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 [I 1][Ag 1+ ] 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 AgC
3
H
5
O
2
. _________________________
____ 8. The Ksp equilibrium expression for lead(II) chloride is Pb
2
Cl(s) <====> 2Pb
2+
(aq) + Cl
1-
(aq).
_________________________
____ 9. When 25 mL of 0.24 mol/L CaCl
2
is mixed with 45 mL of 1.5 mol/L AgNO
3
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
Mg
3
(PO
4
)
2
(s) <====> 3 Mg 2+ (aq) + 2 PO
4
3(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 . __________________________________________________
____ 19. A system at equilibrium means the concentration of reactants is equal to the concentration of products .
_______________________________________________________
____ 20. In a saturated solution of aluminum hydroxide the [Al 3+ ] is always 1/3 the [OH 1– ].
_________________________
____ 21. The pH scale ranges from 0 to 14 . ___________________________________
____ 22. A concentrated weak acid cannot have a lower pH than a dilute strong acid. _________________________
____ 23. A concentrated weak base can have a lower pOH than a dilute strong base. _________________________
____ 24. 1.0 mol/L solutions of weak bases will have a higher pH than 1.0 mol/L solutions of strong bases.
_________________________
____ 25. Conjugate acid base partners differ by a single proton . _________________________
____ 26. Salts containing an anion which is found in a strong acid cannot act like weak bases .
_________________________
____ 27. Salts containing anion which is not found in a strong acid can act like weak bases .
_________________________
____ 28. Salts contain cations found in the alkali metal family cannot act like weak acids .
_________________________
____ 29. Sodium ions have too weak a pull on water's electrons to make donating protons impossible.
_________________________
____ 30. If the pH of an aquatic solution at 95 o C is 4.5 the pOH must be 9.5
.
___________________________________
____ 31. The K b
expression for SO
4
2 ion is K b
= [HSO
4
2-
][OH
1-
] / [SO
4
2-
].
_________________________
____ 32. The K a
expression for H
2
PO
4
1 is K a
= [OH 1][H
3
PO
4
] / [H
2
PO
4
1] _________________________
____ 33. The K b
expression for H
2
PO
4
1 is K b
= [OH 1][H
3
PO
4
] / [H
2
PO
4
1]. _________________________
____ 34. During acid - base titrations the products are always neutral salts and water.
________________________________________
____ 35. When HCl is titrated with NaOH the endpoint is indicated when an excess of HCl turns the indicator a different colour. _________________________
Completion
Complete each sentence or statement.
36. If solutions of barium chloride and sodium sulfate were mixed and a precipitate formed, the precipitate would be _________________________.
37. If solutions of silver nitrate and copper(II) bromide were mixed and a precipitate formed, the precipitate would be _________________________.
38. If solutions of strontium chloride and potassium chromate were mixed and a precipitate formed, the precipitate would be ______________________________.

39. If solutions of lead(II) nitrate and lithium chloride were mixed and a precipitate formed, the precipitate would be _________________________.
40. If solutions of aluminum fluoride and potassium hydroxide were mixed and a precipitate formed, the precipitate would be ______________________________.
41. If solutions of sodium oxalate and magnesium chloride were mixed and a precipitate formed, the precipitate would be ______________________________.
42. If solutions of calcium fluoride and potassium carbonate were mixed and a precipitate formed, the precipitate would be ______________________________.
43. If solutions of sodium phosphate and zinc bromide were mixed and a precipitate formed, the precipitate would be _________________________.
44. If solutions of silver nitrate and potassium cyanide were mixed and a precipitate formed, the precipitate would be _________________________.
45. If solutions of lithium sulfite and barium iodide were mixed and a precipitate formed, the precipitate would be
_________________________.
46. If solutions of barium chloride and sodium sulfate were mixed and a precipitate formed, the equilibrium equation for the precipitate would be _____________________________________________.
47. If solutions of copper(II) nitrate and sodium carbonate were mixed and a precipitate formed, the equilibrium equation for the precipitate would be _____________________________________________.
48. If solutions of iron(II) chloride and potassium phosphate were mixed and a precipitate formed, the equilibrium equation for the precipitate would be _____________________________________________.
49. If solutions of potassium chromate and silver nitrate were mixed and a precipitate formed, the equilibrium equation for the precipitate would be _____________________________________________.
50. If solutions of calcium nitrate and sodium fluoride were mixed and a precipitate formed, the equilibrium equation for the precipitate would be _____________________________________________.
51. When solid magnesium carbonate is in equilibrium with its ions, the ratio of magnesium ion to carbonate ion is ____________________.
52. When solid lead(II) phosphate is in equilibrium with its ions, the ratio of lead(II) ion to phosphate ion is
____________________.
53. When solid barium monohydrogen phosphate is in equilibrium with its ions, the ratio of barium ion to monohydrogen phosphate ion is ____________________.
54. When solid zinc hydroxide is in equilibrium with its ions, the ratio of zinc ion to hydroxide ion is
____________________.
55. When solid mercury(II) iodide is in equilibrium with its ions, the ratio of mercury(II) ion to iodide ion is
____________________.
56. CO(g) + 2H
2
(g)

CH
3
OH(l); during this reaction the entropy ____________________.
57. S(s) + 2N
2
O(g)

SO
2
(g) + 2N
2
(g); during this reaction the entropy ____________________.
58. NH
3
(g) + HCl(g)

NH
4
Cl(s); during this chemical change the algebraic sign for the entropy change is predicted to be ____________________.

59. 4NO(g)

2N
2
O(g) + O
2
(g); during this chemical change the algebraic sign for the entropy change is predicted to be ____________________.
60. A system at equilibrium always has forward and reverse reactions which are
___________________________________.
61. A buffer solution can contain a weak acid and a _____________________________________________.
62. A buffer can contain a weak base and a salt containing
_____________________________________________.
63. A 1.5 mol/L solution of HCl(aq) has a pH of ____________________.
64. The pH of a 0.25 mol/L solution of HCl at 25 o C is ____________________.
65. A solution at 25 o C with a pOH of 3.45 has a pH of ____________________.
66. The [H 1+ ] of a 0.95 mol/L solution of HBr at 25 o C is ____________________.
67. Baking soda, NaHCO
3
, acts like a base because _____________________________________________.
68. The pH of an acidic solution is always ____________________.
69. The pOH of a basic solution is always ____________________.
70. The pOH of an acidic solution is always ____________________.
71. When potassium hydroxide is titrated to an end point by sulfuric acid the salt formed is
_________________________.
72. When nitric acid is titrated to an end point by lithium hydroxide the salt formed is
_________________________.
73. When iron(III) hydroxide is combined with carbonic acid the salt formed is _________________________.
74. Bronsted and Lowry's definition of acids is acids are substances which _________________________.
Essay
75. 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.
76. Shown below is the Haber process for the commercial production of ammonia.
N
2
(g) + 3H
2
(g) <=====> 2NH
3
(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.
77. Acid rain is a serious environmental problem. Given the equations for a variety of chemical reactions which contribute to this problem, discuss how human activity adds to the overall load of acidic substances. Make sure to include in your discussion strong and weak acids and include equilibrium expressions for one weak acid. Also discuss how the oxides of sulfur and nitrogen are formed through combustion and describe how these oxides react with water forming strong and weak acids. Suggest some measures which would reduce the problem.

N
2
(g) + O
2
(g) <====>2NO(g)
2NO(g) + O
2
(g) -------> 2NO
2
(g)
SO
2
(g)
+
H
2
O(g) ------> H
2
SO
3
(aq)
2NO
2
(g) + H
2
O(g)----->HNO
3
(aq) + HNO
2
(aq)
SO
3
(g)
+
H
2
O -------> H
2
SO
4
(aq)
S(s) + O
2
(g) -------> SO
2
(g)
2SO
2
(g) + O
2
(g) -------> 2SO
3
(g)
78. Impurities of sulfur in coal, natural gas and gasoline create environmental problems. Limestone is an abundant natural resource which contains CaCO
3
. Use these equations to discuss how the rain is becoming increasing acidified and suggest potential solutions to our acid rain problems.
N
2
(g) + O
2
(g) <====>2NO(g)
2NO(g) + O
2
(g) -------> 2NO
2
(g)
SO
2
(g)
+
H
2
O(g) ------> H
2
SO
3
(aq)
2NO
2
(g) + H
2
O(g)----->HNO
3
(aq) + HNO
2
(aq)
SO
3
(g)
+
H
2
O -------> H
2
SO
4
(aq)
S(s) + O
2
(g) -------> SO
2
(g)
2SO
2
(g) + O
2
(g) -------> 2SO
3
(g)
CaCO
3
(s) + SO
2
(g) -----> CaSO
3
(g) + CO
2
(g)

MODIFIED TRUE/FALSE
1. ANS: T
LOC: CS2.05
2. ANS: F, only forms
LOC: CS2.05
REF: I
REF: I
OBJ: 7.6
OBJ: 7.6
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, AgC
2
H
3
O
2
LOC: CS1.10
8. ANS: F
PbCl
2
(s) <====> Pb 2+ (aq) + 2Cl 1(aq)
REF: K/U OBJ: 7.6
9. ANS: T
LOC: CS2.05
10. ANS: T
LOC: CS1.01
REF: K/U
REF: K/U
REF: K/U
REF: I
REF: K/U
LOC: CS2.06
REF: I
REF: K/U
OBJ: 7.6
OBJ: 7.1
OBJ: 7.6
OBJ: 7.6
OBJ: 7.1
OBJ: 7.6
OBJ: 7.1
11. ANS: F, Ca(OH)
2
has a higher pH
LOC: CS2.06
12. ANS: T
LOC: CS1.01
13. ANS: F, [D] will decrease
LOC: CS1.03
14. ANS: F, decrease 3/2 as much
LOC: CS1.03
15. ANS: T
LOC: CS1.03
16. ANS: F, will increase 4

's as much
LOC: CS1.03
REF: I
REF: K/U
REF: I
REF: I
REF: I
REF: I
OBJ: 7.3
OBJ: 7.6
OBJ: 7.3
OBJ: 7.3
OBJ: 7.3
OBJ: 7.3
17. ANS: 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
19. ANS: F, forward reaction is equal to the rate of the reverse reaction
REF: K/U OBJ: 7.1 LOC: CS1.02

20. ANS: T
LOC: CS1.02
21. ANS: F, from below 0 and above 14
LOC: CS2.01
22. ANS: F, can have
LOC: CS1.02
23. ANS: T
LOC: CS1.07
24. ANS: F, lower pH
LOC: CS1.08
25. ANS: T
LOC: CS2.06
26. ANS: T
LOC: CS2.07
27. ANS: T
LOC: CS2.07
28. ANS: T
LOC: CS2.07
29. ANS: T
LOC: CS2.07
30. ANS: F, pH + pOH = 14 only at 25 o C
LOC: CS2.06
31. ANS: F
K b
= [HSO
4
1][OH 1] / [SO
4
2]
REF: I OBJ: 8.3
32. ANS: F, K b
expression
LOC: CS1.07
33. ANS: T
LOC: CS2.08
34. ANS: F, are not always
LOC: CS2.08
35. ANS: F, NaOH
LOC: CS2.08
COMPLETION
36. ANS: barium sulfate
LOC: CS1.06
37. ANS: silver bromide
LOC: CS1.06
38. ANS: strontium chromate
LOC: CS1.06
39. ANS: lead(II) chloride
LOC: CS1.06
40. ANS: aluminium hydroxide
LOC: CS1.06
41. ANS: magnesium oxalate
LOC: CS2.07
REF: I
REF: K/U
REF: K/U
REF: K/U
REF: K/U
REF: K/U
REF: K/U
REF: K/U
REF: K/U
REF: K/U
REF: K/U
REF: K/U
REF: K/U
REF: I
REF: I
REF: K/U
REF: MC
REF: MC
REF: K/U
REF: K/U
REF: I
OBJ: 7.1
OBJ: 8.1
OBJ: 8.1
OBJ: 8.2
OBJ: 8.2
OBJ: 8.1
OBJ: 8.3
OBJ: 8.3
OBJ: 8.3
OBJ: 8.3
OBJ: 8.1
OBJ: 8.2
OBJ: 8.3
OBJ: 8.4
OBJ: 8.4
OBJ: 7.6
OBJ: 7.6
OBJ: 7.6
OBJ: 7.6
OBJ: 7.6
OBJ: 7.6

LOC: CS1.06
42. ANS: calcium carbonate
LOC: CS1.06
43. ANS: zinc phosphate
LOC: CS1.06
44. ANS: silver cyanide
LOC: CS1.06
REF: K/U
REF: K/U
REF: K/U
45. ANS: barium sulfite
LOC: CS1.06
REF: K/U
46. ANS: BaSO
4
(s) <====> Ba 2+ (aq) + SO
4
2(aq)
REF: K/U OBJ: 7.6 LOC: CS1.06
47. ANS: CuCO
3
(s) <=======> Cu 2+ (aq) + CO
3
2(aq)
REF: K/U OBJ: 7.6 LOC: CS1.06
48. ANS: Fe
3
(PO
4
)
2
(s) <=====> 3 Fe 2+ (aq) + 2 PO
4
3(aq)
REF: K/U OBJ: 7.6 LOC: CS1.06
49. ANS: Ag
2
CrO
4
(s) <======> 2Ag 1+ (aq) + CrO
4
2(aq)
REF: K/U OBJ: 7.6 LOC: CS1.06
50. ANS: CaF
2
(s) <======> Ca 2+ (aq) + 2F 1(aq)
REF: K/U OBJ: 7.6 LOC: CS1.06
51. ANS: 1:1
LOC: CS1.03
REF: K/U
REF: K/U 52. ANS: 3:2
LOC: CS1.03
53. ANS: 1:1
LOC: CS1.03
REF: K/U
54. ANS: 1:2
LOC: CS1.03
55. ANS: 1:2
LOC: CS1.06
56. ANS: decreases
LOC: CS1.05
57. ANS: increases
LOC: CS1.05
58. ANS: negative
LOC: CS1.05
59. ANS: negative
LOC: CS1.05
REF: K/U
REF: K/U
REF: K/U
REF: K/U
REF: K/U
REF: K/U
60. ANS: occurring at the same rate
LOC: CS1.02
REF: K/U
61. ANS: salt which contains the conjugate base partner
REF: K/U OBJ: 8.5 LOC: CS1.09
62. ANS: the conjugate acid partner of the weak base
OBJ: 7.6
OBJ: 7.6
OBJ: 7.6
OBJ: 7.6
OBJ: 7.6
OBJ: 7.6
OBJ: 7.6
OBJ: 7.6
OBJ: 7.6
OBJ: 7.7
OBJ: 7.7
OBJ: 7.7
OBJ: 7.7
OBJ: 7.1

REF: K/U
63. ANS: – 0.18
LOC: CS2.06
64. ANS: 0.60
LOC: CS2.06
65. ANS: 10.55
LOC: CS2.06
OBJ: 8.5
73. ANS: iron(III) carbonate
LOC: CS2.08
74. ANS: donate protons
LOC: CS1.08
LOC: CS1.09
REF: I
REF: I
REF: I
66. ANS: 0.95 mol/L
LOC: CS2.06
REF: I
67. ANS: HCO
3
1 steals a proton from water forming OH 1 ions
REF: K/U OBJ: 8.3 LOC: CS2.07
REF: K/U 68. ANS: below 7
LOC: CS2.06
69. ANS: below 7
LOC: CS2.06
REF: K/U
REF: K/U 70. ANS: above 7
LOC: CS2.06
71. ANS: potassium sulfate
LOC: CS2.08
72. ANS: lithium nitrate
LOC: CS2.08
REF: K/U
REF: K/U
REF: K/U
REF: K/U
OBJ: 8.2
OBJ: 8.1
OBJ: 8.1
OBJ: 8.1
OBJ: 8.1
OBJ: 8.1
OBJ: 8.1
OBJ: 8.4
OBJ: 8.4
OBJ: 8.4
OBJ: 8.1