This document provides a review of key concepts from Chapter 16, including solubility, supersaturated solutions, colligative properties, factors that affect solubility, and calculations involving molarity, molality, mass percent, and volume percent in solution concentration problems. It contains multiple choice and open response questions about these topics.

1. Chapter 16 Review
=“Solutions
”
Pre-AP Chemistry
Charles Page High School
Stephen L. Cotton

2. 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 ____.

3. 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)?

4. 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?

5. 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?

6. 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?

7. Chapter 16 Review
 Ifthe 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

8. 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 ____.

9. 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?

10. 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?

11. 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?

12. 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?

13. 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?

14. 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?

15. Chapter 16 Review
 Calculate the molality of a
solution prepared by dissolving
175 g KNO3 in 750 g of water.