Solutions Test Preview
Matching
Match each item with the correct statement below.
a. solvation
e. electrolyte
b. weak electrolyte
f. colloid
c. aqueous solution
g. surfactant
d. solvent
____
____
____
____
____
____
____
1.
2.
3.
4.
5.
6.
7.
interferes with hydrogen bonding between water molecules
dissolving medium
homogeneous mixture of water and dissolved substances
Solute ions or molecules are surrounded by solvent molecules.
compound that will conduct current in the liquid state or in aqueous solution
compound that ionizes incompletely in aqueous solution
mixture in which particle size averages between 1 nm and 1000 nm
Match each item with the correct statement below.
a. dispersed phase
e.
b. surface tension
f.
c. Brownian motion
g.
d. dispersion medium
h.
____
____
____
____
____
____
____
8.
9.
10.
11.
12.
13.
14.
Tyndall effect
suspension
solute
emulsion
inward force tending to minimize surface area of a liquid
dissolved particle
mixture in which particle size averages greater that 1000 nm in diameter
Colloidal particles spread throughout a suspension.
phenomenon observed when beam of light passes through a colloid
chaotic movement of colloidal particles
colloid of a liquid in a liquid
Match each item with the correct statement below.
a. Henry's law
d. supersaturated solution
b. immiscible
e. concentration
c. saturated solution
____
____
____
____
15.
16.
17.
18.
describes liquids that are insoluble in one another
solution containing maximum amount of solute
solution containing more solute than can theoretically dissolve at a given temperature
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. molarity
b. molality
e. freezing point depression
c. 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 Choice
Identify 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 bonding
b. covalent bonding
d. ionic attractions
____ 27. What is the shape of the water molecule?
a. linear
c. trigonal planar
b. 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 bonds
b. hydrogen bonds
d. polar covalent bonds
____ 29. Which atom in a water molecule has the greatest electronegativity?
a. one of the hydrogen atoms
b. both hydrogen atoms
c. the oxygen atom
d. 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 bonds
b. ionic bonds
d. polar covalent bonds
____ 31. What is primarily responsible for the surface tension of water?
a. dispersion forces
c. ionic attractions
b. 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 liquid
b. may be increased by detergents
c. is decreased by hydrogen bonding
d. 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 bonds
b. 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 water
____ 37.
____ 38.
____ 39.
____ 40.
____ 41.
____ 42.
____ 43.
____ 44.
b. the molecules of ice are held to each other by covalent bonding
c. ice has a molecular structure in which water molecules are arranged randomly
d. ice has a molecular structure that is an open framework held together by hydrogen bonds
Which is responsible for the high thermal energy required to melt ice?
a. covalent bonding
c. hydrogen bonding
b. dispersion forces
d. ionic attractions
What is the term for the dissolving medium in a solution?
a. solvent
c. solvator
b. solute
d. emulsifier
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.
Which of the following substances is the most soluble in water?
a. sodium chloride
c. bromine
b. methane
d. carbon
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.
Which of the following substances dissolves most readily in gasoline?
a. CH
c. NH
b. HCl
d. NaBr
A solution is a mixture ____.
a. from which the solute can be filtered
b. that has the same properties throughout
c. that is heterogeneous
d. in which a solid solute is always dissolved in a liquid solvent
Predict which one of the following compounds would be insoluble in water.
a. NaCl
c. CF
b. 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. NaCl
b. CI
d. SnS
____ 47. Which of the following substances dissolves most readily in water?
a. BaSO
c. NH
b. CaCO
d. CH
____ 48. What type of compound is always an electrolyte?
a. polar covalent
c. ionic
b. nonpolar covalent
d. network solid
____ 49. An electric current can be conducted by ____.
a. methane gas
c. a salt solution
____ 50.
____ 51.
____ 52.
____ 53.
____ 54.
____ 55.
b. a sugar solution
d. rubbing alcohol
Which of the following compounds conducts electricity only in the molten state?
a. sodium bromide
c. calcium hydroxide
b. magnesium sulfate
d. barium sulfate
Which of the following compounds is a nonelectrolyte?
a. sodium bromide
c. copper chloride
b. magnesium sulfate
d. carbon tetrachloride
Which of the following compounds is an electrolyte?
a. rubbing alcohol
c. carbon tetrachloride
b. sugar
d. sodium hydroxide
Which of the following compounds is a nonelectrolyte when pure, but an electrolyte when dissolved in water?
a. rubbing alcohol
c. carbon tetrachloride
b. sugar
d. ammonia
Which of the following are weak electrolytes in water?
a. ionic compounds that partially dissociate in water
b. ionic compounds that are soluble
c. polar compounds that ionize
d. nonpolar compounds that do not ionize
Which of the following compounds is a weak electrolyte?
a. NaBr
c. KOH
b. HBr
d. NH
____ 56. Which of the following compounds is a strong electrolyte?
a. ammonia
c. sugar
b. acetic acid
d. potassium sulfate
____ 57. Which of the following substances is NOT an electrolyte?
a. KCl
c. LiCl
b. CCl
d.
____ 58. Which of the following is NOT a common hydrate?
a. Epsom salt
c. sugar
b. 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 symbol
b. an asterisk
d. a dot
____ 60. What is another term for the water of hydration?
a. water of solvation
c. water of sublimation
b. water of crystallization
d. water of efflorescence
____ 61. Which compound changes color when it becomes a hydrate?
a. silicon dioxide
c. copper(II) sulfate
b. 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. hygroscopic
b. deliquescent
d. efflorescent
____ 63. A crystal that absorbs water vapor from the air is ____.
a. aqueous
c. hygroscopic
b. deliquescent
d. efflorescent
____ 64. Which of the following mixture types is characterized by the settling of particles?
a. solution
c. colloid
b. suspension
d. hydrate
____ 65. Which of the following mixture types can be filtered to remove solute?
____ 66.
____ 67.
____ 68.
____ 69.
____ 70.
____ 71.
____ 72.
____ 73.
____ 74.
____ 75.
____ 76.
____ 77.
____ 78.
a. suspensions only
c. suspensions and colloids
b. colloids only
d. suspensions and solutions
Which of the following materials is NOT a colloid?
a. glue
c. smoke
b. alloy
d. muddy water
Which of the following mixtures is NOT a colloid?
a. fog
c. paint
b. milk
d. sugar water
An emulsion is which type of mixture?
a. suspension
c. solution
b. colloid
d. gaseous
The solute in a colloidal suspension is called the ____.
a. dissolving phase
c. dispensing phase
b. dispersed phase
d. dispersion medium
What is the size range of particles in a colloid?
a. more than 1000 nm
c. between 1 nm and 1000 nm
b. between 100 nm and 1000 nm
d. between 1 nm and 10 nm
Which of the following types of mixtures exhibit the Tyndall effect?
a. suspensions and colloids
c. colloids and solutions
b. suspensions and solutions
d. colloids only
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.
An emulsion is a colloidal dispersion of a ____.
a. solid in a liquid
c. gas in a liquid
b. liquid in a liquid
d. liquid in a gas
An emulsifying agent is typically characterized by having ____.
a. one polar end
c. two polar ends
b. one nonpolar end
d. one polar end and one nonpolar end
What causes Brownian motion in colloids?
a. molecules of the dispersion medium colliding with dispersed phase particles
b. coagulation of particles of the dispersed phase
c. erratic flashes of light
d. There is no Brownian motion in colloids.
Which of the following usually makes a substance dissolve faster in a solvent?
a. agitating the solution
b. increasing the particle size of the solute
c. lowering the temperature
d. decreasing the number of particles
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 g
b. 34 g
d. 6800 g
What is the solubility of silver nitrate if only 11.1 g can dissolve in 5.0 g of water at 20 C?
a.
c.
at 20 C
at 20 C
b.
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 solvent
b. grams of solute per 100 milliliters of solvent
c. grams of solute per 100 grams of solution
d. 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 solvent
b. temperature and degree of mixing
c. particle size and degree of mixing
d. 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 emulsion
b. saturated
d. supersaturated
____ 82. Which of the following substances is less soluble in hot water than in cold water?
a. CO
c. NaNO
b. 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 liquid
b. directly proportional to the pressure of the gas above the liquid
c. inversely proportional to the pressure of the gas above the liquid
d. 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.
c.
at 25 C
at 20 C
b.
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 atm
b. 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 atm
b. 1.3 atm
d. 12 atm
____ 89. In a concentrated solution there is ____.
a. no solvent
c. a small amount of solute
b. 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. 7M
b. 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 solution
b. 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. 12M
b. 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. 0.40M
b. 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 mol
b. 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. 2.1M
b. 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 g
b. 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 g
b. 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 solute
b. 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 mL
b. 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 mL
b. 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. 0.30M
b. 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. 0.35M
b. 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 mL
b. 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 g
b. 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 mL
b. 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 mL
b. 228 mL
d. 142 mL
____ 109. In which of the following is concentration expressed in percent by volume?
a.
c.
100%
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 lowering
b. supersaturation
d. freezing point depression
____ 111. Colligative properties depend upon the ____.
a. nature of the solute
c. number of solute particles in a solution
b. 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 solvent
b. disrupts crystal formation of the solvent
c. tends to sink to the bottom of the solution
d. 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. 0.17m
b. 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. 1.67
b. 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. 1.67m
b. 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 kg
b. 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 solution
b. 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 C
b. –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 C
b. –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 C
b. 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 = 1.86
C/m; molar mass of water = 18 g)
a. 0.6m
c. 0.8m
b. 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 C
b. 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 amu
b. 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
128. How many grams of copper sulfate pentahydrate (CuSO
water?
129. What mass of KCl (solubility =
6
?
5H O) would you heat to produce 29.8 g of
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 Preview
Answer Section
MATCHING
1. ANS:
STO:
2. ANS:
STO:
3. ANS:
STO:
4. ANS:
STO:
5. ANS:
STO:
6. ANS:
STO:
7. ANS:
STO:
G
SC.A.1.4.2
D
SC.A.1.4.4
C
SC.A.1.4.4
A
SC.A.1.4.4
E
SC.A.1.4.4
B
SC.A.1.4.4
F
SC.A.1.4.4
DIF: L1
REF: p. 447
OBJ: 15.1.1
DIF: L1
REF: p. 450
OBJ: 15.2.1
DIF: L1
REF: p. 450
OBJ: 15.2.1
DIF: L1
REF: p. 451
OBJ: 15.2.2
DIF: L1
REF: p. 452
OBJ: 15.2.3
DIF: L1
REF: p. 453
OBJ: 15.2.3
DIF: L1
REF: p. 460
OBJ: 15.3.2
8. ANS:
STO:
9. ANS:
STO:
10. ANS:
11. ANS:
12. ANS:
13. ANS:
14. ANS:
B
SC.A.1.4.2
G
SC.A.1.4.4
F
A
E
C
H
DIF: L1
REF: p. 447
OBJ: 15.1.1
DIF: L1
REF: p. 450
OBJ: 15.2.1
DIF:
DIF:
DIF:
DIF:
DIF:
L1
L1
L1
L1
L1
REF:
REF:
REF:
REF:
REF:
p. 459
p. 460
p. 461
p. 461
p. 462
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
15.3.1
15.3.2
15.3.2
15.3.2
15.3.2
15.
16.
17.
18.
19.
ANS:
ANS:
ANS:
ANS:
ANS:
OBJ:
B
C
D
A
E
16.2.1
DIF:
DIF:
DIF:
DIF:
DIF:
L1
L1
L1
L1
L1
REF:
REF:
REF:
REF:
REF:
p. 473
p. 473
p. 474
p. 476
p. 480, p. 481
OBJ:
OBJ:
OBJ:
OBJ:
16.1.2
16.1.3
16.1.3
16.1.3
20. ANS:
OBJ:
21. ANS:
OBJ:
22. ANS:
OBJ:
23. ANS:
24. ANS:
D
16.2.1
E
16.3.1
A
16.3.1
B
C
DIF: L1
REF: p. 481, p. 482
DIF: L1
REF: p. 488, p. 489
DIF: L1
REF: p. 487, p. 490
DIF: L1
DIF: L1
REF: p. 491
REF: p. 492
OBJ: 16.4.1
OBJ: 16.4.1
DIF: L1
REF: p. 447
OBJ: 15.1.1
MULTIPLE CHOICE
25. ANS: C
STO: SC.A.1.4.2
26. ANS:
STO:
27. ANS:
STO:
28. ANS:
STO:
29. ANS:
STO:
30. ANS:
STO:
31. ANS:
OBJ:
32. ANS:
STO:
33. ANS:
STO:
34. ANS:
STO:
35. ANS:
STO:
36. ANS:
OBJ:
37. ANS:
STO:
38. ANS:
STO:
39. ANS:
STO:
40. ANS:
STO:
41. ANS:
STO:
42. ANS:
STO:
43. ANS:
STO:
44. ANS:
STO:
45. ANS:
STO:
46. ANS:
STO:
47. ANS:
OBJ:
48. ANS:
STO:
49. ANS:
OBJ:
50. ANS:
51. ANS:
52. ANS:
C
SC.A.1.4.2
D
SC.A.1.4.2
B
SC.A.1.4.2
C
SC.A.2.4.5
A
SC.A.1.4.2
B
15.1.1
A
SC.A.1.4.2
A
SC.A.1.4.2
D
SC.A.1.4.5
C
SC.A.1.4.3
D
15.1.2
C
SC.A.1.4.3
A
SC.A.1.4.4
C
SC.A.1.4.4
A
SC.A.1.4.4
B
SC.A.1.4.4
A
SC.A.1.4.4
B
SC.A.1.4.4
C
SC.A.1.4.4
A
SC.A.1.4.4
B
SC.A.1.4.4
C
15.2.2
C
SC.A.1.4.5
C
15.2.3
D
D
D
DIF: L1
REF: p. 447
OBJ: 15.1.1
DIF: L2
REF: p. 446
OBJ: 15.1.1
DIF: L2
REF: p. 446
OBJ: 15.1.1
DIF: L2
REF: p. 446
OBJ: 15.1.1
DIF: L2
REF: p. 446
OBJ: 15.1.1
DIF: L2
STO: SC.A.1.4.2
DIF: L2
REF: p. 446, p. 447
REF: p. 447
OBJ: 15.1.1
DIF: L2
REF: p. 447
OBJ: 15.1.1
DIF: L3
REF: p. 446
OBJ: 15.1.1
DIF: L1
REF: p. 449
OBJ: 15.1.2
DIF: L2
STO: SC.A.1.4.2
DIF: L3
REF: p. 448, p. 449
REF: p. 449
OBJ: 15.1.2
DIF: L1
REF: p. 450
OBJ: 15.2.1
DIF: L2
REF: p. 450
OBJ: 15.2.1
DIF: L2
REF: p. 451
OBJ: 15.2.2
DIF: L2
REF: p. 451
OBJ: 15.2.2
DIF: L2
REF: p. 451
OBJ: 15.2.2
DIF: L3
REF: p. 450
OBJ: 15.2.2
DIF: L3
REF: p. 451
OBJ: 15.2.2
DIF: L3
REF: p. 451
OBJ: 15.2.2
DIF: L3
REF: p. 451
OBJ: 15.2.2
DIF: L3
STO: SC.A.1.4.4
DIF: L1
REF: p. 451, p. 453
DIF: L1
REF: p. 452, p. 453
DIF: L2
DIF: L2
DIF: L2
REF: p. 452
REF: p. 452
REF: p. 453
REF: p. 452
OBJ: 15.2.3
OBJ: 15.2.3
OBJ: 15.2.3
OBJ: 15.2.3
53.
54.
55.
56.
57.
58.
59.
60.
61.
62.
63.
64.
65.
66.
67.
68.
69.
70.
71.
72.
73.
74.
75.
76.
77.
78.
79.
80.
81.
82.
83.
84.
85.
86.
87.
ANS:
ANS:
ANS:
ANS:
OBJ:
ANS:
OBJ:
ANS:
STO:
ANS:
STO:
ANS:
STO:
ANS:
STO:
ANS:
STO:
ANS:
STO:
ANS:
STO:
ANS:
OBJ:
ANS:
ANS:
ANS:
ANS:
OBJ:
ANS:
ANS:
ANS:
OBJ:
ANS:
ANS:
ANS:
ANS:
OBJ:
ANS:
ANS:
ANS:
ANS:
OBJ:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
OBJ:
ANS:
D
A
D
D
15.2.3
B
15.2.3
C
SC.A.1.4.4
D
SC.A.1.4.4
B
SC.A.1.4.4
C
SC.A.1.4.4
D
SC.A.1.4.4
C
SC.A.1.4.4
B
SC.A.1.4.4
A
15.3.1, 15.3.2
B
D
B
B
15.3.2
C
A
A
15.3.1, 15.3.2
B
D
A
A
16.1.1
C
D
A
A
16.1.3
D
A
B
B
D
A
16.1.4
D
DIF:
DIF:
DIF:
DIF:
L2
L2
L2
L2
REF:
REF:
REF:
REF:
p. 453
OBJ: 15.2.3
p. 453
OBJ: 15.2.3
p. 453
OBJ: 15.2.3
p. 452, p. 453
DIF: L3
REF: p. 452, p. 453
DIF: L1
REF: p. 455
OBJ: 15.2.4
DIF: L1
REF: p. 454
OBJ: 15.2.4
DIF: L2
REF: p. 454
OBJ: 15.2.4
DIF: L2
REF: p. 454
OBJ: 15.2.4
DIF: L2
REF: p. 455
OBJ: 15.2.4
DIF: L2
REF: p. 455
OBJ: 15.2.4
DIF: L1
REF: p. 459
OBJ: 15.3.1
DIF: L1
REF:
STO:
REF:
REF:
REF:
REF:
DIF:
DIF:
DIF:
DIF:
L1
L1
L1
L2
p. 459, p. 460
SC.A.1.4.4
p. 460
OBJ: 15.3.2
p. 460
OBJ: 15.3.2
p. 462
OBJ: 15.3.2
p. 459, p. 460
DIF: L2
DIF: L2
DIF: L2
REF: p. 460
OBJ: 15.3.2
REF: p. 461
OBJ: 15.3.1, 15.3.2
REF: p. 450, p. 459, p. 460, p. 461
DIF:
DIF:
DIF:
DIF:
L2
L2
L3
L2
REF:
REF:
REF:
REF:
p. 462
OBJ: 15.3.2
p. 462
OBJ: 15.3.2
p. 461
OBJ: 15.3.2
p. 471, p. 472
DIF:
DIF:
DIF:
DIF:
L2
L2
L2
L2
REF:
REF:
REF:
REF:
p. 473
OBJ: 16.1.2
p. 473
OBJ: 16.1.2
p. 473
OBJ: 16.1.2
p. 473, p. 474
DIF:
DIF:
DIF:
DIF:
DIF:
DIF:
L2
L2
L2
L2
L3
L1
REF:
REF:
REF:
REF:
REF:
REF:
p. 474
p. 475
p. 474
p. 476
p. 474
p. 476, p. 477
DIF: L2
REF: p. 476, p. 477
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
16.1.3
16.1.3
16.1.3
16.1.3
16.1.3
88.
89.
90.
91.
92.
93.
94.
95.
96.
97.
98.
99.
100.
101.
102.
103.
104.
105.
106.
107.
108.
109.
110.
111.
112.
113.
114.
115.
116.
117.
118.
119.
120.
121.
122.
OBJ:
ANS:
OBJ:
ANS:
ANS:
ANS:
OBJ:
ANS:
ANS:
OBJ:
ANS:
ANS:
OBJ:
ANS:
ANS:
OBJ:
ANS:
OBJ:
ANS:
ANS:
OBJ:
ANS:
OBJ:
ANS:
OBJ:
ANS:
OBJ:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
OBJ:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
OBJ:
ANS:
ANS:
OBJ:
ANS:
ANS:
OBJ:
ANS:
16.1.4
A
16.1.4
B
D
D
16.2.1
B
C
16.2.1
B
A
16.2.1
B
A
16.2.1
D
16.2.1
C
B
16.2.2
D
16.2.2
A
16.2.2
D
16.2.2
C
A
A
C
D
B
B
C
16.3.1
B
B
A
A
A
A
16.4.1
B
B
16.4.1, 16.4.2
D
C
16.4.2
C
DIF: L3
REF: p. 476, p. 477
DIF: L1
DIF: L1
DIF: L1
REF: p. 480
OBJ: 16.2.1
REF: p. 481
OBJ: 16.2.1
REF: p. 480, p. 481
DIF: L2
DIF: L2
REF: p. 480
OBJ: 16.2.1
REF: p. 480, p. 481
DIF: L2
DIF: L2
REF: p. 481
OBJ: 16.2.1
REF: p. 480, p. 482
DIF: L3
DIF: L3
REF: p. 481
OBJ: 16.2.1
REF: p. 481, p. 482
DIF: L3
REF: p. 481, p. 482
DIF: L1
DIF: L2
REF: p. 483
OBJ: 16.2.2
REF: p. 483, p. 484
DIF: L2
REF: p. 483, p. 484
DIF: L2
REF: p. 483, p. 484
DIF: L3
REF: p. 483, p. 484
DIF:
DIF:
DIF:
DIF:
DIF:
DIF:
DIF:
DIF:
L1
L1
L1
L2
L2
L2
L1
L2
REF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
p. 485
p. 485
p. 486
p. 485
p. 485
p. 485
p. 487
p. 487, p. 488
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
16.2.3
16.2.3
16.2.3
16.2.3
16.2.3
16.2.3
16.3.1
DIF:
DIF:
DIF:
DIF:
DIF:
DIF:
L2
L1
L1
L1
L2
L3
REF:
REF:
REF:
REF:
REF:
REF:
p. 488
p. 491
p. 491
p. 492
p. 491
p. 491, p. 492
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
16.3.2
16.4.1
16.4.1
16.4.1
16.4.1
DIF: L1
DIF: L2
REF: p. 494
OBJ: 16.4.2
REF: p. 494, p. 495
DIF: L2
DIF: L3
REF: p. 495
OBJ: 16.4.2
REF: p. 494, p. 496
DIF: L3
REF: p. 494, p. 495
OBJ:
123. ANS:
OBJ:
124. ANS:
OBJ:
16.4.2
C
16.4.2
C
16.4.2
DIF: L3
REF: p. 495, p. 496
DIF: L3
REF: p. 491, p. 494, p. 496
DIF: L2
126. ANS:
4 C
REF: p. 446
OBJ: 15.1.1
DIF: L2
127. ANS:
Molar mass CoCl
REF: p. 448
OBJ: 15.1.2
SHORT ANSWER
125. ANS:
105
STO: SC.A.1.4.3
6H O = 237.9 g
percentage of water =
100% = 45%
DIF: L2
REF: p. 456
128. ANS:
29.8 g
= 1.66 mol
molar mass
5
= 249.6 g
mol CuSO
5H O
5 mol
OBJ: 15.2.4
STO: SC.A.1.4.4
1.66 mol H O = 82.6 g CuSO
DIF: L3
STO: SC.A.1.4.4
129. ANS:
REF: p. 454, p. 456
DIF: L2
130. ANS:
REF: p. 473
S
=
DIF: L2
131. ANS:
=
OBJ: 15.2.4
OBJ: 16.1.2
= 3.8 g/L
REF: p. 476, p. 477
OBJ: 16.1.4
5H O
2.7 mol
= 9.0 L
DIF: L1
132. ANS:
REF: p. 480
OBJ: 16.2.1
DIF: L2
133. ANS:
REF: p. 480, p. 481
OBJ: 16.2.1
DIF: L2
134. ANS:
REF: p. 480, p. 481
OBJ: 16.2.1
DIF: L2
135. ANS:
REF: p. 480, p. 482
OBJ: 16.2.1
DIF: L3
136. ANS:
REF: p. 480, p. 481
OBJ: 16.2.1
DIF: L2
137. ANS:
REF: p. 483, p. 484
OBJ: 16.2.2
% = 2.0%
DIF: L1
138. ANS:
REF: p. 485
OBJ: 16.2.3
DIF: L1
139. ANS:
REF: p. 491
OBJ: 16.4.1
DIF: L2
REF: p. 491, p. 492
140. ANS:
molar mass KNO :
K: 1 39.1 g = 39.1 g
OBJ: 16.4.1
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
141. ANS:
Number of moles = mass of solvent molality
OBJ: 16.4.1
DIF: L2
142. ANS:
REF: p. 491, p. 492
OBJ: 16.4.1
DIF: L2
143. ANS:
REF: p. 492
DIF: L2
144. ANS:
REF: p. 492, p. 493
OBJ: 16.4.1
REF: p. 494, p. 495, p. 496
OBJ: 16.4.2
DIF: L1
146. ANS:
2
REF: p. 446
OBJ: 15.1.1
STO: SC.A.1.4.2
DIF: L3
REF: p. 446
OBJ: 15.1.1
STO: SC.A.1.4.5
=
OBJ: 16.4.1
15
DIF: L3
NUMERIC RESPONSE
145. ANS:
1
147. ANS:
78
DIF: L3
148. ANS:
2
REF: p. 454
OBJ: 15.2.4
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: 15.1.1
150. 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: 15.1.1
151. 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.1.4.2
152. 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: 15.2.1
153. 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.1.4.4
154. 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: 15.2.3
155. 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, 15.3.2
156. 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: 16.1.2
157. 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: 16.1.3
158. 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: 16.1.3
159. 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: 16.3.2
160. 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