Chapter 4 2 When aqueous solutions of AgNO3 and KI are mixed

12) When aqueous solutions of AgNO3 and KI are mixed, AgI precipitates. The balanced net ionic

equation is ________.

A) Ag+ (aq) + (aq) → AgI (s)

B) Ag+ (aq) + NO3– (aq) → AgNO3 (s)

C) Ag+ (aq) + NO3– (aq) → AgNO3 (aq)

D) AgNO3 (aq) + KI (aq) → AgI (s) + KNO3 (aq)

E) AgNO3 (aq) + KI (aq) → AgI (aq) + KNO3 (s)

13) When aqueous solutions of Pb(NO3)2 and NaCl are mixed, PbCl2 precipitates. The balanced net ionic

equation is ________.

A) Pb2+ (aq) + 2Cl– (aq) → PbCl2 (s)

B) Pb2+ (aq) + 2NO3– (aq) → Pb(NO3)2 (s)

C) Pb2+ (aq) + 2NO3– (aq) → Pb(NO3)2 (aq)

D) Pb(NO3)2 (aq) + 2NaCl (aq) → PbCl2 (s) + 2NaNO3 (aq)

E) Pb(NO3)2 (aq) + 2NaCl (aq) → PbCl2 (aq) + 2NaNO3 (s)

14) When H2SO4 is neutralized by NaOH in aqueous solution, the net ionic equation is ________.

A) SO42- (aq) + 2Na+ (aq) → Na2SO4 (aq)

B) SO42- (aq) + 2Na+ (aq) → Na2SO4 (s)

C) H+ (aq) + OH– (aq) → H2O (l)

D) H2SO4 (aq) + 2OH– (aq) → 2H2O (l) + SO42– (aq)

E) 2H+ (aq) + 2NaOH (aq) → 2H2O (l) + 2Na+ (aq)

15) The spectator ions in the reaction between aqueous perchloric acid and aqueous barium hydroxide

are ________.

A) OH– and ClO4–

B) H+, OH– , ClO4–, and Ba2+

C) H+ and OH–

D) H+ and Ba2+

E) ClO4– and Ba2+

16) The spectator ions in the reaction between aqueous chloric acid and aqueous barium hydroxide are

________.

A) OH– and ClO3–

B) H+, OH–, ClO3–, and Ba2+

C) H+ and OH–

D) H+ and Ba2+

E) ClO3– and Ba2+

17) The spectator ions in the reaction between aqueous hydrofluoric acid and aqueous barium hydroxide

are ________.

A) OH–, F–, and Ba2+

B) F– and Ba2+

C) OH– and F–

D) Ba2+ only

E) H+, OH–, F–, and Ba2+

18) The spectator ions in the reaction between aqueous hydrochloric acid and aqueous ammonia are

________.

A) H+ and NH3

B) H+, Cl–, NH3, and NH4+

C) Cl– and NH4+

D) H+, Cl–, and NH4+

E) Cl– only

19) Which of the following are strong acids?

HI

HNO3

HF

HBr

A) HF, HBr

B) HI, HNO3, HF, HBr

C) HI, HF, HBr

D) HNO3, HF, HBr

E) HI, HNO3, HBr

20) Which hydroxides are strong bases?

Sr(OH)2

KOH

NaOH

Ba(OH)2

A) KOH, Ba(OH)2

B) KOH, NaOH

C) KOH, NaOH, Ba(OH)2

D) Sr(OH)2, KOH, NaOH, Ba(OH)2

E) None of these is a strong base.

21) A neutralization reaction between an acid and a metal hydroxide produces ________.

A) water and a salt

B) hydrogen gas

C) oxygen gas

D) sodium hydroxide

E) ammonia

22) Of the metals below, only ________ will not dissolve in an aqueous solution containing nickel ions.

aluminum

chromium

barium

tin

potassium

A) aluminum

B) chromium

C) barium

D) tin

E) potassium

23) Which of these metals is the least easily oxidized?

Na

Au

Fe

Ca

Ag

A) Na

B) Au

C) Fe

D) Ca

E) Ag

24) Which of these metals is the most easily oxidized?

Na

Au

Fe

Ca

Ag

A) Na

B) Au

C) Fe

D) Ca

E) Ag

25) Of the following elements, ________ is the only one that cannot be found in nature in its elemental

form.

Cu

Hg

Au

Ag

Na

A) Cu

B) Hg

C) Au

D) Ag

E) Na

26) Of the following elements, ________ is the most easily oxidized.

oxygen

fluorine

nitrogen

aluminum

gold

A) oxygen

B) fluorine

C) nitrogen

D) aluminum

E) gold

27) Of the following elements, ________ is the least easily oxidized.

zinc

iron

hydrogen

aluminum

lead

A) zinc

B) iron

C) hydrogen

D) aluminum

E) lead

28) Based on the equations below, which metal is the most active?

Pb(NO3)2 (aq) + Ni (s) → Ni(NO3)2 (aq) + Pb (s)

Pb(NO3)2 (aq) + Ag (s) → No reaction

Cu(NO3)2 (aq) + Ni (s) → Ni(NO3)2 (aq) + Cu (s)

A) Ni

B) Ag

C) Cu

D) Pb

E) N

29) In the following reaction, which species is reduced?

Au(s) + 3NO3–(aq) + 6H+(aq) → Au3+(aq) + NO(g) + 3H2O (l)

H+

N+5

O2-

H2O

Au

A) H+

B) N+5

C) O2-

D) H2O

E) Au

28

30) What is the concentration (M) of a NaCl solution prepared by dissolving 9.3 g of NaCl in sufficient

water to give 350 mL of solution?

A) 18

B) 0.16

C) 0.45

D) 27

E) 2.7 × 10-2

31) How many moles of Co2+ are present in 0.200 L of a 0.400 M solution of CoI2?

A) 2.00

B) 0.500

C) 0.160

D) 0.0800

E) 0.0400

32) How many moles of Na+ are present in 343 mL of a 1.27 M solution of Na2SO4?

A) 0.436

B) 0.871

C) 1.31

D) 3.70

E) 11.1

33) How many moles of K+ are present in 343 mL of a 1.27 M solution of K3PO4?

A) 0.436

B) 1.31

C) 0.145

D) 3.70

E) 11.1

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34) What are the respective concentrations (M) of Na+ and SO42- afforded by dissolving 0.500 mol

Na2SO4 in water and diluting to 1.33 L?

A) 0.665 and 0.665

B) 0.665 and 1.33

C) 1.33 and 0.665

D) 0.376 and 0.752

E) 0.752 and 0.376

35) What are the respective concentrations (M) of K+ and PO43– afforded by dissolving 0.800 mol K3PO4

in water and diluting to 1.63 L?

A) 0.800 and 0.800

B) 0.491 and 0.491

C) 0.800 and 0.491

D) 1.44 and 0.491

E) 0.489 and 0.163

36) Calculate the concentration (M) of sodium ions in a solution made by diluting 50.0 mL of a 0.874 M

solution of sodium sulfide to a total volume of 250.0 mL.

A) 0.175

B) 4.37

C) 0.525

D) 0.350

E) 0.874

37) An aqueous ethanol solution (400 mL) was diluted to 4.00 L, giving a concentration of 0.0400 M. The

concentration of the original solution was ________ M.

A) 0.400

B) 0.200

C) 2.00

D) 1.60

E) 4.00

38) The concentration (M) of an aqueous methanol produced when 0.200 L of a 2.00 M solution was

30

diluted to 0.800 L is ________.

A) 0.800

B) 0.200

C) 0.500

D) 0.400

E) 8.00

39) The molarity (M) of an aqueous solution containing 22.5 g of sucrose (C12H22O11) in 35.5 mL of

solution is ________.

A) 0.0657

B) 1.85 ×

C) 1.85

D) 3.52

E) 0.104

40) The molarity (M) of an aqueous solution containing 52.5 g of sucrose (C12H22O11) in 35.5 mL of

solution is ________.

A) 5.46

B) 1.48

C) 0.104

D) 4.32

E) 1.85

41) The molarity (M) of an aqueous solution containing 22.5 g of glucose (C6H12O6) in 35.5 mL of

solution is ________.

A) 3.52

B) 0.634

C) 0.197

D) 0.125

E) 1.85

42) The molarity of an aqueous solution containing 75.3 g of glucose (C6H12O6) in 35.5 mL of solution is

31

________.

A) 1.85

B) 2.12

C) 0.197

D) 3.52

E) 11.8

43) How many grams of sodium chloride are there in 55.0 mL of a 1.90 M aqueous solution of sodium

chloride?

A) 0.105

B) 6.11

C) 3.21

D) 6.11 × 103

E) 12.2

44) How many grams of sodium chloride are there in 550.0 mL of a 1.90 M aqueous solution of sodium

chloride?

A) 61.1

B) 1.05

C) 30.5

D) 6.11 × 104

E) 122

45) The molarity of a solution prepared by diluting 43.72 mL of 1.005 M aqueous K2Cr2O7 to 500. mL is

________.

A) 0.0879

B) 87.9

C) 0.0218

D) 0.0115

E) 0.870

46) The molarity of a solution prepared by diluting 43.72 mL of 5.005 M aqueous K2Cr2O7 to 500. mL is

________.

A) 57.2

B) 0.0044

C) 0.438

D) 0.0879

E) 0.870

47) The concentration of chloride ions in a 0.193 M solution of potassium chloride is ________.

A) 0.0643 M

B) 0.386 M

C) 0.0965 M

D) 0.579 M

E) 0.193 M

48) The concentration of sulfate ions in a 0.233 M solution of sulfuric acid is ________.

A) 0.699 M

B) 0.233 M

C) 0.466 M

D) 0.0777 M

E) 0.155 M

49) The concentration of iodide ions in a 0.193 M solution of barium iodide is ________.

A) 0.193 M

B) 0.386 M

C) 0.0965 M

D) 0.579 M

E) 0.0643 M

33

50) The concentration of species in 500 mL of a 2.104 M solution of sodium sulfate is ________ M sodium

ion and ________ M sulfate ion.

A) 2.104, 1.052

B) 2.104, 2.104

C) 2.104, 4.208

D) 1.052, 1.052

E) 4.208, 2.104

51) When 0.500 mol of HC2H3O2 is combined with enough water to make a 300.0 mL solution, the

concentration of HC2H3O2 is ________ M.

A) 3.33

B) 1.67

C) 0.835

D) 0.00167

E) 0.150

52) In a titration of 35.00 mL of 0.737 M H2SO4, ________ mL of a 0.827 M KOH solution is required for

neutralization.

A) 35.0

B) 1.12

C) 25.8

D) 62.4

E) 39.3

53) Oxalic acid is a diprotic acid. Calculate the percent of oxalic acid (H2C2O4) in a solid given that a

0.7984-g sample of that solid required 37.98 mL of 0.2283 M NaOH for neutralization.

A) 48.89

B) 97.78

C) 28.59

D) 1.086

E) 22.83

54) Oxalic acid is a diprotic acid. If a solid material contains 53.66 percent of oxalic acid (H2C2O4), by

34

mass, then a 0.6543-g sample of that solid will require ________ mL of 0.3483 M NaOH for neutralization.

A) 11.19

B) 97.78

C) 28.59

D) 1.119

E) 22.39

55) A 17.5 mL sample of an acetic acid (CH3CO2H) solution required 29.6 mL of 0.250 M NaOH for

neutralization. The concentration of acetic acid was ________ M.

A) 0.158

B) 0.423

C) 134

D) 6.88

E) 0.214

56) A 25.5 mL aliquot of HCl (aq) of unknown concentration was titrated with 0.113 M NaOH (aq). It took

51.2 mL of the base to reach the endpoint of the titration. The concentration (M) of the acid was ________.

A) 1.02

B) 0.114

C) 0.454

D) 0.113

E) 0.227

57) A 31.5 mL aliquot of HNO3 (aq) of unknown concentration was titrated with 0.0134 M NaOH (aq). It

took 23.9 mL of the base to reach the endpoint of the titration. The concentration (M) of the acid was

________.

A) 0.0102

B) 0.0051

C) 0.0204

D) 0.227

E) 1.02

58) A 31.5 mL aliquot of H2SO4 (aq) of unknown concentration was titrated with 0.0134 M NaOH (aq). It