Question 1

What change will be caused by addition of a small amount of HCl to a solution containing fluoride ions and hydrogen fluoride?

Accepted Answer

A)  The concentration of hydronium ions will increase significantly.
B)  The concentration of fluoride ions will increase as will the concentration of hydronium ions.
C)  The concentration of hydrogen fluoride will decrease and the concentration of fluoride ions will increase.
D)  The concentration of fluoride ion will decrease and the concentration of hydrogen fluoride will increase.
E)  The fluoride ions will precipitate out of solution as its acid salt.F) A) and E)
G) None of the above

Question 2

Calculate the percent ionization of nitrous acid in a solution that is 0.222 M in nitrous acid (HNO2) and 0.278 M in potassium nitrite (KNO2) . The acid dissociation constant of nitrous acid is 4.50 × 10-4.

Accepted Answer

A)  55.6
B)  0.162
C)  15.5
D)  2.78 × 10-3
E)  3.448F) All of the above
G) C) and D)

Question 3

Calculate the maximum concentration (in M) of magnesium ions (Mg+2) in a solution that contains 0.025 M of CO32-. The Ksp of MgCO3 is 3.5 × 10-8.

Accepted Answer

A)  1.8 × 10-5
B)  1.4 × 10-6
C)  2.8 × 10-6
D)  3.2 × 10-10
E)  8.1 × 10-12F) B) and E)
G) A) and B)

Question 4

A 50.0 mL sample of an aqueous H2SO4 solution is titrated with a 0.375 M NaOH solution. The equivalence point is reached with 62.5 mL of the base. The concentration of H2SO4 is __________ M.

Accepted Answer

A)  0.234
B)  0.469
C)  0.150
D)  0.300
E)  0.938F) None of the above
G) B) and D)

Question 5

An assembly of a metal ion and the Lewis bases bonded to it is called a __________.

Accepted Answer

The answer of An assembly of a metal ion and...

Question 6

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

Accepted Answer

A)  KI, HI
B)  AgBr, HBr
C)  CuCl, HCl
D)  CsI, HI
E)  none of the aboveF) A) and B)
G) B) and E)

Question 7

A 25.0 mL sample of a solution of a monoprotic acid is titrated with a 0.115 M NaOH solution. The titration curve above was obtained. Which of the following indicators would be best for this titration?

Accepted Answer

A)  methyl red
B)  bromthymol blue
C)  thymol blue
D)  phenolpthalein
E)  bromocresol purpleF) A) and B)
G) A) and C)

Question 8

In a solution, when the concentrations of a weak acid and its conjugate base are equal,

Accepted Answer

A)  the system is not at equilibrium.
B)  the buffering capacity is significantly decreased.
C)  the -log of the [H+] and the -log of the Ka are equal.
D)  all of the above are true.E) None of the above
F) All of the above

Question 9

Determine the Ksp for magnesium hydroxide (Mg(OH) 2) where the solubility of Mg(OH) 2 is 1.4 × 10-4 M.

Accepted Answer

A)  2.7 × 10-12
B)  1.1 × 10-11
C)  2.0 × 10-8
D)  3.9 × 10-8
E)  1.4 × 10-4F) B) and C)
G) B) and D)

Question 10

The solubility product of a compound is numerically equal to the product of the concentration of the ions involved in the equilibrium, each multiplied by its coefficient in the equilibrium reaction.

Accepted Answer

A) True 
 B)False

Question 11

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.

Accepted Answer

A) True 
 B)False

Question 12

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.

Accepted Answer

A)  0.4
B)  1 × 10-7
C)  0.7
D)  3 × 10-13
E)  4 × 10-2F) None of the above
G) A) and B)

Question 13

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

Accepted Answer

A)  pure water
B)  0.020 M BaCl2
C)  0.015 NaCl
D)  0.020 AgNO3
E)  0.020 KClF) A) and E)
G) None of the above

Question 14

The solubility of a slightly soluble salt is decreased by the presence of a second solute that provides a common ion to the system.

Accepted Answer

A) True 
 B)False

Question 15

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

Accepted Answer

A)  HONH2, HONH3Cl
B)  NaCl, HCl
C)  RbOH, HF
D)  KOH, HNO2
E)  H2SO3, KHSO3F) None of the above
G) B) and E)

Question 16

Metal oxides and hydroxides that are relatively insoluble in neutral water, but are soluble in both strongly acidic and strongly basic solutions are said to be __________.

Accepted Answer

The answer of Metal oxides and hydroxides that are relatively...

Question 17

The solubility of manganese (II) hydroxide (Mn(OH) 2) is 2.2 × 10-5 M. What is the Ksp of MnOH) 2?

Accepted Answer

A)  1.1 × 10-14
B)  4.3 × 10-14
C)  2.1 × 10-14
D)  4.8 × 10-10
E)  2.2 × 10-5F) B) and E)
G) B) and D)

Question 18

A 25.0-mL sample of 0.150 M butanoic acid is titrated with a 0.150 M NaOH solution. What is the pH before any base is added? The Ka of butanoic acid is 1.5 × 10-5.

Accepted Answer

A)  2.83
B)  1.5 × 10-3
C)  4.82
D)  4.00
E)  1.0 × 104F) A) and D)
G) B) and E)

Question 19

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

Accepted Answer

A)  HC6H5O
B)  NaOH
C)  NaCl
D)  C2H5NH2
E)  none of the aboveF) A) and C)
G) None of the above

Question 20

Calculate the percent ionization of formic acid (HCO2H) in a solution that is 0.219 M in formic acid. The Ka of formic acid is 1.77 × 10-4.

Accepted Answer

A)  3.94 × 10-5
B)  0.0180
C)  2.84
D)  0.280
E)  12.2F) All of the above
G) A) and D)

Exam 17: Additional Aspects of Aqueous Equilibria

The solubility of manganese (II) hydroxide (Mn(OH) 2) is 2.2 × 10-5 M. What is the Ksp of MnOH) 2?

Correct AnswerverifiedShow Answer

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.

Correct AnswerverifiedShow Answer

An assembly of a metal ion and the Lewis bases bonded to it is called a __________.

Correct AnswerverifiedShow Answer

A 25.0-mL sample of 0.150 M butanoic acid is titrated with a 0.150 M NaOH solution. What is the pH before any base is added? The Ka of butanoic acid is 1.5 × 10-5.

Correct AnswerverifiedShow Answer

A 50.0 mL sample of an aqueous H2SO4 solution is titrated with a 0.375 M NaOH solution. The equivalence point is reached with 62.5 mL of the base. The concentration of H2SO4 is __________ M.

Correct AnswerverifiedShow Answer

Calculate the maximum concentration (in M) of magnesium ions (Mg+2) in a solution that contains 0.025 M of CO32-. The Ksp of MgCO3 is 3.5 × 10-8.

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Metal oxides and hydroxides that are relatively insoluble in neutral water, but are soluble in both strongly acidic and strongly basic solutions are said to be __________.

Correct AnswerverifiedShow Answer

Calculate the percent ionization of nitrous acid in a solution that is 0.222 M in nitrous acid (HNO2) and 0.278 M in potassium nitrite (KNO2) . The acid dissociation constant of nitrous acid is 4.50 × 10-4.

Correct AnswerverifiedShow Answer

Calculate the percent ionization of formic acid (HCO2H) in a solution that is 0.219 M in formic acid. The Ka of formic acid is 1.77 × 10-4.

Correct AnswerverifiedShow Answer

Determine the Ksp for magnesium hydroxide (Mg(OH) 2) where the solubility of Mg(OH) 2 is 1.4 × 10-4 M.

Correct AnswerverifiedShow Answer

The solubility product of a compound is numerically equal to the product of the concentration of the ions involved in the equilibrium, each multiplied by its coefficient in the equilibrium reaction.

Correct AnswerverifiedShow Answer

What change will be caused by addition of a small amount of HCl to a solution containing fluoride ions and hydrogen fluoride?

Correct AnswerverifiedShow Answer

A 25.0 mL sample of a solution of a monoprotic acid is titrated with a 0.115 M NaOH solution. The titration curve above was obtained. Which of the following indicators would be best for this titration?

Correct AnswerverifiedShow Answer

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.

Correct AnswerverifiedShow Answer

The solubility of a slightly soluble salt is decreased by the presence of a second solute that provides a common ion to the system.

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

In a solution, when the concentrations of a weak acid and its conjugate base are equal,

Correct AnswerverifiedShow Answer

The solubility of manganese (II) hydroxide (Mn(OH) ₂) is 2.2 × 10^-5 M. What is the K_sp of MnOH) ₂?

Correct Answer
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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.

Correct Answer
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A 25.0-mL sample of 0.150 M butanoic acid is titrated with a 0.150 M NaOH solution. What is the pH before any base is added? The K_a of butanoic acid is 1.5 × 10^-5.

Correct Answer
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A 50.0 mL sample of an aqueous H₂SO₄ solution is titrated with a 0.375 M NaOH solution. The equivalence point is reached with 62.5 mL of the base. The concentration of H₂SO₄ is __________ M.

Correct Answer
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Calculate the maximum concentration (in M) of magnesium ions (Mg⁺²) in a solution that contains 0.025 M of CO₃²^-. The K_sp of MgCO₃ is 3.5 × 10^-8.

Correct Answer
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Calculate the percent ionization of nitrous acid in a solution that is 0.222 M in nitrous acid (HNO₂) and 0.278 M in potassium nitrite (KNO₂) . The acid dissociation constant of nitrous acid is 4.50 × 10^-4.

Correct Answer
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Calculate the percent ionization of formic acid (HCO₂H) in a solution that is 0.219 M in formic acid. The K_a of formic acid is 1.77 × 10^-4.

Correct Answer
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Determine the K_sp for magnesium hydroxide (Mg(OH) ₂) where the solubility of Mg(OH) ₂ is 1.4 × 10^-4 M.

Correct Answer
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