AP CHEMISTRY REVIEW:
SOLUTIONS
How many mL o f 10.0 M HCl are
needed to prepare 500. mL of
2.00 M HCl?

A. 1.00 mL
B. 10.0 mL
C. 20.0 mL
D. 100. mL
E. 200. mL

ANSWER: d




A solution is prepared by adding 16 g CH3OH
(molar mass 32 g) to 90. g of H2O (molar mass
18.g). The mol fraction of CH3OH in this solution is
closest to which of the following?

A. 0.10
B. 0.20
C. 0.30
D. 0.40
E. 0.60

ANSWER: A




Which of the following measures of
concentrations changes with
temperature

A. mass percentage
B. mol fraction
C. molarity
D. molality
E. parts per million by mass

Answer: C




A sample of 10.0 mol of butyric acid, HC4H7O2, a weak
acid, is dissolved in 1000. g of water to make a 10.0 molal
solution. Which of the following would be the best method
to determine the molarity of the solution.






A. Titration of the solution with a standard acid
B. measurement of the pH with a pH meter
C. determination of the freezing point of the
solution
D. measurement of the total volume of the
solution
E. measurement of the electrical conductivity of
the solution
Answer: D
The nonvolatile compound ethylene glycol, C2H6O2, forms
nearly ideal solutions with water. What is the vapor
pressure of a solution made from 1.00 mole of C2H6O2
and 9.00 moles of H2O if the vapor pressure of pure water
at the same temperature is 25.0 mm Hg.

A. 2.50 mm Hg
B. 7.50 mm Hg
C. 12.5 mm Hg
D. 22.5 mm Hg
E. 27.5 mm Hg

Answer: d




A 360. mg sample of aspirin, C9H8O4, (molar
mass 180.g) is dissolved in enough water to make
200. mL of solution. What is the molarity of
aspirin in a 50. mL sample of this solution
 A. 0.0800 M
 B. 0.0400 M
 C. 0.0200 M
 D. 0.0100 M
 E. 0.00250 M

Answer: D
The molality of glucose in a 1.0 molar glucose solution can be
obtained by using which of the following?
a. Volume of the solution
b. Temperature of the solution
c. Solubility of glucose in water
d. Density of the solution
ANSWER: d
When 70. mL of 3.0 molar Na2CO3 is added to
30. mL of 1.0 molar NaHCO3 the resulting
concentration of Na+ is
a. 2.0
b. 2.4
c. 4.0
d. 4.5
e. 7.0
M
M
M
M
M
ANSWER: D
Which of the following aqueous solutions has
the highest boiling point?
a. 0.10 M potassium sulfate, K2SO4
b. 0.10 M hydrochloric acid, HCl
c. 0.10 M ammonium nitrate, NH4NO3
d. 0.10 M magnesium sulfate MgSO4
e. 0.20 M sucrose C12H22O11
ANSWER: A
what additional information is necessary to calculate
the molarity of the solution?
The density of the water
II. The density of the solution
III. The molar mass of sucrose
I.
a. I only
b. II only
c. III only
d. I and III
e. II and III
I SEEM TO HAVE LEFT OFF PART OF THE PROBLEM 
ANSWER IS PROBABLY B BECAUSE YOU WOULD HAVE TO HAVE THE
MOLAR MASS OF SUCROSE TO CHANGE GRAMS TO MOLES AND THE
DENSITY OF THE SOLUTION TO FIND LITERS
6. If the temperature of an aqueous solution of NaCl
is increased from 20 C to 90 C, which of the following
statements is true?
a. The density of the solution remains unchanged
b. The molarity of the solution remains unchanged
c. The molality of the solution remains unchanged
d. The mole fraction of the solute decreases
e. The mole fraction of the solute increases
ANSWER: C
7. What
is the molality of a solution of
phosphoric acid, H3PO4, that contains 24.5 g of
phosphoric acid (molar mass 98.0g)
in 100. g of H2O
a. 0.245 m
b. 2.50 m
c. 4.00 m
d. 25.0 m
e. 40.0 m
ANSWER: B
1.The freezing point and electrical conductivities
of three aqueous solutions are given below:
Solution
(0.010 molal)
Sucrose
Freezing point
Electrical conductivity
-.0186 C
Almost zero
Formic acid
-.0213 C
Low
Sodium
-.0361 C
high
formate
Explain the relationship between the freezing point and electrical
conductivity for each of the solutions above.
Account for the differences in the freezing points among
the three solutions. SEE FREE RESPONSE #1 ON SHEET