Chapter 16 Review
=“Solutions”
Chapter 16 Review
If the solubility of a particular solute is
10 g/100 g H2O at 20 oC, which of the
following would represent a
supersaturated solution of that solute:
a) 9 g/100 g H2O at 20 oC, or
b) 11 g/100 g H2O at 20 oC.
 If a crystal added to an aqueous
solution causes many particles to come
out of the solution, the original solution
was ____.

Chapter 16 Review
 Colligative
properties depend upon
the ____.
 What happens to the solubility of a
gas in a liquid, if the partial pressure
of the gas above the liquid
decreases?
 Which of the following substances is
less soluble in hot water than in cold
water: a) CO2(g), or b) KBr(s)?
Chapter 16 Review
 The
solubility of a gas in a liquid is
____ proportional to ____.
 To what concentration variable is
change in boiling point directly
proportional?
 What usually occurs to solubility as
temperature increases?
 What units are generally used to
express solubility?
Chapter 16 Review
 What
factors will usually make a
substance dissolve faster in a
solvent?
 In a concentrated solution, there is a
____ amount of solute.
 What are the three colligative
properties of a solution we have
studied?
Chapter 16 Review
 What
are the solution concentration
units used to express molarity?
 What is the maximum amount of
KCl that can dissolve in 200 g of
water at 20 oC? (the solubility of
KCl is 34 g/100 g H2O at 20 oC)
 What does NOT change when a
solution is diluted by the addition of
more solvent?
Chapter 16 Review
 If
the percent by volume is 2.0 %
and the volume of solution is 250
mL, what is the volume of solute in
solution?
 What two factors affect the solubility
of a particular substance?
 Which of the following equations
yields the number of moles?
a) M x L, or b) M x mass of solution
Chapter 16 Review
 The
volume of alcohol present in
620 mL of a 40.0 % (v/v) solution of
alcohol is ____.
 A solute depresses the freezing
point because the solute ____.
 To increase the solubility of gas at
constant temperature from 1.20 g/L
at 1.4 atm, to 2.3 g/L, the pressure
would have to be increased to ____.
Chapter 16 Review
 What
is the boiling point of a
solution that contains 3 moles of
KBr in 2000 g of water? (Kb = 0.512
oC/m; molar mass of water = 18
g/mol)
 What mass of KCl (solubility 34
g/100 g H2O at 20 oC) can dissolve
in 3.30 x 102 g of water?
Chapter 16 Review
 What
is the freezing point of a
solution that has 5.0 mol of NaI in
1250 g of water? (Kf = 1.86 oC/m;
molar mass of water = 18.0 g/mol)
 How many kilograms of solvent are
in a sample of 0.30 molal solution, if
the sample contains 13 moles of
solute?
Chapter 16 Review
 What
is the molality of a solution
containing 5.0 mol of solute in 3.2 kg
of solvent?
 What is the molarity of a solution
containing 1.2 g of solute in 450 mL
of solution? (molar mass of solute =
24 g/mol)
 How many liters of a 0.30 M solution
are needed to give 2.7 mol of solute?
Chapter 16 Review
 How many liters of a 1.5 M
solution are required to yield 5.0 g
of solute? (molar mass of solute =
30.0 g/mol)
 If the volume of solute is 6.0 mL
and the volume of solution is
300.0 mL, what is the solute’s
percent by volume?
Chapter 16 Review
 If the solubility of a gas is 7.5
g/L at 404 kPa pressure, what
is the solubility of the gas when
the pressure is 202 kPa?
 What
is the number of moles of
solute in 650 mL of a 0.40 M
solution?
Chapter 16 Review
 What is the number of moles of
solute in a 0.3 molal solution
containing 0.10 kg of solvent?
 If 1.0 mL of 6.0 M HCl is added
to 499 mL of water to give
exactly a 500 mL solution, what
is the molarity of the dilute
solution?
Chapter 16 Review
 Calculate the molality of a
solution prepared by dissolving
175 g KNO3 in 750 g of water.