1.In Which of the Following Aqueous Solutions Would You Expect Agbr to Have the Highest

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1.In which of the following aqueous solutions would you expect AgBr to have the highest solubility?

a.0.10 M LiBr

b.0.10 M AgNO3

c.0.20 M NaBr

d.0.15 M KBr

e.pure water

2.In which of the following aqueous solutions would you expect PbCl2 to have the lowest solubility?

a.0.020 M KCl

b.0.020 M BaCl2

c.0.015 M PbNO3

d.pure water

e.0.015 M NaCl

3.Calculate the fluoride ion concentration (in M) in a 1.0-L aqueous solution containing 0.40 mol of HF and 0.10 mol of HCl. (Ka for HF = 6.8 x 10-4)

a.1.0

b.0.40

c.0.016

d.2.7 x 10-3

e.1.4 x 10-3

4.Calculate the percent ionization of HF in a 1.0-L aqueous solution containing 0.30 mol of HF and 0.10 mol of HCl. (Ka for HF = 6.8 x 10-4)

a.33

b.4.1

c.11

d.0.68

e.2.7

5.The pH of a solution containing 0.818 M acetic acid (Ka = 1.76 x 10-5) and 0.172 M sodium acetate is ______.

a.4.077

b.5.432

c.8.568

d.8.370

e.9.922

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6.Which one of the following pairs cannot be mixed together to form a buffer solution?

a.NH3, NH4Cl

b.NaC2H3O2, HCl

c.RbOH, HBr

d.KOH, HF

e.H3PO4, KH2PO4

7.A solution containing which one of the following pairs of substances will be a buffer solution?

a.NaI, HI

b.KBr, HBr

c.RbCl, HCl

d.CsF, HF

e.none of these

8.The Kb of ammonia is 1.8 x 10-5. The pH of a buffer prepared by combining 50.0 mL of 1.00 M ammonia and 50.0 mL of 1.00 M ammonium nitrate is ______.

a.4.63

b.9.26

c.4.74

d.9.37

e.7.00

9.Calculate the pH of a solution prepared by dissolving 0.37 mol of formic acid (HCO2H) and 0.23 mol of sodium formate (NaCO2H) in 1.00 L of solution. Ka = 1.8 x 10-4 for formic acid.

a.2.09

b.10.46

c.3.54

d.2.30

e.3.95

10.Determine the pH of a solution prepared by dissolving 0.75 mol of NH3 and 0.25 mol of NH4Cl in a liter of solution. Kb = 1.8 x 10-4 for NH3.

a.4.27

b.8.78

c.10.73

d.5.22

e.9.78

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11.The pH of a solution prepared by dissolving 0.35 mol of solid CH3NH3Cl (methylamine hydrochloride) in 1.00 L of 1.1 M CH3NH2 (methylamine) is ______. The Kb for methylamine is 4.4 x 10-4.

a.1.66

b.2.86

c.10.15

d.11.14

e.10.64

12.Consider a solution prepared by dissolving 0.35 mol of solid CH3NH3Cl (methylamine hydrochloride) in 1.00 L of 1.1 M CH3NH2 (methylamine). The Kb for methylamine is 4.4 x 10-4. If 10 mL of 0.01 M HCl is added to this buffer solution, the pH of the solution will ______slightly because the HCl reacts with the ______present in the solution.

a. increase, OH-

b. increase, CH3NH2

c. decrease, CH3NH2

d. +

decrease, CH3NH3

e. This is a buffer solution so that the pH doesnot change.

13.Which of the following could be added to a solution of sodium acetate to prepare a buffer?

acetic acid hydrochloric acid ammonium acetate sodium chloride

a.acetic acid only

b.acetic acid or hydrochloric acid

c.hydrochloric acid only

d.ammonium acetate only

e.sodium chloride or ammonium acetate

14.Which of the following could be added to a solution of acetic acid to prepare a buffer?

sodium acetate sodium hydroxide nitric acid hydrofluoric acid

a.sodium acetate only

b.sodium acetate or sodium hydroxide

c.nitric acid only

d.hydrofluoric acid or nitric acid

e.sodium hydroxide only

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15.Consider the titration of 25.0 mL of 0.723 M HClO4 with 0.273 M KOH. The H3O+ concentration before any KOH is added is ______M.

a.0.439

b.1.00 x 10-7

c.0.723

d.2.81 x 10-13

e.0.273

16.Consider the titration of 25.00 mL of 0.723 M HClO4 with 0.273 M KOH. The H3O+ concentration after addition of 10.0 mL of KOH is ______M.

a.0.438

b.1.00 x 10-7

c.0.723

d.2.81 x 10-13

e.0.273

17.Consider the titration of 25.0 mL of 0.723 M HClO4 with 0.273 M KOH. The H3O+ concentration after addition of 66.2 mL of KOH is ______M.

a.0.439

b.1.00 x 10-7

c.0.723

d.2.81 x 10-13

e.0.273

18.Consider the titration of 25.0 mL of 0.723 M HClO4 with 0.273 M KOH. The H3O+ concentration after addition of 80.0 mL of KOH is ______M.

a.0.439

b.1.00 x 10-7

c.0.723

d.2.79 x 10-13

e.3.58 x 10-2

19.A ______yields a titration curve with an initial pH of 1.00, an equivalence point at pH 7.0, and a relatively long, nearly vertical middle section.

a.strong acid titrated by strong base

b.strong base titrated by strong acid

c.weak acid titrated by strong base

d.weak base titrated by strong acid

e.weak base titrated by weak acid

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20.An initial pH of 4.00, an equivalence point at pH 9.35, and a moderately short, nearly vertical middle section correspond to a titration curve for ______.

a.strong acid titrated by strong base

b.strong base titrated by strong acid

c.weak acid titrated by strong base

d.weak base titrated by strong acid

e.weak base titrated by weak acid

21.An initial pH of 13.00, an equivalence point at pH 7.0, and a relatively long, nearly vertical middle section correspond to a titration curve for ______.

a.strong acid titrated by strong base

b.strong base titrated by strong acid

c.weak acid titrated by strong acid

d.weak base titrated by strong acid

e.weak base titrated by weak acid

22.50.50 mL of 0.116 M HF is titrated with 0.1200 M NaOH. How many mL of the base are required to reach the equivalence point? (Ka for HF is 6.8 x 10-4)

a.101

b.50.5

c.52.7

d.24.2

e.48.8

23.50.50 mL of 0.116 M HF is titrated with 0.1200 M NaOH. What is the pH when 25.00 mL of base have been added? (Ka for HF is 6.8 x 10-4)

a.5.118

b.3.146

c.6.168

d.3.547

e.3.189

24.50.50 mL of 0.116 M HF is titrated with 0.1200 M NaOH. What is the pH at the equivalence point? (Ka for HF is 6.8 x 10-4)

a.13.064

b.7.000

c.7.969

d.12.771

e.1.229

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25.50.50 mL of 0.116 M HF is titrated with 0.1200 M NaOH. What is the pH after 50.50 mL of base have been added? (Ka for HF is 6.8 x 10-4)

a.7.000

b.11.300

c.12.778

d.8.119

e.4.631

26.The solubility of which one of the following will not be affected by the pH of the solution?

a.Na3PO4

b.NaF

c.KNO3

d.AlCl3

e.MnS

27.The concentration (in M) of bromide ions in a saturated solution of mercury(II) bromide, Ksp = 8.0 x 10-20, is _____ M.

a.1.4 x 10-10

b.2.0 x 10-20

c.5.4 x 10-7

d.2.7 x 10-7

e.8.0 x 10-20

28.What is the molar solubility of PbS? Ksp(PbS) = 8.0 x 10-28

a.4.0 x 10-28

b.2.8 x 10-14

c.6.4 x 10-55

d.8.0 x 10-19

e.8.0 x 10-28

29.The Ksp for Ag2S is 1.0 x 10-51. What is the molar solubility of Ag2S?

a.1.0 x 10-17

b.7.9 x 10-18

c.6.3 x 10-18

d.8.3 x 10-53

e.1.0 x 10-51

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30.The solubility of Mn(OH)2 is 2.2 x 10-5 mol/L. What is the Ksp of Mn(OH)2?

a.1.1 x 10-14

b.4.3 x 10-14

c.2.1 x 10-14

d.4.8 x 10-10

e.2.2 x 10-5

31.What is the maximum concentration (in M) of chloride ions in a solution that contains 0.100 M Pb2+. The Ksp for lead(II) chloride is 1.0 x 10-4.

a.0.058

b.0.029

c.0.0.0010

d.0.032

e.1.0 x 10-4

32.Calculate the solubility (in M) of aluminum hydroxide, Ksp = 1.9 x 10-33, in 0.0182 M KOH solution.

a.3.2 x 10-28

b.2.9 x 10-9

c.1.2 x 10-11

d.3.1 x 10-12

e.1.9 x 10-33

33.What is the solubility (in M) of PbCl2 in a 0.15 M solution of HCl? (Ksp PbCl2 = 1.6 x 10-5)

a.2.0 x 10-3

b.1.1 x 10-4

c.1.8 x 10-4

d.7.1 x 10-4

e.1.6 x 10-5

34.The Ksp for Zn(OH)2 is 5.0 x 10-17. Determine the molar solubility of Zn(OH)2 in a buffer solution with a pH of 11.50.

a.5.0 x 106

b.1.2 x 10-12

c.1.6 x 10-14

d.5.0 x 10-12

e.5.0 x 10-17

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35.In which one of the following solutions is silver chloride the most soluble?

a.0.181 M HCl

b.0.0176 M NH3

c.0.744 M LiNO3

d.pure water

e.0.181 M NaCl

36.For which salt should the aqueous solubility be most sensitive to pH?

a.Ca(NO3)2

b.CaF2

c.CaCl2

d.CaBr2

e.CaI2

37.In which aqueous system is PbI2 least soluble?

a.H2O

b.0.5 M HI

c.0.2 M HI

d.1.0 M HNO3

e.0.8 M KI

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1.e

2.c

3.d

4.d

5.a

6.c

7.d

8.b

9.c

10.c

11.d

12.c

13.b

14.b

15.c

16.a

17.b

18.d

19.a

20.c

21.b

22.e

23.e

24.c

25.b

26.c

27.c

28.b

29.c

30.b

31.d

32.a

33.d

34.d

35.b

36.b

37.e