Chapter 4 2 Combining aqueous solutions of BaI2 and Na2SO4 affords

B) H+ and OH–

C) Mg+2 and Cl–

D) H+ and Cl–

E) OH– only

8) The net ionic equation for the reaction between aqueous solutions of HF and KOH is __________.

A) HF + KOH → H2O + K+ + F–

B) HF + OH– → H2O + F–

C) HF + K+ + OH– → H2O + KF

D) H+ + OH– → H2O

E) H+ + F– + K+ + OH– → H2O + K+ + F–

9) Combining aqueous solutions of BaI2 and Na2SO4 affords a precipitate of BaSO4. Which ion(s)

is/are spectator ions in the reaction?

A) Ba2+ only

B) Na+ only

C) Ba2+ and SO42-

D) Na+ and I–

E) SO42- and I–

10) Which ion(s) is/are spectator ions in the formation of a precipitate of AgCl via combining aqueous

solutions of CoCl2 and AgNO3?

A) Co2+ and NO3–

B) NO3– and Cl–

C) Co2+ and Ag+

D) Cl–

E) NO3–

11) The balanced net ionic equation for precipitation of CaCO3 when aqueous solutions of Na2CO3 and

CaCl2 are mixed is __________.

A) 2Na+ (aq) + CO32- (aq) → Na2CO3 (aq)

B) 2Na+ (aq) + 2Cl– (aq) → 2NaCl (aq)

C) Na+ (aq) + Cl– (aq) → NaCl (aq)

D) Ca2+ (aq) + CO32- (aq) → CaCO3 (s)

E) Na2CO3 (aq) + CaCl2 (aq) → 2NaCl (aq) + CaCO3 (s)

12) When aqueous solutions of AgN O3 and KI are mixed, AgI precipitates. The balanced net ionic

equation is __________.

A) Ag+ (aq) + I– (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 AgNO3 and NaCl are mixed, AgCl precipitates. The balanced net ionic

equation is __________.

A) Ag+ (aq) + Cl– (aq) → AgCl (s)

B) Ag+ (aq) + NO3– (aq) → AgNO3 (s)

C) Ag+ (aq) + NO3– (aq) → AgNO (aq)

D) AgNO3 (aq) + NaCl (aq) → AgCl (s) + NaNO3 (aq)

E) AgNO3 (aq) + NaCl (aq) → AgCl (aq) + NaNO3 (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) → 2 H2O (l) + SO42- (aq)

E) 2H+ (aq) + 2NaOH (aq) → 2 H2O (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

27

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) When gold dissolves in aqua regia, what is reduced?

A) H+

B) N+5

C) Cl–

D) H2O

E) Au

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

28

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

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

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 __________.

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

31

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 __________.