Solutions Test Preview

Matching

Match each item with the correct statement below.a. solvation e. electrolyteb. weak electrolyte f. colloidc. aqueous solution g. surfactantd. solvent

____ 1. interferes with hydrogen bonding between water molecules____ 2. dissolving medium____ 3. homogeneous mixture of water and dissolved substances____ 4. Solute ions or molecules are surrounded by solvent molecules.____ 5. compound that will conduct current in the liquid state or in aqueous solution____ 6. compound that ionizes incompletely in aqueous solution____ 7. mixture in which particle size averages between 1 nm and 1000 nm

Match each item with the correct statement below.a. dispersed phase e. Tyndall effectb. surface tension f. suspensionc. Brownian motion g. soluted. dispersion medium h. emulsion

____ 8. inward force tending to minimize surface area of a liquid____ 9. dissolved particle____ 10. mixture in which particle size averages greater that 1000 nm in diameter____ 11. Colloidal particles spread throughout a suspension.____ 12. phenomenon observed when beam of light passes through a colloid____ 13. chaotic movement of colloidal particles____ 14. colloid of a liquid in a liquid

Match each item with the correct statement below.a. Henry's law d. supersaturated solutionb. immiscible e. concentrationc. saturated solution

____ 15. describes liquids that are insoluble in one another____ 16. solution containing maximum amount of solute____ 17. solution containing more solute than can theoretically dissolve at a given temperature____ 18. At a given temperature, the solubility of a gas in a liquid is directly proportional to the pressure of the gas

above the liquid.____ 19. measure of the amount of solute dissolved in a specified quantity of solvent

Match each item with the correct statement below.a. boiling point elevation d. molarityb. molality e. freezing point depressionc. mole fraction

____ 20. number of moles of solute dissolved in 1 L of solution____ 21. a colligative property related to the fact that ice will form at higher temperatures in the Great Lakes than in

the ocean____ 22. a colligative property related to a decrease in the vapor pressure of a solution____ 23. number of moles of solute dissolved in 1 kg of solvent____ 24. ratio of moles of solute in solution to total number of moles of both solvent and solute

Multiple ChoiceIdentify the letter of the choice that best completes the statement or answers the question.

____ 25. How does the surface tension of water compare with the surface tensions of most other liquids?a. It is lower.b. It is about the same.c. It is higher.d. It is higher when a surfactant is added.

____ 26. What causes water's low vapor pressure?a. dispersion forces c. hydrogen bondingb. covalent bonding d. ionic attractions

____ 27. What is the shape of the water molecule?a. linear c. trigonal planarb. tetrahedral d. bent

____ 28. Which of the following is primarily responsible for holding water molecules together in the liquid state?a. dispersion forces c. ionic bondsb. hydrogen bonds d. polar covalent bonds

____ 29. Which atom in a water molecule has the greatest electronegativity?a. one of the hydrogen atomsb. both hydrogen atomsc. the oxygen atomd. There is no difference in the electronegativities of the atoms in a water molecule.

____ 30. The bonds between adjacent water molecules are called ____.a. hydrogen bonds c. nonpolar covalent bondsb. ionic bonds d. polar covalent bonds

____ 31. What is primarily responsible for the surface tension of water?a. dispersion forces c. ionic attractionsb. hydrogen bonding d. covalent bonding

____ 32. Which of the following is NOT a result of surface tension in water?a. Surface area is maximized.b. Water has an unusually low vapor pressure.c. Surface appears to have a "skin."d. Drops tend to become spherical.

____ 33. Surface tension ____.a. is the inward force which tends to minimize the surface area of a liquidb. may be increased by detergentsc. is decreased by hydrogen bondingd. causes beads of water to spread out

____ 34. The bonds between the hydrogen and oxygen atoms in a water molecule are ____.a. hydrogen bonds c. nonpolar covalent bondsb. ionic bonds d. polar covalent bonds

____ 35. How much heat is absorbed when 6.30 g of water melts?a. 21 kJ c. 2.10 kJ

b. 0.210 kJ d. 21.0 J____ 36. The fact that ice is less dense than water is related to the fact that ____.

a. the molecular structure of ice is much less orderly than that of waterb. the molecules of ice are held to each other by covalent bondingc. ice has a molecular structure in which water molecules are arranged randomlyd. ice has a molecular structure that is an open framework held together by hydrogen bonds

____ 37. Which is responsible for the high thermal energy required to melt ice?a. covalent bonding c. hydrogen bondingb. dispersion forces d. ionic attractions

____ 38. What is the term for the dissolving medium in a solution?a. solvent c. solvatorb. solute d. emulsifier

____ 39. A solution has which of the following properties?a. Gravity separates its parts.b. The top layer is different in composition than the bottom layer.c. The average diameter of its solute particles usually is less than 1 nm.d. A filter can remove the solute.

____ 40. Which of the following substances is the most soluble in water?a. sodium chloride c. bromineb. methane d. carbon

____ 41. What occurs in solvation?a. Solute ions separate from solvent molecules.b. Solvent molecules surround solute ions.c. Solvent molecules bind covalently to solute molecules.d. Ionic compounds are formed.

____ 42. Which of the following substances dissolves most readily in gasoline?a. CH c. NHb. HCl d. NaBr

____ 43. A solution is a mixture ____.a. from which the solute can be filteredb. that has the same properties throughoutc. that is heterogeneousd. in which a solid solute is always dissolved in a liquid solvent

____ 44. Predict which one of the following compounds would be insoluble in water.a. NaCl c. CFb. HCl d. CuSO

____ 45. Why are two nonpolar substances able to dissolve in each other?a. They have similar attractive forces in their molecules.b. They combine to produce a polar substance.c. There is no attractive force between them.d. Nonpolar substances cannot dissolve in each other.

____ 46. Which of these would you expect to be soluble in the nonpolar solvent carbon disulfide, CS ?a. c. NaClb. CI d. SnS

____ 47. Which of the following substances dissolves most readily in water?a. BaSO c. NHb. CaCO d. CH

____ 48. What type of compound is always an electrolyte?

a. polar covalent c. ionicb. nonpolar covalent d. network solid

____ 49. An electric current can be conducted by ____.a. methane gas c. a salt solutionb. a sugar solution d. rubbing alcohol

____ 50. Which of the following compounds conducts electricity only in the molten state?a. sodium bromide c. calcium hydroxideb. magnesium sulfate d. barium sulfate

____ 51. Which of the following compounds is a nonelectrolyte?a. sodium bromide c. copper chlorideb. magnesium sulfate d. carbon tetrachloride

____ 52. Which of the following compounds is an electrolyte?a. rubbing alcohol c. carbon tetrachlorideb. sugar d. sodium hydroxide

____ 53. Which of the following compounds is a nonelectrolyte when pure, but an electrolyte when dissolved in water?a. rubbing alcohol c. carbon tetrachlorideb. sugar d. ammonia

____ 54. Which of the following are weak electrolytes in water?a. ionic compounds that partially dissociate in waterb. ionic compounds that are solublec. polar compounds that ionized. nonpolar compounds that do not ionize

____ 55. Which of the following compounds is a weak electrolyte?a. NaBr c. KOHb. HBr d. NH

____ 56. Which of the following compounds is a strong electrolyte?a. ammonia c. sugarb. acetic acid d. potassium sulfate

____ 57. Which of the following substances is NOT an electrolyte?a. KCl c. LiClb. CCl d.

____ 58. Which of the following is NOT a common hydrate?a. Epsom salt c. sugarb. borax d. alum

____ 59. Which symbol is used to connect the formula of the compound with the number of water molecules in a hydrate?a. a parenthesis c. a multiplication symbolb. an asterisk d. a dot

____ 60. What is another term for the water of hydration?a. water of solvation c. water of sublimationb. water of crystallization d. water of efflorescence

____ 61. Which compound changes color when it becomes a hydrate?a. silicon dioxide c. copper(II) sulfateb. sodium chloride d. potassium chloride

____ 62. A hydrated crystal that has a water vapor pressure greater than the water vapor pressure of air is called ____.a. a desiccant c. hygroscopicb. deliquescent d. efflorescent

____ 63. A crystal that absorbs water vapor from the air is ____.a. aqueous c. hygroscopicb. deliquescent d. efflorescent

____ 64. Which of the following mixture types is characterized by the settling of particles?a. solution c. colloidb. suspension d. hydrate

____ 65. Which of the following mixture types can be filtered to remove solute?a. suspensions only c. suspensions and colloidsb. colloids only d. suspensions and solutions

____ 66. Which of the following materials is NOT a colloid?a. glue c. smokeb. alloy d. muddy water

____ 67. Which of the following mixtures is NOT a colloid?a. fog c. paintb. milk d. sugar water

____ 68. An emulsion is which type of mixture?a. suspension c. solutionb. colloid d. gaseous

____ 69. The solute in a colloidal suspension is called the ____.a. dissolving phase c. dispensing phaseb. dispersed phase d. dispersion medium

____ 70. What is the size range of particles in a colloid?a. more than 1000 nm c. between 1 nm and 1000 nmb. between 100 nm and 1000 nm d. between 1 nm and 10 nm

____ 71. Which of the following types of mixtures exhibit the Tyndall effect?a. suspensions and colloids c. colloids and solutionsb. suspensions and solutions d. colloids only

____ 72. Which of these statements is correct?a. Particles can be filtered from a suspension.b. A solution is heterogeneous.c. A colloidal system does not exhibit the Tyndall effect.d. The particles in a colloidal system are affected by gravity.

____ 73. An emulsion is a colloidal dispersion of a ____.a. solid in a liquid c. gas in a liquidb. liquid in a liquid d. liquid in a gas

____ 74. An emulsifying agent is typically characterized by having ____.a. one polar end c. two polar endsb. one nonpolar end d. one polar end and one nonpolar end

____ 75. What causes Brownian motion in colloids?a. molecules of the dispersion medium colliding with dispersed phase particlesb. coagulation of particles of the dispersed phasec. erratic flashes of lightd. There is no Brownian motion in colloids.

____ 76. Which of the following usually makes a substance dissolve faster in a solvent?a. agitating the solutionb. increasing the particle size of the solutec. lowering the temperatured. decreasing the number of particles

____ 77. What is the maximum amount of KCl that can dissolve in 200 g of water?(The solubility of KCl is 34 g/100 g H2O at 20 C.)a. 17 g c. 68 gb. 34 g d. 6800 g

____ 78. What is the solubility of silver nitrate if only 11.1 g can dissolve in 5.0 g of water at 20 C?

a.

at 20 C

c.

at 20 Cb.

at 20 C

d.

at 20 C____ 79. Which of the following expressions is generally used for solubility?

a. grams of solute per 100 grams of solventb. grams of solute per 100 milliliters of solventc. grams of solute per 100 grams of solutiond. grams of solute per 100 milliliters of solution

____ 80. Which of the following pairs of factors affects the solubility of a particular substance?a. temperature and the nature of solute and solventb. temperature and degree of mixingc. particle size and degree of mixingd. particle size and temperature

____ 81. If a crystal added to an aqueous solution causes many particles to come out of the solution, the original solution was ____.a. unsaturated c. an emulsionb. saturated d. supersaturated

____ 82. Which of the following substances is less soluble in hot water than in cold water?a. CO c. NaNOb. NaCl d. KBr

____ 83. Which of the following occurs as temperature increases?a. Solubility decreases. c. Solubility remains the same.b. Solubility increases. d. Molarity doubles.

____ 84. The solubility of a gas in a liquid is ____.a. proportional to the square root of the pressure of the gas above the liquidb. directly proportional to the pressure of the gas above the liquidc. inversely proportional to the pressure of the gas above the liquidd. unrelated to the pressure of the gas above the liquid

____ 85. If the solubility of a particular solute is at 20 C, which of the following solution concentrations would represent a supersaturated aqueous solution of that solute?a.

at 25 C

c.

at 20 Cb.

at 15 C

d.

at 20 C____ 86. What happens to the solubility of a gas, in a liquid, if the partial pressure of the gas above the liquid

decreases?a. The solubility decreases. c. The solubility remains the same.b. The solubility increases. d. The solubility cannot be determined.

____ 87. To increase the solubility of a gas at constant temperature from 1.20 g/L, at 1.4 atm, to 2.3 g/L, the pressure would have to be increased to ____.a. 0.37 atm c. 1.37 atmb. 0.7 atm d. 2.7 atm

____ 88. If the solubility of a gas in water is 4.0 g/L when the pressure of the gas above the water is 3.0 atm, what is the pressure of the gas above the water when the solubility of the gas is 1.0 g/L?

a. 0.75 atm c. 4.0 atmb. 1.3 atm d. 12 atm

____ 89. In a concentrated solution there is ____.a. no solvent c. a small amount of soluteb. a large amount of solute d. no solute

____ 90. What is the molarity of a solution that contains 6 moles of solute in 2 liters of solution?a. 6M c. 7Mb. 12M d. 3M

____ 91. In which of the following is the solution concentration expressed in terms of molarity?a. c.

b. d.

____ 92. Which of the following operations yields the number of moles of solute?a. molarity moles of solution c. molarity mass of solutionb. molarity liters of solution d. moles of solution volume of solution

____ 93. What is the molarity of a solution containing 7.0 moles of solute in 569 mL of solution?a. 81M c. 12Mb. 0.081M d. 4.0M

____ 94. What is the molarity of 200 mL of solution in which 2.0 moles of sodium bromide is dissolved?a. 2.0M c. 0.40Mb. 10M d. 4.0M

____ 95. What is the number of moles of solute in 250 mL of a 0.4M solution?a. 0.1 mol c. 0.62 molb. 0.16 mol d. 1.6 mol

____ 96. What is the molarity of a solution containing 56 grams of solute in 959 mL of solution? (molar mass of solute = 26 g/mol)a. 1.5M c. 2.1Mb. 2.2M d. 0.0022M

____ 97. What mass of sucrose, C H O , is needed to make 500.0 mL of a 0.200M solution?a. 34.2 g c. 17.1 gb. 100 g d. 68.4 g

____ 98. What mass of Na SO is needed to make 2.5 L of 2.0M solution? (Na = 23 g; S = 32 g; O = 16 g)a. 178 g c. 356 gb. 284 g d. 710 g

____ 99. What does NOT change when a solution is diluted by the addition of solvent?a. volume of solvent c. number of moles of soluteb. mass of solvent d. molarity of solution

____ 100. How many mL of a 2.0M NaBr solution are needed to make 200.0 mL of 0.50M NaBr?a. 25 mL c. 100 mLb. 50 mL d. 150 mL

____ 101. The volume of 6.00M HCl needed to make 319 mL of 6.80M HCl is ____.a. 0.128 mL c. 281 mLb. 7.8 mL d. 362 mL

____ 102. If 2.0 mL of 6.0M HCl is used to make a 500.0-mL aqueous solution, what is the molarity of the dilute solution?a. 0.024M c. 0.30Mb. 0.24M d. 0.83M

____ 103. To 225 mL of a 0.80M solution of KI, a student adds enough water to make 1.0 L of a more dilute KI solution. What is the molarity of the new solution?a. 180M c. 0.35Mb. 2.8M d. 0.18M

____ 104. If the percent by volume is 2.0% and the volume of solution is 250 mL, what is the volume of solute in solution?a. 0.5 mL c. 5.0 mLb. 1.25 mL d. 12.5 mL

____ 105. In which of the following is concentration expressed in percent by volume?a. 10% (v/v) c. 10% (m/m)b. 10% (m/v) d. 10%

____ 106. If the percent (mass/mass) for a solute is 4% and the mass of the solution is 200 g, what is the mass of solute in solution?a. 8.0 g c. 80 gb. 50 g d. 800 g

____ 107. The volume of alcohol present in 620 mL of a 40.0% (v/v) solution of alcohol is ____.a. 372 mL c. 248 mLb. 40.0 mL d. 580 mL

____ 108. How many milliliters of alcohol are in 167 mL of an 85.0% (v/v) alcohol solution?a. 252 mL c. 145 mLb. 228 mL d. 142 mL

____ 109. In which of the following is concentration expressed in percent by volume?a.

100%

c.

100%b.

100%

d.

100%____ 110. Which of the following is NOT a colligative property of a solution?

a. boiling point elevation c. vapor pressure loweringb. supersaturation d. freezing point depression

____ 111. Colligative properties depend upon the ____.a. nature of the solute c. number of solute particles in a solutionb. nature of the solvent d. freezing point of a solute

____ 112. A solute depresses the freezing point because the solute ____.a. is colder than the solventb. disrupts crystal formation of the solventc. tends to sink to the bottom of the solutiond. has bigger molecules than the solvent

____ 113. The molality of a solution containing 8.1 moles of solute in 4847 g of solvent is ____.a. 39m c. 0.17mb. 1.7m d. 598m

____ 114. Which of the following is an expression of molality?a. c.

b. d.

____ 115. What is the mole fraction of ethanol in a solution of 3.00 moles of ethanol and 5.00 moles of water?a. 0.375 c. 1.67b. 0.6 d. 15

____ 116. What is the molality of a solution containing 8.0 grams of solute in 0.50 kg of solvent? (molar mass of solute = 24 g)a. 0.67m c. 1.67mb. 4m d. 0.17m

____ 117. What is the number of kilograms of solvent in a 0.70 molal solution containing 5.0 grams of solute? (molar mass of solute = 30 g)a. 0.24 kg c. 0.11 kgb. 2.4 kg d. 1.1 kg

____ 118. To which of the following variables is change in boiling point directly proportional?a. molarity of solution c. percent by volume of solutionb. molality of solution d. percent (mass/mass) of solution

____ 119. What is the freezing point of a solution of 0.5 mol of LiBr in 500 mL of water? (K = 1.86 C/m)a. –1.86 C c. –5.58 Cb. –3.72 C d. –7.44 C

____ 120. The freezing point of a solution that contains 0.550 moles of NaI in 615 g of water is ____. (K = 1.86 C/m; molar mass of water = 18 g)a. 1.66 C c. 3.33 Cb. –1.66 C d. –3.33 C

____ 121. What is the boiling point of a solution that contains 3 moles of KBr in 2000 g of water? (K = 0.512 C/m; molar mass of water = 18 g)a. 97 C c. 101.4 Cb. 99.7 C d. 103 C

____ 122. What is the molality of a solution of water and KCl if the freezing point of the solution is –3 C? (K = 1.86C/m; molar mass of water = 18 g)a. 0.6m c. 0.8mb. 1.2m d. 6m

____ 123. What is the boiling point of a solution of 0.1 mole of glucose in 200 mL of water? (K = 0.512 C/m)a. 100.06 C c. 100.26 Cb. 100.13 C d. 100.5 C

____ 124. What is the approximate molar mass of a molecular solute if 300 g of the solute in 1000 g of water causes the solution to have a boiling point of 101 C? (K = 0.512 C/m; K = 1.86 C/m; molar mass of water = 18 g)a. 15 amu c. 150 amub. 30 amu d. 300 amu

Short Answer

125. What is the angle between the bonds of a water molecule?

126. At what temperature does liquid water have its maximum density?

127. What is the percentage of water in the hydrate CoCl 6 ?

128. How many grams of copper sulfate pentahydrate (CuSO 5H O) would you heat to produce 29.8 g of water?

129. What mass of KCl (solubility = at 20 C) can dissolve in 3.30 10 g of water?

130. If the solubility of a gas is 7.5 g/L at 404 kPa pressure, what is the solubility of the gas when the pressure is 202 kPa?

131. How many liters of a 0.30M solution are needed to give 2.7 moles of solute?

132. What is the molarity of a solution containing 9.0 moles of solute in 2500 mL of solution?

133. What is the molarity of a solution containing 1.2 grams of solute in 450 mL of solution? (molar mass of solute = 24 g)

134. What is the number of moles of solute in 650 mL of a 0.40M solution?

135. How many liters of a 1.5M solution are required to yield 5.0 grams of solute? (molar mass of solute = 30.0 g)

136. If 1.0 mL of 6.0M HCl is added to 499 mL of water to give exactly a 500-mL solution, what is the molarity of the dilute solution?

137. If the volume of solute is 6.0 mL and the volume of solution is 300.0 mL, what is the solute's percent by volume?

138. What is the molality of a solution containing 5.0 moles of solute in 3.2 kg of solvent?

139. What is the molality of a solution containing 15 grams of solute in 0.50 kilograms of solvent? (molar mass of solute = 24 g)

140. Calculate the molality of a solution prepared by dissolving 175 g of KNO in 750 g of water.

141. What is the number of moles of solute in a 0.3 molal solution containing 0.10 kg of solvent?

142. How many kilograms of solvent are in a sample of 0.30 molal solution if the sample contains 13 moles of solute?

143. What is the mole fraction of KCl in a 0.20 molal solution of KCl? (molar mass of KCl = 75 g; molar mass of water = 18 g)

144. What is the freezing point of a solution that has 5.0 moles of NaI in 1250 g of water? (K = 1.86 C/m; molar mass of water = 18.0 g)

Numeric Response

145. How many hydrogen bonds can be formed between one hydrogen atom in a water molecule and oxygen atoms of surrounding water molecules?

146. How many nonbonding pairs of electrons are in a water molecule?

147. How many water molecules are in 39 formula units of calcium chloride dihydrate (CaCl2 2H2O)?

148. How many phases are present in a colloid?

Essay

149. What does a surfactant do? Include an example of a surfactant in your discussion.

150. Describe the structure of the water molecule and indicate how this structure is responsible for many of the unique properties of this vital compound.

151. Why is ice less dense than liquid water?

152. Define the terms solute, solvent, and aqueous solution. Provide an example of each.

153. Describe the process of solvation.

154. What is an electrolyte? Give examples and distinguish between a strong electrolyte and a weak electrolyte.

155. Distinguish among a suspension, a colloid, and a solution. Give an example of each.

156. Explain what a saturated solution is. Give a specific example.

157. Discuss the phenomenon of supersaturation. Indicate how crystallization can be initiated in a supersaturated solution.

158. Discuss the different factors that can affect the solubility of a substance. Include specific examples in your discussion.

159. Explain on a particle basis how the addition of a solute affects the boiling point, the freezing point, and the vapor pressure of the solvent.

160. Compare and contrast molarity and molality.

Solutions Test PreviewAnswer Section

MATCHING

1. ANS: G DIF: L1 REF: p. 447 OBJ: 15.1.1STO: SC.A.1.4.2

2. ANS: D DIF: L1 REF: p. 450 OBJ: 15.2.1STO: SC.A.1.4.4

3. ANS: C DIF: L1 REF: p. 450 OBJ: 15.2.1STO: SC.A.1.4.4

4. ANS: A DIF: L1 REF: p. 451 OBJ: 15.2.2STO: SC.A.1.4.4

5. ANS: E DIF: L1 REF: p. 452 OBJ: 15.2.3STO: SC.A.1.4.4

6. ANS: B DIF: L1 REF: p. 453 OBJ: 15.2.3STO: SC.A.1.4.4

7. ANS: F DIF: L1 REF: p. 460 OBJ: 15.3.2STO: SC.A.1.4.4

8. ANS: B DIF: L1 REF: p. 447 OBJ: 15.1.1STO: SC.A.1.4.2

9. ANS: G DIF: L1 REF: p. 450 OBJ: 15.2.1STO: SC.A.1.4.4

10. ANS: F DIF: L1 REF: p. 459 OBJ: 15.3.111. ANS: A DIF: L1 REF: p. 460 OBJ: 15.3.212. ANS: E DIF: L1 REF: p. 461 OBJ: 15.3.213. ANS: C DIF: L1 REF: p. 461 OBJ: 15.3.214. ANS: H DIF: L1 REF: p. 462 OBJ: 15.3.2

15. ANS: B DIF: L1 REF: p. 473 OBJ: 16.1.216. ANS: C DIF: L1 REF: p. 473 OBJ: 16.1.317. ANS: D DIF: L1 REF: p. 474 OBJ: 16.1.318. ANS: A DIF: L1 REF: p. 476 OBJ: 16.1.319. ANS: E DIF: L1 REF: p. 480, p. 481

OBJ: 16.2.1

20. ANS: D DIF: L1 REF: p. 481, p. 482OBJ: 16.2.1

21. ANS: E DIF: L1 REF: p. 488, p. 489OBJ: 16.3.1

22. ANS: A DIF: L1 REF: p. 487, p. 490OBJ: 16.3.1

23. ANS: B DIF: L1 REF: p. 491 OBJ: 16.4.124. ANS: C DIF: L1 REF: p. 492 OBJ: 16.4.1

MULTIPLE CHOICE

25. ANS: C DIF: L1 REF: p. 447 OBJ: 15.1.1STO: SC.A.1.4.2

26. ANS: C DIF: L1 REF: p. 447 OBJ: 15.1.1STO: SC.A.1.4.2

27. ANS: D DIF: L2 REF: p. 446 OBJ: 15.1.1STO: SC.A.1.4.2

28. ANS: B DIF: L2 REF: p. 446 OBJ: 15.1.1STO: SC.A.1.4.2

29. ANS: C DIF: L2 REF: p. 446 OBJ: 15.1.1STO: SC.A.2.4.5

30. ANS: A DIF: L2 REF: p. 446 OBJ: 15.1.1STO: SC.A.1.4.2

31. ANS: B DIF: L2 REF: p. 446, p. 447OBJ: 15.1.1 STO: SC.A.1.4.2

32. ANS: A DIF: L2 REF: p. 447 OBJ: 15.1.1STO: SC.A.1.4.2

33. ANS: A DIF: L2 REF: p. 447 OBJ: 15.1.1STO: SC.A.1.4.2

34. ANS: D DIF: L3 REF: p. 446 OBJ: 15.1.1STO: SC.A.1.4.5

35. ANS: C DIF: L1 REF: p. 449 OBJ: 15.1.2STO: SC.A.1.4.3

36. ANS: D DIF: L2 REF: p. 448, p. 449OBJ: 15.1.2 STO: SC.A.1.4.2

37. ANS: C DIF: L3 REF: p. 449 OBJ: 15.1.2STO: SC.A.1.4.3

38. ANS: A DIF: L1 REF: p. 450 OBJ: 15.2.1STO: SC.A.1.4.4

39. ANS: C DIF: L2 REF: p. 450 OBJ: 15.2.1STO: SC.A.1.4.4

40. ANS: A DIF: L2 REF: p. 451 OBJ: 15.2.2STO: SC.A.1.4.4

41. ANS: B DIF: L2 REF: p. 451 OBJ: 15.2.2STO: SC.A.1.4.4

42. ANS: A DIF: L2 REF: p. 451 OBJ: 15.2.2STO: SC.A.1.4.4

43. ANS: B DIF: L3 REF: p. 450 OBJ: 15.2.2STO: SC.A.1.4.4

44. ANS: C DIF: L3 REF: p. 451 OBJ: 15.2.2STO: SC.A.1.4.4

45. ANS: A DIF: L3 REF: p. 451 OBJ: 15.2.2STO: SC.A.1.4.4

46. ANS: B DIF: L3 REF: p. 451 OBJ: 15.2.2STO: SC.A.1.4.4

47. ANS: C DIF: L3 REF: p. 451, p. 453OBJ: 15.2.2 STO: SC.A.1.4.4

48. ANS: C DIF: L1 REF: p. 452 OBJ: 15.2.3STO: SC.A.1.4.5

49. ANS: C DIF: L1 REF: p. 452, p. 453OBJ: 15.2.3

50. ANS: D DIF: L2 REF: p. 452 OBJ: 15.2.351. ANS: D DIF: L2 REF: p. 452 OBJ: 15.2.352. ANS: D DIF: L2 REF: p. 453 OBJ: 15.2.3

53. ANS: D DIF: L2 REF: p. 453 OBJ: 15.2.354. ANS: A DIF: L2 REF: p. 453 OBJ: 15.2.355. ANS: D DIF: L2 REF: p. 453 OBJ: 15.2.356. ANS: D DIF: L2 REF: p. 452, p. 453

OBJ: 15.2.357. ANS: B DIF: L3 REF: p. 452, p. 453

OBJ: 15.2.358. ANS: C DIF: L1 REF: p. 455 OBJ: 15.2.4

STO: SC.A.1.4.459. ANS: D DIF: L1 REF: p. 454 OBJ: 15.2.4

STO: SC.A.1.4.460. ANS: B DIF: L2 REF: p. 454 OBJ: 15.2.4

STO: SC.A.1.4.461. ANS: C DIF: L2 REF: p. 454 OBJ: 15.2.4

STO: SC.A.1.4.462. ANS: D DIF: L2 REF: p. 455 OBJ: 15.2.4

STO: SC.A.1.4.463. ANS: C DIF: L2 REF: p. 455 OBJ: 15.2.4

STO: SC.A.1.4.464. ANS: B DIF: L1 REF: p. 459 OBJ: 15.3.1

STO: SC.A.1.4.465. ANS: A DIF: L1 REF: p. 459, p. 460

OBJ: 15.3.1, 15.3.2 STO: SC.A.1.4.466. ANS: B DIF: L1 REF: p. 460 OBJ: 15.3.267. ANS: D DIF: L1 REF: p. 460 OBJ: 15.3.268. ANS: B DIF: L1 REF: p. 462 OBJ: 15.3.269. ANS: B DIF: L2 REF: p. 459, p. 460

OBJ: 15.3.270. ANS: C DIF: L2 REF: p. 460 OBJ: 15.3.271. ANS: A DIF: L2 REF: p. 461 OBJ: 15.3.1, 15.3.272. ANS: A DIF: L2 REF: p. 450, p. 459, p. 460, p. 461

OBJ: 15.3.1, 15.3.273. ANS: B DIF: L2 REF: p. 462 OBJ: 15.3.274. ANS: D DIF: L2 REF: p. 462 OBJ: 15.3.275. ANS: A DIF: L3 REF: p. 461 OBJ: 15.3.276. ANS: A DIF: L2 REF: p. 471, p. 472

OBJ: 16.1.177. ANS: C DIF: L2 REF: p. 473 OBJ: 16.1.278. ANS: D DIF: L2 REF: p. 473 OBJ: 16.1.279. ANS: A DIF: L2 REF: p. 473 OBJ: 16.1.280. ANS: A DIF: L2 REF: p. 473, p. 474

OBJ: 16.1.381. ANS: D DIF: L2 REF: p. 474 OBJ: 16.1.382. ANS: A DIF: L2 REF: p. 475 OBJ: 16.1.383. ANS: B DIF: L2 REF: p. 474 OBJ: 16.1.384. ANS: B DIF: L2 REF: p. 476 OBJ: 16.1.385. ANS: D DIF: L3 REF: p. 474 OBJ: 16.1.386. ANS: A DIF: L1 REF: p. 476, p. 477

OBJ: 16.1.487. ANS: D DIF: L2 REF: p. 476, p. 477

OBJ: 16.1.488. ANS: A DIF: L3 REF: p. 476, p. 477

OBJ: 16.1.489. ANS: B DIF: L1 REF: p. 480 OBJ: 16.2.190. ANS: D DIF: L1 REF: p. 481 OBJ: 16.2.191. ANS: D DIF: L1 REF: p. 480, p. 481

OBJ: 16.2.192. ANS: B DIF: L2 REF: p. 480 OBJ: 16.2.193. ANS: C DIF: L2 REF: p. 480, p. 481

OBJ: 16.2.194. ANS: B DIF: L2 REF: p. 481 OBJ: 16.2.195. ANS: A DIF: L2 REF: p. 480, p. 482

OBJ: 16.2.196. ANS: B DIF: L3 REF: p. 481 OBJ: 16.2.197. ANS: A DIF: L3 REF: p. 481, p. 482

OBJ: 16.2.198. ANS: D DIF: L3 REF: p. 481, p. 482

OBJ: 16.2.199. ANS: C DIF: L1 REF: p. 483 OBJ: 16.2.2

100. ANS: B DIF: L2 REF: p. 483, p. 484OBJ: 16.2.2

101. ANS: D DIF: L2 REF: p. 483, p. 484OBJ: 16.2.2

102. ANS: A DIF: L2 REF: p. 483, p. 484OBJ: 16.2.2

103. ANS: D DIF: L3 REF: p. 483, p. 484OBJ: 16.2.2

104. ANS: C DIF: L1 REF: p. 485 OBJ: 16.2.3105. ANS: A DIF: L1 REF: p. 485 OBJ: 16.2.3106. ANS: A DIF: L1 REF: p. 486 OBJ: 16.2.3107. ANS: C DIF: L2 REF: p. 485 OBJ: 16.2.3108. ANS: D DIF: L2 REF: p. 485 OBJ: 16.2.3109. ANS: B DIF: L2 REF: p. 485 OBJ: 16.2.3110. ANS: B DIF: L1 REF: p. 487 OBJ: 16.3.1111. ANS: C DIF: L2 REF: p. 487, p. 488

OBJ: 16.3.1112. ANS: B DIF: L2 REF: p. 488 OBJ: 16.3.2113. ANS: B DIF: L1 REF: p. 491 OBJ: 16.4.1114. ANS: A DIF: L1 REF: p. 491 OBJ: 16.4.1115. ANS: A DIF: L1 REF: p. 492 OBJ: 16.4.1116. ANS: A DIF: L2 REF: p. 491 OBJ: 16.4.1117. ANS: A DIF: L3 REF: p. 491, p. 492

OBJ: 16.4.1118. ANS: B DIF: L1 REF: p. 494 OBJ: 16.4.2119. ANS: B DIF: L2 REF: p. 494, p. 495

OBJ: 16.4.1, 16.4.2120. ANS: D DIF: L2 REF: p. 495 OBJ: 16.4.2121. ANS: C DIF: L3 REF: p. 494, p. 496

OBJ: 16.4.2122. ANS: C DIF: L3 REF: p. 494, p. 495

OBJ: 16.4.2123. ANS: C DIF: L3 REF: p. 495, p. 496

OBJ: 16.4.2124. ANS: C DIF: L3 REF: p. 491, p. 494, p. 496

OBJ: 16.4.2

SHORT ANSWER

125. ANS:105

DIF: L2 REF: p. 446 OBJ: 15.1.1126. ANS:

4 C

DIF: L2 REF: p. 448 OBJ: 15.1.2 STO: SC.A.1.4.3127. ANS:

Molar mass CoCl 6H O = 237.9 g

percentage of water = 100% = 45%

DIF: L2 REF: p. 456 OBJ: 15.2.4 STO: SC.A.1.4.4128. ANS:

29.8 g = 1.66 mol molar mass 5 = 249.6 g mol CuSO 5H O 5 mol

1.66 mol H O = 82.6 g CuSO 5H O

DIF: L3 REF: p. 454, p. 456 OBJ: 15.2.4STO: SC.A.1.4.4

129. ANS:

DIF: L2 REF: p. 473 OBJ: 16.1.2130. ANS:

S = = = 3.8 g/L

DIF: L2 REF: p. 476, p. 477 OBJ: 16.1.4

131. ANS:

2.7 mol = 9.0 L

DIF: L1 REF: p. 480 OBJ: 16.2.1132. ANS:

DIF: L2 REF: p. 480, p. 481 OBJ: 16.2.1133. ANS:

DIF: L2 REF: p. 480, p. 481 OBJ: 16.2.1134. ANS:

DIF: L2 REF: p. 480, p. 482 OBJ: 16.2.1135. ANS:

DIF: L3 REF: p. 480, p. 481 OBJ: 16.2.1136. ANS:

DIF: L2 REF: p. 483, p. 484 OBJ: 16.2.2137. ANS:

% = 2.0%

DIF: L1 REF: p. 485 OBJ: 16.2.3138. ANS:

DIF: L1 REF: p. 491 OBJ: 16.4.1139. ANS:

DIF: L2 REF: p. 491, p. 492 OBJ: 16.4.1140. ANS:

molar mass KNO : K: 1 39.1 g = 39.1 g N: 1 14.0 g = 14.0 g O: 3 16.0 g = 48.0 g molar mass = 101.1 g

DIF: L2 REF: p. 491, p. 492 OBJ: 16.4.1141. ANS:

Number of moles = mass of solvent molality

DIF: L2 REF: p. 491, p. 492 OBJ: 16.4.1142. ANS:

DIF: L2 REF: p. 492 OBJ: 16.4.1143. ANS:

DIF: L2 REF: p. 492, p. 493 OBJ: 16.4.1144. ANS:

= 15

DIF: L3 REF: p. 494, p. 495, p. 496 OBJ: 16.4.2

NUMERIC RESPONSE

145. ANS:1

DIF: L1 REF: p. 446 OBJ: 15.1.1 STO: SC.A.1.4.2146. ANS:

2

DIF: L3 REF: p. 446 OBJ: 15.1.1 STO: SC.A.1.4.5147. ANS:

78

DIF: L3 REF: p. 454 OBJ: 15.2.4148. ANS:

2

DIF: L2 REF: p. 460 OBJ: 15.3.2

ESSAY

149. ANS:Surfactants are surface active agents used to decrease surface tension. Detergents and soaps are examples of surfactants. When added to beads of water on a greasy surface, for example, the detergent molecules interfere with the hydrogen bonding between water molecules and cause the water to spread out.

DIF: L2 REF: p. 447 OBJ: 15.1.1150. ANS:

Water is a simple triatomic molecule. Each O—H covalent bond in the water molecule is polar. Because of its greater electronegativity, the oxygen atom attracts the electron pair of the covalent O—H bond and acquires a partial negative charge. The hydrogen atoms, being less electronegative than the oxygen, acquire a partial positive charge. The atoms of the water molecule are joined at a 105 angle. As a result, the partial charges on the individual atoms do not cancel one another and the molecule is polar. Because water molecules are polar, they attract one another. The hydrogen of one molecule is attracted to the oxygen of another molecule. This attraction is termed hydrogen bonding and it is stronger than other polar attractions.

DIF: L3 REF: p. 446, p. 447 OBJ: 15.1.1151. ANS:

The structure of ice is a regular, open framework in which water molecules are farther apart from each other than they are in liquid water. When ice melts, this open framework collapses and the water molecules move closer together. As a result, liquid water is denser than ice.

DIF: L2 REF: p. 449 OBJ: 15.1.2 STO: SC.A.1.4.2152. ANS:

A solute is the dissolved material in a solution. A solvent is the dissolving medium in a solution. An aqueous solution is any sample of water that contains one or more dissolved substances. Aqueous solutions are homogeneous mixtures. Sodium chloride (NaCl) in water is an example of an aqueous solution. In this solution, water is the solvent and sodium chloride is the solute.

DIF: L2 REF: p. 450 OBJ: 15.2.1153. ANS:

The process by which the positive and negative ions of an ionic solid become surrounded by solvent molecules is called solvation. For example, polar water molecules attract solute ions in solutions of ionic salts. This causes the solute particles to separate from the bulk of the solute.

DIF: L3 REF: p. 451 OBJ: 15.2.2 STO: SC.A.1.4.4154. ANS:

An electrolyte is any substance that will conduct an electric current in aqueous solution or in the molten state. Strong electrolytes are substances that are completely, or almost completely, ionized in water. Examples of strong electrolytes are sodium chloride and sodium hydroxide. Weak electrolytes are substances that are only slightly dissociated in water. Examples of weak electrolytes are mercury(II) chloride and ammonia.

DIF: L3 REF: p. 452, p. 453 OBJ: 15.2.3155. ANS:

Suspensions are heterogeneous mixtures out of which some particles will settle upon standing. Particles in a typical suspension have an average diameter greater than 1000 nm. Suspensions exhibit the Tyndall effect, which is the scattering of light in all directions by the particles in the suspension. An example of a suspension is a sand-water mixture. Colloids are mixtures containing particles that are intermediate in size between the particles in suspensions and the particles in solutions. The range in particle diameter of a colloid is between 1 nm and 1000 nm. Colloids exhibit the Tyndall effect. An example of a colloid is gelatin. A solution is a homogeneous mixture. The particles in a solution have an average diameter of 1 nm or less. Solutions do not exhibit the Tyndall effect. An example of a solution is an oil-gasoline mixture.

DIF: L2 REF: p. 450, p. 459, p. 460, p. 461 OBJ: 15.3.1, 15.3.2156. ANS:

A saturated solution contains the maximum amount of solute for a given amount of solvent at a constant temperature. For example, no more than 36.2 g of sodium chloride will dissolve in 100 g of water. In a saturated solution, a dynamic equilibrium exists between the solid and its dissolved ions. In this equilibrium, as many ions are going out of the solution as are going in per unit time.

DIF: L2 REF: p. 472, p. 473 OBJ: 16.1.2157. ANS:

A solution that contains more solute than it can theoretically hold at a given temperature is a supersaturated solution. Crystallization can be initiated by adding a seed crystal to the solution or by exposing the solution to a rough surface. The latter can be done by scratching the inside of the container holding the solution.

DIF: L2 REF: p. 474, p. 475 OBJ: 16.1.3158. ANS:

The factors are temperature, pressure, and the nature of the solute and solvent. Specific examples include the following. Potassium nitrate is more soluble in water at high temperature than at low temperature. Gases are less soluble at high temperatures than at low temperatures. The solubility of a particular gas increases as the partial pressure of that gas above the solution increases. Sodium nitrate is much more soluble in water than is barium sulfate, regardless of temperature, because the attractive forces between the ions in BaSO are stronger than the attractive force of the solvent molecules.

DIF: L3 REF: p. 474, p. 475 OBJ: 16.1.3159. ANS:

Boiling point elevation, freezing point lowering, and vapor pressure lowering are colligative properties. They depend on the number of particles in solution and not on the chemical nature of the solute. Boiling point elevation: Additional attractive forces exist between solute and solvent; they must be overcome for the solution to boil. Kinetic energy must be added to overcome these forces. Freezing point lowering: More kinetic energy must be withdrawn from a solution because the solute particles are surrounded by shells of solvent molecules. These shells interfere with the formation of the orderly pattern that the particles assume as the solvent changes from liquid to solid. Vapor pressure lowering: The formation of solvent shells around the solute particles reduces the number of solvent particles that have sufficient kinetic energy to vaporize.

DIF: L3 REF: p. 487, p. 488, p. 490 OBJ: 16.3.2160. ANS:

Molarity is a quantitative measure of the concentration of a solution. It is defined as the number of moles of solute present in 1 L of solution. Molality is also a quantitative measure of the concentration of a solution. It is defined as the number of moles of solute present in 1 kg of solvent. Molarity is a ratio of moles of solute to 1 L of solution. Molality is a ratio of moles of solute to 1kg of solvent.

Molarity: ; Molality:

DIF: L2 REF: p. 480, p. 491 OBJ: 16.2.1, 16.4.1