Chemistry, 7e (McMurry/Fay)
Chapter 4 Reactions in Aqueous Solutions
4.1 Multiple-Choice Questions
1) Molarity is defined as
A) moles of solute per liter of solution.
B) moles of solute per liter of solvent.
C) moles of solvent per liter of solution.
D) moles of solvent per liter of solvent.
2) What is the concentration of FeBr3 in a solution prepared by dissolving 10.0 g of FeBr3 in enough water
to make 275 mL of solution?
A) 1.23 × 10-4 M
B) 0.123 M
C) 1.23 M
D) 1.23 × 103 M
3) How many grams of KNO3 are needed to make 250. mL of a solution that is 0.135 M?
A) 1.71 g
B) 0.341 g
C) 3.41 g
D) 6.82 g
4) What volume of a 0.540 M KOH solution contains 15.5 g of KOH?
A) 0.54 L
B) 0.51 L
C) 1.95 L
D) 8.47 L
5) Which statement about diluted solutions is false? When a solution is diluted
A) the concentration of the solution decreases.
B) the molarity of the solution decreases.
C) the number of moles of solute remains unchanged.
D) the number of moles of solvent remains unchanged.
6) What is the concentration of HNO3 in the final solution when 70.0 mL of a 6.00 M HNO3 solution is
diluted with pure water to a total volume of 0.15 L?
A) 3.57 × 10-2 M
B) 2.80 M
C) 12.6 M
D) 1.75 M
7) How many milliliters of a 6.0 M HNO3 solution are needed to make 0.25 L of a 3.5 M HNO3 solution?
A) 686 mL
B) 428 mL
C) 146 mL
D) 119 mL
8) A student prepared a stock solution by dissolving 20.0 g of NaOH in enough water to make 150. mL of
solution. She then took 15.0 mL of the stock solution and diluted it with enough water to make 65.0 mL of
a final solution. What is the concentration of NaOH for the final solution?
A) 0.769 M
B) 0.548 M
C) 1.40 M
D) 1.82 M
9) What is the concentration of NO3– ions in a solution prepared by dissolving 15.0 g of Ba(NO3)2 in
enough water to produce 300. mL of solution?
A) 0.057 M
B) 0.191 M
C) 0.573M
D) 0.382 M
10) If the reaction of phosphate ion with water is ignored, what is the total concentration of ions in a
solution prepared by dissolving 3.00 g of Na3PO4 in enough water to make 350. mL of solution?
A) 0.0183 M
B) 0.209 M
C) 0.0523 M
D) 0.323 M
11) What is the concentration of an AlBr3 solution if 150. mL of the solution contains 250. mg of Br– ion?
A) 6.95 × 10-3 M
B) 2.08 × 10-2 M
C) 1.67 M
D) 6.23 × 10-3 M
12) A student dissolved 3.00 g of Ca(NO3)2 in enough water to make 100. mL of stock solution. He took
4.00 mL of the solution then diluted it with water to give 275 mL of a final solution. How many grams of
NO3– ion are there in the final solution?
A) 0.329 g
B) 0.00073 g
C) 0.0453 g
D) 0.0906 g
13) Identify the statement that is true about nonelectrolytes.
A) Nonelectrolytes dissolve in water to produce ions.
B) Nonelectrolytes do not dissociate in water.
C) Nonelectrolytes conduct electricity.
D) Most nonelectrolytes are ionic compounds.
14) Acetic acid (CH3CO2H), formic acid (HCO2H), hydrofluoric acid (HF), ammonia (NH3), and
methylamine (CH3NH2) are commonly classified as
A) acids.
B) nonelectrolytes.
C) strong electrolytes.
D) weak electrolytes.
15) Water (H2O), methyl alcohol (CH3OH), ethyl alcohol (CH3CH2OH), ethylene glycol
(HOCH2CH2OH), and sucrose (C12H22O11) are commonly classified as
A) bases.
B) nonelectrolytes.
C) strong electrolytes.
D) weak electrolytes.
5
16) In a solution prepared by mixing CH3OH with H2O the major species present are
A) CH3OH and H2O.
B) CH3OH, H+, and OH–.
C) CH3+, OH–, and H2O.
D) CH3O–, H+, and H2O.
17) What is the molar concentration of sodium ions in a 0.350 M Na3PO4 solution?
A) 0.117 M
B) 0.350 M
C) 1.05 M
D) 1.40 M
18) The reaction 2 HNO3(aq) + Ba(OH)2(aq) → Ba(NO3)2(aq) + 2 H2O(l) is best classified as a(n)
A) acid-base neutralization reaction.
B) oxidation-reduction reaction.
C) precipitation reaction.
D) single replacement reaction.
19) The reaction Na3PO4(aq) + 3 AgNO3(aq) → Ag3PO4(s) + 3 NaNO3(aq) is best classified as a(n)
A) acid-base neutralization reaction.
B) oxidation-reduction reaction.
C) precipitation reaction.
D) single replacement reaction.
20) The reaction C6H12O6(s) + 6 O2(g) → 6 CO2(g) + 6 H2O(l) is best classified as a(n)
A) acid-base neutralization reaction.
B) double replacement reaction.
C) oxidation-reduction reaction.
D) precipitation reaction.
21) The combustion reaction CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(l) can be classified as a(n)
A) acid-base neutralization reaction.
B) double replacement reaction.
C) oxidation-reduction reaction.
D) precipitation reaction.
22) Write a balanced net ionic equation for the reaction of Pb(NO3)2(aq) with NaI(aq).
A) Pb(NO3)2(aq) + 2 NaI(aq) → PbI2(s) + 2 NaNO3(aq)
B) Pb2+(aq) + 2 NO3–(aq) + 2 Na+(aq) + 2 I–(aq) → Pb2+(aq) + 2 I–(aq) + 2 Na+(aq) + 2 NO3–(aq)
C) Pb2+(aq) + 2 NO3–(aq) + 2 Na+(aq) + 2 I–(aq) → PbI2(s) + 2 Na+(aq) + 2 NO3–(aq)
D) Pb2+(aq) + 2 I–(aq) → PbI2(s)
23) Write a balanced net ionic equation for the reaction of H2SO4(aq) with Ba(OH)2(aq).
A) H2SO4(aq) + Ba(OH)2(aq) → BaSO4(s) + 2 H2O(l)
B) 2 H+(aq) + SO42-(aq) + Ba2+(aq) + 2 OH–(aq) → BaSO4(s) + 2 H2O(l)
C) H+(aq) + OH+(aq) → H2O(l)
D) Ba2+(aq) + SO42-(aq) → BaSO4(s)
24) Write a balanced net ionic equation for the reaction of AgNO3(aq) with Cu(s).
A) AgNO3(aq) + Cu(s) → Ag(s) + CuNO3(aq)
B) Ag+(aq) + Cu(s) → Ag(s) + Cu+(aq)
C) 2 AgNO3(aq) + Cu(s) → 2 Ag(s) + CuNO3(aq)
D) 2Ag+(aq) + Cu(s) → 2 Ag(s) + Cu2+(aq)
25) Write a balanced net ionic equation for the reaction of NiBr2(aq) with (NH4)2S(aq).
A) NiBr2(aq) + (NH4)2S(aq) → NiS(s) + 2 NH4Br(aq)
B) Ni2+(aq) + 2 Br–(aq) + 2 NH4+(aq) + S2-(aq) → NiS(s) + 2 NH4+(aq) + 2 Br–(aq)
C) Ni2+(aq) + 2 Br–(aq) + 2 NH4+(aq) + S2-(aq) → NiS(s) + 2 NH4Br(s)
D) Ni2+(aq) + S2-(aq) → NiS(s)
26) In the reaction AgNO3(aq) + HI(aq) → AgI(s) + HNO3(aq) the spectator ions are
A) Ag+ and NO3–.
B) Ag+ and I–.
C) H+ and I–.
D) H+ and NO3–.
27) Which one of the following compounds is insoluble in water?
A) NH4SO4
B) Ba(OH)2
C) Ca3(PO4)2
D) Rb2CO3
28) Which pair of compounds is insoluble in water?
A) AgNO3 and KNO3
B) Na2S and CuS
C) (NH4)2SO4 and AgI
D) PbSO4 and Pb3(PO4)2
29) Which one of the following compounds is soluble in water?
A) BaSO4
B) AgCl
C) Pb(ClO4)2
D) Ca(OH)2
30) Which pair of compounds is soluble in water?
A) AgCl and AgBr
B) CdS and (NH4)2S
C) KClO4 and Ba(ClO4)2
D) K2SO4 and BaSO4
31) Phthalic acid is a diprotic acid having the formula HO2CC6H4CO2H that can be converted to a salt
by reaction with base. Which of the following is expected to be most soluble in water?
A) HO2CC6H4CO2H
B) HO2CC6H4CO2Na
C) HO2CC6H4CO2K
D) NaO2CC6H4CO2Na
32) What reagent could be used to separate Br– from SO42- when added to an aqueous solution
containing both?
A) AgNO3(aq)
B) Ba(OH)2(aq)
C) CuSO4(aq)
D) NaI(aq)
33) What reagent could not be used to separate Cl– from S2– when added to an aqueous solution
containing both?
A) AgNO3(aq)
B) Ca(NO3)2(aq)
C) Cu(NO3)2(aq)
D) Fe(NO3)3(aq)
34) When K2SO4(aq) and Pb(NO3)2(aq) are mixed, a white colored precipitate forms which is
A) KNO3.
B) K2SO3.
C) Pb.
D) PbSO4.
35) When Na2CrO4(aq) and AgNO3(aq) are mixed, a red colored precipitate forms which is
A) Ag.
B) Ag2CrO4.
C) AgNO2.
D) NaNO3.
36) What reagent would distinguish between Ag+ and Fe3+?
A) NaClO3
B) NaI
C) NaNO3
D) NaOH
37) When 50.0 mL of a 1.00 M solution of Fe(NO3)3 are mixed with 50.0 mL of a 1.00 M solution of NaOH,
a precipitate forms. What is the identity of the precipitate?
Fe(NO3)3(aq) + 3 NaOH(aq) → Fe(OH)3(s) + 3 NaNO3(aq)
A) Fe(NO3)3
B) NaOH
C) Fe(OH)3
D) NaNO3
38) Which of the following compounds is not an Arrhenius acid?
A) HF
B) KOH
C) HClO
D) H2SO3
39) What ion is provided when Arrhenius bases dissolve in water?
A) H+
B) Na+
C) Cl–
D) OH–
40) When dissolved in water, LiOH behaves as
A) an acid that forms Li+ and OH– ions.
B) an acid that forms LiO– and H+ ions.
C) a base that forms Li+ and OH– ions.
D) a base that forms LiO– and H+ ions.
41) Which of the following compounds is an Arrhenius base in water?
A) C6H12O6
B) CH3COOH
C) KCl
D) NH2CH2CH2NH2
42) Which of the following compounds is an Arrhenius base in water?
A) CH3CH3
B) CH3SH
C) HOCl
D) KOH
43) Which one of the following compounds behaves as an acid when dissolved in water?
A) CH3OCH3
B) CH4
C) H2SO3
D) KOH
44) When dissolved in water, of HClO4, NH3, KOH, HI, and CH3OH which are acids?
A) NH3 and KOH
B) HClO4 and HI
C) only HI
D) only KOH
45) When dissolved in water, of HClO4, NH3, KOH, HI, and CH3OH which are bases?
A) NH3 and KOH
B) HClO4 and HI
C) only HI
D) NH3, KOH, and CH3OH
13
46) Which of the following is not a strong acid?
A) HF
B) HCl
C) HBr
D) HI
47) How many H+ ions can the acid, H2CO3, donate per molecule?
A) 0
B) 1
C) 2
D) 3
48) How many H+ ions can the acid H3PO4 donate per molecule?
A) 0
B) 1
C) 2
D) 3
49) How many H+ ions can the acid CH3CO2H donate per molecule?
A) 1
B) 2
C) 3
D) 4
50) Write a net ionic equation for the neutralization reaction of HCN(aq) with NaOH(aq).
A) HCN(aq) + NaOH(aq) → NaCN(aq) + H2O(l)
B) HCN(aq) + Na+(aq) + OH–(aq) → Na+(aq) + CN–(aq) + H2O(l)
C) HCN(aq) + OH–(aq) → CN–(aq) + H2O(l)
D) H+(aq) + OH–(aq) → H2O(l)
51) Write a net ionic equation for the neutralization reaction of CH3CO2H(aq) with CsOH(aq).
A) CH3CO2H(aq) + CsOH(aq) → CH3CO2Cs(aq) + H2O(l)
B) CH3CO2–(aq) + H+(aq) + Cs+(aq) + OH–(aq) → CH3CO2–(aq) + Cs+ + H2O(l)
C) CH3CO2H(aq) + Cs+(aq) + OH–(aq) → CH3CO2Cs(s) + H2O(l)
D) CH3CO2H(aq) + OH–(aq) → CH3CO2–(aq) + H2O(l)
52) Write a net ionic equation for the neutralization reaction of H3PO4(aq) with Ba(OH)2(aq).
A) 2 H3PO4(aq) + 3 Ba(OH)2(aq) → Ba3(PO4)2(s) + 6 H2O(l)
B) 2 H3PO4(aq) + 3 Ba2+(aq) + 6 OH–(aq) → Ba3(PO4)2(s) + 6 H2O(l)
C) 6 H+(aq) + 2 PO43–(aq) + 3 Ba2+(aq) + 6 OH–(aq) → Ba3(PO4)2(s) + 6 H2O(l)
D) H+(aq) + OH–(aq) → H2O(l)
53) The name of H2SO3 is
A) sulfurous acid.
B) sulfuric acid.
C) hydrosulfuric acid.
D) hydrosulfurous acid.
54) The chemical formula for nitric acid is
A) HNO2(aq).
B) HNO3(aq).
C) H2NO3(aq).
D) H2NO2(aq).
55) By analogy with the oxoacids of sulfur, H2TeO3 would be named
A) hydrotellurous acid.
B) pertelluric acid.
C) telluric acid.
D) tellurous acid.
56) How many milliliters of 0.300 M Li2S are needed to react with 25.00 mL of 0.315 M AgNO3?
Li2S(aq) + 2 AgNO3(aq) → 2 LiNO3(aq) + Ag2S(s)
A) 13.1 mL
B) 226.2 mL
C) 6.05 mL
D) 1.31 mL
57) How many grams of BaCl2 are formed when 35.00 mL of 0.00237 M Ba(OH)2 reacts with excess Cl2
gas?
2 Ba(OH)2(aq) + 2 Cl2(g) → Ba(OCl)2(aq) + BaCl2(s) + 2 H2O(l)
A) 0.00864 g
B) 0.0173 g
C) 0.0346 g
D) 0.0829 g
58) When 125 mL of 0.500 M AgNO3 is added to 100. mL of 0.500 M NH4Cl, how many grams of AgCl
are formed?
AgNO3(aq) + NH4Cl(aq) → AgCl(s) + NH4NO3(aq)
A) 7.17 g
B) 8.96 g
C) 13.3 g
D) 25.8 g
59) How many milliliters of 0.100 M FeCl3 are needed to react with an excess of Na2S to produce 2.75 g of
Fe2S3 if the percent yield for the reaction is 65.0%?
3 Na2S(aq) + 2 FeCl3(aq) → Fe2S3(s) + 6 NaCl(aq)
A) 25.4 mL
B) 43.0 mL
C) 50.1 mL
D) 102 mL
60) If 200. mL of 0.100 M Na2SO4 is added to 200. mL of 0.150 M NaCl, what is the concentration of Na+
ions in the final solution? Assume that the volumes are additive.
A) 0.05 M
B) 0.175 M
C) 0.125 M
D) 0.250 M
61) When 50.0 mL of a 1.00 M solution of Fe(NO3)3 are mixed with 50.0 mL of a 1.00 M solution of NaOH,
a precipitate forms. How many moles of precipitate is formed?
Fe(NO3)3(aq) + 3 NaOH(aq) → Fe(OH)3(s) + 3 NaNO3(aq)
A) 0.33 moles
B) 1.00 mole
C) 0.05 moles
D) 0.017 moles
62) When 50.0 mL of a 1.00M solution of Fe(NO3)3 are mixed with 50.0mL of a 1.00 M solution of NaOH,
a precipitate forms. What ions remain after the reaction is complete?
Fe(NO3)3(aq) + 3 NaOH(aq) → Fe(OH)3(s) + 3 NaNO3(aq)
A) Fe3+ and OH–
B) Fe3+, Na+, and OH–
C) Fe3+, OH–, Na+, and NO3–
D) Na+ and NO3–
63) What is the oxidation number of the sulfur atom in S8?
A) -2
B) 0
C) +6
D) +8
64) What is the oxidation number of the chromium atom in K2Cr2O4?
A) -2
B) +3
C) +6
D) +7
65) What is the oxidation number of the sulfur atom in SO2?
A) -2
B) +2
C) -4
D) +4
66) What is the oxidation number change for the manganese atom in the following unbalanced reduction
half reaction?
MnO4–(aq) + H+(aq) → Mn2+(aq) + H2O(l)
A) -7
B) -5
C) +5
D) +7
67) What is the oxidation number change for the iron atom in the following reaction?
2 Fe2O3(s) + 3 C(s) → 4 Fe(s) + 3 CO2(g)
A) -6
B) -3
C) +3
D) +6
68) The oxidation state of chlorine in ClO4– is
A) 0
B) +5
C) -5
D) +7
69) In the following reaction, Cl2 is
2 Rb(s) + Cl2(g) → 2 RbCl(s)
A) the reducing agent.
B) the oxidizing agent.
C) oxidized.
D) the electron donor.
70) Which species functions as the oxidizing agent in the following reduction-oxidation reaction?
5 Fe2+(aq) + MnO4–(aq) + 8 H+(aq) → Mn2+(aq) + 5 Fe3+(aq) + 4 H2O(l)
A) Fe2+(aq)
B) H+(aq)
C) Mn2+(aq)
D) MnO4–(aq)
71) Which species functions as the reducing agent in the following reduction-oxidation reaction?
2 P(s) + 3 Br2(l) → 2 PBr3(l)
A) Br–(aq)
B) Br2(l)
C) P(s)
D) P3+(aq)
72) Which species functions as the reducing agent in the following reduction-oxidation reaction?
ZnO(s) + C(s) → Zn(s) + CO(g)
A) C(s)
B) CO(g)
C) Zn(s)
D) ZnO(s)