Chapter 15 Problem Set KEY
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Chemistry
Date
Apr 3, 2024
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CHEM 1411 Chapter 15 Problem Set Key Spring 2024 1 | P a g e Chapter 15 Problem Set Key 1.
Define the following terms. a.
Lewis acid Electron pair acceptor b.
Lewis base Electron pair donor c.
Formation constant K
f
The equilibrium constant for the formation of a coordination complex/complex ion. d.
Dissociation constant K
D
The equilibrium constant for the dissociation of a coordination complex/complex ion. e.
Solubility product constant K
sp
The equilibrium constant for solubility equilibria. 2.
Determine whether the following statement is true or false. If it is false, explain why. A Lewis acid must have a lone pair of electrons. a.
True b.
False Explanation if false: Lewis acids are electron-pair acceptors
; Lewis bases must have a lone pair of electrons because they are electron-pair donors
. 3.
Complete the following dissolution reaction and write the K
sp
expression for each of the following reactions. a.
MgCO
3
(s)
⇋
Mg
2+
(aq) + CO
3
2
─
(aq)
K
sp
= [Mg
2+
][CO
3
2
─
] b.
Li
2
S (s)
⇋
2 Li
+
(aq) + S
2
─
(aq) K
sp
= [Li
+
]
2
[S
2
─
] c.
SrF
2
(s)
⇋
Sr
2+
(aq) + 2 F
─
(aq) K
sp
= [Sr
2+
] [F
─
]
2
d.
Na
2
CrO
4
(s)
⇋
2 Na
+
+ CrO
4
2─
K
sp
= [Na
+
]
2
[CrO
4
2─
] e.
Ba(OH)
2
(s)
⇋
Ba
2+
+ 2 OH
─
K
sp
= [Ba
2+
][OH
─
]
2
f.
Ag(S
2
O
3
)
2
(s)
⇋
Ag
+
+ 2 S
2
O
3
2─
K
sp
= [Ag
+
] [S
2
O
3
2─
]
2
g.
AlBr
3
(s)
⇋
Al
3+
+ 3 Br
─
K
sp
= [Al
3+
][Br
─
]
3
h.
Cu(NO
3
)
2
(s)
⇋
Cu
2+
+ 2 NO
3
─
K
sp
= [Cu
2+
][NO
3
─
]
2
Formation Constant Application 4.
Consider the formation of silver diammonia, which has a K
f
= 1.7 × 10
7
. Ag
+
(aq)
+ 2 NH
3
(aq)
⇄
[Ag(NH
3
)
2
]
+
(aq)
a.
Write the formation constant expression. 𝑲
?
=
[??(?𝑯
?
)
?
+
]
[??
+
][?𝑯
?
]
?
CHEM 1411 Chapter 15 Problem Set Key Spring 2024 2 | P a g e b.
Find the concentration of silver diammonia if [Ag
+
] = 0.001 M and [NH
3
] = 0.003 M. Express your answer to 3 sf. [Ag(NH
3
)
2
+
] = 0.153 M _ 5.
Consider the formation of iron (III) hexacyanide, which has a K
f
= 2 × 10
43
. Fe
3+
(aq)
+ 6 CN
-
(aq)
⇄
[Fe(CN)
6
]
3-
(aq)
a.
Write the formation constant expression. 𝑲
?
=
[𝑭?(??)
𝟔
?−
]
[𝑭?
?+
][??
−
]
𝟔
b.
Find the concentration of cyanide after 86% of the initial concentration of Fe
3+
has been converted to [Fe(CN)
6
]
3-
. Express your answer to 3 sf. [CN
-
] = 8.21 × 10
-8
M _
6.
Consider the formation of zinc tetroxide, which has a K
f
= 2 × 10
15
. Zn
2+
(aq)
+ 4 OH
-
(aq)
⇄
[Zn(OH)
4
]
2-
(aq)
a.
Write the formation constant expression. 𝑲
?
=
[??(?𝑯)
?
?−
]
[??
?+
][?𝑯
−
]
?
b.
Find the concentration of hydroxide after 42% of the initial concentration of Zn
2+
has been converted to [Zn(OH)
4
]
2-
. Express your answer to 3 sf. [OH
-
] = 1.38 × 10
-4
M _
CHEM 1411 Chapter 15 Problem Set Key Spring 2024 3 | P a g e c.
What is the pH after 42% of the initial concentration of Zn
2+
has been converted to [Zn(OH)
4
]
2-
? pH = 10.14 _ K
sp
and Molar Solubility 7.
What is the K
sp
variable dependent on? a.
Concentrations of dissolution products b.
Concentration of solid c.
Temperature of the dissolution d.
Volume of the solution 8.
When can K
sp
values be compared to predict solubility at 25 °C? The compounds must have the same total number of ions in the formula. Example: one could compare the K
sp
’s of AgCl, AgBr, CaCO
3
, and NiSO
4
but CaF
2
cannot be compared since it has 3 ions in total in the formula. a.
Using this assumption, what solution at 25°C has the greatest solubility? Explain below.
a.
CaF
2
K
sp
= 3.2e-11 b.
Tl
2
OH K
sp
= 6.0e-22 c.
PbCl
2
K
sp
= 1.7e-5 d.
Ba(IO
3
)
2
K
sp
= 7.1e-11 Explanation of choice: Because all the compounds have the same total number of ions, it is known that PbCl
2
has the largest K
sp
so it has the greatest solubility. 9.
Aqueous solutions of lithium carbonate and cadmium (II) chloride are combined, precipitating cadmium carbonate. a.
Write the solubility equilibrium system for the formation of cadmium carbonate. Cd
2+
(aq)
+ CO
3
2-
(aq)
⇄
CdCO
3
(s)
b.
Write the K
sp
expression. 𝑲
??
= [??
?+
][??
?
?−
]
c.
Calculate the molar solubility of cadmium carbonate (M and g/L) if the K
sp
= 5.2 × 10
─
12
at 25˚C
. s = 2.3 × 10
-6
M _
s = 3.9 × 10
-4
g/L _
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CHEM 1411 Chapter 15 Problem Set Key Spring 2024 4 | P a g e d.
Using the molar solubility, determine the concentrations of cadmium (II) and carbonate ions. [Cd
2+
] = 2.3 × 10
-6
M _ [CO
3
2-
] = 2.3 × 10
-6
M _ 10.
Aqueous solutions of sodium fluoride and magnesium nitrate are combined, precipitating magnesium fluoride. a.
Write the solubility equilibrium system for the formation of magnesium fluoride. Mg
2+
(aq)
+ 2 F
-
(aq)
⇄
MgF
2
(s)
b.
Write the K
sp
expression. 𝑲
??
= [??
?+
][𝑭
−
]
?
c.
Calculate the molar solubility of magnesium fluoride (M and g/L) if the K
sp
= 6.4 × 10
─
9
at 25˚C
. s = 1.2 × 10
-3
M _
s = 0.073 g/L _ d.
Using the molar solubility, determine the concentrations of magnesium and fluoride ions. [Mg
2+
] = 1.2 × 10
-3
M _ [F
-
] = 2.4 × 10
-3
M _ 11.
Aqueous solutions of barium acetate and potassium phosphate are combined, precipitating barium phosphate. a.
Write the solubility equilibrium system for the formation of barium phosphate. 3 Ba
2+
(aq)
+ 2 PO
4
3-
(aq)
⇄
Ba
3
(PO
4
)
2
(s)
CHEM 1411 Chapter 15 Problem Set Key Spring 2024 5 | P a g e b.
Write the K
sp
expression. 𝑲
??
= [??
?+
]
?
[??
?
?−
]
?
c.
Calculate the molar solubility of barium phosphate (M and g/L) if the K
sp
= 6.0 × 10
-39
at 25˚C.
s = 1.1 × 10
-8
M _
s = 6.7 × 10
-6
g/L _ d.
Using the molar solubility, determine the concentrations of barium and phosphate ions. [Ba
2+
] = 3.3 × 10
-8
M _ [PO
4
3-
] = 2.2 × 10
-8
M _ e.
Determine the Q
sp
if [Ba
2+
] = 1.5 x 10
─7
M and [PO
4
3─
] = 4.0 x 10
─6
M. Would precipitate form? Precipitate will form because Q
sp
> K
sp
Q
sp
= _ 5.40 x 10
─32
_ 12.
Describe the reaction direction and predict whether precipitation occurs or not if: a.
Q
sp
> K
sp
Reaction proceeds backwards, precipitation observed (solution is saturated) b.
Q
sp
< K
sp
Reaction proceeds forward, no precipitation occurs (solution is unsaturated) c.
Q
sp
= K
sp
The solution is saturated, no change will occur
CHEM 1411 Chapter 15 Problem Set Key Spring 2024 6 | P a g e 13.
Complete the table. Compound K
sp
Q Precipitation formed? TlSCN 1.6 × 10
─4
1.6 × 10
─14
No Cu
2
S 2.5 x 10
─48
3.2 x 10
─45
Yes Cr(OH)
3
6.7 × 10
─31
4.2 × 10
─29
Yes SrSO
4
3.2 × 10
─7
7.7 × 10
─10
No PbCrO
4
2.0 x 10
─16
4.2 x 10
─12
Yes 14.
What is the common ion effect? Write an example of an ionic compound that when added to a solution of MgCO
3
would be subject to the common ion effect. The solubility of an ionic compound is decreased in a solution containing a common ion that is produced by the dissolution of an ionic compound. Examples include: MgF
2
, Mg(OH)
2
, MnS or CaCO
3
, SrCO
3
, BaCO
3
, MnCO
3
, CoCO
3
and most other carbonate compounds excluding group 1A. 15.
An experiment was prepared with multiple solutions barium chromate. Predict the what occurs with respect to the concentration of Ba
2+
and CrO
4
2-
, along with the solid BaCrO
4
as each compound was added to each beaker of barium chromate solution. a.
Additional water was added.
Additional water only further dilutes the solution. It does not change the number of moles in the solution but does lower the molar concentration. b.
BaF
2
was added.
A common ion was added which shifts the solubility equilibrium to the left. It lowers the concentration of chromate ion and increase the solid BaCrO
4
in solution. c.
AgBr was added.
The compound does not contain a common ion, has no effect. d.
CuCrO
4
was added.
A common ion was added which shifts the solubility equilibrium to the left. It lowers the concentration of chromate ion and increase the solid BaCrO
4
in solution. 16.
A beaker with 450 mL of water had 0.045 g of AgBrO
3
added. Determine the Q
sp
. Will it dissolve completely? (K
sp
= 5.5 x 10
─5
) Q
sp
< K
sp
no precipitation occurs. Q
sp
= __ 1.80 x 10
─
7
_
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CHEM 1411 Chapter 15 Problem Set Key Spring 2024 7 | P a g e 17.
Calcium sulfide is added to a solution containing 0.50 M Cu
+
and 0.50 M Ag
+
ions. Cu
2
S has K
sp
= 2.5 × 10
-48
and Ag
2
S has K
sp
= 1.6 × 10
-49
. a.
Write the K
sp
expression for both complex ions. 𝑲
??
= [??
+
]
?
[𝑺
?−
]
𝑲
??
= [??
+
]
?
[𝑺
?−
]
b.
What is the threshold concentration of sulfide ions needed to precipitate Cu
2
S? [S
2-
] = 1.0 × 10
-47
M _ c.
What is the threshold concentration of sulfide ions needed to precipitate Ag
2
S? [S
2-
] = 6.4 × 10
-49
M _ d.
Which compound will precipitate first when calcium sulfide is added in increasing increments? Ag
2
S 18.
Strontium chloride is added to a solution containing 0.310 M SO
3
2-
and 0.265 M CrO
4
2-
ions. SrSO
3
has K
sp
= 3.2 × 10
-7
and SrCrO
4
has K
sp
= 3.6 × 10
-5
. a.
Write the K
sp
expression for both complex ions. 𝑲
??
= [𝑺?
?+
][𝑺?
?
?−
]
𝑲
??
= [𝑺?
?+
][???
?
?−
]
b.
What is the threshold concentration of strontium ions needed to precipitate SrSO
3
? [Sr
2+
] = 1.0 × 10
-6
M _ c.
What the threshold concentration of strontium ions needed to precipitate SrCrO
4
? [Sr
2+
] = 1.4 × 10
-4
M _ d.
Which compound will precipitate first when strontium chloride is added in increasing increments? SrSO
3
CHEM 1411 Chapter 15 Problem Set Key Spring 2024 8 | P a g e 19.
Sodium hydroxide is added to a solution containing 0.75 M Sn
2+
and 0.65 M Fe
3+
ions. Sn(OH)
2
has K
sp
= 3.0 × 10
-27
and Fe(OH)
3
has K
sp
= 4.0 × 10
-38
. a.
Write the K
sp
expression for both complex ions. 𝑲
??
= [𝑺?
?+
][?𝑯
−
]
?
𝑲
??
= [𝑭?
?+
][?𝑯
−
]
?
b.
What concentration of hydroxide ions are needed to precipitate Sn(OH)
2
? [OH
-
] = 6.3 × 10
-14
M _ c.
What concentration of hydroxide ions are needed to precipitate Fe(OH)
3
? [OH
-
] = 3.94 × 10
-13
M _ d.
Which compound will precipitate first when sodium hydroxide is added in increasing increments? Sn(OH)
2
i.
What is the pH required to precipitate the compound chosen? _ pH = 0.80
_ 20.
Use the following reaction and information to solve the following questions. Cu(OH)
2
(s)
⇋
Cu
2+
(aq)
+ 2 OH
─
(aq)
K
so
= 4.8 x 10
─20
a.
Write the K
sp
expression. K
sp
= [Cu
2+
] [OH
─
]
2
b.
What is the molar solubility when K
so
= 4.8 x 10
─20
at 25°C? s = ___
2.3 x 10
-7
M
_ c.
What is the pOH of the solution when the concentration of Cu
2+
is 0.54 M? pOH = ___ 9.53 _
CHEM 1411 Chapter 15 Problem Set Key Spring 2024 9 | P a g e d.
Write the reaction for formation of copper (II) tetraammonia ([Cu(NH
3
)
4
]
2+
) (K
f
= 6.8 x 10
12
). Cu
2+
(aq)
+ 4 NH
3
(aq)
⇋
[Cu(NH
3
)
4
]
2+
(aq)
e.
Write the overall reaction for the formation of Cu(NH
3
)
4
2+
from Cu(OH)
2
and ammonia. Cu(OH)
2
(s)
+ 4 NH
3
(aq)
⇋
[Cu(NH
3
)
4
]
2+
(aq)
+ 2 OH
-
(aq)
f.
Write the K
overall expression for the given reaction. 𝑲
?????𝒍𝒍
= 𝑲
??
𝑲
?
=
[??(?𝑯
?
)
?
?+
][?𝑯
−
]
?
[?𝑯
?
]
?
g.
Determine the K
overall
. K
overall
= ____ 3.26 x 10
-7
_ h.
What is the concentration of Cu(NH
3
)
4
2+
when the solution has 500 mg/L of ammonia with a pH of 7.45? __ 3.03 M _
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- 13. What is the molar solubility of Pbl2 in an aqueous solution containing 0.15 M Nal? The Ksp of Pblz is 1.4x10-8. a. 6.2x107 M b. 9.3x10-8 M 4.7x10-8 M d. 1.6x107 M e. 2.5x107 M Only typedc solutionarrow_forwardI need help with this problemarrow_forwardAfter adding the water how was the equilibrium affected? If a compound was removed how? Explain the effect of water addition using Le Chatelier's Principle.arrow_forward
- The solubility product expression for La2(CO3)3 is Ksp = __. a) [La3+]3[CO32-]2 b) [La2+]3[CO32-]2 c) [La3+]2[CO32-]3 d) [2La3+]2[3CO32-]3 e) [2La3+][3CO32-]arrow_forwardWhat is the Kf expression for the following complexation reaction? Al* (aq) + 6F (aq) TAIF* (aq) Select one: | AIF| K = Al- || F]° A. | AIF ° | A || F| K = | A13+ ][ F| Kf = | AIF,3- 1 C. | AP || F]° Kf = | AIF-| D. B.arrow_forward0 Calculate the minimum concentration of Cr³+ required in a 0.095 M (aq) NaF solution in order to initiate a precipitate of chromium (III) fluoride. (For CrF3, Ksp = 6.6 x 10-¹¹) A. 0.023 M B. 0.032 M C. 6.9 × 10-10 M 2.9 x 10¹9 M 7.7 x 108 M D. E.arrow_forward
- Please don't provide handwritten solution ....arrow_forwardA solution is prepared such that the initial concentration of A2+ is 1.50x103 M and the initial concentration of X is 4.60x10-3 M. A2+ and X are allowed to react as shown below to establish equilibrium with the complex AX2+. In a colorimetry experiment, the equilibrium concentration of the complex AX2+ is determined to be 8.9x10-4 M. A2* (aq) + X (aq) =Ax2+ (aq) %3D Complete the ICE table below by selecting the correct value or expression to place in the ICE table from the drop-down menu. A2+ (aq) X (ад) АХ2+ (aq) Initial concentration Change in concentration Equilibrium concentration expression Equilibrium concentration valuearrow_forwardWhat is the solubility-product expression for La(IO3)3 (s)? A. Ksp = [La3+] [IO3-]1/3 B. Ksp = [La3+] [IO3-] C. Ksp = [La3+]3 [IO3-] D. Ksp = [La3+]3 [IO3-]arrow_forward
- For AgOH, Ksp = 1.5 x 10-8. What is the molar solubility of AgOH in a solution containing 0.1 M of NH3 buffered at pH = 7? (K;[Ag(NH3)2')= 1.6 x 107). A. 0.20 M B. 0.025 M C. 0.25 M D. 0.05 Marrow_forwardAccording to the equilibrium equation, which ion(s) do you have when solution dissolved?Explain how you know the identity of the ion(s) present.arrow_forwardWhat is the equilibrium constant expression for the Ksp of Fe2S3? a. Ksp = [2Fe3+]2 [3S2-]3 b. Ksp = [2Fe3+] [3S2-] c. Ksp = [Fe3+]2 [S2-]3 d. Ksp = [Fe3+] [ S2-]arrow_forward
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