Chapter 4 1 What is the molar concentration of sulfate ions in a

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Chemistry, 6e (McMurry/Fay)

Chapter 4 Reactions in Aqueous Solutions

4.1 Multiple-Choice Questions

1) The reaction HNO3(aq) + KOH(aq) → KNO3(aq) + H2O(l) is best classified as a(n)

A) acid-base neutralization reaction.

B) oxidation-reduction reaction.

C) precipitation reaction.

D) single replacement reaction.

2) 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.

3) The reaction Pb(NO3)2(aq) + K2SO4(aq) → PbSO4(s) + 2 KNO3(aq) is best classified as a(n)

A) acid-base neutralization reaction.

B) oxidation-reduction reaction.

C) precipitation reaction.

D) single replacement reaction.

4) 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.

5) The reaction Cu(s) + 2 AgNO3(aq) → Cu(NO3)2(aq) + 2 Ag(s) is best classified as a(n)

A) acid-base neutralization reaction.

B) double replacement reaction.

C) oxidation-reduction reaction.

D) precipitation reaction.

6) 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.

7) 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.

8) HBr, HCl, HClO4, KBr, and NaCl are all classified as

A) acids.

B) nonelectrolytes.

C) strong electrolytes.

D) weak electrolytes.

9) 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.

10) 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.

11) 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

12) 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

13) What is the molar concentration of sulfate ions in a 0.150 M Na2SO4 solution?

A) 0.075 M

B) 0.150 M

C) 0.300 M

D) 0.450 M

14) 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)

15) 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)

16) Write a balanced net ionic equation for the reaction of Na2CO3(s) and HCl(aq).

A) Na2CO3(s) + 2 HCl(aq) → 2 NaCl(aq) + H2O(l) + CO2(g)

B) 2Na+(aq) + CO32-(aq) + 2H+(aq) + 2Cl–(aq) → 2Na+(aq) + 2Cl–(aq) + H2O(l) + CO2(g)

C) Na2CO3(s) + 2 H+(aq) → 2 Na+(aq) + H2O(l) + CO2(g)

D) CO32-(aq) + 2 H+(aq) → H2O(l) + CO2(g)

17) 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)

18) Write a balanced net ionic equation for the reaction of AgNO3(aq) with KBr(aq).

A) AgNO3(aq) + KBr(aq) → AgBr(aq) + KNO3(s)

B) Ag+(aq) + NO3–(aq) + K+(aq) + Br–(aq) → Ag+(aq) + Br–(aq) + KNO3(s)

C) Ag+(aq) + NO3–(aq) + K+(aq) + Br–(aq) → AgBr(s) + K+(aq) + NO3–(aq)

D) Ag+(aq) + Br–(aq) → AgBr(s)

19) Write a balanced net ionic equation for the reaction of CdCl2(aq) with Na2S(aq).

A) CdCl2(aq) + Na2S(aq) → CdS (aq) + 2 NaCl(aq)

B) Cd2+(aq) + 2 Cl–(aq) + 2 Na+(aq) + S2-(aq) → CdS(s) + 2 NaCl(aq)

C) Cd2+(aq) + S2-(aq) → CdS(s)

D) Cd2+(aq) + 2 Cl–(aq) + 2 Na+(aq) + S2-(aq) → CdS(s) + 2 Na+(aq)

20) 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)

21) 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–

22) Which one of the following compounds is insoluble in water?

A) K2SO4

B) NaNO3

C) PbSO4

D) Rb2CO3

23) 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

24) Which one of the following compounds is soluble in water?

A) Ag3PO4

B) CuS

C) Pb(NO3)2

D) ZnCO3

25) Which pair of compounds is soluble in water?

A) AgBr and AgI

B) CdS and (NH4)2S

C) KI and Ba(NO3)2

D) NaNO3 and CuCO3

26) 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) NaO2CC6H4CO2K

27) The mixing of which pair of reactants will result in a precipitation reaction?

A) CsI(aq) + NaOH(aq)

B) HCl(aq) + Ca(OH)2(aq)

C) K2SO4(aq) + Ba(NO3)2(aq)

D) NaNO3(aq) + NH4Cl(aq)

28) The mixing of which pair of reactants will result in a precipitation reaction?

A) Cu(NO3)2(aq) + Na2CO3(aq)

B) K2SO4(aq) + Cu(NO3)2(aq)

C) NaClO4(aq) + (NH4)2S(aq)

D) NH4Br(aq) + NaI(aq)

29) What reagent could be used to separate Br– from NO3– when added to an aqueous solution

containing both?

A) AgNO3(aq)

B) Ba(OH)2(aq)

C) CuSO4(aq)

D) NaI(aq)

30) What reagent could not be used to separate Cl– from OH– 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)

31) Predict the products of a reaction between AgNO3(aq) and KBr(aq).

A) Ag(s) and NO(g)

B) Ag(s) and Br2(l)

C) AgBr(s) and KNO3(aq)

D) AgNO3(aq) and KBr(aq)

32) Predict the products of a reaction between Ba(NO3)2(aq) and K2SO4(aq).

A) Ba(s), KNO3(aq) and K2SO3(aq)

B) BaSO3(s) and KNO2(aq)

C) BaSO3(s) and KNO3(aq)

D) BaSO4(s) and KNO3(aq)

33) Which pair of reactants will produce a precipitate when mixed together?

A) HCl(aq) and NaOH(aq)

B) HCl(aq) and Na2CO3(aq)

C) HCl(aq) and Na2S(aq)

D) HCl(aq) and Pb(NO3)2(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 Ba2+ and Pb2+?

A) NaCl

B) NaNO3

C) Na2SO4

D) Na2S2O3

37) What reagent would distinguish between Ag+ and Fe3+?

A) NaClO3

B) NaI

C) NaNO3

D) NaOH

38) Which of the following compounds is not an Arrhenius acid?

A) CH3CO2H

B) CH3NH2

C) HNO3

D) H2SO4

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) HOClO2

C) H2SO4

D) NH3

42) Which of the following compounds is an Arrhenius base in water?

A) CH3OH

B) CH3CO2H

C) HOCl

D) KOH

43) Which one of the following compounds behaves as an acid when dissolved in water?

A) BaO

B) CH4

C) HBr

D) KOH

44) When dissolved in water, of HClO4, Ca(OH)2, KOH, HI, which are acids?

A) Ca(OH)2 and KOH

B) HClO4 and HI

C) only HI

D) only KOH

45) When dissolved in water, of HClO4, Ca(OH)2, KOH, HI, which are bases?

A) Ca(OH)2 and KOH

B) HClO4 and HI

C) only HI

D) only KOH

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) An aqueous solution of HI is named

A) hydriodic acid.

B) hydroiodous acid.

C) iodic acid.

D) iodous acid.

54) The chemical formula for sulfurous acid is

A) H2S(aq).

B) H2SO3(aq).

C) H2SO4(aq).

D) H2S2O7(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) What is the oxidation number of the sulfur atom in S8?

A) –2

B) 0

C) +6

D) +8

57) What is the oxidation number of the sulfur atom in H2SO4?

A) -2

B) +2

C) +4

D) +6

58) What is the oxidation number of the chromium atom in K2Cr2O7?

A) -2

B) +2

C) +6

D) +7

59) What is the oxidation number of the oxygen atom in H2O2?

A) -2

B) -1

C) +1

D) +2

60) In which compound is the oxidation state of oxygen not –2?

A) MgO

B) Li2O

C) Na2O2

D) Al2O3

61) In which compound is the oxidation state of hydrogen not +1?

A) H2O

B) H2O2

C) NaH

D) Na2HSO4

62) 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

63) 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

64) Which species functions as the oxidizing agent in the following reduction-oxidation reaction?

Zn(s) + Cu2+(aq) → Cu(s) + Zn2+(aq)

A) Cu(s)

B) Cu2+(aq)

C) Zn(s)

D) Zn2+(aq)

65) 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)

66) 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)

67) 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)

68) Disproportionation is a reaction in which a substance is both oxidized and reduced in the reaction.

Which is a disproportionation reaction?

A) ClO3–(aq) + 3 Cu(s) + 6 H+(aq) → Cl–(aq) + 3 Cu2+(aq) + 3 H2O(l)

B) ClO–(aq) + Pb(OH)4–(aq) → Cl–(aq) + PbO2(s) + H2O(l) + 2 OH–(aq)

C) 6 Cl–(aq) + Cr2O72-(aq) + 14 H+(aq) → 3 Cl2(g) + 2 Cr3+(aq) + 7 H2O(l)

D) Cl2(g) + 2 OH–(aq) → Cl–(aq) + ClO–(aq) + H2O(l)

69) In the reaction 2 H2O2(l) → 2 H2O(l) + O2(g) oxygen is

A) both oxidized and reduced.

B) neither oxidized nor reduced.

C) only oxidized.

D) only reduced.

70) Using the following portion of the activity series for oxidation half-reactions, determine which

combination of reactants will result in a reaction.

Na(s) → Na+(aq) + e–

Cr(s) → Cr3+(aq) + 3e–

A) Na(s) with Cr(s)

B) Na(s) with Cr3+(aq)

C) Na+(aq) with Cr3+(aq)

D) Na+(aq) with Cr(s)

71) Using the following portion of the activity series for oxidation half reactions

K(s) → K+(aq) + e–

Al(s) → Al3+(aq) + 3e–

Fe(s) → Fe2+(aq) + 2e–

Sn(s) → Sn2+(aq) + 2e–

determine which reaction will occur.

A) Al3+(aq) with Fe(s)

B) Al(s) with Sn(s)

C) K+(aq) with Fe2+(aq)

D) K(s) with Sn2+(aq)

72) Using the following portion of the activity series for oxidation half reactions

Ca(s) → Ca2+(aq) + 2e–

Mg(s) → Mg2+(aq) + 2e–

Zn(s) → Zn2+(aq) + 2e–

Cu(s) → Cu2+(aq) + 2e–

determine which reaction will not occur.

A) Ca(s) with Cu2+(aq)

B) Ca(s) with Zn2+(aq)

C) Zn(s) with Cu2+(aq)

D) Zn(s) with Mg2+(aq)

73) Using the following portion of the activity series for oxidation half reactions

Mg(s) → Mg2+(aq) + 2e–

Zn(s) → Zn2+(aq) + 2e–

Cu(s) → Cu2+(aq) + 2e–

indicate which pairs of reactions will occur.

A) Cu(s) with Zn2+(aq) and Zn(s) with Mg2+(aq)

B) Mg(s) with Cu2+(aq) and Zn2+(aq) with Mg2+(aq)

C) Mg(s) with Cu(s) and Zn(s) with Cu(s)

D) Mg(s) with Zn2+(aq) and Zn(s) with Cu2+(aq)

74) Using the following portion of the activity series for oxidation half reactions

K(s) → K+(aq) + e–

Al(s) → Al3+(aq) + 3e–

Fe(s) → Fe2+(aq) + 2e–

Sn(s) → Sn2+(aq) + 2e–

determine which pairs of reactions will occur.

A) Al(s) with Fe2+(aq) and Sn(s) with K+(aq)

B) Fe(s) with Al(s) and Al3+(aq) with Sn2+(aq)

C) Fe(s) with Sn2+(aq) and Al(s) with Sn2+(aq)

D) K(s) with Al3+(aq) and Fe(s) with Al3+(aq)

75) Using the following sequence of reactions, determine the order of reducing agents (strongest to

weakest).

A + B+ → A+ + B

A + C+ → A+ + C

B + C+ → no reaction

A) A > B > C

B) A > C > B

C) B > C > A

D) C+ > B+ > A+

76) Using the following sequence of reactions, determine the order of oxidizing agents (strongest to

weakest).

Q + U+ → Q+ + U

U + W+ → U+ + W

Q + W+ → Q+ + W

A) Q > U > W

B) W > U > Q

C) Q+ > U+ > W+

D) W+ > U+ > Q+

77) Coinage metals are metals that are not easily oxidized. Based on the activity series, which metal

would be least desirable as a coinage metal?

A) Al

B) Au

C) Mg

D) Mn

78) Based on the activity series, which metal dissolves in hydrochloric acid to produce hydrogen gas?

A) Ag

B) Au

C) Co

D) Cu

79) Which elements will react rapidly with aqueous H+ ions and also with liquid H2O?

A) Al, Cr, Fe, Mn, Zn

B) Au, Co, Cu, Ni, Sn

C) Au, Li, K, Ni, Sn

D) Ba, Ca, Li, K, Na

80) Which elements will not react with liquid water but will react with aqueous H+ ions?

A) Ag, Cu, Hg, Pt

B) Al, Cr, Mn, Zn

C) Ba, Ca, Li, Na

D) Ag, Au, Ca, K

81) Which elements will not react with liquid water or with aqueous H+ ions?

A) Ag, Au, Hg, Pt

B) Ba, Ca, Li, K

C) Co, Cu, Ni, Sn

D) Cr, Fe, Mn, Zn

82) In the unbalanced equation shown below how many moles of electrons are transferred per mole of

reducing agent?

C2O42– (aq) + MnO4–(aq) → CO2(aq) + Mn2+(aq)

A) 1

B) 2

C) 5

D) 10

83) What are the coefficients in front of NO3–(aq) and Cu(s) when the following redox equation is

balanced in an acidic solution:

_____ NO3–(aq) + _____ Cu(s) → _____ NO(g) + _____ Cu2+(aq)?

A) 2, 3

B) 2, 6

C) 3, 4

D) 3, 6

84) What is true when the following equation is balanced in basic solution?

P(s) + PO43-(aq) → HPO32-(aq)

A) H+ appears on the left side of the equation.

B) H+ appears on the right side of the equation.

C) OH– appears on the left side of the equation.

D) OH– appears on the right side of the equation.

85) What are the coefficients in front of NO3–(aq) and Zn(s) when the following equation is balanced in

a basic solution?

_____ NO3–(aq) + _____ Zn(s) → _____ Zn2+(aq) + _____ NO(g)

A) 2, 3

B) 2, 5

C) 3, 2

D) 3, 4

86) What are the coefficients in front of Fe(s) and O3(g) when the following equation is balanced in a

basic solution?

_____ Fe(s) + _____ O3(g) → _____ Fe2O3(s) + _____ O2(g)

A) 2, 2

B) 2, 3

C) 3, 2

D) 3, 4

87) What are the coefficients in front of BrO3–(aq) and Br–(aq) when the following equation is balanced

in an acidic solution?

_____ BrO3–(aq) + _____ Br–(aq) → _____ Br2(aq)

A) 1, 3

B) 1, 5

C) 2, 3

D) 2, 5

88) Determine the number of water molecules necessary to balance the following chemical equation.

Cr2O72-(aq) + Cl–(aq) + H+(aq) → Cr3+(aq) + Cl2(g) + _____ H2O(l)

A) 3

B) 5

C) 7

D) 14

89) Determine the number of water molecules necessary to balance the reduction half reaction of

____ MnO4–(aq) → ____ MnO2(s) that occurs in a basic solution.

A) 2

B) 3

C) 4

D) 5

90) Determine the number of water molecules necessary to balance the reduction half reaction of

____ MnO4–(aq) → ____ Mn2+(aq)that occurs in an acidic solution.

A) 2

B) 4

C) 5

D) 7

91) Determine the number of water molecules necessary to balance the reduction half reaction of

____ ClO3–(aq) → ____ Cl– (aq)that occurs in an acidic solution.

A) 1

B) 3

C) 5

D) 7

92) What is the oxidation half reaction in the following chemical reaction?

Zn(s) + 2 H+(aq) → Zn2+(aq) + H2(g)

A) Zn(s) → Zn2+(aq) + 2e–

B) Zn2+(aq) + 2e– → Zn(s)

C) 2 H+(aq) + 2e– → H2(g)

D) H2(g) → 2 H+(aq) + 2e–