Chapter 13—Solutions
MULTIPLE CHOICE
2. Sugar in water is an example of which solute-solvent combination?
a. gas-liquid
c. solid-liquid
b. liquid-liquid
d. liquid-solid
ANS: C
PTS: 1
DIF: II
OBJ: 13-1.2
3. A substance whose water solution conducts a current is a(n)
a. nonelectrolyte.
c. nonpolar substance.
b. electrolyte.
d. solute.
ANS: B
PTS: 1
DIF: I
OBJ: 13-1.4
4. To conduct electricity, a solution must contain
a. nonpolar molecules.
c. ions.
b. polar molecules.
d. free electrons.
ANS: C
PTS: 1
DIF: I
OBJ: 13-1.4
7. Which of the following will dissolve most rapidly?
a. sugar cubes in cold water
c. powdered sugar in cold water
b. sugar cubes in hot water
d. powdered sugar in hot water
ANS: D
PTS: 1
DIF: I
8. The rule like dissolves like is used to predict
a. solubility.
b. equilibrium.
ANS: A
PTS: 1
OBJ: 13-2.1
c. reactivity.
d. phase.
DIF: I
OBJ: 13-2.3
9. Which of the following is an example of a polar solvent?
a. carbon tetrachloride
c. water
b. benzene
d. gasoline
ANS: C
PTS: 1
DIF: II
OBJ: 13-2.3
12. What is the molality of a solution that contains 5.10 mol KNO3 in 4.47 kg water?
a. 0.315 m
c. 1.02 m
b. 0.779 m
d. 1.14 m
ANS: D
PTS: 1
DIF: III
OBJ: 13-3.1
13. The concentration of a water solution of NaCl is 2.48 m, and it contains 806 g of water. How much
NaCl is in the solution?
a. 2.00 g
c. 117 g
b. 89.3 g
d. 224 g
ANS: C
PTS: 1
DIF: III
OBJ: 13-3.2
Chapter 14—Ions in Aqueous Solutions and Colligative Properties
MULTIPLE CHOICE
2. How many moles of ions are produced by the dissociation of 1 mol of MgCl2?
a. 0
c. 2 mol
b. 1 mol
d. 3 mol
ANS: D
PTS: 1
DIF: II
OBJ: 14-1.1
3. How many moles of ions are produced by the dissociation of 1 mol of Al2(CO3)3?
a. 2 mol
c. 5 mol
b. 4 mol
d. 11 mol
ANS: C
PTS: 1
DIF: II
OBJ: 14-1.1
5. Which of the following is the right side of the equation for dissolving K2S(s)?
a. 2K+(aq) + S2–(aq)
c. K2+(aq) + S2–(aq)
2+
2–
b. K2 (aq) + S (aq)
d. 2K(aq) + S(aq)
ANS: A
PTS: 1
DIF: II
OBJ: 14-1.1
6. Which compound dissociates to produce the ions Ca2+(aq) and NO3–(aq)?
a. CaNO3(s)
c. Ca(NO3)2(s)
b. Ca2NO3
d. Ca2(NO3)3
ANS: C
PTS: 1
DIF: II
OBJ: 14-1.1
7. When solutions of two ionic compounds are combined and a solid forms, the process is called
a. hydration.
c. solvation.
b. precipitation.
d. dissociation.
ANS: B
PTS: 1
DIF: I
OBJ: 14-1.2
General Solubility Guidelines--Use Your Solubility Chart
1. Most sodium, potassium, and ammonium
compounds are soluble in water.
2. Most nitrates, acetates, and chlorates are soluble.
3. Most chlorides are soluble, except those of silver,
mercury(I), and lead. Lead(II) chloride is soluble in
hot water.
4. Most sulfates are soluble, except those of barium,
strontium, and lead.
5. Most carbonates, phosphates, and silicates are
insoluble, except those of sodium, potassium, and
ammonium.
6. Most sulfides are insoluble, except those of calcium,
strontium, sodium, potassium, and ammonium.
9. Which of the following pairs of solutions produce a precipitate when combined?
a. Cu(NO3)2 and NaCl
c. Cu(NO3)2 and K2CO3
b. Fe(NO3)3 and MgCl2
d. CaCl2 and NaNO3
ANS: C
PTS: 1
DIF: II
OBJ: 14-1.2
10. When solutions of NH4OH and K2SO4 are combined, what precipitate(s) forms?
a. (NH4)2SO4
c. (NH4)2SO4 and KOH
b. KOH
d. none of the above
ANS: D
PTS: 1
DIF: II
OBJ: 14-1.2
11. What is the spectator ion in the equation Cu2+(aq) + Zn2+(aq) + 2S2–(aq)
a. Cu2+(aq)
c. S2–(aq)
2+
b. Zn (aq)
d. none of the above
ANS: D
PTS: 1
DIF: II
CuS(s) + ZnS(s)?
OBJ: 14-1.2
Chapter 8—Chemical Equations and Reactions
MULTIPLE CHOICE
1. A solid produced by a chemical reaction in solution that separates from the solution is called
a. a precipitate.
c. a molecule.
b. a reactant.
d. the mass of the product.
ANS: A
PTS: 1
DIF: I
OBJ: 8-1.1
5. To balance a chemical equation, it may be necessary to adjust the
a. coefficients.
c. formulas of the products.
b. subscripts.
d. number of products.
ANS: A
PTS: 1
DIF: I
OBJ: 8-1.2
6. In an equation, the symbol for a substance in water solution is followed by
a. (1).
c. (aq).
b. (g).
d. (s).
ANS: C
PTS: 1
7. When the equation Fe3O4 + Al
a. 3
b. 4
ANS: D
PTS: 1
DIF: I
OBJ: 8-1.3
Al2O3 + Fe is correctly balanced, what is the coefficient of Fe?
c. 6
d. 9
DIF: III
OBJ: 8-1.4
8. Which coefficients correctly balance the formula equation NH4NO2(s)
a. 1, 2, 2
c. 2, 1, 1
b. 1, 1, 2
d. 2, 2, 2
ANS: B
PTS: 1
DIF: III
N2(g) + H2O(l)?
OBJ: 8-1.4
11. The equation AX A + X is the general equation for a
a. synthesis reaction.
c. combustion reaction.
b. decomposition reaction.
d. single-replacement reaction.
ANS: B
PTS: 1
DIF: II
OBJ: 8-2.1
12. The equation AX + BY AY + BX is the general equation for a
a. synthesis reaction.
c. single-replacement reaction.
b. decomposition reaction.
d. double-replacement reaction.
ANS: D
PTS: 1
DIF: II
OBJ: 8-2.1
13. The equation A + X AX is the general equation for a(n)
a. combustion reaction.
c. synthesis reaction.
b. ionic reaction.
d. double-replacement reaction.
ANS: C
PTS: 1
DIF: II
OBJ: 8-2.1
14. The equation A + BX AX + B is the general equation for a
a. double-replacement reaction.
c. single-replacement reaction.
b. decomposition reaction.
d. combustion reaction.
ANS: C
PTS: 1
15. The reaction 2Mg(s) + O2(g)
a. synthesis reaction.
b. decomposition reaction.
ANS: A
DIF: II
2MgO(s) is a
PTS: 1
16. In the equation 2Al(s) + 3Fe(NO3)2(aq)
a. nitrate.
b. water.
ANS: C
PTS: 1
OBJ: 8-2.1
c. single-replacement reaction.
d. double-replacement reaction.
DIF: II
OBJ: 8-2.2
3Fe(s) + 2Al(NO3)3(aq), iron has been replaced by
c. aluminum.
d. nitrogen.
DIF: II
OBJ: 8-2.4
18. What is the balanced equation when aluminum reacts with copper(II) sulfate?
a. Al + Cu2S Al2S + Cu
c. Al + CuSO4 AlSO4 + Cu
b. 2Al + 3CuSO4 Al2(SO4)3 + 3Cu
d. 2Al + Cu2SO4 Al2SO4 + 2Cu
ANS: B
PTS: 1
DIF: III
OBJ: 8-2.5
Chapter 9—Stoichiometry
MULTIPLE CHOICE
4. In the reaction N2 + 3H2
a. 1:1
b. 1:2
ANS: B
5. In the reaction 2Al2O3
a. 10:6
b. 3:4
ANS: D
2NH3, what is the mole ratio of nitrogen to ammonia?
c. 1:3
d. 2:3
PTS: 1
DIF: III
OBJ: 9-1.3
4Al + 3O2, what is the mole ratio of aluminum to oxygen?
c. 2:3
d. 4:3
PTS: 1
DIF: III
OBJ: 9-1.3
6. In the reaction C + 2H2
a. 1:1
b. 2:1
ANS: B
PTS: 1
7. In the reaction N2 + 3H2
a. 1:1
b. 2:1
ANS: C
ANS: B
OBJ: 9-1.3
DIF: III
OBJ: 9-1.3
2H2O, how many grams of water are produced from 6.00 mol of
c. 54.0 g
d. 108 g
PTS: 1
11. For the reaction 2Fe + O2
iron?
a. 71.8 g
b. 574 g
DIF: III
2NH3, what is the mole ratio of hydrogen to ammonia?
c. 3:2
d. 6:8
PTS: 1
10. For the reaction 2H2 + O2
hydrogen?
a. 2.00 g
b. 6.00 g
ANS: D
CH4, what is the mole ratio of hydrogen to methane?
c. 1:2
d. 2:4
DIF: III
OBJ: 9-2.2
2FeO, how many grams of iron oxide are produced from 8.00 mol of
PTS: 1
c. 712 g
d. 1310 g
DIF: III
OBJ: 9-2.2
14. For the reaction 2Na + 2H2O 2NaOH + H2, how many grams of hydrogen are produced if 120. g of
sodium and 80. g of water are available?
a. 4.5 g
c. 80. g
b. 44 g
d. 200. g
ANS: A
PTS: 1
DIF: III
OBJ: 9-2.4
15. For the reaction Mg + 2HCl H2 + MgCl2, calculate the percent yield of magnesium chloride if 100.
g of magnesium react with excess hydrochloric acid to yield 330. g of magnesium chloride.
a. 71.8%
c. 81.6%
b. 74.3%
d. 84.2%
ANS: D
PTS: 1
DIF: III
OBJ: 9-3.4
16. When the limiting reactant in a chemical reaction is completely used, the
a. excess reactants begin combining.
c. reaction speeds up.
b. reaction slows down.
d. reaction stops.
ANS: D
PTS: 1
DIF: I
OBJ: 9-3.1