Master List for Chapter 7
Modified True/False
Indicate whether the sentence or statement is true or false. If false, change the identified word or phrase to
make the sentence or statement true.
____
1. A precipitate forms when the ion product for the precipitate exceeds the Ksp. _________________________
____
2. When a solution of silver nitrate is mixed with a solution of potassium iodide a precipitate of lead iodide never
forms when [I1-][Ag1+] exceeds the Ksp. _________________________
____
3. A solution of lead(II) nitrate is mixed with a solution of sodium iodide and a precipitate forms. The precipitate is
lead(II) iodide. _________________________
____
4. When a precipitate forms at the bottom of a container after 2 unsaturated solutions are mixed, the solid
precipitate is always in equilibrium with its liberated ions in solution. _________________________
____
5. Ksp values are temperature dependent. _________________________
____
6. More potassium bromide can dissolve in distilled water than in a solution of potassium chloride.
_________________________
____
7. The formula for silver acetate is AgC3H5O2. _________________________
____
8. The Ksp equilibrium expression for lead(II) chloride is Pb2Cl(s) <====> 2Pb2+(aq) + Cl1-(aq).
_________________________
____
9. When 25 mL of 0.24 mol/L CaCl2 is mixed with 45 mL of 1.5 mol/L AgNO3 a precipitate of AgCl forms since
the Ksp of AgCl is 1.8  10-10. _________________________
____ 10. The Ksp's of CuCl and TlCl are 1.910-7 and 1.8  10-4 respectively. This means TlCl is more soluble than
CuCl. _________________________
____ 11. The pH of 0.0050 mol/L solutions of Ca(OH)2 and NaOH are compared. The NaOH has a higher pH.
______________________________
____ 12. The Ksp expression for magnesium phosphate is
Mg3(PO4)2(s) <====> 3 Mg2+(aq) + 2 PO43-(aq). _________________________
____ 13. For the gaseous equilibrium shown, 3A + B <====> C + 2D, some C is added to the system. The quantity of D
will rise. _________________________
____ 14. For the gaseous equilibrium shown, 2A + 3B <====> C + 2D + heat.
If the temperature of the system is decreased, the quantity of B will increase 3/2 as much as the quantity of A.
______________________________
____ 15. For the gaseous equilibrium shown, 3A + B <====> 4C + D + heat.
If some B is removed from the system, the quantity of C will decrease 4's as much as the quantity of D
decreases. _________________________
____ 16. For the gaseous equilibrium shown, 2A + 3B <====> 4C + D + heat.
If some B is added to the system, the quantity of C will decrease 4's as much as the quantity of D decreases.
______________________________
____ 17. In a saturated solution of silver carbonate, the quantity of silver ion = the quantity of carbonate ion.
_________________________________________________________________
____ 18. In a saturated solution of cobalt(II) hydroxide, the quantity of cobalt(II) ion is double the quantity of hydroxide
ion. __________________________________________________
Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
____ 19. When solid lead(II) phosphate is in equilibrium with its ions, the ratio of lead(II) ions to phosphate ions is which
of the following?
a. 1:1
d. 2:3
b. 1:2
e. 3:2
c.
2:1
____ 20. When solid zinc hydroxide is in equilibrium with its ions, the ratio of zinc ion to hydroxide ion is which of the
following?
a. 1:2
d. 1:3
b. 2:1
e. 2:3
c.
1:1
____ 21. When solid aluminum hydroxide is in equilibrium with its ions, the ratio of aluminum ion to hydroxide ion is
which of the following?
a. 1:1
d. 1:3
b. 2:1
e. 3:1
c.
1:2
____ 22. When solid plumbous sulfate is in equilibrium with its ions, the ratio of plumbous ion to sulfate ion is which of
the following?
a. 1:2
d. 3:1
b. 2:1
e. 1:3
c.
1:1
____ 23. When solid barium fluoride is in equilibrium with its ions, the ratio of fluoride ion to barium ion is which of the
following?
a. 1:1
d. 2:3
b. 1:2
e. 3:2
c.
2:1
____ 24. In a saturated solution of silver phosphate, the concentration of silver ion is 4.5  10-4 mol/L. The Ksp of silver
phosphate would be which of the following?
a. 6.8  10-8
d. 1.0  10-11
b. 1.4  10-14
e. none of the above
c.
1.5  10-15
____ 25. In a saturated solution of lead(II) chloride, the concentration of chloride ion is 6.2  10-4 mol/L. The Ksp of
lead(II) chloride would be which of the following?
a. 1.9  10-7
d. 2.3  10-17
b. 6.0  10-11
e. none of the above
c.
1.2  10-10
____ 26. In a saturated solution of silver sulfite, the concentration of silver ion is 3.6  10-4 mol/L. The Ksp of silver
sulfite would be which of the following?
a. 6.5  10-8
d. 7.6  10-19
b. 2.3  10-11
e. none of the above
c.
1.2  10-11
____ 27. In a saturated solution of aluminum hydroxide, the concentration of aluminum ion is 2.4  10-8 mol/L. The Ksp
of aluminum hydroxide would be which of the following?
a.
b.
c.
1.7  10-15
4.2  10-23
1.0  10-30
d.
e.
9.0  10-30
none of the above
____ 28. In a saturated solution of NiCO3, the concentration of nickel(II) ion is 7.6  10-4 mol/L. The Ksp of nickel(II)
carbonate would be which of the following?
a. 5.8  10-7
d. 7.6  10-4
b. 1.2  10-6
e. none of the above
c.
4.4  10-10
____ 29. In a saturated solution of PbBr2, the concentration of Br1- is 8.2  10-2 mol/L. The [Pb2+] in mol/L is which of
the following?
a. 8.2  10-2
d. 0.24
b. 4.1  10-2
e. none of the above
c.
0.16
____ 30. In a saturated solution of Al(OH)3 the concentration of OH1- is 2.6  10-5 mol/L. The concentration of Al3+ in
mol/L is which of the following?
a. 2.6  10-5
d. 7.8  10-5
b. 5.2  10-5
e. 8.7  10-4
c.
7.8  10-15
____ 31. For the equilibrium system below, which of the following would result in an increase in the quantity of PCl 5(g)?
PCl3(g) + Cl2(g) <=====> PCl5(g) + 45 kJ
a. increasing temperature
d. removing some Cl2(g)
b. increasing the size of the container
e. injecting some He gas
c.
decreasing temperature
____ 32. For the equilibrium system below, which of the following would result in a decrease in the quantity of PCl 5(g)?
PCl3(g) + Cl2(g) <=====> PCl5(g) + 45 kJ
a. increasing temperature
d. decreasing the size of the container
b. adding some Cl2(g)
e. injecting some He gas
c.
decreasing temperature
____ 33. For the equilibrium system below, which of the following would result in an increase in the quantity of Cl 2(g)?
PCl3(g) + Cl2(g) <=====> PCl5(g) + 45 kJ
a. adding some PCl3(g)
d. increasing the volume of the container
b. removing some PCl5(g)
e. injecting some He gas
c.
decreasing temperature
____ 34. For the equilibrium system below, which of the following would result in an increase in the quantity of H2(g)?
H2(g) + I2(g) <=====> 2HI(g) + 65 kJ
a. removing some I2(g)
d. both b and c
b. removing some HI(g)
e. both a and b
c.
decreasing temperature
____ 35. For the equilibrium system below, which of the following would result in an decrease in the quantity of H2(g)?
H2(g) + I2(g) <=====> 2HI(g) + 65 kJ
a. increasing temperature
b. adding some HI(g)
c. decreasing the volume of the container
d. increasing the volume of the container
____ 36.
____ 37.
____ 38.
____ 39.
____ 40.
____ 41.
____ 42.
____ 43.
e. none of the above
For the equilibrium system below, which of the following would result in an increase in the quantity of CO(g)?
2H2(g) + CO(g) <=====> CH3OH(g) + 92 kJ
a. decreasing temperature
b. decreasing the volume of the container
c. adding some CH3OH
d. both a and b
e. both b and c
Some CO2 is removed from the equilibrium system shown below. Which of the following statements is/are true
when the equilibrium responds to this stress?
CO(NH2)2(g) + H2O(g) + 45 kJ <=====> CO2(g) + 2 NH3
a. heat is released as the equilibrium shifts to replace the removed CO2
b. the quantity of NH3 will rise twice as much as CO2
c. the quantity of H2O(g) will rise
d. both a and b are true
e. both b and c are true
1.2 mol of CH3OH(g) are injected into a 2.0 L container and the following equilibrium becomes established.
2H2(g) + CO(g) <=====> CH3OH(g) + 92 kJ
If at equilibrium 1.0 mol of CH3OH is still in the container the Ke must be which of the following?
a. 25
d. 12.5
b. 125
e. 0.032
c.
0.0080
1.6 mol of CH3OH(g) are injected into a 4.0 L container and the following equilibrium becomes established.
2H2(g) + CO(g) <=====> CH3OH(g) + 92 kJ
If at equilibrium 0.80 mol of CH3OH is still in the container the Ke must be which of the following?
a. 0.78
d. 0.16
b. 25
e. 6.25
c.
5.0
2.4 mol of PCl5(g) are injected into a 2.0 L container and the following equilibrium becomes established.
PCl5(g) <=====> PCl3(g) + Cl2(g)
If at equilibrium 1.0 mol of PCl5(g) is still in the container the Ke must be which of the following?
a. 2.0
d. 0.98
b. 1.4
e. 1.02
c.
0.71
4.5 mol of HI(g) are injected into a 5.0 L container and the following equilibrium was established.
H2(g) + I2(g) <=====> 2HI(g) + 65 kJ
If at equilibrium there was 4.0 mol of HI(g) left the Ke for this equilibrium must be which of the following?
a. 8.0
d. 0.063
b. 16
e. 0.016
c.
64
For the equilibrium system below, which of the following would result in a decrease in the quantity of H2(g)?
N2(g) + 3H2(g) <=====> 2NH3(g) + 94 kJ
a. decreasing the volume of the container
d. removing some ammonia gas
b. decreasing the temperature
e. none of the above
c.
adding some ammonia gas
6.0 mol of ammonia gas is injected into a 3.0 L container. At equilibrium 1.5 mol of hydrogen gas is found in the
container. The number of moles of ammonia gas left in the container must be which of the following?
____ 44.
____ 45.
____ 46.
____ 47.
____ 48.
____ 49.
____ 50.
____ 51.
N2(g) + 3H2(g) <=====> 2NH3(g) + 94 kJ
a. 2.0
d. 5.0
b. 3.0
e. 4.5
c.
4.0
10.0 mol of ammonia gas is injected into a 4.0 L container. At equilibrium 1.2 mol of hydrogen gas is found in
the container. The number of moles of ammonia gas left in the container must be which of the following?
N2(g) + 3H2(g) <=====> 2NH3(g) + 94 kJ
a. 6.8
d. 8.8
b. 6.4
e. 9.2
c.
8.6
10.0 mol of ammonia gas is injected into a 4.0 L container. At equilibrium 1.2 mol of nitrogen gas is found in the
container. The number of moles of ammonia gas left in the container must be which of the following?
N2(g) + 3H2(g) <=====> 2NH3(g) + 94 kJ
a. 8.8
d. 6.4
b. 2.4
e. 9.2
c.
7.6
10.0 mol of ammonia gas is injected into a 4.0 L container. At equilibrium 1.2 mol of hydrogen gas is found in
the container. The Ke for this equilibrium must be which of the following?
N2(g) + 3H2(g) <=====> 2NH3(g) + 94 kJ
a. 1.8  103
d. 3.0
b. 5.6  10-4
e. 2.8
c.
73
4.5 mol of HI(g) are injected into a 5.0 L container and the following equilibrium was established.
H2(g) + I2(g) <=====> 2HI(g) + 65 kJ
If the Ke = 64 the concentration, in mol/L, of HI left in the container is which of the following?
a. 0.042
d. 0.82
b. 0.084
e. 0.041
c.
0.80
The equilibrium system shown below was analyzed and the concentrations of HI(g), H2(g), and I2(g) were
found, in mol/L, to be 4.4, 3.2, 1.5 respectively. The equilibrium constant must be which of the following?
H2(g) + I2(g) <=====> 2HI(g) + 65 kJ
a. 4.0
d. 1.1
b. 0.25
e. 0.16
c.
0.92
The equilibrium system shown below was analyzed and the concentrations of H2(g), I2(g) and HI(g), were
found, in mol/L, to be 4.2, 3.8, 1.6 respectively. The equilibrium constant must be which of the following?
H2(g) + I2(g) <=====> 2HI(g) + 65 kJ
a. 0.10
d. 2.3
b. 28
e. 1.4
c.
0.16
The equilibrium shown below was analyzed and the concentrations of PCl5(g), PCl3(g) and Cl2(g) were found,
in mol/L, to be 4.5, 2.6 and 1.2. The equilibrium constant must be which of the following?
PCl5(g) <=====> PCl3(g) + Cl2(g)
a. 1.4
d. 0.84
b. 0.69
e. 1.2
c.
9.8
Which of the following systems would be considered to be at equilibrium:
I. an open flask with 2.0 mL of perfume
II. a closed flask with 10 mL of water
____ 52.
____ 53.
____ 54.
____ 55.
____ 56.
III. an open flask with 10 mL of water
IV. a closed flask with an ice cube and 10 mL of water
a. I
d. II
b. I and II
e. III
c.
II and IV
6.4 g of potassium hydroxide crystals are placed in 1.5 L of distilled water. After 2 days a few crystals are still
visible. The condition this system is in is best described as which of the following?
a. at minimum entropy
d. at equilibrium
b. at maximum enthalpy
e. supersaturated
c.
saturated
A flask contains this equilibrium
Fe3+(aq) + SCN1-(aq) <======> FeSCN1-(aq)
What is observed if a few drops of iron(II) chloride is added to this equilibrium?
a. it becomes darker red
d. nothing happens
b. it becomes lighter red
e. none of the above
c.
it becomes colourless
A flask contains this equilibrium
Fe3+(aq) + SCN1-(aq) <======> FeSCN1-(aq)
What is observed if a few drops of iron(III) chloride is added to this equilibrium?
a. it becomes darker red
d. nothing happens
b. it becomes lighter red
e. none of the above
c.
it becomes colourless
A full syringe contains this equilibrium
2 NO2(g) <======> N2O4(g)
If nitrogen dioxide gas is brown and the other gas is colourless, what is observed when the syringe is used to
compress this gas mixture?
a. the mixture gets darker
d. the mixture gets lighter
b. the mixture gets darker then lighter
e. none of the above
c.
the mixture get lighter then darker
If the equilibrium shown below is heated at a constant pressure.
H2(g) + I2(g) <=====> 2HI(g) + 65 kJ
What is most likely to happen?
a. Ke gets larger
d. both a and c
b. Ke gets smaller
e. both b and c
c.
[H2] gets smaller
____ 57. If the equilibrium shown below is cooled at a constant pressure.
H2(g) + I2(g) <=====> 2HI(g) + 65 kJ
What is most likely to happen?
a. Ke decreases
d. both a and c
b. Ke increases
e. both b and c
c.
[HI] increases
____ 58. A closed flask contains this equilibrium
2 NO2(g) (brown gas) <======> N2O4(g) (colourless gas)
When the equilibrium is heated at a constant pressure it gets browner. This must mean which of the following?
a. Ke is very large
d. both a and b
b. it is endothermic
e. both a and c
c.
it is exothermic
____ 59. Consider this equilibrium
N2(g) + 3H2(g) <=====> 2NH3(g) + 94 kJ
____ 60.
____ 61.
____ 62.
____ 63.
____ 64.
____ 65.
____ 66.
If some nitrogen gas were injected into this system at constant temperature and pressure the system would most
likely experience which of the following?
a. an increase in [hydrogen]
d. an increase in [ammonia]
b. a decrease in [ammonia]
e. both c and d
c.
a decrease in [hydrogen]
If the equilibrium constant for an equilibrium system is decreased by an increase in temperature then
a. [reactants] and [products] decreases
b. [reactants] and [products] increases
c. [reactants] increases and [products] decreases
d. [reactants] decreases and [products] increases
e. none of the above
If the equilibrium constant for an equilibrium system is increased by an increase in temperature then
a. [reactants] and [products] decreases
b. [reactants] and [products] increases
c. [reactants] increases and [products] decreases
d. [reactants] decreases and [products] increases
e. none of the above
If the equilibrium constant for an equilibrium system is increased by a decrease in temperature then
a. [reactants] and [products] decreases
b. [reactants] and [products] increases
c. [reactants] increases and [products] decreases
d. [reactants] decreases and [products] increases
e. none of the above
If the equilibrium constant for an equilibrium system is decreased by a decrease in temperature then
a. [reactants] and [products] decreases
b. [reactants] and [products] increases
c. [reactants] increases and [products] decreases
d. [reactants] decreases and [products] increases
e. none of the above
Which equilibrium shows an increase in [products] when the volume decreases?
I. 2H2(g) + O2(g) <====> 2H2O(g)
II. Cl2(g) + PCl3(g) <====> PCl5 (g)
III. H2(g) + I2(g) <====> 2HI(g)
IV. 2NH3(g) <====> N2 + 3H2(g)
a. I
d. III and IV
b. I and II
e. II
c.
IV
Which equilibrium shows a decrease in [products] when the volume decreases?
I. 2H2(g) + O2(g) <====> 2H2O(g)
II. Cl2(g) + PCl3(g) <====> PCl5 (g)
III. H2(g) + I2(g) <====> 2HI(g)
IV. 2NH3(g) <====> N2 + 3H2(g)
a. I
d. III and IV
b. I and II
e. II
c.
IV
Which equilibrium shows a increase in [products] when the volume increases?
I. 2H2(g) + O2(g) <====> 2H2O(g)
II. Cl2(g) + PCl3(g) <====> PCl5 (g)
III. H2(g) + I2(g) <====> 2HI(g)
____ 67.
____ 68.
____ 69.
____ 70.
IV. 2NH3(g) <====> N2 + 3H2(g)
a. I
d. III and IV
b. I and II
e. II
c.
IV
Which equilibrium shows a decrease in [products] when the volume increases?
I. 2H2(g) + O2(g) <====> 2H2O(g)
II. Cl2(g) + PCl3(g) <====> PCl5 (g)
III. H2(g) + I2(g) <====> 2HI(g)
IV. 2NH3(g) <====> N2 + 3H2(g)
a. I
d. III and IV
b. I and II
e. II
c.
IV
Consider the following system at equilibrium:
C2H2(g) + Br2(g) + 44 kJ <======> C2HBr2(g)
Which of the following actions would cause the Ke to increase?
I. increasing the volume at constant pressure and temperature
II. decreasing the volume at constant pressure and temperature
III. increasing the temperature
IV. adding bromine gas at constant temperature and pressure
V. removing ethyne gas at constant temperature and pressure
VI. decreasing the temperature
a. I and II
d. III
b. III and VI
e. VI
c.
IV and V
Consider the following system at equilibrium:
C2H2(g) + Br2(g) + 44 kJ <======> C2H2Br2(g)
Which of the following actions would cause the Ke to decrease?
I. increasing the volume at constant pressure and temperature
II. decreasing the volume at constant pressure and temperature
III. increasing the temperature
IV. adding bromine gas at constant temperature and pressure
V. removing ethyne gas at constant temperature and pressure
VI. decreasing the temperature
a. I and II
d. III
b. III and VI
e. VI
c.
IV and V
Consider this equilibrium
N2(g) + H2(g) <=====> NH3(g) + 94 kJ
The equilibrium law expression for the balanced chemical equation would be
a. [N2][H2] / [NH3]
d. [NH ]2 / [H ]3[N ]
3
2
2
b. [NH3] / [H2][N2]
e. 2[NH ]2 / 3[H ]3[N ]
3
2
2
c.
2
[NH3] / [H2][N2]
____ 71. Consider this equilibrium
4HCl(g) + O2(g) <=====> 2H2O(g) + 2Cl2(g)
The equilibrium law expression for the balanced chemical equation would be
a. [HCl][O2] / [H2O][Cl2]
d. [HCl]4[O ] / [H O]2[Cl ]2
2
2
2
b. [H O]2[Cl ]2/ [HCl]4[O ]
e. [H2O][Cl2]/HCl][O2]
2
2
2
c.
2[H2O][Cl2]/ 4[HCl][O2]
Completion
Complete each sentence or statement.
72. If solutions of barium chloride and sodium sulfate were mixed and a precipitate formed, the precipitate would be
_________________________.
73. If solutions of silver nitrate and copper(II) bromide were mixed and a precipitate formed, the precipitate would
be _________________________.
74. If solutions of strontium chloride and potassium chromate were mixed and a precipitate formed, the precipitate
would be ______________________________.
75. If solutions of lead(II) nitrate and lithium chloride were mixed and a precipitate formed, the precipitate would be
_________________________.
76. If solutions of aluminum fluoride and potassium hydroxide were mixed and a precipitate formed, the precipitate
would be ______________________________.
77. If solutions of sodium oxalate and magnesium chloride were mixed and a precipitate formed, the precipitate
would be ______________________________.
78. If solutions of calcium fluoride and potassium carbonate were mixed and a precipitate formed, the precipitate
would be ______________________________.
79. If solutions of sodium phosphate and zinc bromide were mixed and a precipitate formed, the precipitate would
be _________________________.
80. If solutions of silver nitrate and potassium cyanide were mixed and a precipitate formed, the precipitate would be
_________________________.
81. If solutions of lithium sulfite and barium iodide were mixed and a precipitate formed, the precipitate would be
_________________________.
82. If solutions of barium chloride and sodium sulfate were mixed and a precipitate formed, the equilibrium equation
for the precipitate would be _____________________________________________.
83. If solutions of copper(II) nitrate and sodium carbonate were mixed and a precipitate formed, the equilibrium
equation for the precipitate would be _____________________________________________.
84. If solutions of iron(II) chloride and potassium phosphate were mixed and a precipitate formed, the equilibrium
equation for the precipitate would be _____________________________________________.
85. If solutions of potassium chromate and silver nitrate were mixed and a precipitate formed, the equilibrium
equation for the precipitate would be _____________________________________________.
86. If solutions of calcium nitrate and sodium fluoride were mixed and a precipitate formed, the equilibrium
equation for the precipitate would be _____________________________________________.
87. When solid magnesium carbonate is in equilibrium with its ions, the ratio of magnesium ion to carbonate ion is
____________________.
88. When solid lead(II) phosphate is in equilibrium with its ions, the ratio of lead(II) ion to phosphate ion is
____________________.
89. When solid barium monohydrogen phosphate is in equilibrium with its ions, the ratio of barium ion to
monohydrogen phosphate ion is ____________________.
90. When solid zinc hydroxide is in equilibrium with its ions, the ratio of zinc ion to hydroxide ion is
____________________.
91. When solid mercury(II) iodide is in equilibrium with its ions, the ratio of mercury(II) ion to iodide ion is
____________________.
92. CO(g) + 2H2(g)  CH3OH(l); during this reaction the entropy ____________________.
93. S(s) + 2N2O(g)  SO2(g) + 2N2(g); during this reaction the entropy ____________________.
94. NH3(g) + HCl(g)  NH4Cl(s); during this chemical change the algebraic sign for the entropy change is
predicted to be ____________________.
95. 4NO(g)  2N2O(g) + O2(g); during this chemical change the algebraic sign for the entropy change is predicted
to be ____________________.
Matching
Look at the entropy and enthalpy changes below and match them to spontaneity choices below.
a.
S is positive, H is positive
b.
S is negative, H is positive
c.
S is positive, H is negative
d.
S is negative, H is negative
____
____
____
____
96.
97.
98.
99.
spontaneity temperature dependent, spontaneous at high T
spontaneous at all temperatures
nonspontaneous, proceeds only with continuous input of energy
spontaneity temperature dependent, spontaneous at low T
Short Answer
100. Consider the equilibrium below:
If 1.5 mol of PCl5 was placed in a 1.0 L container and allowed to reach equilibrium, what would the value of Ke
be if at equilibrium [PCl5] = 1.2 mol/L?
PCl3(g) + Cl2(g) <=====> PCl5(g)
101. Consider the equilibrium below:
If 1.2 mol of H2 and 1.2 mol of O2 was placed in a 1.0 L container and allowed to reach equilibrium, what
would the value of Ke be if at equilibrium [HI] = 0.40 mol/L?
H2(g) + I2(g) <=====> 2HI(g)
102. Consider the equilibrium below:
If 1.2 mol of HI was placed in a 1.0 L container and allowed to reach equilibrium what would the value of Ke be
if at equilibrium [HI] = 0.40 mol/L.
H2(g) + I2(g) <=====> 2HI(g)
103. Consider the equilibrium below:
If 1.6 mol of HI was placed in a 1.0 L container and allowed to reach equilibrium, what would the equilibrium
concentrations be for H2(g), I2(g) and HI(g) if the Ke = 36?
H2(g) + I2(g) <=====> 2HI(g)
104. Consider the equilibrium below:
If 3.4 mol of HI was placed in a 2.0 L container and allowed to reach equilibrium, what would the equilibrium
concentrations be for H2(g), I2(g) and HI(g) if the Ke = 49?
H2(g) + I2(g) <=====> 2HI(g)
105. The equilibrium system shown below has a Ke = 1.4  10-4. If [A] = 0.24 mol/L, what is the [D]?
3A(g) + B(s) <=====> C(s) + 2D(g)
106. The equilibrium system shown below has a Ke = 8.3  10-2. If [D] = 0.38 mol/L, what is the [A]?
2A(g) + B(s) <=====> C(s) + 3D(g)
107. The equilibrium shown below was analyzed and found to contain 1.4 moles of SO2(g), 2.5 moles of NO2(g), 5.2
moles of SO3(g), and 6.4 moles of NO(g) in a 2.0 L container. How many moles of SO2(g) would have to be
added to increase the equilibrium concentration of SO3(g) to 2.8 mol/L?
SO2(g) + NO2(g) <====> SO3(g) + NO(g)
108. The Ke for the equilibrium shown below is 50. Some methane and hydrogen sulfide are added to a container and
at equilibrium the concentrations of methane and hydrogen sulfide are found to be 0.24 mol/L and 0.36 mol/L
respectively. What are the equilibrium concentrations of carbon disulfide and hydrogen gas?
CH4(g) + 2H2S(g) <====> CS2(g) + 4H2(g)
109. 8.0 moles of pure ammonia gas were injected into a 2.0-L flask and allowed to reach equilibrium according to
the equation shown below. If the equilibrium mixture was analyzed and found to contain 2.0 moles of nitrogen
gas, calculate the value of the equilibrium constant.
2NH3(g) <====> 2N2(g) + 3H2(g)
110. 9.0 moles of pure ammonia gas were injected into a 3.0 L flask and allowed to reach equilibrium according to
the equation shown below. If the equilibrium mixture was analyzed and found to contain 3.0 moles of hydrogen
gas, calculate the value of the equilibrium constant.
2NH3(g) <====> 2N2(g) + 3H2(g)
Problem
111. If the solubility of AgC2H3O2 is 5.0  10-2 mol/L, what is its Ksp?
112. If the solubility of AgBr is 8.8  10-7 mol/L, what is its Ksp?
113. If the solubility of Ag2CO3 is 1.3  10-4 mol/L, what is its Ksp?
114. If the solubility of Cu2S is 7.4  10-17 mol/L, what is its Ksp?
115. If the solubility of CaF2 is 2.3  10-4 mol/L, what is its Ksp?
116. If the solubility of Mg(OH)2 is 1.3  10-4 mol/L, what is its Ksp?
117. If the solubility of Pb(IO3)2 is 4.0  10-5 mol/L, what is its Ksp?
118. If the solubility of Al(OH)3 is 3.2  10-09 mol/L, what is its Ksp?
119. If the solubility of Zn3(PO4)2 is 3.4  10-8 mol/L, what is its Ksp?
120. If the concentration of Pb2+ is found to be 2.3  10-9 mol/L in a saturated solution of Pb3(PO4)2, what is the
Ksp of Pb3(PO4)2 ?
121. If the concentration of Fe3+ is found to be 2.2  10-10 mol/L in a saturated solution of Fe(OH)3, what is the
Ksp of Fe(OH)3?
122. If the concentration of Zn2+ is found to be 1.7  10-5 mol/L in a saturated solution of this salt, what is the Ksp
of Zn(OH)2?
123. If the concentration of Ba2+ is found to be 4.2  10-8 mol/L in a saturated solution of this salt, what is the
Ksp of Ba3(PO4)2?
124. If the concentration of Pb2+ is found to be 1.6  10-2 mol/L in a saturated solution of PbCl2, what is the Ksp of
PbCl2?
125. If the concentration of CrO42- is found to be 6.5  10-5 mol/L in a saturated solution of Ag2CrO4, what is the
Ksp of Ag2CrO4?
126. If the concentration of I-1 is found to be 2.4  10-3 mol/L in a saturated solution of PbI2, what is the Ksp of
PbI2?
127. If the concentration of PO43- is found to be 7.1  10-6 mol/L in a saturated solution of Mg3(PO4)2, what is the
Ksp of Mg3(PO4)2?
128. If the concentration of CN1- is found to be 1.4  10-6 mol/L in a saturated solution of AgCN, what is the Ksp of
AgCN?
129. If the concentration of CO32- is found to be 1.3  10-4 mol/L in a saturated solution of Ag2CO3, what is the
Ksp of Ag2CO3?
130. If 1.7 L of a saturated solution of AgC2H3O2 is found to contain 14.1 g of AgC2H3O2, what is the Ksp of
AgC2H3O2.
131. If 2.6 L of a saturated solution of MgCO3 is found to contain 1.1 g of MgCO3, what is the Ksp of MgCO3.
132. If 12 L of a saturated solution of PbSO4 is found to contain 0.46 g of PbSO4, what is the Ksp of PbSO4
133. If 1.4 L of a saturated solution of Ag2CO3 is found to contain 0.049g of Ag2CO3, what is the Ksp of Ag2CO3.
134. If 5.6 L of a saturated solution of Ag2CrO4 is found to contain 0.12 g of Ag2CrO4, what is the Ksp of
Ag2CrO4.
135. If 24 L of a saturated solution of Cu(OH)2 is found to contain 8.0  10-4 g of Cu(OH)2, what is the Ksp of
Cu(OH)2.
136. If 32 L of a saturated solution of Pb(IO3)2 is found to contain 0.72 g of Pb(IO3)2, what is the Ksp of Pb(IO3)2.
137. If 76 L of a saturated solution of Mg(OH)2 is found to contain 0.58 g of Mg(OH)2, what is the Ksp of Mg(OH)2.
138. If 4.5 L of a saturated solution of AgBr is found to contain 4.5  10-4 g of Ag, what is the Ksp of AgBr.
139. If 85 mL of a saturated solution of BaSO4 is found to contain 4.5  10-2 g of Ba, what is the Ksp of BaSO4.
140. If 25 mL of a saturated solution of CaCO3 is found to contain 5.6  10-5 g of Ca, what is the Ksp of CaCO3.
141. If 55 L of a saturated solution of AgCN is found to contain 7.8  10-3 g of Ag, what is the Ksp of AgCN.
142. What mass of Ag2CO3 would be found in 1.4 L of a saturated solution if the Ksp of Ag2CO3 is 8.2  10-12?
143. What mass of Cu2S would be found in 34 L of a saturated solution of Cu2S if the Ksp of Cu2S is 1.6  10-48?
144. What mass of PbCl2 would be found in 0.48 L of a saturated solution of PbCl2 if the Ksp of PbCl2 is 1.6 
10-5?
145. What mass of Mg(OH)2 would be found in 7.6  102 mL of a saturated solution of Mg(OH)2 if the Ksp of
Mg(OH)2 is 9.0  10-12?
146. What is the solubility, in mol/L, of AgC2H3O2 in a 0.45 mol/L solution of AgNO3 if the Ksp of AgC2H3O2 is
2.5  10-3?
147. What is the solubility, in mol/L, of AgCl in a 0.0045 mol/L solution of NaCl if the Ksp of AgCl is 1.8  10-10
mol/L?
148. What is the solubility, in mol/L, of MgCO3 in a 0.65 mol/L solution of MgCl2 if the Ksp of MgCO3 is 2.5 
10-5?
149. What is the solubility, in mol/L, of CaF2 in a 0.65 mol/L solution of NaF, if the Ksp of CaF2 is 4.9  10-11?
150. What is the solubility of Mg(OH)2 in a 0.55 mol/L solution of KOH if the Ksp of Mg(OH)2 is 9.0  10-12?
151. If 45 mL of a 0.45 mol/L solution of AgNO3 was mixed with 85 mL of a 1.35  10-2 mol/L solution of NaCl,
would a precipitate form? Calculate the ion product for the potential precipitate. The Ksp of AgCl(s) is 1.8 
10-10.
152. If 145 mL of a 0.0078 mol/L solution of CuNO3 was mixed with 195 mL of a 1.48  10-3 mol/L solution of KI,
would a precipitate form? Calculate the ion product for the potential precipitate. The Ksp of CuI is 1  10-12.
153. If 365 mL of a 0.0054 mol/L solution of Pb(NO3)2 was mixed with 595 mL of a 6.34  10-4 mol/L solution of
KI, would a precipitate form? Calculate the ion product for the potential precipitate. The Ksp of PbI2 is 7.9 
10-9.
154. If 845 mL of a 2.5  10-5 mol/L solution of Ni(NO3)2 was mixed with 195 mL of a 4.86  10-2 mol/L solution
of KOH, would a precipitate form?. Calculate the ion product for the potential precipitate. The Ksp of
Ni(OH)2(s) is 6  10-16.
155. If 78 mL of a 0.0026 mol/L solution of Zn(NO3)2 was mixed with 45 mL of a 7.13  10-3 mol/L solution of
K2CO3, would a precipitate form? Calculate the ion product for the potential precipitate. The Ksp of ZnCO3 is
1.0  10-10.
156. Find the temperature at which the reaction below is spontaneous given this data
Hfo of NH3(g) = - 46 kJ/mol, So of NH3(g) = 192.5 J/molK, So of N2(g) = 191.5 J/molK,
130.6 J/molK.
N2(g) + 3H2(g) <=====> 2NH3(g)
So of H2(g) =
157. The production of lime, CaO, from limestone, CaCO3, is accomplished by heating limestone until it
decomposes. Find the temperature at which the reaction below is spontaneous given the following data:
Hfo of CaCO3(s) = - 1207 kJ/mol, Hfo of CaO(s) = - 635.5 kJ/mol, Hfo of CO2(g) = - 394 kJ/mol,
CaCO3(s) = 92.9 J/molK, So of CaO(s) = 40 J/molK, So of CO2(g) = 213.6 J/molK.
So
CaCO3(s) <=====> CaO(s) + CO2(g)
Essay
158. Given this equilibrium
2A(g) + 3B(g) <=====> C(g) + 4D(g) + energy
Discuss what happens to this equilibrium if the temperature increases while the pressure is held constant. Make
sure to include a discussion of the rates of the forward and reverse reactions as well as changes in the
concentrations of A, B, C and D.
159. Shown below is the Haber process for the commercial production of ammonia.
N2(g) + 3H2(g) <=====> 2NH3(g) + 92 kJ
Discuss how Haber maximized the production of ammonia by manipulating this equilibrium. Also point out the
importance of this industrial process to a growing world population. Make sure to establish a link between
ammonia and protein.
Master List for Chapter 7
Answer Section
MODIFIED TRUE/FALSE
1. ANS: T
LOC: CS2.05
2. ANS: F, only forms
LOC: CS2.05
3. ANS: T
LOC: CS2.05
4. ANS: T
LOC: CS2.01
5. ANS: T
LOC: CS2.01
6. ANS: T
LOC: CS2.05
7. ANS: F, AgC2H3O2
LOC: CS1.10
8. ANS: F
PbCl2(s) <====> Pb2+(aq) + 2Cl1-(aq)
9.
10.
11.
12.
13.
14.
15.
16.
17.
REF:
ANS:
LOC:
ANS:
LOC:
ANS:
LOC:
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LOC:
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LOC:
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LOC:
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LOC:
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LOC:
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REF: I
OBJ: 7.6
REF: I
OBJ: 7.6
REF: K/U
OBJ: 7.6
REF: K/U
OBJ: 7.1
REF: K/U
OBJ: 7.6
REF: I
OBJ: 7.6
REF: K/U
OBJ: 7.1
K/U
OBJ: 7.6
LOC: CS2.06
T
REF: I
OBJ: 7.6
CS2.05
T
REF: K/U
OBJ: 7.1
CS1.01
F, Ca(OH)2 has a higher pH
REF: I
OBJ: 7.3
CS2.06
T
REF: K/U
OBJ: 7.6
CS1.01
F, [D] will decrease
REF: I
OBJ: 7.3
CS1.03
F, decrease 3/2 as much
REF: I
OBJ: 7.3
CS1.03
T
REF: I
OBJ: 7.3
CS1.03
F, will increase 4's as much
REF: I
OBJ: 7.3
CS1.03
F, the quantity of silver ion is double the quantity of carbonate ion
REF: K/U
OBJ: 7.6
LOC: CS1.06
18. ANS: F, the quantity of hydroxide ion is double the quantity of cobalt(II) ion
REF:
K/U
OBJ: 7.6
LOC: CS1.06
MULTIPLE CHOICE
19. ANS: E
REF: I
OBJ: 7.1
LOC: CS1.06
20.
21.
22.
23.
24.
25.
26.
27.
28.
29.
30.
31.
32.
33.
34.
35.
36.
37.
38.
39.
40.
41.
42.
43.
44.
45.
46.
47.
48.
49.
50.
51.
52.
53.
54.
55.
56.
57.
58.
59.
60.
61.
62.
63.
64.
65.
66.
67.
68.
ANS:
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ANS:
A
D
C
B
B
C
B
D
A
B
E
C
A
D
A
E
C
B
B
E
D
C
C
D
E
C
A
C
A
C
B
D
D
D
A
B
B
E
A
E
C
D
D
C
B
C
C
B
D
REF:
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K/U
K/U
K/U
K/U
I
I
I
I
I
I
I
I
I
I
I
I
I
I
I
I
I
I
I
I
I
I
I
I
I
I
I
K/U
I
I
I
I
I
I
I
I
K/U
K/U
K/U
K/U
K/U
K/U
K/U
K/U
K/U
OBJ:
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OBJ:
7.1
7.1
7.1
7.1
7.6
7.6
7.6
7.6
7.6
7.6
7.6
7.3
7.3
7.3
7.3
7.3
7.3
7.3
7.5
7.5
7.5
7.5
7.5
7.5
7.5
7.5
7.5
7.5
7.5
7.5
7.5
7.1
7.1
7.3
7.3
7.3
7.2
7.3
7.3
7.3
7.3
7.3
7.3
7.3
7.3
7.3
7.3
7.3
7.3
LOC:
LOC:
LOC:
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CS1.06
CS1.06
CS1.06
CS1.06
CS2.06
CS2.06
CS2.06
CS2.06
CS2.06
CS2.06
CS2.06
CS1.03
CS1.03
CS1.03
CS1.03
CS1.03
CS1.03
CS1.03
CS2.06
CS2.06
CS2.06
CS2.06
CS2.06
CS2.06
CS2.06
CS2.06
CS2.06
CS2.06
CS2.06
CS2.06
CS2.06
CS1.01
CS1.06
CS1.03
CS1.03
CS1.03
CS2.06
CS2.06
CS1.03
CS1.03
CS1.03
CS1.03
CS1.03
CS1.03
CS1.03
CS1.03
CS1.03
CS1.03
CS1.03
69. ANS: E
70. ANS: D
71. ANS: B
REF: K/U
REF: I
REF: I
OBJ: 7.3
OBJ: 7.2
OBJ: 7.2
LOC: CS1.03
LOC: CS1.02
LOC: CS1.02
REF: K/U
OBJ: 7.6
REF: K/U
OBJ: 7.6
REF: K/U
OBJ: 7.6
REF: K/U
OBJ: 7.6
REF: K/U
OBJ: 7.6
REF: K/U
OBJ: 7.6
REF: K/U
OBJ: 7.6
REF: K/U
OBJ: 7.6
REF: K/U
OBJ: 7.6
REF: K/U
OBJ: 7.6
COMPLETION
72. ANS:
LOC:
73. ANS:
LOC:
74. ANS:
LOC:
75. ANS:
LOC:
76. ANS:
LOC:
77. ANS:
LOC:
78. ANS:
LOC:
79. ANS:
LOC:
80. ANS:
LOC:
81. ANS:
LOC:
barium sulfate
CS1.06
silver bromide
CS1.06
strontium chromate
CS1.06
lead(II) chloride
CS1.06
aluminium hydroxide
CS1.06
magnesium oxalate
CS1.06
calcium carbonate
CS1.06
zinc phosphate
CS1.06
silver cyanide
CS1.06
barium sulfite
CS1.06
82. ANS: BaSO4(s) <====> Ba2+(aq) + SO42-(aq)
REF:
K/U
OBJ: 7.6
LOC: CS1.06
2+
83. ANS: CuCO3(s) <=======> Cu (aq) + CO32-(aq)
REF:
K/U
OBJ: 7.6
REF:
K/U
OBJ: 7.6
REF:
K/U
REF:
ANS:
LOC:
ANS:
LOC:
ANS:
LOC:
ANS:
K/U
1:1
CS1.03
3:2
CS1.03
1:1
CS1.03
1:2
LOC: CS1.06
84. ANS: Fe3(PO4)2(s) <=====> 3 Fe2+(aq) + 2 PO43-(aq)
LOC: CS1.06
85. ANS: Ag2CrO4(s) <======> 2Ag1+(aq) + CrO42-(aq)
OBJ: 7.6
LOC: CS1.06
2+
186. ANS: CaF2(s) <======> Ca (aq) + 2F (aq)
87.
88.
89.
90.
OBJ: 7.6
LOC: CS1.06
REF: K/U
OBJ: 7.6
REF: K/U
OBJ: 7.6
REF: K/U
OBJ: 7.6
REF: K/U
OBJ: 7.6
91.
92.
93.
94.
95.
LOC:
ANS:
LOC:
ANS:
LOC:
ANS:
LOC:
ANS:
LOC:
ANS:
LOC:
CS1.03
1:2
CS1.06
decreases
CS1.05
increases
CS1.05
negative
CS1.05
negative
CS1.05
REF: K/U
OBJ: 7.6
REF: K/U
OBJ: 7.7
REF: K/U
OBJ: 7.7
REF: K/U
OBJ: 7.7
REF: K/U
OBJ: 7.7
OBJ:
OBJ:
OBJ:
OBJ:
LOC:
LOC:
LOC:
LOC:
MATCHING
96.
97.
98.
99.
ANS:
ANS:
ANS:
ANS:
A
C
B
D
REF:
REF:
REF:
REF:
K/U
K/U
K/U
K/U
7.7
7.7
7.7
7.7
CS1.05
CS1.05
CS1.05
CS1.05
SHORT ANSWER
100. ANS:
mol/L
PCl3(g) + Cl2(g) <=====>
initial
shift
0.3
@E
0.3
Ke = 1.2 / 0.3  0.3 = 13
REF: I
101. ANS:
OBJ: 7.5
0.3
0.3
PCl5(g)
1.5
0.3
1.2
LOC: CS2.06
mol/L
H2(g) + I2(g) <=====>
initial
1.2
1.2
shift
–0.20
–0.20
@E
1.0
1.0
2
Ke = (0.40) / (1.0  1.0) = 0.16
REF: I
102. ANS:
OBJ: 7.5
mol/L
H2(g) +
initial
shift
0.40
@E
0.40
Ke = (0.40)2 / (0.40  0.40) = 1.0
REF: I
103. ANS:
OBJ: 7.5
2HI(g)
0.40
0.40
LOC: CS2.06
I2(g) <=====>
2HI(g)
1.2
0.40
0.40
LOC: CS2.06
–0.80
0.40
mol/L
initial
shift
@E
H2(g) +
I2(g) <=====>
1.6
´
–2
2HI(g)

´

2
2
Ke = (1.6  2) / ( ) = 36 (take the square root of both sides)
1.6  2 /  = 6
6 = 1.6 –2
8 = 1.6
= 0.20 mol/L = [H2] = [I2]; [HI] = 1.6  2(0.20) = 1.2 mol/L
REF: I
104. ANS:
mol/L
initial
shift
@E
OBJ: 7.5
H2(g) +
1.6  2
LOC: CS2.06
I2(g) <=====>
2HI(g)
1.7
´
–2

´

Ke = (1.7  2)2 / (2) = 49 (take the square root of both sides)
1.7  2 /  = 7
7 = 1.7 –2
9 = 1.7
= 0.019 mol/L = [H2] = [I2]; [HI] = 1.7  2(0.019) = 1.3 mol/L
REF: I
OBJ: 7.5
105. ANS:
1.4  10-4 = [D]2 / (0.24)3
[D]2 = (1.4  10-4)(0.24)3
[D] = 1.4  10-3 mol/L
LOC: CS2.06
REF: I
OBJ: 7.5
106. ANS:
8.3  10-2 = [0.38]3 / [A]2
[A]2 = [0.38]3 / 8.3  10-2
[A] = 0.81 mol/L
LOC: CS2.06
REF: I
OBJ: 7.5
LOC: CS2.06
107. ANS:
Ke = 2.6  3.2 / 0.7  1.25 = 9.5
mol/L
SO2(g) +
NO2(g)<====>
initial
0.70
1.25
upset
+
shift
–0.2
–0.2
@E
1.05
0.50 + 
9.51 = (2.8  3.4) / (0.50 + )(1.05)
(9.51) (0.50 + )(1.05) = 2.8  3.4
9.984 + 4.992 = 9.52
= 4.528 / 9.984 = 0.45 mol/L  2L = 0.91 moles of SO2(g)
1.7  2
SO3(g) +
2.6
NO(g)
3.2
0.2
2.8
0.2
3.4
REF: I
OBJ: 7.5
LOC: CS2.06
108. ANS:
mol/L
CH4(g) +
2H2S(g) <====>
@E
0.24
0.36
4
50 = (4) () / (0.24)(0.36)
50 = 2565 / 0.0864
5 = (50)(0.0864)(256)
= 4.1 mol/L = [CS2]; [H2] = 16 mol/L
REF: I
OBJ: 7.5
109. ANS:
mol/L
2NH3(g)
initial
4.0
shift
–2.0
@E
2.0
3
Ke = (3.0) (1.0) / (2.0)2 = 6.8
I
OBJ: 7.5
4H2(g)
4
LOC: CS2.06
<====>
N2(g)
+
3H2(g)
1.0
1.0
REF: I
OBJ: 7.5
110. ANS:
mol/L
2NH3(g)
initial
3.0
shift
–0.66
@E
2.33
3
Ke = (1.0) (0.33) / (2.33)2 = 6.1  10-2
REF:
CS2(g) +

3.0
3.0
LOC: CS2.06
<====>
N2(g)+
3H2(g)
0.33
0.33
1.0
1.0
LOC: CS2.06
PROBLEM
111. ANS:
AgC2H3O2(s) <====>
@E
Ag1+(aq)
5.0  10-2
+
C2H3O21-(aq)
5.0  10-2
Ksp = (5.0  10-2)2 = 2.5  10-3
REF: I
OBJ: 7.6
112. ANS:
AgBr(s) <====> Ag1+(aq)
@E
LOC: CS2.06
+ Br1-(aq)
8.8  10-7
8.8  10-7
Ksp = (8.8  10-7)2 = 7.7  10-13
REF: I
OBJ: 7.6
113. ANS:
Ag2CO3(s) <====> 2Ag1+(aq)
@E
LOC: CS2.06
2 * 1.3 10-4
CO32-(aq)
1.3 10-4
Ksp = ( 2 * 1.3  10-4)2  1.3  10-4 = 8.8  10-12
REF: I
114. ANS:
Cu2S(s) <====>
@E
OBJ: 7.6
LOC: CS2.06
2Cu1+(aq)
2 * 7.4  10-17
+
S2-(aq)
7.4  10-17
Ksp = ( 2 * 7.4  10-17)2  7.4  10-17 = 1.6  10-48
REF: I
115. ANS:
CaF2(s) <====>
@E
OBJ: 7.6
LOC: CS2.06
Ca2+(aq)
2.3  10-4
+
2F1-(aq)
2 * 2.3  10-4
+
2OH1-(aq)
2 * 1.3  10-4
+
2IO31-(aq)
2 * 4.0  10-5
+
3 OH1-(aq)
3 * 3.2  10-09
Ksp = 2.3  10-4 ( 2 * 2.3  10-4 )2 = 4.9  10-11
REF: I
OBJ: 7.6
116. ANS:
Mg(OH)2(s) <====>
@E
LOC: CS2.06
Mg2+(aq)
1.3  10-4
Ksp = 1.3  10-4 ( 2 * 1.3  10-4)2 = 8.8  10-12
REF: I
OBJ: 7.6
117. ANS:
Pb(IO3)2(s) <====>
@E
LOC: CS2.06
Pb2+(aq)
4.0  10-5
Ksp = 4.0  10-5 ( 2 * 4.0  10-5 )2 = 2.6  10-13
REF: I
OBJ: 7.6
118. ANS:
Al(OH)3(s) <====>
@E
LOC: CS2.06
Al3+(aq)
3.2  10-09
Ksp = 3.2  10-09 ( 3 * 3.2  10-09 )3 = 2.8  10-33
REF: I
OBJ: 7.6
119. ANS:
Zn3(PO4)2(s) <====>
@E
LOC: CS2.06
3 Zn2+(aq)
3  3.4  10-8
+
2 PO43-(aq)
2 * 3.4  10-8
Ksp = (3  3.4  10-8)3 ( 2  3.4  10-8 )2 = 4.9  10-36
REF: I
OBJ: 7.6
120. ANS:
Pb3(PO4)2(s) <====>
LOC: CS2.06
3 Pb2+(aq)
+
2 PO43-(aq)
2.3  10-9
@E
2/3 * 2.3  10-9
Ksp = (2.3  10-9 )3 ( 2/3  2.3  10-9 )2 = 2.6  10-44
REF: I
OBJ: 7.6
121. ANS:
Fe(OH)3(s) <====>
@E
LOC: CS2.06
Fe3+(aq)
2.2  10-10
+
3 OH1-(aq)
2.2  10-10
+
2OH1-(aq)
2  1.7  10-5
Ksp = 2.2  10-10 ( 3  2.2  10-10 )3 = 6.3  10-38
REF: I
OBJ: 7.6
122. ANS:
Zn(OH)2(s) <====>
@E
LOC: CS2.06
Zn2+(aq)
1.7  10-5
Ksp = 1.7  10-5 ( 2  1.7  10-5 )2 = 2.0  10-14
REF: I
OBJ: 7.6
123. ANS:
Ba3(PO4)2(s) <====>
@E
LOC: CS2.06
3 Ba2+(aq)
4.2  10-8
+
2 PO43-(aq)
2/3  4.2  10-8
Ksp = (4.2  10-8 )3 ( 2/3  4.2  10-8 )2 = 5.8  10-38
REF: I
124. ANS:
PbCl2(s) <====>
@E
OBJ: 7.6
LOC: CS2.06
Pb2+(aq)
1.6  10-2
+
2Cl1-(aq)
2  1.6  10-2
+
CO32-(aq)
6.5  10-5
Ksp = 1.6  10-2 ( 2  1.6  10-2 )2 = 1.6  10-5
REF: I
OBJ: 7.6
125. ANS:
Ag2CO3(s) <====>
@E
LOC: CS2.06
2Ag1+(aq)
2  6.5  10-5
Ksp = ( 2  6.5  10-5 )2  6.5  10-5 = 1.1  10-12
REF: I
126. ANS:
PbI2(s) <====>
@E
OBJ: 7.6
LOC: CS2.06
Pb2+(aq)
1/2  2.4  10-3
Ksp = 1/2  2.4  10-3 (2.4  10-3 )2 = 6.9  10-9
REF:
I
OBJ: 7.6
LOC: CS2.06
+
2I1-(aq)
2.4  10-3
127. ANS:
Mg3(PO4)2(s) <====>
@E
3 Mg2+(aq)
+
2 PO43-(aq)
7.1  10-6
+
CN1-(aq)
1.4  10-6
3/2  7.1  10-6
Ksp = (3/2  7.1  10-6 )3 ( 7.1  10-6 )2 = 6.1  10-26
REF: I
128. ANS:
AgCN(s) <====>
@E
OBJ: 7.6
LOC: CS2.06
Ag1+(aq)
1.4  10-6
Ksp = (1.4  10-6)2
Ksp = 2.0  10-12
REF: I
OBJ: 7.6
129. ANS:
Ag2CO3(s) <====>
LOC: CS2.06
+
2Ag1+(aq)
2 * 1.3  10-4
@E
CO32-(aq)
1.3  10-4
Ksp = ( 2 * 1.3  10-4 )2  1.3  10-4
Ksp = 8.8  10-12
REF: I
130. ANS:
OBJ: 7.6
AgC2H3O2(s) <====>
LOC: CS2.03
Ag1+(aq)
(14.1g /166.91 g/mol) / 1.7 L)
@E
+
C2H3O21-(aq)
(14.1g /166.91 g/mol) / 1.7 L)
Ksp = (14.1g /166.91 g/mol) / 1.7 L)2
Ksp = 2.4  10-3
REF: I
131. ANS:
MgCO3(s) <====>
@E
OBJ: 7.6
LOC: CS2.06
Mg2+(aq)
1.1 g / 84.314 g/mol / 2.6 L
+
CO32-(aq)
1.1 g / 84.314 g/mol / 2.6 L
+
SO42-(aq)
0.46 g / 303.26 g/mol / 12 L
+
CO32-(aq)
Ksp = (1.1 g / 84.314 g/mol / 2.6 L )2 = 2.5  10-5
REF: I
132. ANS:
PbSO4(s) <====>
@E
OBJ: 7.6
LOC: CS2.06
Pb2+(aq)
0.46 g / 303.26 g/mol / 12 L
Ksp = (0.46 g / 303.26 g/mol / 12 L )2 = 1.6  10-8
REF: I
133. ANS:
Ag2CO3(s) <====>
OBJ: 7.6
LOC: CS2.06
2 Ag1+(aq)
@E
2  ( 0.049 g / 275.75 g/mol / 1.4 L)
0.049 g / 275.75 g/mol / 1.4 L
Ksp = (2  ( 0.049 g / 275.75 g/mol / 1.4 L) )2(0.049 g / 275.75 g/mol / 1.4 L) = 8.2  10-12
REF: I
134. ANS:
OBJ: 7.6
Ag2CrO4(s) <====>
@E
LOC: CS2.06
2 Ag1+(aq)
+
2  ( 0.12 g / 331.73 g/mol / 5.6 L)
CrO42-(aq)
0.12 g / 331.73 g/mol / 5.6 L
Ksp = (2  ( 0.12 g / 331.73 g/mol / 5.6 L) )2(0.12 g / 331.73 g/mol / 5.6 L) = 1.1  10-12
REF: I
135. ANS:
Cu(OH)2(s) <====>
@E
OBJ: 7.6
LOC: CS2.06
Cu2+(aq)
8.0  10-4 g / 97.561 g/mol / 24 L
+
2OH1-(aq)
2  8.0  10-4 g / 97.561 g/mol / 24 L
Ksp = (8.0  10-4 g / 97.561 g/mol / 24 L )(8.0  10-4 g / 97.561 g/mol / 24 L )2 = 1.6  10-19
REF: I
136. ANS:
OBJ: 7.6
Pb(IO3)2(s) <====>
LOC: CS2.06
Pb2+(aq)
0.72 g / 557.01 g/mol / 32 L
@E
+
2IO31-(aq)
2  (0.72 g / 557.01 g/mol / 32 L)
Ksp = (0.72 g / 557.01 g/mol / 32 L )(2  (0.72 g / 557.01 g/mol / 32 L) )2 = 2.6  10-13
REF: I
OBJ: 7.6
137. ANS:
Mg(OH)2(s) <====>
@E
LOC: CS2.06
Mg2+(aq)
0.58 g / 58.32 g/mol / 76 L
+
2OH1-(aq)
2  0.58 g / 58.32 g/mol / 76 L
Ksp = (0.58 g / 58.32 g/mol / 76 L )(2  0.58 g / 58.32 g/mol / 76 L )2 = 9.0  10-12
REF: I
138. ANS:
AgBr(s) <====>
@E
OBJ: 7.6
LOC: CS2.06
Ag1+(aq)
4.5  10-4 g/107.87 g/mol / 4.5 L
+
Br1-(aq)
4.5  10-4 g/107.87 g/mol / 4.5 L
+
SO42-(aq)
Ksp = ( 4.5  10-4 g/107.87 g/mol / 4.5 L )2
Ksp = 8.6  10-13
REF: I
139. ANS:
BaSO4(s) <====>
@E
OBJ: 7.6
LOC: CS2.06
Ba2+(aq)
4.5  10-2 g/137.33 g/mol / 0.085 L
Ksp = ( 4.5  10-2 g/137.33 g/mol / 0.085 L )2 = 2.1  10-9
4.5  10-2 g/137.33 g/mol / 0.085 L
REF: I
140. ANS:
OBJ: 7.6
CaCO3(s) <====>
LOC: CS2.06
Ca2+(aq)
+
5.6  10-5 g /40.078 g/mol / 0.025 L
@E
CO32-(aq)
5.6  10-5 g /40.078 g/mol / 0.025 L
Ksp = ( 5.6  10-5 g /40.078 g/mol / 0.025 L )2 = 3.1  10-9
REF: I
141. ANS:
OBJ: 7.6
AgCN(s) <====>
@E
LOC: CS2.06
Ag1+(aq)
-3
7.8  10 g /107.87 g/mol / 0.055 L
+
CN1-(aq)
-3
7.8  10 g /107.87 g/mol / 0.055 L
Ksp = ( 7.8  10-3 g /107.87 g/mol / 0.055 L )2 = 1.7  10-12
REF: I
OBJ: 7.6
142. ANS:
Ag2CrO4(s) <====>
@E
LOC: CS2.06
2 Ag1+(aq)
2
+
CrO42-(aq)

8.2  10-12 = 43
= 1.27  10-2 mol/L
mAg2CO3 = (1.27  10-2 mol/L)(1.4 L)(331.73 g/mol) = 4.9  10-2 g
REF: I
143. ANS:
Cu2S(s) <====>
@E
OBJ: 7.6
LOC: CS2.04
2 Cu1+(aq)
2
+
S2-(aq)

+
2 Cl1-(aq)
2
+
2 OH1-(aq)
1.6  10-48 = 43
= 7.4  10-17 mol/L
mCu2S = (7.4  10-17 mol/L)(34 L)(159.16 g/mol = 4.0  10-13 g
REF: I
144. ANS:
PbCl2(s) <====>
@E
OBJ: 7.6
LOC: CS2.04
Pb2+(aq)

1.6  10-5 = 43
= 1.59  10-2 mol/L
mCu2S = (1.59  10-2 mol/L)(0.48 L)(278.11 g/mol = 2.1 g
REF: I
OBJ: 7.6
145. ANS:
Mg(OH)2(s) <====>
LOC: CS2.04
Mg2+(aq)
2

@E
9.0  10-12 = 43
= 1.3  10-4 mol/L
mCu2S = (1.3  10-4 mol/L mol/L)(0.76 L)(58.32 g/mol) = 5.8  10-3 g
REF: I
OBJ: 7.6
146. ANS:
AgC2H3O2(s) <====>
initial
@E
LOC: CS2.04
Ag1+(aq)
0.45 mol/L
0.45 mol/L + (negligible)
C2H3O21-(aq)
+

2.5  10-3 = 0.45 
solubility = 5.6  10-3 mol/L
REF: I
OBJ: 7.6
147. ANS:
AgCl(s) <=====> Ag1+(aq)
initial
@E
LOC: CS2.04
+
Cl1-(aq)
0.0045 mol/L
0.0045 +  (negligible)

0.0045  = 1.8  10-10
solubility = 4.0  10-8 mol/L
REF: I
148. ANS:
MgCO3(s) <====>
OBJ: 7.6
LOC: CS2.04
Mg2+(aq)
0.65 mol/L
0.65 mol/L + (negligible)
initial
@E
+
CO32-(aq)

´
2.5  10-5 = 0.65 
solubility = 3.9  10-5 mol/L
REF: I
OBJ: 7.6
149. ANS:
CaF2(s) <=====> Ca2+(aq) +
initial
@E
LOC: CS2.04
2F1-(aq)
0.65
0.65 + 2 (negligible)
0.652 = 4.9  10-11
solubility = 1.2  10-10 mol/L
REF:
I
OBJ: 7.6
LOC: CS2.04
150. ANS:
Mg(OH)2(s) <====>
initial
@E
Mg2+(aq)
+

1 OH1 (aq)
0.55 mol/L
0.55 + 2 (negligible)
9.0  10-12 = 0.552 
solubility = 3.9  10-5 mol/L
REF: I
OBJ: 7.6
LOC: CS2.04
151. ANS:
AgNO3(aq) + NaCl(aq)  AgCl(s) + NaNO3(aq)
[Ag1+] = (0.45 mol/L)(0.045 L) / (0.045 L + 0.085) L
[Cl1-] = (1.35  10-2 mol/L)(0.085 L) / (0.045 L + 0.085) L
ion product AgCl is [Ag1+][Cl1-] = 1.4  10-3 > Ksp, yes a precipitate forms
REF: I
OBJ: 7.6
LOC: CS2.05
152. ANS:
CuNO3(aq) + KI(aq)  CuI(s) + KNO3(aq)
[Cu1+] = (0.0078 mol/L)(0.145 L) / (0.145 + 0.195) L
[I1-] = (1.48  10-3 mol/L)(0.195 L) / (0.145 + 0.195) L
ion product CuI is [Cu1+][I1-] = 2.8  10-6 > Ksp, yes a precipitate forms
REF: I
OBJ: 7.6
LOC: CS2.05
153. ANS:
Pb(NO3)2(aq) + 2KI(aq)  PbI2(s) + 2KNO3(aq)
[Pb2+] = (0.0054 mol/L)(0.365 L) / (0.365 L + 0.595) L
[I1-] = (6.34  10-4 mol/L)(0.595 L) / (0.365 L + 0.595) L
ion product PbI2 is [Pb2+][I1-]2 = 3.2  10-10 < Ksp, no precipitate forms
REF: I
OBJ: 7.6
LOC: CS2.05
154. ANS:
Ni(NO3)2(aq) + 2KOH(aq)  Ni(OH)2(s) + 2KNO3(aq)
[Ni2+] = (2.5  10-5 mol/L)(0.845 L) / (0.845 L + 0.195) L
[OH1-] = (4.86  10-2 mol/L)(0.195 L) / (0.845 L + 0.195) L
ion product Ni(OH)2 is [Ni2+][OH1-]2 = 1.7  10-9 > Ksp of Ni(OH)2, yes a precipitate occurs
REF: I
OBJ: 7.6
LOC: CS2.05
155. ANS:
Zn(NO3)2(aq) + K2CO3(aq)  ZnCO3(s) + 2KNO3(aq)
[Zn2+] = (0.0026 mol/L)(0.078 L) / (0.078 L + 0.045) L
[CO32-] = (7.13  10-3 mol/L)(0.045 L) / (0.078 L + 0.045) L
ion product ZnCO3 is [Zn2+][CO32-] = 4.3  10-6 > Ksp of ZnCO3, yes a precipitate occurs
REF: I
OBJ: 7.6
LOC: CS2.05
156. ANS:
T = H / S = (-46 kJ/mol  2 mol) – 0 / (192.5 J/molK  2 mol) – (130.6 J/mol K  3 mol + 191.5 J/molK  1
mol)
T = - 92 kJ / (385 J/K) – (391.8 J/K + 191.5 J/K)
T = – 92 000 J / – 198.3 J/K
T = 4.6  102 K
REF: I
OBJ: 7.7
LOC: CS1.05
157. ANS:
T = H / S = ((-635.5 kJ + (-394 kJ)) - (-1207 kJ) / (40 J/K + 213.6 J/lK - 92.9 J/K)
T = 177 500 J / (160.7 J/K)
T = 1.10  103 K
REF:
I
OBJ: 7.7
LOC: CS1.05
ESSAY
158. ANS:
Rates of forward and reverse reactions will both increase, but the reverse rate increases at a faster rate than the
forward rate. The rate of growth of the reverse rate slows down gradually and the rate of growth of the forward
rate speeds up until both rates are equal at a new equilibrium. The concentration of A and B both increase, A
increases 2/3 as much as B increases (or B increases 3/2 as much as A increases. Concentrations of C and D both
decrease, D decreases 4 times as much as C (or C decreases 1/4 as much as D decreases). When a new
equilibrium is reached the concentrations of A, B, C and D no longer change, but the new levels are different
than the original levels.
REF: C
OBJ: 7.3
LOC: CS1.03
159. ANS:
High temperatures do not favour the production of ammonia even though it speeds up the reaction rates. High
pressures favour the production of ammonia by forcing the equilibrium to the side with fewer molecules. He
discovered the introduction of a catalyst, iron oxide, increased the production of ammonia without the use of
extreme temperatures.
Ammonia dissolves in water in the soil forming ammonium ion that is converted into nitrates in the soil, which is
assimilated by plants into amino acids and ultimately protein. This greatly enhances mans ability to provide
relatively cheap food for a growing population.
REF:
C
OBJ: 7.4
LOC: CS1.03