Unit 8 Progress Check: MCQ - SUPERTALLTEACHER
AP Chemistry
Unit 8 Progress Check: MCQ
Scoring Guide
1. Pure water autoionizes as shown in the equation above. Based on this information, which of the following is correct?
The autoionization equilibrium for pure water favors the formation of reactants at
A
.
compared to
The autoionization equilibrium for pure water produces the same amount of
ions at
and
B
.
C At
,
for pure water.
D At
,
for pure water.
2.
at
Based on the information above, which of the following is true for a sample of pure water at
?
A
B
C
D
3.
The endothermic autoionization of pure water is represented by the chemical equation shown
above. The of pure water is measured to be 7.00 at
and 6.02 at
. Which of the
following statements best explains these observations?
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Page 1 of 20
AP Chemistry
Unit 8 Progress Check: MCQ
A At the higher temperature water dissociates less, B At the higher temperature water dissociates less, C At the higher temperature water dissociates more, D At the higher temperature water dissociates more,
Scoring Guide
, and the water becomes basic. , and the water remains neutral. , and the water becomes acidic. , and the water remains neutral.
4. Which of the following gives the best estimate for the of a ?
A
because
is a strong acid.
B
because
is a weak acid.
C
because
is a weak base.
D
because
is a strong base.
solution at
5. Which of the following gives the best estimate for the of a ?
solution at
Copyright ? 2017. The College Board. These materials are part of a College Board program. Use or distribution of these materials online or in print beyond your school's participation in the program is prohibited.
Page 2 of 20
AP Chemistry
Unit 8 Progress Check: MCQ
A
because
is a strong acid.
B
because
is a strong acid.
C
because
is a strong base.
D
because
is a strong base.
Scoring Guide
6. Which of the following is the correct mathematical relationship to use to calculate the of a aqueous solution?
A
B
C
D
7.
at
Initial
Percent Ionization
Equilibrium
0.150
3.4%
0.100
4.2%
0.0500
5.8%
The equilibrium for the acid ionization of
is represented by the equation above and the
table gives the percent ionization for
at different initial concentrations of the weak acid at
. Based on the information, which of the following is true for a
aqueous solution of
?
Copyright ? 2017. The College Board. These materials are part of a College Board program. Use or distribution of these materials online or in print beyond your school's participation in the program is prohibited.
Page 3 of 20
AP Chemistry
Unit 8 Progress Check: MCQ
It has a larger percent ionization, a lower
A
solution does. It has a larger percent ionization, a lower
B
solution does. It has a lower percent ionization, a larger
C
solution does. It has a lower percent ionization, a larger
D
solution.
, and a lower than a
, and a higher
than a
, and a higher
than a
, and a higher than a
Scoring Guide
8.
The reaction between
and water is represented above. A solution that is initially
in
has a of 11.28. Which of the following correctly predicts the of a solution for which
, and why?
The will be lower than 11.28 because decreasing the initial concentration of
A
equilibrium concentration of the conjugate acid
.
increases the
The will be lower than 11.28 because the equilibrium concentration of
B
when the initial concentration of the base decreases.
ions decreases
The will be higher than 11.28 because decreasing the initial concentration of
C
the equilibrium concentration of the conjugate acid
.
decreases
The will be higher than 11.28 because the equilibrium concentration of
D
when the initial concentration of the base decreases.
ions increases
9.
The acid ionization equilibrium for
at
is shown above. A
aqueous solution of
this acid has a of about 4.2. If a solution with an initial concentration of
of
is
allowed to reach equilibrium at the same temperature, which of the following correctly predicts its
, and why?
Copyright ? 2017. The College Board. These materials are part of a College Board program. Use or distribution of these materials online or in print beyond your school's participation in the program is prohibited.
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AP Chemistry
Scoring Guide
Unit 8 Progress Check: MCQ
The will be higher than 4.2 because increasing the concentration of the weak acid decreases
A
the percent ionization.
The will be higher than 4.2 because, for weak acid solutions, the
B
the initial concentration of the weak acid.
is directly proportional to
The will be lower than 4.2 because increasing the concentration of the weak acid produces
C
more
to establish equilibrium.
The will be lower than 4.2 because the
D
concentration of the weak acid.
of the weak acid is inversely proportional to the initial
10. The weak acid
has a
and
calculate the of the solution?
A
of 4.76. A solution is prepared by mixing
of
of
. Which of the following can be used to
B
C
D
11. Which of the following provides the correct mathematical expression to calculate the of a
solution made by mixing
of
and
of
at
?
Copyright ? 2017. The College Board. These materials are part of a College Board program. Use or distribution of these materials online or in print beyond your school's participation in the program is prohibited.
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