M
PRACTICE
3. If 100 ml of water are added to 50 ml of a
12 M HCl solution, what is the molarity of
the diluted solution?
4.0 M
PERCENT BY MASS
% solute = g solute
g solution
x 100
PRACTICE
1. Calculate the % of sugar in a solution made
by dissolving 25.0 g of sugar in 100. g of
water.
20.0 %
PRACTICE
2. How many g of sugar are contained in 325 g
of a solution that is 8.55 % sugar?
27.8 g
PRACTICE
3. How many grams of solution are needed to
have 36.5 g of sugar in a solution that is 15.0 %
sugar?
243 g
SOLUTION STOICHIOMETRY
1. What volume of 0.100 M HCl is needed to
neutralize 25.0 ml of a 0.350 M NaOH
solution?
CONT.
2. Pb(NO3)2 +
37.5 ml
0.500 M
2 KCl → 2KNO3 + PbCl2
28.0 ml
M=?
3. Ba(NO3)2 + Na2SO4 → BaSO4 + 2NaNO3.
How many grams of BaSO4 are produced by the
reaction of 43.7 ml of 0.650 M Ba(NO3)2?
4. How many grams of Ag2CrO4 are produced by
reacting 75.5 ml of 0.100 M AgNO3 according to the
equation:
2 AgNO3 + K2CrO4 → Ag2CrO4 + 2KNO3
NET IONIC EQUATIONS
 Precipitation reactions – two solutions are mixed and form a
precipitate (solid)
 To determine what forms a precipitate use the solubility
rules in your packet.
 Soluble – dissolves in water, exists as ____________ (aq)
Ex: KBr
 Insoluble – does not dissolve, remains a _____________
(s)
PRECIPITATES
SOLUBLE OR INSOLUBLE?
1. KNO3 ____________
soluble
2. MgCl2 _____________
soluble
3. PbCl2 _______________
insoluble
4. K3PO4 ____________
soluble
SOLUBLE OR INSOLUBLE?
5. Ca3(PO4)2 __________
insoluble
6. BaSO4 _____________
insoluble
7. Cu(C2H3O2)2 ___________
soluble
8. PbCrO4 _______________
insoluble
WRITING NET IONIC EQUATIONS
1. Pb(NO3)2 + ZnCl2 →
Pb+2(aq) + 2 Cl- (aq) → PbCl2(s)
CONT
2. CuCl2 + K2CrO4 →
Cu+2(aq) + CrO4-2(aq) → CuCrO4(s)
CONT.
3. Ba(NO3)2 + Na2SO4 →
Ba+2(aq) + SO4-2(aq) → BaSO4(s)
CONT.
4. NaOH + CuCl2 →
Cu+2(aq) + 2OH- → Cu(OH)2(s)
CONT.
5. KNO3 + NaCl →
No Reaction (NR)