Test Bank Chapter 3 Composition of Substances and Solutions

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Chapter 03: Composition of Substances and Solutions

1. Which of the following compounds contains the largest number of atoms? (Outcome # 1,2) DOK 2
2. 1.00 mole of NH₃
3. 1.00 mole of H₂SO₄
4. 1.00 mole of HBr
5. What is the molar mass of (NH₄)₃PO₄? (Outcome # 1,2) DOK 2
6. 113 g
7. 121 g
8. 149 g
9. What is the mass in grams of 6.022 x 10²³ molecules of CO₂? (Outcome # 1,2) DOK 3
10. 22 g
11. 44 g
12. 66 g
13. What is the total number of atoms contained in 2.00 moles of iron? (Outcome # 1,2) DOK 2
14. 118
15. 6.02 x 10²³
16. 1.2 x 10²⁴
17. What is the molar mass of K₂CO₃? (Outcome # 1,2) DOK 2
18. 138 g/mol
19. 106 g/mol
20. 99 g/mol
21. What is the total number of atoms contained in 1.00 mole of sodium? (Outcome # 1,2,9) DOK 2
22. 118
23. 6.02 x 10²³
24. 1.2 x 10²⁴
25. If a hazardous bottle is labeled 20.2 percent by mass Hydrochloric Acid, HCl, with a density of 1.096 g/mL, calculate the molarity of the HCl solution. (Outcome # 1,2,5,8,9,10) (DOK 3)
26. 6.07 M
27. 0.22 M
28. 14.7 M
29. To dilute a HCl solution from 0.500 M to 0.100 M the final volume must be: (Outcome # 1,2,4,5,8) DOK 2
30. 1/5 the original volume
31. 5 times the original volume
32. 50 L
33. How would you prepare a 1 M solution of sodium hydroxide? (Outcome # 5) (DOK 3)
34. add 40.0 grams of sodium hydroxide to 1 L of water
35. add 40.0 grams of sodium hydroxide to 100 L of water
36. add 40.0 grams of sodium hydroxide to 10 L of water
37. How would you prepare a 0.5 M solution of sodium hydroxide? (Outcome # 5) (DOK 3) (Paired item 1)
38. add 40.0 grams of sodium hydroxide to 1 L of water
39. add 20.0 grams of sodium hydroxide to 1 L of water
40. add 20.0 grams of sodium hydroxide to 10 L of water
41. An experiment requires 15.0 mL of a 0.100 M solution of HCl. If you have a 12.0 M HCl stock solution in the laboratory, how would you prepare enough 0.1 M solution to run at least 3 experiments? (Outcome # 5) (DOK 3)
42. add 0.833 mL 12 M HCl stock solution to 99.167 mL water
43. add 0.833 mL 12 M HCl stock solution to 49.167 mL water
44. add 0.833 mL 12 M HCl stock solution to 199.167 mL water
45. What is the mass in grams of 1.59 moles of aluminum oxide? (Outcome # 2) (DOK 2)
46. 162 g
47. 0.0156 g
48. 64.1 g
49. What is the mass in grams of 0.852 moles of ferric oxide? (Outcome # 2) (DOK 3) (Paired item 1)
50. 5.34 x 10^-3 g
51. 187 g
52. 136 g
53. How many moles are in 1.77 kg of cuprous sulfate? (Outcome # 2) (DOK 3)
54. 7.93 x 10^-3 moles
55. 7.93 moles
56. 395 moles
57. How many grams are in 2.05 x 10²³ molecules of dinitrogen pentoxide? (Outcome # 2) (DOK 3)
58. 317 g
59. 36.8 g
60. 0.00315 g
61. How many grams are in 1.02 x 10²² molecules of nitric acid? (Outcome # 2) (DOK 3) (Paired item 1)
62. 1.07 g
63. 3720 g
64. 2.69 x 10^-4 g
65. What is the total number of atoms contained in 2.11 moles of nickel? (Outcome # 2) (DOK 2)
66. 2.85 x 10²³ atoms
67. 1.27 x 10²⁴ atoms
68. 3.50 x 10^-24 atoms
69. How many atoms are in 1.00 mole of Au? (Outcome # 2) (DOK 2) (Paired item 1)
70. 6.02 x 10²³ atoms
71. 1.66 x 10^-24 atoms
72. 197 atoms
73. A 44.8 g rhodium sample contains how many rhodium atoms? (Outcome # 2) (DOK 3)
74. 2.62 x 10²³ atoms
75. 6.02 x 10²³ atoms
76. 2.70 x 10²⁵ atoms
77. What is the molar mass of potassium nitrate? (Outcome # 2) (DOK 2)
78. 85.10 g/mol
79. 140.20 g/mol
80. 101.10 g/mol
81. Commercial grade fuming nitric acid contains about 90% HNO₃ by mass with a density of 1.50 g/mL, calculate the molarity of the HNO₃ solution. (Outcome # 9) (DOK 3)
82. 0.214 M
83. 21.4 M
84. 2.14 M
85. Which of the following is a method used to allow scientists to determine an empirical formula and identify an organic compound by combusting a sample and the resulting combustion products are quantitatively analyzed? (Outcome # 7) (DOK 1)
86. gravimetric analysis
87. combustion analysis
88. thermal analysis
89. A 3.00 g sample of unknown hydrocarbon is prepared for combustion analysis. After the hydrocarbon undergoes complete combustion, 8.80 g of CO₂ and 5.40 g of H₂O are produced. What is the empirical formula of the unknown? (Outcome # 7) (DOK 3)
90. CH₃
91. CH
92. CH₂
93. A 0.125 g sample of unknown hydrocarbon is prepared for combustion analysis. After the hydrocarbon undergoes complete combustion, 0.4225 g of CO₂ and 0.0865 g of H₂O are produced. What is the empirical formula of the unknown? (Outcome # 7) (DOK 3) (Paired item 1)
94. CH₃
95. CH
96. CH₂
97. An unknown organic compound (0.315 g) containing only C, H, and O produces 0.771 of CO₂ and 0.105 g of H₂O when it undergoes complete combustion. The approximate molar mass is 108 g/mol. Which of the following compounds could be the identification of the unknown? (Outcome # 7) (DOK 3)
98. para-Cresol, CH₃C₆H₄(OH)
99. Benzyl alcohol, C₆H₅CH₂OH
100. 1,2-Benzoquinone, C₆H₄O₂
101. Which of the following is an experimental technique used to determine the mass percent of elements found in a compound? (Outcome # 7) (DOK 1)
102. gravimetric analysis
103. mass analysis
104. elemental analysis
105. An unknown hydrocarbon compound was analyzed for hydrogen by elemental analysis and results show that it contains 15.88 % H. What is the empirical formula? (Outcome # 7) (DOK 2)
106. C₄H₉
107. C₈H₁₈
108. C₁₂H₂₇
109. A 5.91 g unknown sample analyzed by elemental analysis revealed a composition of 37.51 % C. In addition, it was determined that the sample contains 1.4830 x 10²³ hydrogen atoms and 1.2966 x 10²³ oxygen atoms. What is the empirical formula? (Outcome # 7) (DOK 3)
110. C₆H₈O₇
111. C₅H₆O₃
112. C₈H₁₆O₅
113. What is the concentration in ppm of a 3.7 L solution (d = 1.00 g/mL) containing 4.21 x 10^-7 kg of the pesticide DDT? (Outcome # 8) (DOK 2)
114. 1.14 x 10^-1 ppm
115. 1.14 x 10² ppm
116. 1.14 x 10¹ ppm
117. When a salt is dissolved in water, it is represented by the following notation in a chemical reaction? (Outcome # 6) (DOK 1)
118. (aq)
119. (l)
120. (s)
121. How is a solid phase represented in a chemical reaction? (Outcome # 6) (DOK 1)
122. (s)
123. (g)
124. (l)
125. How is a liquid phase represented in a chemical reaction? (Outcome # 6) (DOK 1)
126. (s)
127. (g)
128. (l)
129. How is a gas phase represented in a chemical reaction? (Outcome # 6) (DOK 1)
130. (s)
131. (g)
132. (l)
133. What are the proper units for molar mass in chemistry? (Outcome # 6) (DOK 1)
134. amu
135. g/mol
136. g/mmol
137. How many atoms can be found in a mole of mercury? (Outcome # 2) (DOK 2)
138. 201 atoms
139. 6.02 x 10²³ atoms
140. 1.21 x 10²⁶ atoms
141. A 21.8 g sample of water contains how many water molecules? (Outcome # 2) (DOK 3)
142. 7.29 x 10²³ molecules
143. 6.02 x 10²³ molecules
144. 2.01 x 10^-24 molecules
145. A sample has a molar mass of 143 g/mol, identify the sample. (Outcome # 2) (DOK 1)
146. AuCl
147. AcCl
148. AgCl
149. What is the molar mass of 2.50 g of an unknown sample dissolved in 130. mL of water with a concentration of 0.480 M? (Outcome # 4) (DOK 3)
150. 0.062 g/mol
151. 8.65 g/mol
152. 40.1 g/mol
153. 2.50 g of an unknown base is dissolved in 289 mL of water and has a concentration of 0.216 M. What is the identification of the unknown base? (Outcome # 4) (DOK 3)
154. NaOH
155. LiOH
156. KOH
157. How many grams of Hydrogen are present in three moles of Hydrogen? (Outcome # 1,5,9) (DOK 1)
158. two grams
159. six grams
160. one gram
161. Which of the following compounds contains the largest number of atoms? (Outcome # 1,9) (DOK 2)
162. 1.00 mole of NH₃
163. 1.00 mole of H₂SO₄
164. 1.00 mole of HBr
165. How many atoms are in 12.8 g of copper metal? (Outcome # 6) (DOK 2)
166. 7.71 x 10²⁴ atoms
167. 1.21 x 10²³ atoms
168. 3.34 x 10^-25 atoms
169. How many grams contain 1.45 x 10²¹ zinc atoms? (Outcome # 6) (DOK 2)
170. 1.57 x 10^-1 g
171. 5.71 x 10⁴⁶ g
172. 2.41 x 10^-3 g
173. How many moles are in 11.0 g of silver metal? (Outcome # 6) (DOK 1)
174. 9.81 moles
175. 1.19 x 10³ moles
176. 1.02 x 10^-1 moles
177. What is Avogadro’s number? (Outcome # 6) (DOK 1)
178. 6.022 x 10²³ particles/mole
179. 6.022 x 10²² particles/mole
180. 6.022 x 10²⁴ particles/mole
181. Which of the following 85.0 g samples contain the greatest number of atoms? (Outcome # 6) (DOK 3)
182. zinc
183. gold
184. zirconium
185. Which of the following 49.5 g samples contain the fewest number of atoms? (Outcome # 6) (DOK 3) (Paired item 1)
186. lead
187. platinum
188. iron
189. How many atoms are in 1 mole of calcium? (Outcome # 6) (DOK 1)
190. 6.022 x 10²³ atoms
191. 6.022 x 10^-23 atoms
192. 6.022 x 10²² atoms
193. How many moles contain 6.022 x 10²³ lithium atoms? (Outcome # 6) (DOK 1)
194. 6.022 x 10²³ moles
195. 1 mole
196. 2 moles