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62. If all of the chloride in a 3.734-g sample of an unknown metal chloride is precipitated as
AgCl with 70.90 mL of 0.2010 M AgNO3, what is the percentage of chloride in the sample?
A)
50.52%
B)
13.53%
C)
1.425%
D)
7.391%
E)
none of the above
63. A mixture of BaCl2 and NaCl is analyzed by precipitating all the barium as BaSO4. After
addition of an excess of Na2SO4 to a 3.725-g sample of the mixture, the mass of precipitate
collected is 2.734 g. What is the mass percentage of barium chloride in the mixture?
A)
82.28%
B)
73.40%
C)
43.18%
D)
65.47%
E)
19.60%
64. A 3.00-g sample of an alloy (containing only Pb and Sn) was dissolved in nitric acid
(HNO3). Sulfuric acid was added to this solution, which precipitated 2.37 g of PbSO4.
Assuming that all of the lead was precipitated, what is the percentage of Sn in the sample?
(molar mass of PbSO4 = 303.3 g/mol)
A)
46.0% Sn
B)
0.781% Sn
C)
79.0% Sn
D)
54.0% Sn
E)
1.62% Sn
65. A mixture contained no fluorine compound except methyl fluoroacetate, FCH2COOCH3
(molar mass = 92.07 g/mol). When chemically treated, all the fluorine was converted to
CaF2 (molar mass = 78.08 g/mol). The mass of CaF2 obtained was 35.8 g. Find the mass of
methyl fluoroacetate in the original mixture.
A)
60.7 g
B)
84.4 g
C)
30.4 g
D)
42.2 g
E)
21.1 g
66. A 1.59-g sample of a metal chloride, MCl2, is dissolved in water and treated with excess
aqueous silver nitrate. The silver chloride that formed weighed 3.60 g. Calculate the molar
mass of M.
A)
70.9 g/mol
B)
28 g/mol
C)
55.9 g/mol
D)
63 g/mol
E)
72.4 g/mol
67. You have 88.6 mL of a 2.50 M solution of Na2CrO4(aq). You also have 125 mL of a 2.50 M
solution of AgNO3(aq). Calculate the concentration of Na+ after the two solutions are mixed
together.
A)
0.00 M
B)
1.04 M
C)
2.07 M
D)
5.00 M
E)
0.443 M
68. You have 75.0 mL of a 2.50 M solution of Na2CrO4(aq). You also have 125 mL of a 2.01 M
solution of AgNO3(aq). Calculate the concentration of CrO42– after the two solutions are
mixed together.
A)
0.00 M
B)
0.309 M
C)
0.938 M
D)
0.251 M
E)
2.50 M
69. You have 75.0 mL of a 2.50 M solution of Na2CrO4(aq). You also have 125 mL of a 1.72 M
solution of AgNO3(aq). Calculate the concentration of Ag+ after the two solutions are mixed
together.
A)
0.00 M
B)
0.538 M
C)
1.08 M
D)
0.088 M
E)
0.215 M
70. You have 75.0 mL of a 2.50 M solution of Na2CrO4(aq). You also have 125 mL of a 1.88 M
solution of AgNO3(aq). Calculate the concentration of NO3– after the two solutions are
mixed together.
A)
0.00 M
B)
0.588 M
C)
1.18 M
D)
2.35 M
E)
4.50 M
71. You mix 55 mL of 1.00 M silver nitrate with 25 mL of 0.84 M sodium chloride. What mass
of silver chloride should you form?
A)
3.0 g
B)
6.0 g
C)
3.3 g
D)
6.6
E)
none of these
72. When solutions of carbonic acid and potassium hydroxide react, which of the following are
NOT present in the complete ionic equation?
A)
hydrogen ion
B)
carbonate ion
C)
potassium ion
D)
hydroxide ion
E)
water
73. When solutions of acetic acid and sodium hydroxide react, which of the following are NOT
present in the net ionic equation?
I.
hydrogen ion
II.
acetate ion
III.
sodium ion
IV.
hydroxide ion
A)
I and II
B)
I, II, and III
C)
I and IV
D)
I and III
E)
II and III
74. When solutions of carbonic acid and aluminum hydroxide react, which of the following are
NOT present in the net ionic equation?
I.
hydrogen ion
II.
carbonate ion
III.
aluminum ion
IV.
hydroxide ion
A)
I and II
B)
I, II, and III
C)
I and IV
D)
I and III
E)
II and III
75. When solutions of carbonic acid and copper(II) hydroxide react, which of the following are
spectator ions?
A)
hydrogen ion
B)
carbonate ion
C)
copper(II) ion
D)
hydroxide ion
E)
none of these
76. In the balanced molecular equation for the neutralization of sodium hydroxide with sulfuric
acid, the products are:
A)
NaSO4 + H2O
B)
NaSO3 + 2H2O
C)
2NaSO4 + H2O
D)
Na2S + 2H2O
E)
Na2SO4 + 2H2O
77. A 0.307-g sample of an unknown triprotic acid is titrated to the third equivalence point
using 35.2 mL of 0.106 M NaOH. Calculate the molar mass of the acid.
A)
247 g/mol
B)
171 g/mol
C)
165 g/mol
D)
151 g/mol
E)
82.7 g/mol
78. An unknown diprotic acid requires 44.39 mL of 0.111 M NaOH to completely neutralize a
0.580-g sample. Calculate the approximate molar mass of the acid.
A)
406 g/mol
B)
235 g/mol
C)
118 g/mol
D)
59 g/mol
E)
203 g/mol
79. You have separate solutions of HCl and H2SO4 with the same concentrations in terms of
molarity. You wish to neutralize a solution of NaOH. Which acid solution would require
more volume (in mL) to neutralize the base?
A)
The HCl solution.
B)
The H2SO4 solution.
C)
You need to know the acid concentrations to answer this question.
D)
You need to know the volume and concentration of the NaOH solution to answer
this question.
E)
C and D
80. What mass of NaOH is required to react exactly with 25.0 mL of 2.7 M H2SO4?
A)
2.7 g
B)
0.7 g
C)
5.4 g
D)
135 g
E)
none of these
81. With what volume of 5.00 M HF will 4.72 g of calcium hydroxide react completely,
according to the following reaction?
A)
12.7 mL
B)
127 mL
C)
637 mL
D)
25.5 mL
E)
39.2 mL
82. Sulfamic acid, HSO3NH2 (molar mass = 97.1 g/mol), is a strong monoprotic acid that can be
used to standardize a strong base:
A 0.165-g sample of HSO3NH2 required 19.4 mL of an aqueous solution of KOH for a
complete reaction. What is the molarity of the KOH solution?
A)
0.00170 M
B)
8.76 M
C)
0.0876 M
D)
0.0330 M
E)
none of these
83. A student weighs out 0.512 g of KHP (molar mass = 204.22 g/mol) and titrates to the
equivalence point with 36.78 mL of a stock NaOH solution. What is the concentration of the
stock NaOH solution? KHP is an acid with one acidic proton.
A)
0.00251 M
B)
0.092 M
C)
0.0139 M
D)
0.0682 M
E)
none of these
84. A chemical that changes color at the endpoint of a reaction is called a colorimeter.
85. In which of the following does nitrogen have an oxidation state of +4?
A)
HNO3
B)
NO2
C)
N2O
D)
NH4Cl
E)
NaNO2
86. The oxidation state of iodine in IO3– is:
A)
0
B)
+3
C)
–3
D)
+5
E)
–5
87. The oxidation state of chlorine in ClO– is:
A)
0
B)
+1
C)
-1
D)
+3
E)
-3
88. Which of the following statements is not true?
A)
When a metal reacts with a nonmetal, an ionic compound is formed.
B)
A metal-nonmetal reaction can always be assumed to be an oxidation-reduction
reaction.
C)
Two nonmetals can undergo an oxidation-reduction reaction.
D)
When two nonmetals react, the compound formed is ionic.
E)
A metal-nonmetal reaction involves electron transfer.
89. In the reaction 2Ca(s) + O2(g) → 2CaO(s), which species is oxidized?
A)
O2
B)
O2–
C)
Ca
D)
Ca2+
E)
none of these
90. In the reaction 2Cs(s) + Cl2(g) → 2CsCl(s), Cl2 is
A)
the reducing agent
B)
the oxidizing agent
C)
oxidized
D)
the electron donor
E)
two of these
91. In the reaction N2(g) + 3H2(g) → 2NH3(g), N2 is
A)
oxidized
B)
reduced
C)
the electron donor
D)
the reducing agent
E)
two of these
92. In the reaction P4(s) + 10Cl2(g) → 4PCl5(s), the reducing agent is
A)
chlorine
B)
PCl5
C)
phosphorus
D)
Cl–
E)
none of these
93. In the reaction C(s) + O2(g) → CO2(g) carbon is __________.
A)
the reducing agent
B)
the electron acceptor
C)
reduced
D)
the oxidizing agent
E)
more than one of these
94. Which of the following reactions does not involve oxidation-reduction?
A)
CH4 + 3O2 → 2H2O + CO2
B)
Zn + 2HCl → ZnCl2 + H2
C)
2Na + 2H2O → 2NaOH + H2
D)
MnO2 + 4HCl → Cl2 + 2H2O + MnCl2
E)
All are oxidation-reduction reactions.
95. Which of the following are oxidation-reduction reactions?
I.
PCl3 + Cl2 → PCl5
II.
Cu + 2AgNO3 → Cu(NO3)2 + 2Ag
III.
CO2 + 2LiOH → Li2CO3 + H2O
IV.
FeCl2 + 2NaOH → Fe(OH)2 + 2NaCl
A)
III
B)
IV
C)
I and II
D)
I, II, and III
E)
I, II, III, and IV
96. Which of the following statements is(are) true? Oxidation and reduction
A)
cannot occur independently of each other
B)
accompany all chemical changes
C)
describe the loss and gain of electron(s), respectively
D)
result in a change in the oxidation states of the species involved
E)
A, C, and D
97. In the reaction Zn + H2SO4 → ZnSO4 + H2, which, if any, element is oxidized?
A)
zinc
B)
hydrogen
C)
sulfur
D)
oxygen
E)
none of these
98. In the following reaction, which species is oxidized?
8NaI + 5H2SO4 → 4I2 + H2S + 4Na2SO4 + 4H2O
A)
sodium
B)
iodine
C)
sulfur
D)
hydrogen
E)
oxygen
99. How many of the following are oxidation-reduction reactions?
NaOH + HCl → NaCl + H2O
Cu + 2AgNO3 → 2Ag + Cu(NO3)2
Mg(OH)2 → MgO + H2O
N2 + 3H2 → 2NH3
A)
0
B)
1
C)
2
D)
3
E)
4
100. In the reaction shown below, what species is oxidized?
2NaI + Br2 → 2NaBr + I2
A)
Na+
B)
I–
C)
Br2
D)
Br–
E)
I2
101. Oxidation is the gain of electrons.
102. A reducing agent is an electron donor.
103. Balance the following oxidation-reduction reaction using the oxidation number method:
Fe3+ + I– → Fe2+ + I2
In the balanced equation, the coefficient of Fe2+ is
A)
1
B)
2
C)
3
D)
4
E)
none of these
104. Balance the following oxidation-reduction reaction using the oxidation number method:
Fe + Br2 → Fe3+ + Br–
In the balanced equation, the coefficient of Br– is
A)
2
B)
3
C)
4
D)
6
E)
none of these
105. Consider the following unbalanced oxidation-reduction reaction:
Fe2+ + Br2 → Fe3+ + Br–
In the balanced equation, the number of electrons transferred is
A)
1
B)
3
C)
2
D)
4
E)
none of these
106. The MnO4– is often used to analyze for the Fe2+ content of an aqueous solution via the
reaction
MnO4–(aq) + Fe2+(aq) + H+(aq) → Fe3+(aq) + Mn2+(aq) + H2O(l)
What is the ratio of Fe2+ : MnO4– in the balanced equation?
A)
1 : 1
B)
2 : 1
C)
3 : 1
D)
4 : 1
E)
5 : 1
107. Given the reaction:
2MnO4– + 5H2O2 + 6H+ → 2Mn2+ + 8H2O + 5O2
determine the number of electrons involved in this reaction.
A)
10
B)
8
C)
6
D)
4
E)
2
108. A molecule with an unequal charge distribution is said to be a __________ molecule.
109. Soluble ionic compounds containing the hydroxide ion are called strong __________.
110. A __________ is a substance dissolved in a liquid to make a solution.
111. A __________ electrolyte dissociates to a great extent in an aqueous solution.
112. Molarity is defined as __________ of solute per volume of solution in ___________.
113. Cu(OH)2(s)
114. FeCl3(aq) + Na2SO4(aq)
115. Precipitation of BaSO4 from solution
116. Neutralization of sulfuric acid
117. Combustion reaction
118. Dissolution of calcium hydroxide with another reagent
119. Formation of hydrogen gas
120. Balance the following equation: C3H5(NO3)3 → N2 + CO2 + H2O + O2
121. Balance the following equation: KI + HNO3 → KNO3 + NO + I2 + H2O
