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Clicker Questions
Chapter 17
Barbara Mowery
York College
© 2015 Pearson Education, Inc.
Adding bromide ion to a
saturated aqueous solution of
_______ decreases its
solubility in water.
a.
b.
c.
d.
BaSO4
Li2CO3
PbS
AgBr
© 2015 Pearson Education, Inc.
Adding bromide ion to a
saturated aqueous solution of
_______ decreases its
solubility in water.
a.
b.
c.
d.
BaSO4
Li2CO3
PbS
AgBr
© 2015 Pearson Education, Inc.
Which of the following
mixtures could be used to
prepare an effective buffer
solution?
a.
b.
c.
d.
HCl and KCl
HNO3 and KNO3
HCl and NH4Cl
NH3 and NH4Cl
© 2015 Pearson Education, Inc.
Which of the following
mixtures could be used to
prepare an effective buffer
solution?
a.
b.
c.
d.
HCl and KCl
HNO3 and KNO3
HCl and NH4Cl
NH3 and NH4Cl
© 2015 Pearson Education, Inc.
Which solution has the
greatest buffer capacity?
a. 1 L of solution containing 0.1 M NH3
and 0.1 M NH4Cl
b. 1 L of solution containing 0.05 M NH3
and 0.05 M NH4Cl
c. 1 L of solution containing 0.1 M NH3
and 0.01 M NH4Cl
d. 1 L of solution containing 0.5 M NH3
and 0.5 M NH4Cl
© 2015 Pearson Education, Inc.
Which solution has the
greatest buffer capacity?
a. 1 L of solution containing 0.1 M NH3
and 0.1 M NH4Cl
b. 1 L of solution containing 0.05 M NH3
and 0.05 M NH4Cl
c. 1 L of solution containing 0.1 M NH3
and 0.01 M NH4Cl
d. 1 L of solution containing 0.5 M NH3
and 0.5 M NH4Cl
© 2015 Pearson Education, Inc.
Select the best acid or base to
pair with its conjugate salt to
prepare a buffer with pH ≈ 8.5.
a.
b.
c.
d.
acetic acid, Ka = 1.8 x 10−5
ammonia, Kb = 1.8 x 10−5
hydroxylamine, Kb = 1.1 x 10−8
citric acid, Ka = 7.4 x 10−4
© 2015 Pearson Education, Inc.
Select the best acid or base to
pair with its conjugate salt to
prepare a buffer with pH ≈ 8.5.
a.
b.
c.
d.
acetic acid, Ka = 1.8 x 10−5
ammonia, Kb = 1.8 x 10−5
hydroxylamine, Kb = 1.1 x 10−8
citric acid, Ka = 7.4 x 10−4
© 2015 Pearson Education, Inc.
For HCN, Ka = 4.9 10−10.
What is the pH of a buffer
solution in which [HCN] =
0.100 M = [KCN]?
a.
b.
c.
d.
4.7
7.0
9.3
14.0
© 2015 Pearson Education, Inc.
For HCN, Ka = 4.9 10−10.
What is the pH of a buffer
solution in which [HCN] =
0.100 M = [KCN]?
a.
b.
c.
d.
4.7
7.0
9.3
14.0
© 2015 Pearson Education, Inc.
For HCN, Ka = 4.9 10−10.
[HCN] = 0.100 M, [KCN] = 0.200 M,
pH of buffer solution = _____.
a.
b.
c.
d.
7.0
9.0
9.3
9.6
© 2015 Pearson Education, Inc.
For HCN, Ka = 4.9 10−10.
[HCN] = 0.100 M, [KCN] = 0.200 M,
pH of buffer solution = _____.
a.
b.
c.
d.
7.0
9.0
9.3
9.6
© 2015 Pearson Education, Inc.
For HCN, Ka = 4.9 10−10.
[HCN] = 1.00 M, [KCN] = 0.100 M,
pH of buffer solution = _____.
a.
b.
c.
d.
7.0
8.3
9.0
9.3
© 2015 Pearson Education, Inc.
For HCN, Ka = 4.9 10−10.
[HCN] = 1.00 M, [KCN] = 0.100 M,
pH of buffer solution = _____.
a.
b.
c.
d.
7.0
8.3
9.0
9.3
© 2015 Pearson Education, Inc.
Select the correct representation
of the Henderson-Hasselbach
equation?
a. Ka = [H+][A−]
b. Kw = [H+][OH−] = 10−14
c. pH = pKa +
d. pKa = pH +
© 2015 Pearson Education, Inc.
Select the correct representation
of the Henderson-Hasselbach
equation?
a. Ka = [H+][A−]
b. Kw = [H+][OH−] = 10−14
[base]
c. pH = pKa + log
[acid]
d. pKa = pH +
© 2015 Pearson Education, Inc.
When titrating a weak base
with a strong acid, a good
indicator to use would be
a.
b.
c.
d.
methyl red (color change at pH = 5).
bromothymol blue (change at pH = 7).
phenolphthalein (change at pH = 9).
None of the above
© 2015 Pearson Education, Inc.
When titrating a weak base
with a strong acid, a good
indicator to use would be
a.
b.
c.
d.
methyl red (color change at pH = 5).
bromothymol blue (change at pH = 7).
phenolphthalein (change at pH = 9).
None of the above
© 2015 Pearson Education, Inc.
When titrating a weak acid
with a strong base, a good
indicator to use would be
a.
b.
c.
d.
methyl red (color change at pH = 5).
bromothymol blue (change at pH = 7).
phenolphthalein (change at pH = 9).
None of the above
© 2015 Pearson Education, Inc.
When titrating a weak acid
with a strong base, a good
indicator to use would be
a.
b.
c.
d.
methyl red (color change at pH = 5).
bromothymol blue (change at pH = 7).
phenolphthalein (change at pH = 9).
None of the above
© 2015 Pearson Education, Inc.
For BaCO3, Ksp = 5.0 10−9.
2+
What is [Ba ] in a saturated
aqueous solution of BaCO3?
a.
b.
c.
d.
7.1 10−5 M
1.0 10−8 M
2.5 10−9 M
5.0 10−9 M
© 2015 Pearson Education, Inc.
For BaCO3, Ksp = 5.0 10−9.
2+
What is [Ba ] in a saturated
aqueous solution of BaCO3?
a.
b.
c.
d.
7.1 10−5 M
1.0 10−8 M
2.5 10−9 M
5.0 10−9 M
© 2015 Pearson Education, Inc.
For BaF2, Ksp = 1.7 10−6.
What is [Ba2+] in a saturated
aqueous solution of BaF2?
a.
b.
c.
d.
1.7 10−6 M
3.4 10−6 M
7.6 10−3 M
1.5 10−2 M
© 2015 Pearson Education, Inc.
For BaF2, Ksp = 1.7 10−6.
What is [Ba2+] in a saturated
aqueous solution of BaF2?
a.
b.
c.
d.
1.7 10−6 M
3.4 10−6 M
7.6 10−3 M
1.5 10−2 M
© 2015 Pearson Education, Inc.
Select the correct Ksp expression
for the dissolution of silver sulfate,
Ag2SO4.
a.
b.
c.
d.
[Ag+][SO42−]
[Ag+]2[SO42−]
[Ag+] [SO42−]2
(2[Ag+])2[SO42−]
© 2015 Pearson Education, Inc.
Select the correct Ksp expression
for the dissolution of silver sulfate,
Ag2SO4.
a.
b.
c.
d.
[Ag+][SO42−]
[Ag+]2[SO42−]
[Ag+] [SO42−]2
(2[Ag+])2[SO42−]
© 2015 Pearson Education, Inc.
For BaF2, Ksp = 1.7 10−6.
1−
What is [F ] in a saturated
aqueous solution of BaF2?
a.
b.
c.
d.
1.7 10−6 M
5.7 10−5 M
7.6 10−3 M
1.5 10−2 M
© 2015 Pearson Education, Inc.
For BaF2, Ksp = 1.7 10−6.
1−
What is [F ] in a saturated
aqueous solution of BaF2?
a.
b.
c.
d.
1.7 10−6 M
5.7 10−5 M
7.6 10−3 M
1.5 10−2 M
© 2015 Pearson Education, Inc.
−6
10 .
For BaF2, Ksp = 1.7
If
KF is added to a saturated
solution so that [F1−] = 0.10 M,
what is [Ba2+]?
a.
b.
c.
d.
1.7 10−6 M
1.7 10−5 M
1.7 10−4 M
1.7 10−3 M
© 2015 Pearson Education, Inc.
−6
10 .
For BaF2, Ksp = 1.7
If
KF is added to a saturated
solution so that [F1−] = 0.10 M,
what is [Ba2+]?
a.
b.
c.
d.
1.7 10−6 M
1.7 10−5 M
1.7 10−4 M
1.7 10−3 M
© 2015 Pearson Education, Inc.
Silver bromide is insoluble in
water, but dissolves in
aqueous ammonia, due to the
formation of _______.
a.
b.
c.
d.
Ag(NH3)21+
Ag(NH3)2+
NH3Br1−
NH4Br
© 2015 Pearson Education, Inc.
Silver bromide is insoluble in
water, but dissolves in
aqueous ammonia, due to the
formation of _______.
a.
b.
c.
d.
Ag(NH3)21+
Ag(NH3)2+
NH3Br1−
NH4Br
© 2015 Pearson Education, Inc.
Which ion will precipitate first
when sulfide ion is added to a
solution containing all of the
ions below?
a.
b.
c.
d.
Hg2+
Pb2+
Zn2+
Cd2+
© 2015 Pearson Education, Inc.
Which ion will precipitate first
when sulfide ion is added to a
solution containing all of the
ions below?
a.
b.
c.
d.
Hg2+
Pb2+
Zn2+
Cd2+
© 2015 Pearson Education, Inc.
Which ion will precipitate
when HCl is added to a
solution containing all of the
ions below?
a.
b.
c.
d.
Zn2+
Pb2+
Al3+
Ba2+
© 2015 Pearson Education, Inc.
Which ion will precipitate
when HCl is added to a
solution containing all of the
ions below?
a.
b.
c.
d.
Zn2+
Pb2+
Al3+
Ba2+
© 2015 Pearson Education, Inc.
Which ion will precipitate
when phosphate ion is added
to a solution containing all of
the ions below?
a.
b.
c.
d.
K1+
Ba2+
Na1+
NH41+
© 2015 Pearson Education, Inc.
Which ion will precipitate
when phosphate ion is added
to a solution containing all of
the ions below?
a.
b.
c.
d.
K1+
Ba2+
Na1+
NH41+
© 2015 Pearson Education, Inc.
Which ion will form a precipitate
upon addition of chloride ion,
hydrogen sulfide, ammonium
sulfide, or ammonium hydrogen
phosphate?
a.
b.
c.
d.
Ba1+
Na2+
K1+
NH41+
© 2015 Pearson Education, Inc.
Which ion will form a precipitate
upon addition of chloride ion,
hydrogen sulfide, ammonium
sulfide, or ammonium hydrogen
phosphate?
a.
b.
c.
d.
Ba1+
Na2+
K1+
NH41+
© 2015 Pearson Education, Inc.