The pH of a solution that contains 0.818 M acetic acid (Ka = 1.76 × 10- 5) and 0.172 M sodium acetate is _.

A) 8.57 B) 9.92 C) 4.08 D) 5.43 E) 8.37 A) 8.57 B) 9.92 C) 4.08 D) 5.43 E) 8.37

Calculate the pH of a solution prepared by dissolving 0.250 mol of benzoic acid (C7H5O2H) and 0.150 mol of sodium benzoate (NaC7H5O2) in water sufficient to yield 1.00 L of solution. The Ka of benzoic acid is 6.50 × 10- 5.

A) 4.19 B) 2.39 C) 10.0 D) 3.97 E) 4.41 A) 4.19 B) 2.39 C) 10.0 D) 3.97 E) 4.41

A 25.0 mL sample of 0.723 M HClO4 is titrated with a 0.27 M KOH solution. The H3O+ concentration after the addition of 80.0 mL of KOH is M.

A) 1.0 × 10- 7 B) 0.44 C) 2.8 × 10- 13 D) 0.72 E) 3.6 × 10- 2 A) 1.0 × 10- 7 B) 0.44 C) 2.8 × 10- 13 D) 0.72 E) 3.6 × 10- 2

What is the solubility (in M) of PbCl2 in a 0.15 M solution of HCl? The Ksp of PbCl2 is 1.6 × 10- 5. 78)

A) 1.8 × 10- 4 B) 1.6 × 10- 5 C) 7.1 × 10- 4 D) 2.0 × 10- 3 E) 1.1 × 10- 4 A) 1.8 × 10- 4 B) 1.6 × 10- 5 C) 7.1 × 10- 4 D) 2.0 × 10- 3 E) 1.1 × 10- 4

Of the substances below, will decrease the solubility of Pb(OH)2 in a saturated solution.

A) Pb(NO3)2 B) NaNO3 C) H2O2 D) NaCl E) HNO3 A) Pb(NO3)2 B) NaNO3 C) H2O2 D) NaCl E) HNO3

In which of the following aqueous solutions would you expect PbCl2to have the lowest solubility?

A) pure water B) 0.015 M NaCl C) 0.020 M KCl D) 0.015 M PbNO3 E) 0.020 M BaCl2 A) pure water B) 0.015 M NaCl C) 0.020 M KCl D) 0.015 M PbNO3 E) 0.020 M BaCl2

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.

A) 4.562 B) 3.490 C) 13.86 D) 10.51 E) 3.210 A) 4.562 B) 3.490 C) 13.86 D) 10.51 E) 3.210

Exam 17: Additional Aspects of Equilibria

A 25.0 mL sample of a solution of an unknown compound is titrated with a 0.115 M NaOH solution. The titration curve above was obtained. The unknown compound is .

(Multiple Choice)

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Question 41

A 25.0 mL sample of an acetic acid solution is titrated with a 0.175 M NaOH solution. The equivalence point is reached when 37.5 mL of the base is added. The concentration of acetic acid is M

(Multiple Choice)

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Question 42

What are the principal organs that regulate the pH of the carbonic acid- bicarbonate buffer system in the blood?

(Multiple Choice)

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Question 43

The K_bof ammonia is 1.77 × 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 .

(Multiple Choice)

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Question 44

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

(Multiple Choice)

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Question 45

The pH of a solution that contains 0.818 M acetic acid (K_a= 1.76 × 10^-⁵) and 0.172 M sodium acetate is _.

(Multiple Choice)

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Question 46

Calculate the pH of a solution prepared by dissolving 0.250 mol of benzoic acid (C₇H₅O₂H) and 0.150 mol of sodium benzoate (NaC₇H₅O₂) in water sufficient to yield 1.00 L of solution. The K_aof benzoic acid is 6.50 × 10^-⁵.

(Multiple Choice)

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Question 47

A 25.0 mL sample of 0.723 M HClO₄is titrated with a 0.27 M KOH solution. The H₃O⁺ concentration after the addition of 80.0 mL of KOH is M.

(Multiple Choice)

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Question 48

The solubility of slightly soluble salts containing basic anions is proportional to the pH of the solution.

(True/False)

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Question 49

A solution of HF is titrated with a 0.150 M NaOH solution. Based on the table above, the best indicator for this reaction is . The K_aof hydrofluoric acid is 6.8 × 10^-⁴.

(Multiple Choice)

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Question 50

What is the solubility (in M) of PbCl₂in a 0.15 M solution of HCl? The K_spof PbCl₂is 1.6 × 10^-⁵. 78)

(Multiple Choice)

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Question 51

The extent of ionization of a weak electrolyte is increased by adding to the solution a strong electrolyte that has an ion in common with the weak electrolyte.

(True/False)

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Question 52

Calculate the maximum concentration (in M) of silver ions (Ag⁺) in a solution that contains 0.025 M of CO₃²^-. The K_spof Ag₂CO₃is 8.1 × 10^-¹².

(Multiple Choice)

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Question 53

Why does fluoride treatment render teeth more resistant to decay?

(Multiple Choice)

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Question 54

The primary buffer system that controls the pH of the blood is the _ _ buffer system.

(Multiple Choice)

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Question 55

Of the substances below, will decrease the solubility of Pb(OH)₂in a saturated solution.

(Multiple Choice)

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Question 56

In which of the following aqueous solutions would you expect PbCl₂to have the lowest solubility?

(Multiple Choice)

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Question 57

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

(Multiple Choice)

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Question 58

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.

(Multiple Choice)

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Question 59

How many milliliters of 0.120 M NaOH are required to titrate 50.0 mL of 0.0998 M butanoic acid to the equivalence point? The K_aof butanoic acid is 1.5 × 10^-⁵.

(Multiple Choice)

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Question 60

Showing 41 - 60 of 88

Exam 17: Additional Aspects of Equilibria

A 25.0 mL sample of a solution of an unknown compound is titrated with a 0.115 M NaOH solution. The titration curve above was obtained. The unknown compound is .

A 25.0 mL sample of an acetic acid solution is titrated with a 0.175 M NaOH solution. The equivalence point is reached when 37.5 mL of the base is added. The concentration of acetic acid is M

What are the principal organs that regulate the pH of the carbonic acid- bicarbonate buffer system in the blood?

The Kb of ammonia is 1.77 × 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 solution containing which one of the following pairs of substances will be a buffer solution?

The pH of a solution that contains 0.818 M acetic acid (Ka = 1.76 × 10- 5) and 0.172 M sodium acetate is _.

Calculate the pH of a solution prepared by dissolving 0.250 mol of benzoic acid (C7H5O2H) and 0.150 mol of sodium benzoate (NaC7H5O2) in water sufficient to yield 1.00 L of solution. The Ka of benzoic acid is 6.50 × 10- 5.

A 25.0 mL sample of 0.723 M HClO4 is titrated with a 0.27 M KOH solution. The H3O+ concentration after the addition of 80.0 mL of KOH is M.

The solubility of slightly soluble salts containing basic anions is proportional to the pH of the solution.

A solution of HF is titrated with a 0.150 M NaOH solution. Based on the table above, the best indicator for this reaction is . The Ka of hydrofluoric acid is 6.8 × 10- 4.

What is the solubility (in M) of PbCl2 in a 0.15 M solution of HCl? The Ksp of PbCl2 is 1.6 × 10- 5. 78)

The extent of ionization of a weak electrolyte is increased by adding to the solution a strong electrolyte that has an ion in common with the weak electrolyte.

Calculate the maximum concentration (in M) of silver ions (Ag+) in a solution that contains 0.025 M of CO32- . The Ksp of Ag2CO3 is 8.1 × 10- 12.

Why does fluoride treatment render teeth more resistant to decay?

The primary buffer system that controls the pH of the blood is the _ _ buffer system.

Of the substances below, will decrease the solubility of Pb(OH)2 in a saturated solution.

In which of the following aqueous solutions would you expect PbCl2to have the lowest solubility?

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

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.

How many milliliters of 0.120 M NaOH are required to titrate 50.0 mL of 0.0998 M butanoic acid to the equivalence point? The Ka of butanoic acid is 1.5 × 10- 5.

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The K_bof ammonia is 1.77 × 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 .

The pH of a solution that contains 0.818 M acetic acid (K_a= 1.76 × 10^-⁵) and 0.172 M sodium acetate is _.

Calculate the pH of a solution prepared by dissolving 0.250 mol of benzoic acid (C₇H₅O₂H) and 0.150 mol of sodium benzoate (NaC₇H₅O₂) in water sufficient to yield 1.00 L of solution. The K_aof benzoic acid is 6.50 × 10^-⁵.

A 25.0 mL sample of 0.723 M HClO₄is titrated with a 0.27 M KOH solution. The H₃O⁺ concentration after the addition of 80.0 mL of KOH is M.

A solution of HF is titrated with a 0.150 M NaOH solution. Based on the table above, the best indicator for this reaction is . The K_aof hydrofluoric acid is 6.8 × 10^-⁴.

What is the solubility (in M) of PbCl₂in a 0.15 M solution of HCl? The K_spof PbCl₂is 1.6 × 10^-⁵. 78)

Calculate the maximum concentration (in M) of silver ions (Ag⁺) in a solution that contains 0.025 M of CO₃²^-. The K_spof Ag₂CO₃is 8.1 × 10^-¹².

Of the substances below, will decrease the solubility of Pb(OH)₂in a saturated solution.

In which of the following aqueous solutions would you expect PbCl₂to have the lowest solubility?

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.

How many milliliters of 0.120 M NaOH are required to titrate 50.0 mL of 0.0998 M butanoic acid to the equivalence point? The K_aof butanoic acid is 1.5 × 10^-⁵.