Question 1

The solubility of lead(II)  chloride is 0.45 g/100 mL of solution. What is the Ksp of PbCl2?

Accepted Answer

A)  4.9 × 10 −2
B)  1.7 × 10 −5
C)  8.5 × 10 −6
D)  4.2 × 10 −6
E)  −6F) A) and B)
G) A) and C)

Question 2

When a weak acid is titrated with a weak base, the pH at the equivalence point

Accepted Answer

A)  is greater than 7.0.
B)  is equal to 7.0.
C)  is less than 7.0.
D)  is determined by the sizes of K a and K b.
E)  is no longer affected by addition of base.F) B) and C)
G) A) and B)

Question 3

A 50.0-mL sample of 0.50 M HCl is titrated with 0.50 M NaOH. What is the pH of the solution after 28.0 mL of NaOH have been added to the acid?

Accepted Answer

A)  0.85
B)  0.75
C)  0.66
D)  0.49
E)  3.8F) A) and D)
G) B) and E)

Question 4

You need to prepare a buffer solution with a pH of 4.00, using NaF and HF. What ratio of the ratio of [base]/[acid] should be used in making the buffer? For HF, Ka = 7.2 × 10−4.

Accepted Answer

A)  [base]/[acid] = 0.14
B)  [base]/[acid] = 0.42
C)  [base]/[acid] = 2.36
D)  [base]/[acid] = 7.20
E)  None of these choices are correct.F) A) and B)
G) B) and E)

Question 5

Write the ion product expression for magnesium fluoride, MgF2.

Accepted Answer

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Question 6

What is the [H3O+] in a buffer that consists of 0.30 M HCOOH and 0.20 M HCOONa? For HCOOH, Ka = 1.7 × 10−4

Accepted Answer

A)  1.1 × 10 −4  M
B)  2.6 × 10 −4  M
C)  4.3 × 10 −4 M
D)  6.7 × 10 −5 M
E)  None of these choices are correct.F) A) and C)
G) C) and E)

Question 7

The salts X(NO3) 2 and Y(NO3) 2 (where X+ and Y+ are metal ions)  are dissolved in water to give a solution which is 0.1 M in each of them. Using the Ksp values listed below, decide which aqueous reagent, if any, will definitely precipitate X+ before precipitating Y+ from solution. Given Ksp values:XCl2, 1 × 10−5 YCl2, 1 × 10−10 X(OH) 2, 1 × 10−10 Y(OH) 2, 1 × 10−5

Accepted Answer

A)  1 M NaCl
B)  1 M HCl
C)  1 M HNO 3
D)  1 M NaOH
E)  None of these choices are correct.F) A) and E)
G) B) and E)

Question 8

The salts X(NO3) 2 and Y(NO3) 2 (where X+ and Y+ are metal ions)  are dissolved in water to give a solution which is 0.1 M in each of them. Using the Ksp values listed below, decide which aqueous reagent, if any, will definitely precipitate X+ before precipitating Y+ from solution. Given Ksp values:XCl2, 1 × 10−5 YCl2, 1 × 10−10 X(OH) 2, 1 × 10−10 Y(OH) 2, 1 × 10−5

Accepted Answer

A)  1 M NH 3
B)  1 M HCl
C)  1 M HNO 3
D)  1 M NaCl
E)  None of these choices are correct.F) B) and E)
G) A) and B)

Question 9

Which one of the following is the best representation of the titration curve that will be obtained in the titration of a weak diprotic acid H2A (0.10 mol L−1)  with a strong base of the same concentration? 2A (0.10 mol L−1)  with a strong base of the same concentration?   A) A B) B C) C D) D E) E" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)  A
B)  B
C)  C
D)  D
E)  EF) B) and E)
G) None of the above

Question 10

What is the maximum amount of sodium sulfate that can be added to 1.00 L of 0.0020 M Ca(NO3) 2 before precipitation of calcium sulfate begins? Ksp = 2.4 × 10−5 for calcium sulfate.

Accepted Answer

A)  1.2 × 10 −2 mol
B)  4.9 × 10 −3 mol
C)  3.5 × 10 −3 mol
D)  1.2 × 10 −5 mol
E)  4.8 × 10 −8 molF) A) and D)
G) B) and E)

Question 11

A sample of a monoprotic acid (HA)  weighing 0.384 g is dissolved in water and the solution is titrated with aqueous NaOH. If 30.0 mL of 0.100 M NaOH is required to reach the equivalence point, what is the molar mass of HA?

Accepted Answer

A)  37.0 g/mol
B)  81.0 g/mol
C)  128 g/mol
D)  20.3 g/mol
E)  211 g/molF) C) and D)
G) A) and D)

Question 12

The salts X(NO3) 2 and Y(NO3) 2 (where X+ and Y+ are metal ions)  are dissolved in water to give a solution which is 0.1 M in each of them. Using the Ksp values listed below, decide which aqueous reagent, if any, will definitely precipitate X+ before precipitating Y+ from solution. Given Ksp values:XCl2, 1 × 10−5 YCl2, 1 × 10−10 X(OH) 2, 1 × 10−10 Y(OH) 2, 1 × 10−5

Accepted Answer

A)  1 M NaNO 3
B)  1 M HCl
C)  1 M HNO 3
D)  1 M NaCl
E)  None of these choices are correct.F) A) and B)
G) B) and C)

Question 13

What is the [H3O+] in a solution that consists of 1.2 M HClO and 2.3 M NaClO? Ka = 3.5 × 10−8

Accepted Answer

A)  7.8 × 10 −9  M
B)  1.8 × 10 −8  M
C)  6.7 × 10 −8  M
D)  1.6 × 10 −7  M
E)  None of these choices are correct.F) B) and C)
G) D) and E)

Question 14

A popular buffer solution consists of carbonate (CO32−)  and hydrogen carbonate (HCO3−)  conjugate acid-base pair. Which, if any, of the following such buffers can neutralize the greatest amount of added hydrochloric acid, while remaining within its buffer range?

Accepted Answer

A)  1 L of 0.9 M CO 3 2− and 0.1 M HCO 3 −
B)  1 L of 0.1 M CO 3 2− and 0.9 M HCO 3 −
C)  1 L of 0.5 M CO 3 2− and 0.5 M HCO 3 −
D)  1 L of 0.1 M CO32− and 0.1 M HCO3−
E)  They can all neutralize the same amount of hydrochloric acid.F) A) and E)
G) D) and E)

Exam 19: Ionic Equilibria in Aqueous Systems

When a weak acid is titrated with a weak base, the pH at the equivalence point

Correct Answer
verified

Which one of the following is the best representation of the titration curve that will be obtained in the titration of a weak diprotic acid H₂A (0.10 mol L⁻¹) with a strong base of the same concentration?

Correct Answer
verified

You need to prepare a buffer solution with a pH of 4.00, using NaF and HF. What ratio of the ratio of [base]/[acid] should be used in making the buffer? For HF, K_a = 7.2 × 10⁻⁴.

Correct Answer
verified

A sample of a monoprotic acid (HA) weighing 0.384 g is dissolved in water and the solution is titrated with aqueous NaOH. If 30.0 mL of 0.100 M NaOH is required to reach the equivalence point, what is the molar mass of HA?

Correct Answer
verified

A popular buffer solution consists of carbonate (CO₃²⁻) and hydrogen carbonate (HCO₃⁻) conjugate acid-base pair. Which, if any, of the following such buffers can neutralize the greatest amount of added hydrochloric acid, while remaining within its buffer range?

Correct Answer
verified

A 50.0-mL sample of 0.50 M HCl is titrated with 0.50 M NaOH. What is the pH of the solution after 28.0 mL of NaOH have been added to the acid?

Correct Answer
verified

What is the maximum amount of sodium sulfate that can be added to 1.00 L of 0.0020 M Ca(NO₃) ₂before precipitation of calcium sulfate begins? K_sp = 2.4 × 10⁻⁵ for calcium sulfate.

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

What is the [H₃O⁺] in a solution that consists of 1.2 M HClO and 2.3 M NaClO? K_a = 3.5 × 10⁻⁸

Correct Answer
verified

Correct Answer
verified

The solubility of lead(II) chloride is 0.45 g/100 mL of solution. What is the K_sp of PbCl₂?

Correct Answer
verified

Write the ion product expression for magnesium fluoride, MgF₂.

Correct Answer
verified

What is the [H₃O⁺] in a buffer that consists of 0.30 M HCOOH and 0.20 M HCOONa? For HCOOH, K_a = 1.7 × 10⁻⁴

Correct Answer
verified

Exam 19: Ionic Equilibria in Aqueous Systems

When a weak acid is titrated with a weak base, the pH at the equivalence point

Correct AnswerverifiedShow Answer

Which one of the following is the best representation of the titration curve that will be obtained in the titration of a weak diprotic acid H2A (0.10 mol L−1) with a strong base of the same concentration?

Correct AnswerverifiedShow Answer

You need to prepare a buffer solution with a pH of 4.00, using NaF and HF. What ratio of the ratio of [base]/[acid] should be used in making the buffer? For HF, Ka = 7.2 × 10−4.

Correct AnswerverifiedShow Answer

A sample of a monoprotic acid (HA) weighing 0.384 g is dissolved in water and the solution is titrated with aqueous NaOH. If 30.0 mL of 0.100 M NaOH is required to reach the equivalence point, what is the molar mass of HA?

Correct AnswerverifiedShow Answer

A popular buffer solution consists of carbonate (CO32−) and hydrogen carbonate (HCO3−) conjugate acid-base pair. Which, if any, of the following such buffers can neutralize the greatest amount of added hydrochloric acid, while remaining within its buffer range?

Correct AnswerverifiedShow Answer

A 50.0-mL sample of 0.50 M HCl is titrated with 0.50 M NaOH. What is the pH of the solution after 28.0 mL of NaOH have been added to the acid?

Correct AnswerverifiedShow Answer

What is the maximum amount of sodium sulfate that can be added to 1.00 L of 0.0020 M Ca(NO3) 2 before precipitation of calcium sulfate begins? Ksp = 2.4 × 10−5 for calcium sulfate.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

What is the [H3O+] in a solution that consists of 1.2 M HClO and 2.3 M NaClO? Ka = 3.5 × 10−8

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

The solubility of lead(II) chloride is 0.45 g/100 mL of solution. What is the Ksp of PbCl2?

Correct AnswerverifiedShow Answer

Write the ion product expression for magnesium fluoride, MgF2.

Correct AnswerverifiedShow Answer

What is the [H3O+] in a buffer that consists of 0.30 M HCOOH and 0.20 M HCOONa? For HCOOH, Ka = 1.7 × 10−4

Correct AnswerverifiedShow Answer

Correct Answer
verified

Which one of the following is the best representation of the titration curve that will be obtained in the titration of a weak diprotic acid H₂A (0.10 mol L⁻¹) with a strong base of the same concentration?

Correct Answer
verified

You need to prepare a buffer solution with a pH of 4.00, using NaF and HF. What ratio of the ratio of [base]/[acid] should be used in making the buffer? For HF, K_a = 7.2 × 10⁻⁴.

Correct Answer
verified

Correct Answer
verified

A popular buffer solution consists of carbonate (CO₃²⁻) and hydrogen carbonate (HCO₃⁻) conjugate acid-base pair. Which, if any, of the following such buffers can neutralize the greatest amount of added hydrochloric acid, while remaining within its buffer range?

Correct Answer
verified

Correct Answer
verified

What is the maximum amount of sodium sulfate that can be added to 1.00 L of 0.0020 M Ca(NO₃) ₂before precipitation of calcium sulfate begins? K_sp = 2.4 × 10⁻⁵ for calcium sulfate.

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

What is the [H₃O⁺] in a solution that consists of 1.2 M HClO and 2.3 M NaClO? K_a = 3.5 × 10⁻⁸

Correct Answer
verified

Correct Answer
verified

The solubility of lead(II) chloride is 0.45 g/100 mL of solution. What is the K_sp of PbCl₂?

Correct Answer
verified

Write the ion product expression for magnesium fluoride, MgF₂.

Correct Answer
verified

What is the [H₃O⁺] in a buffer that consists of 0.30 M HCOOH and 0.20 M HCOONa? For HCOOH, K_a = 1.7 × 10⁻⁴

Correct Answer
verified