Question 1

What is the molar solubility of silver sulfate (Ag2SO4) in water? The solubility-product constant for Ag2SO4 is 1.5 × 10-5 at 25°C.

Accepted Answer

A)  1.9 × 10-3
B)  2.5 × 10-2
C)  5.5 × 10-3
D)  1.6 × 10-2
E)  5.0 × 10-6F) B) and D)
G) None of the above

Question 2

Calculate the pH of a solution prepared by dissolving 0.150 mol of acetic acid and 0.300 mol of sodium acetate in water sufficient to yield 1.00 L of solution. The Ka of acetic acid is 1.76 × 10-5.

Accepted Answer

A)  2.516
B)  3.892
C)  4.502
D)  10.158
E)  5.056F) A) and D)
G) B) and E)

Question 3

The pH of a solution that contains 0.818 M acetic acid (Ka = 1.76 × 10-5) and 0.182 M sodium acetate is __________.

Accepted Answer

A)  4.102
B)  5.407
C)  8.593
D)  8.370
E)  9.898F) A) and C)
G) A) and D)

Question 4

The pH of a solution prepared by dissolving 0.350 mol of solid dimethylamine hydrochloride ((CH3) 2NH2Cl) in 1.00 L of 1.10 M dimethylamine ((CH3) 2NH) is __________. The Kb for methylamine is 5.40 × 10-4. (Assume the final volume is 1.00 L.)

Accepted Answer

A)  1.66
B)  2.77
C)  11.23
D)  11.14
E)  none of the aboveF) B) and D)
G) A) and B)

Question 5

Calculate the pH of a solution that is 0.210 M in nitrous acid (HNO2) and 0.290 M in potassium nitrite (KNO2) . The acid dissociation constant of nitrous acid is 4.50 × 10-4.

Accepted Answer

A)  3.487
B)  3.210
C)  13.86
D)  10.51
E)  4.562F) A) and D)
G) A) and E)

Question 6

The concentration of fluoride ions in a saturated solution of barium fluoride is __________ M. The solubility product constant of BaF2 is 1.7 × 10-6.

Accepted Answer

A)  3.8 × 10-4
B)  3.0 × 10-3
C)  1.5 × 10-2
D)  7.5 × 10-3
E)  1.4 × 10-4F) All of the above
G) D) and E)

Question 7

Of the following solutions, which has the greatest buffering capacity?

Accepted Answer

A)  0.821 M HF and 0.217 M NaF
B)  0.821 M HF and 0.909 M NaF
C)  0.100 M HF and 0.217 M NaF
D)  0.121 M HF and 0.667 M NaF
E)  They are all buffer solutions and would all have the same capacity.F) A) and C)
G) A) and E)

Question 8

The Kb of ammonia is 1.76 × 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 __________.

Accepted Answer

A)  4.632
B)  9.246
C)  4.742
D)  9.372
E)  none of the aboveF) A) and B)
G) A) and C)

Question 9

A 25.0 mL sample of 0.723 M HClO4 is titrated with a 0.273 M KOH solution. The H3O+ concentration after the addition of 60.0 mL of KOH is __________ M.

Accepted Answer

A)  0.0181
B)  0.430
C)  0.0200
D)  0.273
E)  none of the aboveF) C) and E)
G) C) and D) C

Question 10

Calculate the percent ionization of formic acid (HCO2H) in a solution that is 0.311 M in formic acid and 0.189 M in sodium formate (NaHCO2) . The Ka of formic acid is 1.77 × 10-4.

Accepted Answer

A)  37.8
B)  0.0937
C)  11.3
D)  1.06 × 10-3
E)  3.529F) A) and B)
G) None of the above

Question 11

Of the following solutions, which has the greatest buffering capacity?

Accepted Answer

A)  0.521 M HC2H3O2 and 0.217 M NaC2H3O2
B)  0.821 M HC2H3O2 and 0.713 M NaC2H3O2
C)  0.365M HC2H3O2 and 0.497 M NaC2H3O2
D)  0.121 M HC2H3O2 and 0.116 M NaC2H3O2E) B) and C)
F) A) and B) B

Question 12

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

Accepted Answer

A)  Ca(NO3) 2
B)  CaF2
C)  CaCl2
D)  CaBr2
E)  CaI2F) A) and C)
G) B) and D)

Question 13

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

Accepted Answer

A)  0.181 M HCl
B)  0.0176 M NH3
C)  0.744 M LiNO3
D)  pure water
E)  0.181 M NaClF) A) and B)
G) D) and E)

Question 14

Human blood is __________.

Accepted Answer

A)  neutral
B)  very basic
C)  slightly acidic
D)  very acidic
E)  slightly basicF) A) and E)
G) A) and D)

Question 15

In which of the following aqueous solutions would you expect CuBr to have the highest solubility?

Accepted Answer

A)  pure water
B)  0.10 M AgNO3
C)  0.20 M NaBr
D)  0.15 M KBr
E)  0.10 M LiBrF) None of the above
G) A) and B)

Question 16

The addition of hydrofluoric acid and __________ to water produces a buffer solution.

Accepted Answer

A)  HCl
B)  NaNO3
C)  NaCl
D)  NaOH
E)  NaBrF) A) and B)
G) A) and C)

Question 17

A 25.0 mL sample of 0.150 M hypochlorous acid is titrated with a 0.150 M NaOH solution. What is the pH after 26.0 mL of base is added? The Ka of hypochlorous acid is 3.0 × 10-8.

Accepted Answer

A)  2.54
B)  11.47
C)  7.00
D)  7.51
E)  7.54F) B) and D)
G) A) and D)

Question 18

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

Accepted Answer

A)  NaI, HI
B)  KBr, HBr
C)  RbCl, HCl
D)  CsF, HF
E)  none of the aboveF) A) and E)
G) C) and D)

Question 19

Suppose you have just added 100.0 ml of a solution containing 0.5000 moles of acetic acid per liter to 400.0 ml of 0.5000 M NaOH. What is the final pH? The Ka of acetic acid is 1.77 × 10-5.

Accepted Answer

13.48

Question 20

Why does fluoride treatment render teeth more resistant to decay?

Accepted Answer

A)  Fluoride kills the bacteria in the mouth that make the acids that decay teeth.
B)  Fluoride stimulates production of tooth enamel to replace that lost to decay.
C)  Fluoride reduces saliva production, keeping teeth drier and thus reducing decay.
D)  Fluoride converts hydroxyapatite to fluoroapatite that is less reactive with acids.
E)  Fluoride dissolves plaque, reducing its decaying contact with teeth.F) A) and E)
G) B) and D)

Exam 17: Additional Aspects of Aqueous Equilibria

What is the molar solubility of silver sulfate (Ag2SO4) in water? The solubility-product constant for Ag2SO4 is 1.5 × 10-5 at 25°C.

Correct AnswerverifiedShow Answer

Calculate the pH of a solution prepared by dissolving 0.150 mol of acetic acid and 0.300 mol of sodium acetate in water sufficient to yield 1.00 L of solution. The Ka of acetic acid is 1.76 × 10-5.

Correct AnswerverifiedShow Answer

The pH of a solution that contains 0.818 M acetic acid (Ka = 1.76 × 10-5) and 0.182 M sodium acetate is __________.

Correct AnswerverifiedShow Answer

The pH of a solution prepared by dissolving 0.350 mol of solid dimethylamine hydrochloride ((CH3) 2NH2Cl) in 1.00 L of 1.10 M dimethylamine ((CH3) 2NH) is __________. The Kb for methylamine is 5.40 × 10-4. (Assume the final volume is 1.00 L.)

Correct AnswerverifiedShow Answer

Calculate the pH of a solution that is 0.210 M in nitrous acid (HNO2) and 0.290 M in potassium nitrite (KNO2) . The acid dissociation constant of nitrous acid is 4.50 × 10-4.

Correct AnswerverifiedShow Answer

The concentration of fluoride ions in a saturated solution of barium fluoride is __________ M. The solubility product constant of BaF2 is 1.7 × 10-6.

Correct AnswerverifiedShow Answer

Of the following solutions, which has the greatest buffering capacity?

Correct AnswerverifiedShow Answer

The Kb of ammonia is 1.76 × 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 __________.

Correct AnswerverifiedShow Answer

A 25.0 mL sample of 0.723 M HClO4 is titrated with a 0.273 M KOH solution. The H3O+ concentration after the addition of 60.0 mL of KOH is __________ M.

Correct AnswerverifiedC

Calculate the percent ionization of formic acid (HCO2H) in a solution that is 0.311 M in formic acid and 0.189 M in sodium formate (NaHCO2) . The Ka of formic acid is 1.77 × 10-4.

Correct AnswerverifiedShow Answer

Of the following solutions, which has the greatest buffering capacity?

Correct AnswerverifiedB

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Human blood is __________.

Correct AnswerverifiedShow Answer

In which of the following aqueous solutions would you expect CuBr to have the highest solubility?

Correct AnswerverifiedShow Answer

The addition of hydrofluoric acid and __________ to water produces a buffer solution.

Correct AnswerverifiedShow Answer

A 25.0 mL sample of 0.150 M hypochlorous acid is titrated with a 0.150 M NaOH solution. What is the pH after 26.0 mL of base is added? The Ka of hypochlorous acid is 3.0 × 10-8.

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Suppose you have just added 100.0 ml of a solution containing 0.5000 moles of acetic acid per liter to 400.0 ml of 0.5000 M NaOH. What is the final pH? The Ka of acetic acid is 1.77 × 10-5.

Correct Answerverified13.48

Why does fluoride treatment render teeth more resistant to decay?

Correct AnswerverifiedShow Answer

What is the molar solubility of silver sulfate (Ag₂SO₄) in water? The solubility-product constant for Ag₂SO₄ is 1.5 × 10^-5 at 25°C.

Correct Answer
verified

Calculate the pH of a solution prepared by dissolving 0.150 mol of acetic acid and 0.300 mol of sodium acetate in water sufficient to yield 1.00 L of solution. The K_a of acetic acid is 1.76 × 10^-5.

Correct Answer
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The pH of a solution that contains 0.818 M acetic acid (K_a = 1.76 × 10^-5) and 0.182 M sodium acetate is __________.

Correct Answer
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The pH of a solution prepared by dissolving 0.350 mol of solid dimethylamine hydrochloride ((CH₃) ₂NH₂Cl) in 1.00 L of 1.10 M dimethylamine ((CH₃) ₂NH) is __________. The K_b for methylamine is 5.40 × 10^-4. (Assume the final volume is 1.00 L.)

Correct Answer
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Calculate the pH of a solution that is 0.210 M in nitrous acid (HNO₂) and 0.290 M in potassium nitrite (KNO₂) . The acid dissociation constant of nitrous acid is 4.50 × 10^-4.

Correct Answer
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The concentration of fluoride ions in a saturated solution of barium fluoride is __________ M. The solubility product constant of BaF₂ is 1.7 × 10^-6.

Correct Answer
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Correct Answer
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The K_b of ammonia is 1.76 × 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 __________.

Correct Answer
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A 25.0 mL sample of 0.723 M HClO₄ is titrated with a 0.273 M KOH solution. The H₃O⁺ concentration after the addition of 60.0 mL of KOH is __________ M.

Correct Answer
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C

Calculate the percent ionization of formic acid (HCO₂H) in a solution that is 0.311 M in formic acid and 0.189 M in sodium formate (NaHCO₂) . The K_a of formic acid is 1.77 × 10^-4.

Correct Answer
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Correct Answer
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B

Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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A 25.0 mL sample of 0.150 M hypochlorous acid is titrated with a 0.150 M NaOH solution. What is the pH after 26.0 mL of base is added? The K_a of hypochlorous acid is 3.0 × 10^-8.

Correct Answer
verified

Correct Answer
verified

Suppose you have just added 100.0 ml of a solution containing 0.5000 moles of acetic acid per liter to 400.0 ml of 0.5000 M NaOH. What is the final pH? The K_a of acetic acid is 1.77 × 10^-5.

Correct Answer
verified
13.48

Correct Answer
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