Exam Prep Solutions and Colloids Chapter 11 2nd Edition

Supplemental Test Items to accompany OpenStax Chemistry. Note that not all chapters of OpenStax Chemistry have accompanying test items. Building on the community-oriented nature of OpenStax resources, we invite you to submit items to be considered for future inclusion.

Chapter 11: Solutions and Colloids

1. Based off the molecular polarity of water, which of the following molecules would be soluble in water? (Outcome # 4) (DOK 2)
2. glucose, methanol, and ethanol
3. carbon dioxide, methane, methanol
4. glucose, carbon dioxide, ethanol
5. Which of the following would be a strong electrolyte in solution? (Outcome # 6) (DOK 2)
6. PbI₂
7. KCl
8. Al(OH)₃
9. Which of the following would be a weak electrolyte in solution? (Outcome # 6) (DOK 2)
10. acetic acid
11. sulfuric acid
12. hydroiodic acid
13. Which of the following when dissolved in deionized water would make a poor conducting solution? (Outcome # 6) (DOK 2)
14. baking soda
15. sugar
16. salt
17. Which of the following when dissolved in deionized water would make a good conducting solution? (Outcome # 6) (DOK 2) (Paired item 1)
18. methanol
19. sugar
20. baking soda
21. For an experiment, you are asked to prepare a 2 m strong electrolytic solution. Which of the following salts would you use? (Outcome # 6) (DOK 3)
22. an alkali salt
23. an alkaline salt
24. either an alkali or an alkaline salt
25. Which of the following substances would be a poor choice for making conductive solutions? (Outcome # 6) (DOK 3)
26. C₆H₁₂O₆, CH₃OH, CH₃CH₂OH
27. HCl, KBr, HNO₃
28. NaOH, KOH, LiOH
29. Which of the following would be soluble in water? (Outcome # 9) (DOK 2)
30. sugar, NaCl, HCl
31. sugar, NaOH, ethane
32. sugar, HNO₃, methane
33. How would you purify salt water so that it becomes potable? (Outcome # 2) (DOK 1)
34. gravity filtration
35. vacuum filtration
36. distillation
37. Which of the following would conduct electricity? (Outcome # 2) (DOK 3)
38. solid NaCl
39. NaCl solution
40. both solid NaCl and a NaCl solution
41. At what temperature does salt water freeze? (Outcome # 7) (DOK 1)
42. 0 °C
43. below 0 °C
44. above 0 °C
45. If you want to boil a pot of water containing salt, at what temperature would boiling begin? (Outcome # 7) (DOK 1)
46. 100 °C
47. below 100 °C
48. above 100 °C
49. What happens to the freezing point of water when ethylene glycol is added? (Outcome # 8) (DOK 2)
50. Ethylene glycol has no effect on the freezing point of water.
51. Ethylene glycol will interfere with the organization of water molecules during the freezing process therefore increasing the freezing point of water.
52. Ethylene glycol will interfere with the organization of water molecules during the freezing process therefore reducing the freezing point of water.
53. Which of the following is a colligative property? (Outcome # 8) (DOK 1)
54. boiling-point elevation
55. temperature of a solution
56. color of a solution
57. Which of the following is a not a colligative property? (Outcome # 8) (DOK 1) (Paired item 1)
58. boiling-point elevation
59. temperature of a solution
60. Freezing-point depression
61. Assuming all the salts below are the same concentration, which salt would lower the freezing point of water the most? (Outcome # 8) (DOK 1)
62. NaCl
63. KBr
64. CaCl₂
65. Which salt would lower the freezing point of a solvent the most? (Outcome # 8) (DOK 2)
66. 1.5m NaCl
67. 0.5m CaCl₂
68. 1.25m Na₂SO₄
69. What would be the best method for raising the boiling point of water in a kettle by a few degrees Celsius? (Outcome # 8) (DOK 3)
70. increase the temperature of the stove
71. add some table salt to the water
72. increase the temperature of the stove and increase the surface area by transferring the water to a larger kettle
73. What would be the best method for lowering the freezing point of water in an ice tray that is in the freezer? (Outcome # 8) (DOK 3)
74. decrease the temperature of the freezer
75. decrease the temperature of the freezer and increase the surface area by transferring the water to a larger ice tray
76. add some table salt to the water
77. Patients who enter the emergency room dehydrated are usually given sterile saline solution intravenously. The solution administered is isotonic to prevent cell damage. What would happen if the solution was hypotonic? (Outcome # 6) (DOK 3)
78. Hypotonic solutions have a higher osmotic pressure than that within cells so hemolysis can occur.
79. Hypotonic solutions have a lower osmotic pressure than that within cells so hemolysis can occur.
80. Hypotonic solutions have the same osmotic pressure as that within cells so hemolysis can occur.
81. Patients who enter the emergency room dehydrated are usually given sterile saline solution intravenously. The solution administered is isotonic to prevent cell damage. What would happen if the solution was hypertonic? (Outcome # 6) (DOK 3) (Paired item 1)
82. Hypertonic solutions have the same osmotic pressure as that within cells so crenation can occur.
83. Hypertonic solutions have a lower osmotic pressure than that within cells so crenation can occur.
84. Hypertonic solutions have a higher osmotic pressure than that within cells so crenation can occur.
85. Which type of solution has a lower osmotic pressure than that within cells? (Outcome # 6) (DOK 1)
86. hypertonic
87. hypotonic
88. isotonic
89. Which type of solution has a higher osmotic pressure than that within cells? (Outcome # 6) (DOK 1)
90. isotonic
91. hypertonic
92. hypotonic
93. Which type of solution has the same osmotic pressure as that within cells? (Outcome # 6) (DOK 1)
94. hypertonic
95. isotonic
96. hypotonic
97. What is the osmolarity of a 2 M NaCl solution? (Outcome # 6) (DOK 1)
98. 2 osmol
99. 6 osmol
100. 4 osmol
101. A KCl solution is 0.500 M. What is the osmolarity? (Outcome # 6) (DOK 1) (Paired item 1)
102. 1 osmol
103. 2 osmol
104. 4 osmol
105. 45.8 g of NaCl is dissolved in 500. mL of a water (d = 1.00 g/mL) and is placed in the freezer at -1 °C overnight. Which statement best describes what would happen to the solution? (Outcome # 3) (DOK 3)
106. The freezing point of the NaCl solution would be -5.83 °C, so the solution would not freeze.
107. The freezing point of the NaCl solution would be 5.83 °C, so the solution would freeze.
108. The freezing point of the NaCl solution would be -2.92 °C, so the solution would not freeze.
109. 17.1 g of calcium chloride is dissolved in 750. mL of a water (d = 1.00 g/mL) and is placed in the freezer at -2 °C overnight. Which statement best describes what would happen to the solution? (Outcome # 3) (DOK 3) (Paired item 1)
110. The freezing point of the calcium chloride solution would be 1.15 °C, so the solution would freeze.
111. The freezing point of the calcium chloride solution would be -1.15 °C, so the solution would freeze.
112. The freezing point of the calcium chloride solution would be -0.382 °C, so the solution would freeze.
113. How would you be able to increase the boiling point of water on a hotplate? (Outcome # 3) (DOK 2)
114. increase the temperature of the hotplate
115. add less water and increase the temperature of the hotplate
116. add some NaCl to the water
117. How would you increase the concentration of a 1 M NaCl solution? (Outcome # 3) (DOK 1)
118. decant some of the solution down the sink
119. bring the solution to near boiling until desired volume is achieved
120. decrease the temperature of the salt solution to near freezing
121. The solubility of NaCH₃CO₂ in water is ~1.23 g/mL. What would be the best method for preparing a supersaturated NaCH₃CO₂ solution? (Outcome # 3) (DOK 2)
122. add 130 g of NaCH₃CO₂ to 100 mL of H₂O at 80 °C while stirring until all the solid dissolves, then let the solution cool to room temperature
123. add 123 g of NaCH₃CO₂ to 200 mL of H₂O at 80 °C while stirring until all the solid dissolves, then let the solution cool to room temperature
124. add 130 g of NaCH₃CO₂ to 100 mL of H₂O at room temperature while stirring until all the solid dissolves
125. The solubility of KCl in water is ~344 g/L. What would be the best method for preparing a 100 mL saturated KCl solution? (Outcome # 3) (DOK 2)
126. add 38.0 g of KCl to 100 mL of H₂O at room temperature while stirring
127. add 30.0 g of KCl to 100 mL of H₂O at room temperature while stirring
128. add 34.0 g of KCl to 100 mL of H₂O at room temperature while stirring