Chapter 15 - Aqueous Ionic Equilibrium
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Chapter 15 - Aqueous Ionic Equilibrium: General Chemistry: 2022FA-CHEM-001B-202
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Chapter 15 - Aqueous Ionic Equilibrium Due
Oct 23 at 11:59pm
Points
22
Questions
22
Available
Aug 29 at 12am - Dec 4 at 11:59pm
Time Limit
None
Allowed Attempts
2
Instructions
Attempt History
Attempt
Time
Score
KEPT
Attempt 2 9 minutes
22 out of 22
LATEST
Attempt 2 9 minutes
22 out of 22
Attempt 1 433 minutes
20 out of 22
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10/13/22, 2:00 AM
Chapter 15 - Aqueous Ionic Equilibrium: General Chemistry: 2022FA-CHEM-001B-202
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Score for this attempt: 22
out of 22
Submitted Oct 13 at 2am
This attempt took 9 minutes.
1 / 1 pts
Question 1
An important buffer in the blood is a mixture of ________.
carbonic acid and bicarbonate ion acetic acid and bicarbonate ion acetic acid and carbonate ion sodium chloride and hydrochloric acid hydrochloric acid and sodium hydroxide 1 / 1 pts
Question 2
Identify a good buffer.
significant amounts of both a weak acid and a strong acid significant amounts of both a weak acid and its conjugate base small amounts of both a weak acid and its conjugate base significant amounts of both a strong acid and a strong base small amounts of both a strong acid and a strong base
10/13/22, 2:00 AM
Chapter 15 - Aqueous Ionic Equilibrium: General Chemistry: 2022FA-CHEM-001B-202
https://sjeccd.instructure.com/courses/32359/quizzes/198733
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1 / 1 pts
Question 3
If the pKa of HCHO
is 3.74 and the pH of an HCHO
/NaCHO
solution is
3.11, which of the following is TRUE?
2
2
2 [HCHO
] = [NaCHO
]
2
2
[HCHO
] < [NaCHO
]
2
2
[HCHO
] << [NaCHO
]
2
2
It is not possible to make a buffer of this pH from HCHO
and NaCHO
.
2
2
[HCHO
] > [NaCHO
]
2
2
1 / 1 pts
Question 4
Calculate the pH of a buffer that is 0.225 M HC
H
O
and 0.162 M
KC
H
O
. The K
for HC
H
O
is 1.8 × 10
.
2
3
2
2
3
2
a
2
3
2
-5
4.89 9.11 4.74 4.60 9.26 1 / 1 pts
Question 5
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Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M
NH
Cl with 200.0 mL of 0.12 M NH
. The K
for NH
is 1.8 × 10
.
4
3
b
3
-5
9.26 4.55 4.74 9.06 9.45 1 / 1 pts
Question 6
Calculate the pH of a solution formed by mixing 200.0 mL of 0.30 M HClO
with 300.0 mL of 0.20 M KClO. The K
for HClO is 2.9 × 10
.
a
-8
7.06 8.01 6.46 7.54 5.99 1 / 1 pts
Question 7
A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in NaF. Calculate
the pH of the solution after the addition of 100.0 mL of 1.00 M HCl. The K
a
10/13/22, 2:00 AM
Chapter 15 - Aqueous Ionic Equilibrium: General Chemistry: 2022FA-CHEM-001B-202
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for HF is 3.5 × 10
.
-4
3.09 3.46 2.78 3.82 4.11 1 / 1 pts
Question 8
A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in LiF. Calculate the
pH of the solution after the addition of 0.150 moles of solid LiOH. Assume
no volume change upon the addition of base. The K
for HF is 3.5 × 10
.
a
-4
3.46 2.85 3.63 4.06 4.24 1 / 1 pts
Question 9
Define buffer capacity.
10/13/22, 2:00 AM
Chapter 15 - Aqueous Ionic Equilibrium: General Chemistry: 2022FA-CHEM-001B-202
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Buffer capacity is the amount of acid or base that can be added to a buffer
without destroying its effectiveness.
Buffer capacity is the amount of base that can be added until all of the acid
is used up.
Buffer capacity is the amount of acid that can be added until all of the acid
is used up.
Buffer capacity is the amount of acid that can be added until all of the base
is used up.
Buffer capacity is the amount of base that can be added until all of the
base is used up.
1 / 1 pts
Question 10
When titrating a strong monoprotic acid and KOH at 25°C, the
pH will be equal to 7 at the equivalence point. titration will require more moles of acid than base to reach the equivalence
point.
pH will be greater than 7 at the equivalence point. pH will be less than 7 at the equivalence point.
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titration will require more moles of base than acid to reach the equivalence
point.
1 / 1 pts
Question 11
When titrating a weak monoprotic acid with NaOH at 25°C, the
pH will be greater than 7 at the equivalence point. titration will require more moles of acid than base to reach the equivalence
point.
titration will require more moles of base than acid to reach the equivalence
point.
pH will be less than 7 at the equivalence point. pH will be equal to 7 at the equivalence point. 1 / 1 pts
Question 12
A 100.0 mL sample of 0.18 M HClO
is titrated with 0.27 M LiOH.
Determine the pH of the solution before the addition of any LiOH.
4
1.05 1.57
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1.74 0.74 0.57 1 / 1 pts
Question 13
A 100.0 mL sample of 0.18 M HClO
is titrated with 0.27 M LiOH.
Determine the pH of the solution after the addition of 30.0 mL of LiOH.
4
2.00 1.21 1.12 2.86 0.86 1 / 1 pts
Question 14
A 100.0 mL sample of 0.10 M NH
is titrated with 0.10 M HNO
.
Determine the pH of the solution after the addition of 50.0 mL of HNO
.
The K
of NH
is 1.8 × 10
.
3
3
3
b
3
-5
10.34 4.74 9.26
10/13/22, 2:00 AM
Chapter 15 - Aqueous Ionic Equilibrium: General Chemistry: 2022FA-CHEM-001B-202
https://sjeccd.instructure.com/courses/32359/quizzes/198733
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7.05 7.78 1 / 1 pts
Question 15
Determine the molar solubility of AgBr in a solution containing 0.150 M
NaBr. K
(AgBr) = 7.7 × 10
.
sp
-13
0.150 M 8.8 × 10
M
-7
5.8 × 10
M
-5
3.9 × 10
M
-13 5.1 × 10
M
-12
1 / 1 pts
Question 16
The molar solubility of ZnS is 1.6 × 10
M in pure water. Calculate the
K
for ZnS.
-12
sp
1.6 × 10
-35
8.0 × 10
-13
3.2 × 10
-12
6.80 × 10
-5
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2.6 × 10
-24
1 / 1 pts
Question 17
The molar solubility of Ag
S is 1.26 × 10
M in pure water. Calculate the
K
for Ag
S.
2
-16
sp
2
1.12 × 10
-8
1.59 × 10
-32
8.00 × 10
-48
6.81 × 10
-63
3.78 × 10
-12
1 / 1 pts
Question 18
Give the equation for an unsaturated solution in comparing Q with K
.
sp
Q = K
sp
Q ≠
K
sp
none of the above Q < K
sp
Q > K
sp
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Chapter 15 - Aqueous Ionic Equilibrium: General Chemistry: 2022FA-CHEM-001B-202
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1 / 1 pts
Question 19
A solution containing AgNO
is mixed with a solution of NaCl to form a
solution that is 0.10 M in AgNO
and 0.075 M in NaCl. What will happen
once these solutions are mixed? K
(AgCl) = 1.77 × 10
.
3
3
sp
-10
Nothing will happen since the molar solubility of AgCl is higher than the
solution concentrations.
There is not enough information to say anything about this solution. Silver chloride will precipitate out of solution, leaving an unsaturated
solution of AgCl.
Nothing will happen since NaCl and AgNO
are both soluble compounds.
3
Silver chloride will precipitate out of solution, leaving a saturated AgCl
solution.
1 / 1 pts
Question 20
A solution containing CaCl
is mixed with a solution of Li
C
O
to form a
solution that is 3.5 × 10
M in calcium ion and 2.33 × 10
M in oxalate
ion. What will happen once these solutions are mixed? K
(CaC
O
) =
2.3 × 10
.
2
2
2
4
-4
-4 sp
2
4
-9
There is not enough information to determine. A precipitate will form since Q > K
for calcium oxalate.
sp
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Chapter 15 - Aqueous Ionic Equilibrium: General Chemistry: 2022FA-CHEM-001B-202
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A precipitate will form as calcium oxalate is not soluble to any extent. Nothing will happen since both calcium chloride and lithium oxalate are
soluble compounds.
Nothing will happen K
> Q for all possible precipitants.
sp
1 / 1 pts
Question 21
A solution contains 0.021 M Cl
and 0.017 M I
. A solution containing
copper (I) ions is added to selectively precipitate one of the ions. At what
concentration of copper (I) ion will a precipitate begin to form? What is the
identity of the precipitate? K
(CuCl) = 1.0 × 10
, K
(CuI) = 5.1 × 10
.
sp
-6
sp
-12
4.8 × 10
M, CuCl
-5
No precipitate will form at any concentration of copper (I). 4.8 × 10
M, CuI
-5
3.0 × 10
M, CuCl
-10
3.0 × 10
M, CuI
-10 1 / 1 pts
Question 22
A solution contains 2.2 × 10
M in Cu
and 0.33 M in LiCN. If the K for
Cu(CN)
is 1.0 × 10
, how much copper ion remains at equilibrium?
-3 2+
f
4
2-
25
2.9 × 10
M
-27
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6.7 × 10
M
-28
1.9 x 10
M
-26
3.8 × 10
M
-24
4.6 × 10
M
-25 Quiz Score: 22
out of 22
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