Test Bank General Chemistry, 10th edition 35
126. What is the balanced oxidation half-reaction provided below?
Zn(s) + 2H+(aq) → Zn2+(aq) + H2(g)
A)
Zn2+(aq) + 2e− → Zn(s)
B)
Zn2+(aq) + e− → Zn(s)
C)
Zn(s) → Zn2+(aq) + 2e−
D)
2H+(aq) + 2e− → H2(g)
E)
2H+(aq) → H2(g) + 2e−
127. All of the following half-reactions are balanced except
A)
NO3–(aq) + 4H+(aq) + 3e– → NO(g) + 2H2O(l).
B)
H3PO3(aq) + H2O(l) → H3PO4(aq) + 2H+(aq) + 2e–.
C)
2Ta(s) + 5H2O(l) → Ta2O5(s) + 10H+(aq) + 10e–.
D)
2H2O(l) + 2e– → H2(g) + 2OH–(aq).
E)
H2O2(aq) → 2OH–(aq) + 2e–.
128. What is the balanced reduction half-reaction for the reaction
3Mg(s) + N2(g) → Mg3N2(s)
A)
Mg2+ + 2e− → Mg
B)
Mg → Mg2+ + 2e−
C)
Mg2+ → Mg + 2e−
D)
N2 + 6e− → 2N3−
E)
N2 → 2N3−+ 6e−
129. The following reaction occurs in basic solution:
_ H2O(aq) + _ MnO4–(aq) + _ ClO–(aq) → _ MnO2(s) + _ ClO4–(aq) + _ OH–(aq)
Test Bank General Chemistry, 10th edition 36
When the equation is properly balanced, what is the sum of the lowest whole-number
coefficients?
A)
20
B)
9
C)
10
D)
6
E)
12
130. When the following equation is balanced, what is the lowest whole-number coefficient for
SO2?
____ HBrO3(aq) + ____ SO2(g) + ____ H2O(l) → ____ Br2(aq) + ____ H2SO4(aq)
A)
7
B)
10
C)
8
D)
4
E)
5
131. The following reaction occurs in basic solution. What is the sum of the lowest whole-
number coefficients in the balanced equation?
____ MnO4–(aq) + ____ NH3(aq) → ____ NO3–(aq) + ____ MnO2(s)
A)
9
B)
18
C)
12
D)
29
E)
23
132. In basic solution, H2O2 oxidizes Cr3+ to CrO42– and is reduced to OH–. What is the lowest
whole-number coefficient for OH– in the balanced net ionic equation?
A)
6
B)
10
C)
4
D)
16
E)
8
133. The following change occurs in acidic solution:
____ S2–(aq) + ____ Cr2O72–(aq) → ____ S(s) + ____ Cr3+(aq)
In the balanced equation, for every mole of Cr2O72– that reacts, _____ mol of H+ are
consumed.
A)
7
B)
10
C)
5
D)
14
E)
8
134. Which of the following do you need to know to be able to calculate the molarity of a salt
solution?
I. the mass of salt added
II. the molar mass of the salt
III. the volume of water added
IV. the total volume of the solution
A)
II and III only
B)
I, II, and IV only
C)
I, II, and III only
D)
I and III only
E)
You need all of the information.
135. Each of the following containers illustrates a solution in which the black spheres represent
solute.
Which is the most concentrated solution?
A)
A
B)
All have the same concentration.
C)
B
D)
C
E)
D
136. A student must prepare 5.00 L of 0.100 M Na2CO3 (106 g/mol). Which is the best procedure
for preparing this solution?
A)
Measure 53.0 g Na2CO3 and add 5.00 kg of H2O.
B)
Measure 10.6 g Na2CO3 and add 5.00 kg of H2O.
C)
Measure 53.0 g Na2CO3 and add H2O until the final homogeneous solution has a
volume of 5.00 L.
D)
Measure 10.6 g Na2CO3 and add H2O until the final homogeneous solution has a
volume of 5.00 L.
E)
Measure 53.0 g Na2CO3 and add 5.00 L of H2O.
137. What mass of Na2CO3 is present in 0.650 L of a 0.505 M Na2CO3 solution?
A)
34.8 g
B)
68.9 g
C)
53.5 g
D)
136 g
E)
82.3 g
Test Bank General Chemistry, 10th edition 39
138. What is the molarity of an NaI solution that contains 7.3 g of NaI in 28.0 mL of solution?
A)
1.7 M
B)
0.049 M
C)
0.0038 M
D)
0.00019 M
E)
0.26 M
139. In order to prepare a standard 1.00 M solution of oxalic acid from H2C2O4 · 2H2O
(126.07 g/mol), 7.564 g of oxalic acid dihydrate should be dissolved in
A)
enough water to make 60.0 g of solution.
B)
52.436 g of water.
C)
60.0 g of water.
D)
enough water to make 60.0 mL of solution.
E)
60.0 cm3 of water.
140. A 29.0-g sample of NaOH is dissolved in water, and the solution is diluted to give a final
volume of 1.60 L. The molarity of the final solution is
A)
18.1 M.
B)
0.453 M.
C)
0.725 M.
D)
0.0552 M.
E)
0.862 M.
141. What is the molarity of hydrochloric acid in a solution containing 88.5 g of HCl in 215 mL
of solution?
A)
0.412 M
B)
0.00243 M
C)
2.43 M
D)
412 M
E)
11.3 M
Test Bank General Chemistry, 10th edition 40
142. What mass of oxalic acid dihydrate, H2C2O4 · 2H2O, is required to prepare 250.0 mL of a
1.32 M solution of oxalic acid?
A)
126 g
B)
41.6 g
C)
119 g
D)
166 g
E)
29.7 g
143. How many grams of lithium nitrate, LiNO3 (68.9 g/mol), are required to prepare 342.6 mL
of a 0.783 M LiNO3 solution?
A)
0.00389 g
B)
18.5 g
C)
0.0541 g
D)
30.1 g
E)
0.00635 g
144. How many moles of sulfate ions are there in a 0.545-L solution of 0.489 M Al2(SO4)3?
A)
0.267 mol
B)
0.800 mol
C)
3.34 mol
D)
0.0888 mol
E)
2.69 mol
145. What volume of 0.745 M Na2CO3 (106 g/mol) solution contains 50.3 g of Na2CO3?
A)
0.354 L
B)
7.16 103 L
C)
0.637 L
D)
3.97 103 L
Test Bank General Chemistry, 10th edition 41
E)
1.57 L
146. Which of the following solutions contains the largest number of moles of dissolved
particles?
A)
25. mL of 5.0 M sodium chloride
B)
25. mL of 2.0 M sulfuric acid
C)
200. mL of 0.10 M sodium hydroxide
D)
50. mL of 1.0 M hydrochloric acid
E)
100. mL of 0.5 M nitric acid
147. Which substance would produce 2 mol of particles per mole of solute when dissolved in
water?
A)
NH4CH3COO
B)
CH2O
C)
CO2
D)
SO2
E)
Al(NO3)3
148. How many moles of KOH are present in 25.4 mL of 0.965 M KOH?
A)
2.63 10−2
mol
B)
26.3 mol
C)
2.45 10−2
mol
D)
24.5 mol
E)
0.965 mol
149. What mass of H3PO4 (98.0 g/mol) is present in 36.2 L of a 0.0827 M solution of H3PO4?
A)
0.0305 g
B)
0.00341 g
Test Bank General Chemistry, 10th edition 42
C)
2.93 102 g
D)
4.29 104 g
E)
4.47 g
150. Calculate the molarity of a solution that contains 32.5 g of NaOH (40.0 g/mol) in 469 mL of
solution.
A)
0.381 M
B)
2.77 103 M
C)
0.577 M
D)
3.81 105 M
E)
1.73 M
151. What volume of 0.76 M sodium bromide, NaBr, contains 8.8 10–4 mol of bromide ions?
A)
0.58 mL
B)
0.67 L
C)
1.2 mL
D)
0.86 L
E)
0.67 mL
152. To dilute 1.00 L of a 0.600 M to 0.100 M, the final volume must be
A)
60 L.
B)
0.7 L.
C)
1/6 the original volume.
D)
More information is needed to answer this question.
E)
6 times the original volume.
153. What is the final concentration of HCl in a solution prepared by addition of 930.0 mL of
8.77 M HCl to 468.0 mL of 3.22 M HCl? Assume volumes are additive.
A)
6.00 M
B)
0.00858 M
C)
12.0 M
D)
6.91 M
E)
5.08 M
154. In order to dilute 35.5 mL of 0.533 M HCl to 0.100 M, the volume of water that must be
added is
A)
28.8 mL.
B)
6.66 mL.
C)
1.89 102 mL.
D)
1.50 10–3 mL.
E)
1.54 102 mL.
155. What volume of 2.52 M HCl is required to prepare 176.5 mL of 0.449 M HCl?
A)
9.91 102 mL
B)
1.56 102 mL
C)
31.4 mL
D)
0.0318 mL
E)
2.00 102 mL
156. A dilute solution is prepared by transferring 45.00 mL of a 0.5616 M stock solution to a
400.0 mL volumetric flask and diluting to mark. What is the molarity of this dilute
solution?
A)
0.06318 M
B)
0.1264 M
C)
0.04992 M
D)
0.01580 M
E)
0.2808 M
Test Bank General Chemistry, 10th edition 44
157. In order to determine the amount of chloride ion in a solution by using gravimetric analysis,
which of the following should you add to the solution?
A)
NaNO3(aq)
B)
Al(NO3)3(aq)
C)
NaCl(aq)
D)
AgNO3(aq)
E)
Mg(NO3)2(aq)
158. The concentration of sulfate in a sample of wastewater is to be determined by using
gravimetric analysis. To a 100.0-mL sample of the wastewater is added an excess of
calcium nitrate, forming the insoluble calcium sulfate (136.1 g/mol) according to the
balanced equation given below. The solid calcium sulfate is dried, and its mass is measured
to be 0.7272 g. What was the concentration of sulfate in the original wastewater sample?
SO42–(aq) + Ca(NO3)2(aq) → CaSO4(s) + 2NO3–(aq)
A)
0.05343 M
B)
0.9897 M
C)
18.72 M
D)
1.872 M
E)
9.897 M
159. The concentration of Pb2+ in a sample of wastewater is to be determined by using
gravimetric analysis. To a 100.0-mL sample of the wastewater is added an excess of
sodium carbonate, forming the insoluble lead (II) carbonate (267.2092 g/mol) according to
the balanced equation given below. The solid lead (II) carbonate is dried, and its mass is
measured to be 0.4078 g. What was the concentration of Pb2+ in the original wastewater
sample?
Pb2+(aq) + Na2CO3(aq) → PbCO3(s) + 2Na+(aq)
A)
0.01526 M
B)
0.001526 M
C)
1.090 M
D)
0.004078 M
E)
65.52 M
160. What minimum mass of copper (II) nitrate must be added to 30.0 mL of a 0.0387 M
phosphate solution in order to completely precipitate all of the phosphate as solid copper (II)
phosphate?
2PO43–(aq) + 3Cu(NO3)2(aq) → Cu3(PO4)2(s) + 6NO3–(aq)
A)
0.218 g
B)
0.653 g
C)
0.145 g
D)
0.0726 g
E)
0.327 g
161. The reaction of HCl with NaOH is represented by the equation
HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)
What volume of 0.631 M HCl is required to titrate 15.8 mL of 0.321 M NaOH?
A)
3.20 mL
B)
1.58 mL
C)
8.04 mL
D)
15.8 mL
E)
31.1 mL
162. The reaction of H2SO4 with NaOH is represented by the equation
H2SO4(aq) + 2NaOH(aq) → Na2SO4(aq) + 2H2O(l)
What volume of 0.587 M H2SO4 is required to neutralize 12.7 mL of 0.302 M NaOH?
A)
3.27 mL
B)
1.70 mL
C)
6.53 mL
D)
12.7 mL
E)
24.7 mL
Test Bank General Chemistry, 10th edition 46
163. In a volumetric analysis experiment, a solution of sodium oxalate (Na2C2O4) in acidic
solution is titrated with a solution of potassium permanganate (KMnO4) according to the
following balanced chemical equation:
2KMnO4(aq) + 8H2SO4(aq) + 5Na2C2O4(aq) → 2MnSO4(aq) + 8H2O(l) + 10CO2(g) +
5Na2SO4(aq) + K2SO4(aq)
What volume of 0.0388 M KMnO4 is required to titrate 0.134 g of Na2C2O4 dissolved in
20.0 mL of solution?
A)
1.38 mL
B)
3.45 mL
C)
10.3 mL
D)
25.8 mL
E)
20.0 mL
164. In a volumetric analysis experiment, an acidic aqueous solution of methanol (CH3OH) is
titrated with a solution of potassium dichromate (K2Cr2O7) according to the following
balanced chemical equation:
2K2Cr2O7(aq) + 8H2SO4(aq) + 3CH3OH(aq) → 2Cr2(SO4)3(aq) + 11H2O(l) + 3HCOOH(aq)
+ 2K2SO4(aq)
What volume of 0.00389 M K2Cr2O7 is required to titrate 1.77 g of CH3OH dissolved in
20.0 mL of solution?
A)
21.3 mL
B)
683 mL
C)
9.47 mL
D)
20.0 mL
E)
303 mL
165. A 50.00-mL sample of a weak acid is titrated with 0.0955 M NaOH. At the endpoint, it is
found that 32.56 mL of titrant was used. What was the concentration of the weak acid?
A)
0.0622 M
B)
3.11 M
C)
0.0955 M
D)
5.87 10–5 M
E)
0.147 M
Test Bank General Chemistry, 10th edition 47
166. A 40.00-mL sample of a weak base is titrated with 0.0935 M HCl. At the endpoint, it is
found that 32.87 mL of titrant was used. What was the concentration of the weak base?
A)
0.114 M
B)
7.11 10–5 M
C)
3.07 M
D)
0.0935 M
E)
0.0768 M
167. In a volumetric analysis experiment, a solution of sodium oxalate (Na2C2O4) in acidic
solution is titrated with a solution of potassium permanganate (KMnO4) according to the
following balanced chemical equation:
2KMnO4(aq) + 8H2SO4(aq) + 5Na2C2O4(aq) → 2MnSO4(aq) + 8H2O(l) + 10CO2(g) +
5Na2SO4(aq) + K2SO4(aq)
It required 25.0 mL of 0.0448 M KMnO4 to reach the endpoint. What mass of Na2C2O4 was
present initially?
A)
2.40 g
B)
0.0600 g
C)
15.0 g
D)
0.150 g
E)
0.375 g
168. In a volumetric analysis experiment, an acidic aqueous solution of methanol (CH3OH) is
titrated with a solution of potassium dichromate (K2Cr2O7) according to the following
balanced chemical equation:
2K2Cr2O7(aq) + 8H2SO4(aq) + 3CH3OH(aq) → 2Cr2(SO4)3(aq) + 11H2O(l) + 3HCOOH(aq)
+ 2K2SO4(aq)
It required 43.91 mL of 0.0435 M K2Cr2O7 to reach the endpoint. What mass of CH3OH
was present initially?
A)
0.0918 g
B)
2.09 g
C)
0.929 g
D)
0.0612 g
E)
0.0408 g
169. An impure sample of benzoic acid (C6H5COOH, 122.12 g/mol) is titrated with 0.8067 M
NaOH. A 5.109-g sample requires 36.97 mL of titrant to reach the endpoint. What is the
percent by mass of benzoic acid in the sample?
C6H5COOH(aq) + NaOH(aq) → NaC6H5COO(aq) + H2O(l)
A)
0.02442 %
B)
2.982 %
C)
100.0 %
D)
24.42 %
E)
71.29 %