testbank to accompany gob chemistry, 3e - el paso ... 8... · web viewgeneral, organic, and...
TRANSCRIPT
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This set includes all problems but you can focus only on the following numbers; 10-14, 22-24, 26-36, 50-57 and 64-65. The exam will come from those problems.
General, Organic, and Biological Chemistry, 3e (Timberlake) Chapter 8
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Solutions8.1
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Multiple-Choice Questions1)
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The O-H bond in water is polar because A)
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it is an ionic bond. B)
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oxygen is much more electronegative than hydrogen. C)
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oxygen occupies more space than hydrogen. D)
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hydrogen is much more electronegative than oxygen. E)
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it is a hydrogen bond.
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2)
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A hydrogen bond is A)
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an attraction between a hydrogen atom attached to N, O, or F and an N, O, or F atom. B)
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a covalent bond between H and O. C)
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an ionic bond between H and another atom. D)
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a bond that is stronger than a covalent bond. E)
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the polar O-H bond in water.
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3)
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Hydrogen bonds are a major factor in the structure of A)
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DNA. B)
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hydrogen chloride. C)
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dry ice. D)
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air. E)
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table salt.
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4)
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In a liquid, the strength of the intermolecular interactions is considered A)
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very weak. B)
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weak. C)
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moderate. D)
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strong. E)
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very strong.
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5)
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In a solution, the solvent A)
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is a liquid. B)
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can be a liquid or gas. C)
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can be a solid, liquid, or gas. D)
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is never a solid. E)
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is the substance present in the smallest concentration.
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6)
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In water, the melting point is unusually high because of A)
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covalent bonds in the individual molecules. B)
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ionic bonds in the individual molecules. C)
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hydrogen bonding between the molecules. D)
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dispersion forces between the molecules. E)
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the heat content of the hydrogen-oxygen bonds.
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7)
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Which of the following molecules can form hydrogen bonds? A)
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CH4B)
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NaH C)
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NH3D)
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BH3E)
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HI
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8)
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Water has a boiling point of 100 °C, and alcohol has a boiling point of 78 °C, even though water is a smaller molecule. This large difference in boiling point is due to
A)
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weak dispersion forces in the alcohol molecules. B)
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ionic bonds between the water molecules. C)
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covalent bonds in the ethanol molecules. D)
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stronger hydrogen bonds between the water molecules. E)
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stronger hydrogen bonds between the alcohol molecules.
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9)
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A solution is prepared by dissolving 2 g of KCl in 100 g of H2O. In this solution, H2O is the A)
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solute. B)
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solvent. C)
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solution. D)
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solid. E)
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ionic compound.
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10)
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Oil does not dissolve in water because A)
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oil is polar. B)
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oil is nonpolar. C)
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water is nonpolar. D)
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water is saturated. E)
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oil is hydrated.
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11)
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When KCl dissolves in water A)
74
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the Cl- ions are attracted to dissolved K+ ions. B)
75
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the Cl- ions are attracted to the partially negative oxygen atoms of the water molecule. C)
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the K+ ions are attracted to Cl- ions on the KCl crystal. D)
77
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the K+ ions are attracted to the partially negative oxygen atoms of the water molecule. E)
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the K+ ions are attracted to the partially positive hydrogen atoms of the water molecule.
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80
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12)
81
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Water is a polar solvent and hexane (C6H14) is a nonpolar solvent. Which of the following correctly describes the solubility of the solute?
A)
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mineral oil, soluble in water B)
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CaCl2, soluble in hexane C)
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HaHCO3, soluble in water D)
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CCl4, soluble in water E)
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octane, soluble in water
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13)
88
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In water, a substance that ionizes completely in solution is called a A)
89
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weak electrolyte. B)
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nonelectrolyte. C)
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semiconductor. D)
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nonconductor. E)
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strong electrolyte.
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14)
95
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In water, a substance that partially ionizes in solution is called a A)
96
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weak electrolyte. B)
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nonelectrolyte. C)
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semiconductor. D)
99
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nonconductor. E)
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strong electrolyte.
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15)
102
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An equivalent is A)
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the amount of ion that has a 1+ charge. B)
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the amount of ion that has a 1- charge. C)
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the amount of ion that carries 1 mole of electrical charge. D)
106
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1 mole of any ion. E)
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1 mole of an ionic compound.
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16)
109
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How many equivalents are present in 5.0 g of Al3+? A)
110
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15 Eq B)
111
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0.56 Eq C)
112
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0.19 Eq D)
113
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0.37 Eq E)
114
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3 Eq
115
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17)
116
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How many equivalents are present in 5.0 moles of Al3+? A)
117
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15 Eq B)
118
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1.3 Eq C)
119
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5.0 Eq D)
120
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0.67 Eq E)
121
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3.0 Eq
122
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123
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18)
124
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An intravenous replacement solution contains 4.0 mEq/L of Ca2+ ions. How many grams of Ca2+ are in 3.0 L of the solution?
A)
125
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0.24 g B)
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0.80 g C)
127
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0.40 g D)
128
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240 g E)
129
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4.0 g
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19)
131
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When some of the sugar added to iced tea remains undissolved at the bottom of the glass, the solution is
A)
132
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dilute. B)
133
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polar. C)
134
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nonpolar. D)
135
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saturated. E)
136
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unsaturated.
137
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20)
138
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The solubility of KI is 50 g in 100 g of H2O at 20 °C. If 110 grams of KI are added to 200 grams of H2O,
A)
139
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all of the KI will dissolve. B)
140
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the solution will freeze. C)
141
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the solution will start boiling. D)
142
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a saturated solution will form. E)
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the solution will be unsaturated.
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21)
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An increase in the temperature of a solution usually A)
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increases the boiling point. B)
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increases the solubility of a gas in the solution. C)
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increases the solubility of a solid solute in the solution. D)
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decreases the solubility of a solid solute in the solution. E)
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decreases the solubility of a liquid solute in the solution.
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22)
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Which one of the following compounds will NOT be soluble in water? A)
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NaOH B)
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PbS C)
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K2SO4 D)
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LiNO3E)
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MgCl2
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23)
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Which one of the following compounds will NOT be soluble in water? A)
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LiOH B)
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K2S C)
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BaSO4 D)
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NaNO3 E)
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MgCl2
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24)
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Which one of the following compounds will be soluble in water? A)
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AgCl B)
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Cu(OH)2 C)
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LiCl D)
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CaSO4 E)
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PbCO3
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25)
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Which one of the following compounds will be soluble in water? A)
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AgBr B)
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Cu(OH)2C)
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NaH4Cl D)
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CaCO3 E)
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PbS
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26)
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When solutions of KCl and Pb(NO3)2 are mixed, a precipitate forms. Which of the following is the balanced equation for the double replacement reaction that occurs?
A)
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KCl(aq) + Pb(NO3)2 (aq) → KNO3 (aq) + PbCl2 (s) B)
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KNO3 (aq) + PbCl2 (s) → KCl(aq) + Pb(NO3)2 (aq) C)
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K+ (aq) + NO3-(aq) → KNO3 (aq) D)
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2KCl (aq) + Pb(NO3)2 (aq) → 2 KNO3 (aq) + PbCl2 (s) E)
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KCl(aq) + Pb(NO3)2 (aq) → KNO3 (aq) + PbCl(s)
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27)
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When solutions of NaCl and AgNO3 are mixed, A)
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a precipitate of AgCl forms. B)
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a precipitate of NaNO3 forms. C)
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no precipitate forms. D)
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precipitate of NaNO3 and AgCl form. E)
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a precipitate of AgCl2 forms.
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28)
194
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The mass/mass percent concentration refers to A)
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grams of solute in 1 kg of solvent. B)
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grams of solute in 1 kg of solution. C)
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grams of solute in 100 g of solvent. D)
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grams of solute in 100 g of solution. E)
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grams of solvent in 100 g of solution.
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29)
201
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The mass/volume percent concentration refers to A)
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grams of solute in 1 L of solvent. B)
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grams of solute in 1 L of solution. C)
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grams of solute in 100 mL of solvent. D)
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grams of solute in 100 mL of solution. E)
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grams of solvent in 100 mL of solution.
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30)
208
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What is the concentration, in m/m%, of a solution prepared from 50.0 g NaCl and 150.0 g of water?
A)
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0.250% B)
210
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33.3% C)
211
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40.0% D)
212
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25.0% E)
213
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3.00%
214
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31)
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Rubbing alcohol is 70.% isopropyl alcohol by volume. How many mL of isopropyl alcohol are in a 1 pint (473 mL) container?
A)
216
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70. mL B)
217
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0.15 mL C)
218
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680 mL D)
219
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470 mL E)
220
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330 mL
221
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32)
222
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What is the concentration, in m/v%, of a solution prepared from 50. g NaCl and 2.5 L of water?
A)
223
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5.0% B)
224
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2.0% C)
225
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0.020% D)
226
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0.050% E)
227
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20.%
228
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33)
229
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How many grams of glucose are needed to prepare 400. mL of a 2.0%(m/v) glucose solution?
A)
230
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800. g B)
231
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0.0050 g C)
232
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8.0 g D)
233
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2.0 g E)
234
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200. g
235
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34)
236
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A patient needs to receive 85 grams of glucose every 12 hours. What volume of a 5.0%(m/v) glucose solution needs to be administered to the patient each 12 hours?
A)
237
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1700 mL B)
238
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60 mL C)
239
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6000 mL D)
240
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17 mL E)
241
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204 mL
242
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35)
243
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What volume (mL) of a 15% (m/v) NaOH solution contains 120 g NaOH? A)
244
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18 mL B)
245
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0.13 mL C)
246
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13 mL D)
247
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120 mL E)
248
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8.0 x 102 mL
249
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36)
250
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How many milliliters of a 25% (m/v) NaOH solution would contain 75 g of NaOH? A)
251
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25 mL B)
252
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75 mL C)
253
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33 mL D)
254
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19 mL E)
255
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3.0 x 102 mL
256
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37)
257
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A(n) __________ is a type of colloid in which a liquid is dispersed in another liquid or a solid. A)
258
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suspension B)
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aerosol C)
260
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foam D)
261
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sol E)
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emulsion
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38)
264
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A homogeneous mixture that does not settle out upon standing is A)
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an element. B)
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a colloid. C)
267
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a suspension. D)
268
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homogeneous. E)
269
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hydrated.
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39)
271
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In the process known as osmosis, __________ moves through a semipermeable membrane into an area of __________ concentration.
A)
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solute; lower solute B)
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solute; higher solute C)
274
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solvent; lower solute D)
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solvent; lower solvent E)
276
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solvent; higher solvent
277
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For the question(s) that follow, consider a 4% starch solution and a 10% starch solution separated by a semipermeable membrane.
40)
278
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Which starch solution will decrease in volume as osmosis occurs? A)
279
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4% B)
280
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10% C)
281
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Neither exerts osmotic pressure. D)
282
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They exert equal osmotic pressures. E)
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They exert opposite osmotic pressures.
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41)
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The process that occurs in this system is A)
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filtration. B)
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hydration. C)
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neutralization. D)
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dialysis. E)
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osmosis.
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42)
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Which of the following also occurs in this system? A)
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Water flows equally in both directions. B)
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There is a net flow of water from the 4% starch solution into the 10% starch solution. C)
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There is a net flow of water from the 10% starch solution into the 4% starch solution. D)
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Water does not cross the membrane at all. E)
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Starch moves out of the 10% starch solution into the 4% starch solution.
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43)
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A solution with the same osmotic pressure as the blood is A)
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isotonic to the blood. B)
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hypotonic to the blood. C)
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hypertonic to the blood. D)
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nontonic to the blood. E)
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molar to the blood.
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44)
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A solution that has an osmotic pressure less than that of red blood cells is called A)
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saturated. B)
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hypertonic. C)
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isotonic. D)
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hypotonic. E)
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unsaturated.
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45)
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A red blood cell will undergo crenation in A)
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water. B)
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0.5% NaCl. C)
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3% glucose. D)
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5% glucose. E)
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7% NaCl.
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46)
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Which solution is isotonic to a red blood cell? A)
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water B)
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0.5% NaCl C)
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2% glucose D)
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0.9% NaCl E)
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10% glucose
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47)
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A red blood cell will undergo hemolysis in A)
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water. B)
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0.9% NaCl. C)
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5% glucose. D)
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5% NaCl. E)
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10% glucose.
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48)
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The process by which a semipermeable membrane allows water molecules, small molecules, and ions to pass through while retaining large particles is called
A)
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osmotic pressure. B)
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dialysis. C)
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solvation. D)
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dilution. E)
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hydration.
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49)
342
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An aqueous mixture containing starch (a colloid), NaCl, glucose, and albumin (a colloid) is placed in a dialyzing bag and immersed in distilled water. Which of the following correctly describes the location of the indicated substance after dialysis?
A)
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albumin, inside B)
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starch outside C)
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albumin inside and outside D)
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water inside only E)
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starch inside and outside
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50)
349
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What is the molarity of a solution that contains 17 g of NH3 in 0.50 L of solution? A)
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34 M B)
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2.0 M C)
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0.50 M D)
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0.029 M E)
354
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1.0 M
355
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51)
356
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What is the molarity of a solution that contains 3.25 moles of NaNO3 in 250. mL of solution?
A)
357
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3.25 M B)
358
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6.50 M C)
359
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0.0130 M D)
360
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13.0 M E)
361
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2.60 M
362
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52)
363
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When 200. mL of water are added to 100. mL of 12% KCl solution the final concentration of KCl is (Assume the volumes add.)
A)
364
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12%. B)
365
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4.0%. C)
366
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36%. D)
367
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6.0%. E)
368
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8.0%.
369
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53)
370
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The molarity (M) of a solution refers to A)
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moles of solute/L of solution. B)
372
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moles of solute/L of solvent. C)
373
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moles of solute/100 mL of solution. D)
374
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grams of solute/100 mL of solution. E)
375
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grams of solute/L of solution.
376
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54)
377
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What is the molarity of a solution containing 5.0 moles of KCl in 2.0 L of solution? A)
378
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2.5 M B)
379
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1.0 M C)
380
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5.0 M D)
381
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10. M E)
382
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2.0 M
383
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55)
384
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What is the molarity of a solution which contains 58.5 g of sodium chloride dissolved in 0.500 L of solution?
A)
385
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0.500 M B)
386
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1.00 M C)
387
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1.50 M D)
388
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2.00 M E)
389
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4.00 M
390
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56)
391
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How many moles of CaCl2 are in 250 mL of a 3.0 M of CaCl2 solution? A)
392
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750 moles B)
393
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1.3 moles C)
394
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83 moles D)
395
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0.75 mole E)
396
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3.0 moles
397
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57)
398
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What volume of a 1.5 M KOH solution is needed to provide 3.0 moles of KOH? A)
399
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3.0 L B)
400
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0.50 L C)
401
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2.0 L D)
402
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4.5 L E)
403
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0.22 L
404
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58)
405
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During the process of diluting a solution to a lower concentration, A)
406
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the amount of solute does not change. B)
407
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the amount of solvent does not change. C)
408
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there is more solute in the concentrated solution. D)
409
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the volume of the solution does not change. E)
410
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water is removed from the concentrated solution.
411
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59)
412
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According to Henry's law, the solubility of a gas in a liquid A)
413
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decreases as the gas pressure above the liquid increases. B)
414
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increases as the gas pressure above the liquid increases. C)
415
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remains the same as the temperature increases. D)
416
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depends on the liquid polarity. E)
417
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depends on the liquid density.
418
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419
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60)
420
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What is the molarity of a KCl solution made by diluting 75.0 mL of a 0.200 M solution to a final volume of 100. mL?
A)
421
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0.267 M B)
422
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0.150 M C)
423
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0.200 M D)
424
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6.67 M E)
425
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0.100 M
426
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61)
427
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What volume of 2.5% (m/v) KOH can be prepared from 125 mL of a 5.0% KOH solution? A)
428
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0.0040 mL B)
429
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63 mL C)
430
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0.10 mL D)
431
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125 mL E)
432
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250 mL
433
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62)
434
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What volume of 0.10 M NaOH can be prepared from 250. mL of 0.30 M NaOH? A)
435
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0.075 L B)
436
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0.25 L C)
437
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0.75 L D)
438
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0.083 L E)
439
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750 L
440
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63)
441
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What volume of a 2.00 M KCl solution is required to prepare 500. mL of a 0.100 M KCl solution?
A)
442
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0.0400 mL B)
443
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25.0 mL C)
444
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2.00 mL D)
445
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1.00 x mL E)
446
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5.00 x mL
447
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64)
448
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What is the new mass/volume (m/v)% of a KOH solution that is prepared by diluting 110 mL of a 6% (m/v) KOH solution to 330 mL?
A)
449
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2% B)
450
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1% C)
451
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6% D)
452
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12% E)
453
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18%
454
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65)
455
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Use the reaction: 2AgNO3(aq) + H2SO4(aq) → Ag2SO4(s) + 2H2O(l)What volume of 0.123 M AgNO3(aq) is needed to form 0.657 g of Ag2SO4(s)?
A)
456
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34.2 L B)
457
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17.1 mL C)
458
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34.2 mL D)
459
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10.7 mL E)
460
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53.4 mL
461
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8.2
462
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Bimodal Questions1)
463
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Acetic acid can be classified as a __________. A)
464
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gas B)
465
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solid C)
466
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weak electrolyte D)
467
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strong electrolyte E)
468
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ionic compound
469
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2)
470
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NaCl can be classified as a __________. A)
471
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gas B)
472
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liquid C)
473
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weak electrolyte D)
474
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strong electrolyte E)
475
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nonelectrolyte
476
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3)
477
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Methanol, CH3OH, can be classified as a __________. A)
478
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gas B)
479
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solid C)
480
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weak electrolyte D)
481
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strong electrolyte E)
482
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nonelectrolyte
483
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4)
484
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Using a kidney machine to remove waste products from the blood is known as __________. A)
485
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osmosis B)
486
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osmolysis C)
487
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autolysis D)
488
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hemolysis E)
489
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hemodialysis
490
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5)
491
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A mixture in which one component settles is called a(n) __________. A)
492
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solution B)
493
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colloid C)
494
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suspension D)
495
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electrolyte E)
496
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nonelectrolyte
497
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6)
498
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The molarity of a solution of 5.0 g of KCl in 100. mL of solution is __________. A)
499
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0.038 M B)
500
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0.067 M C)
501
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0.67 M D)
502
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0.13 M E)
503
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1.3 M
504
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505
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7)
506
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If 100. mL of water is added to 25 mL of 5.0 M NaCl, the final concentration is __________. A)
507
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25 M B)
508
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1.0 M C)
509
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5.0 M D)
510
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2.0 M E)
511
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1.3 M Answer :
512
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B
8.3
513
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Short Answer Questions1)
514
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Is barium sulfate, BaSO4, soluble or insoluble in water? Answer :
515
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insoluble
2)
516
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In the following equation, __________ will precipitate out of water solution.
NaCl + AgNO3 → AgCl + NaNO3
517
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3)
518
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In the following equation, __________ will precipitate from solution.
BaCl2 + H2SO4 → BaSO4 + 2HCl
519
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4)
520
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The number of moles of a compound dissolved in one liter of a solution is called the __________.
521
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5)
522
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A substance that carries an electric current when dissolved in water is called a(n) __________.
523
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6)
524
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A substance that produces only a small number of ions in solution is known as a __________ electrolyte.
525
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7)
526
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A solution of sodium carbonate, Na2CO3, that has a molarity of 0.0100 M contains __________ equivalents of carbonate per liter of the solution.
527
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8)
528
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A solution of sodium carbonate, Na2CO3, that has a molarity of 0.0100 M contains __________ equivalents of sodium ions per liter of the solution.
529
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9)
530
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Substances whose particles in solution scatter light and pass through filters but cannot pass through semipermeable membranes are called __________.
531
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532
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8.4
533
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Matching QuestionsIdentify the term defined in each description.
1)
534
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a solution that contains the highest amount of solute that dissolves at a given temperature
535
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A)
536
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hydration B)
537
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saturated
C)
538
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unsaturated 2)
539
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the major attraction between water molecules
540
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D)
541
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hydrogen bonding
3)
542
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the association of several water molecules with ions produced in a solution
543
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E)
544
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hypertonic F)
545
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hypotonic
4)
546
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a solution in which more solute can be dissolved
5)
547
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a solution that has a higher osmotic pressure than the red blood cells of the body
548
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549
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550
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551
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552
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553
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554
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555
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556
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Match the type of mixture with the appropriate characteristics.
6)
557
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a mixture of sodium chloride in water
558
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A)
559
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colloid B)
560
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suspension 7)
561
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a mixture whose particles settle on standing
562
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C)
563
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solution
8)
564
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a homogeneous mixture in which suspended particles cannot pass through a semipermeable membrane
9)
565
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a mixture whose particles cannot be separated by filters or semipermeable membranes
10)
566
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a mixture whose particles can be separated by filters
567
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568
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Compare the osmotic pressure of these solutions to the osmotic pressure of red blood cells.
11)
577
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water
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A)
579
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hypotonic
12)
580
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0.5% NaCl
581
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B)
582
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isotonic
13)
583
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7% glucose
584
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C)
585
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hypertonic
14)
586
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5% glucose
15)
587
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0.9% NaCl
588
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589
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590
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591
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592
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593
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594
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595
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596
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Indicate whether each of the following compounds dissolves in water to give ions, molecules, or both.
16)
597
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NaCl, a strong electrolyte
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A)
599
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both
17)
600
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HI, a weak electrolyte
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B)
602
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ions
18)
603
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CH3CH3OH, a nonelectrolyte
604
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C)
605
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molecules
19)
606
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KNO3, a strong electrolyte
20)
607
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glucose, a nonelectrolyte
21)
608
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H2CO3, a weak electrolyte
609
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610
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611
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612
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613
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614
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615
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616
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617
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619
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620