Question 1

The end point in a titration is defined as the point when the indicator changes color.

Accepted Answer

A) True 
 B)False

Question 2

Calculate the solubility of lead(II)  iodide, PbI2, in 0.025 M KI. Ksp = 7.9 × 10−9

Accepted Answer

A)  4.5 × 10 −2  M
B)  2.8 × 10 −2  M
C)  8.9 × 10 −5  M
D)  5.0 × 10 −5  M
E)  1.3 × 10 −5  MF) A) and B)
G) B) and D)

Question 3

A solution is prepared by adding 4.50 mol of sodium hydroxide to 1.00 L of 1.00 M Co(NO3) 2. What is the equilibrium concentration of cobalt ions? Kf = 5.0 × 109 for Co(OH) 42−

Accepted Answer

A)  1.1 × 10 −2 M
B)  1.4 × 10 −5 M
C)  3.2 × 10 −9 M
D)  2.0 × 10 −10 M
E)  4.9 × 10 −13 MF) B) and D)
G) C) and D) C

Question 4

A formic acid buffer containing 0.50 M HCOOH and 0.50 M HCOONa has a pH of 3.77. What will the pH be after 0.010 mol of NaOH has been added to 100.0 mL of the buffer?

Accepted Answer

A)  3.67
B)  3.78
C)  3.81
D)  3.85
E)  3.95F) D) and E)
G) B) and D)

Question 5

A buffer is prepared by adding 1.00 L of 1.0 M HCl to 750 mL of 1.5 M NaHCOO. What is the pH of this buffer? Ka = 1.7 × 10−4

Accepted Answer

A)  2.87
B)  3.72
C)  3.82
D)  3.95
E)  4.66F) None of the above
G) A) and C)

Question 6

The indicator propyl red has Ka = 3.3 × 10−6. What would be the approximate pH range over which it would change color?

Accepted Answer

A)  3.5−5.5
B)  4.5−6.5
C)  5.5−7.5
D)  6.5−8.5
E)  None of these choices are correct.F) A) and B)
G) A) and D)

Question 7

Calculate the solubility of strontium fluoride, SrF2, in pure water. Ksp = 2.6 × 10−9

Accepted Answer

A)  1.4 × 10 −3  M
B)  3.4 × 10 −4  M
C)  8.7 × 10 −4  M
D)  5.1 × 10 −5  M
E)  −5  MF) All of the above
G) B) and D)

Question 8

Calculate the solubility of zinc hydroxide, Zn(OH) 2, in 1.00 M NaOH. Ksp = 3.0 × 10−16 for Zn(OH) 2, Kf = 3.0 × 1015 for Zn(OH) 42−

Accepted Answer

A)  0.60 M
B)  0.52 M
C)  0.37 M
D)  0.32 M
E)  0.24 MF) A) and B)
G) A) and C)

Question 9

A 35.0-mL sample of 0.20 M LiOH is titrated with 0.25 M HCl. What is the pH of the solution after 23.0 mL of HCl have been added to the base?

Accepted Answer

A)  1.26
B)  1.67
C)  12.33
D)  12.74
E)  13.03F) A) and E)
G) None of the above

Question 10

Buffer solutions with the component concentrations shown below were prepared. Which of them should have the lowest pH?

Accepted Answer

A)  [CH3COOH] = 0.25 M, [CH3COO−] = 0.25 M
B)  [CH 3COOH] = 0.75 M, [CH 3COO −] = 0.75 M
C)  [CH 3COOH] = 0.75 M, [CH 3COO −] = 0.25 M
D)  [CH 3COOH] = 0.25 M, [CH 3COO −] = 0.75 M
E)  [CH 3COOH] = 1.00 M, [CH 3COO −] = 1.00 MF) A) and D)
G) A) and C)

Question 11

What is the maximum mass of KCl that can be added to 1.0 L of a 0.010 M lead(II)  chloride solution without causing any precipitation of lead(II)  chloride? Assume that addition of KCl does not affect the solution volume. For lead(II)  chloride, Ksp = 1.6 × 10−5.

Accepted Answer

A)  3.0 g
B)  1.5 g
C)  0.8 g
D)  1.0 g
E)  0.2 gF) A) and E)
G) A) and B)

Question 12

A buffer is prepared by adding 100 mL of 0.50 M sodium hydroxide to 100 mL of 0.75 M propanoic acid. Is this a buffer solution, and if so, what is its pH?

Accepted Answer

A)  It is a buffer, pH > pK a of propanoic acid.
B)  It is a buffer, pH a of propanoic acid.
C)  It is a buffer, pH = pK a of propanoic acid.
D)  It is a buffer, pH = pK b of sodium propanoate.
E)  Since sodium hydroxide is a strong base, this is not a buffer.F) B) and E)
G) B) and C)

Question 13

The solubility of salt MX (solubility product constant Ksp) in water will always be greater than that of salt MX3 (solubility product constant K'sp) provided that Ksp > K'sp.

Accepted Answer

A) True 
 B)False

Question 14

When a strong 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 equal to the p K a of the acid.
E)  is equal to the p K b of the base.F) B) and E)
G) All of the above

Question 15

A solution is prepared by mixing 50.0 mL of 0.50 M Cu(NO3) 2 with 50.0 mL of 0.50 M Co(NO3) 2. Sodium hydroxide is added to the mixture. Which hydroxide precipitates first and what concentration of hydroxide ions present in solution will accomplish the separation? Ksp = 2.2 × 10−20 for Cu(OH) 2, Ksp = 1.3 × 10−15 for Co(OH) 2

Accepted Answer

A)  Co(OH) 2; [OH −] = 6.9 × 10 −6 M
B)  Co(OH) 2; [OH −] = 2.6 × 10 −7 M
C)  Cu(OH) 2; [OH −] = 1.8 × 10 −7 M
D)  Cu(OH) 2; [OH −] = 1.1 × 10 −9 M
E)  Cu(OH) 2; [OH −] = 1.0 × 10 −17 MF) A) and C)
G) A) and E) D

Question 16

Consider the dissolution of MnS in water (Ksp = 3.0 × 10−14) . MnS(s)  + H2O(l)  ⇄ Mn2+(aq)  + HS−(aq)  + OH−(aq) 
How is the solubility of manganese(II)  sulfide affected by the addition of aqueous potassium hydroxide to the system?

Accepted Answer

A)  The solubility will be unchanged.
B)  The solubility will decrease.
C)  The solubility will increase.
D)  The amount of KOH added must be known before its effect can be predicted.
E)  The p K a of H 2S is needed before a reliable prediction can be made.F) A) and C)
G) D) and E)

Question 17

When a strong acid is titrated with a strong 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, but is not 3.5.
D)  is equal to the p K a of the acid.
E)  is equal to 3.5.F) A) and B)
G) A) and C)

Question 18

An acetic acid buffer containing 0.50 M CH3COOH and 0.50 M CH3COONa has a pH of 4.74. What will the pH be after 0.0020 mol of HCl has been added to 100.0 mL of the buffer?

Accepted Answer

A)  4.77
B)  4.71
C)  4.68
D)  4.62
E)  None of these choices are correct.F) None of the above
G) A) and E) B

Question 19

Which one of the following pairs of 0.100 mol L−1 solutions, when mixed, will produce a buffer solution?

Accepted Answer

A)  50. mL of aqueous CH 3COOH and 25. mL of aqueous HCl
B)  50. mL of aqueous CH 3COOH and 100. mL of aqueous NaOH
C)  50. mL of aqueous NaOH and 25. mL of aqueous HCl
D)  50. mL of aqueous CH 3COONa and 25. mL of aqueous NaOH
E)  50. mL of aqueous CH 3COOH and 25. mL of aqueous CH 3COONaF) C) and D)
G) B) and E)

Question 20

A saturated solution of calcium hydroxide, Ca(OH) 2, is in contact with excess solid Ca(OH) 2. Which of the following statements correctly describes what will happen when aqueous HCl (a strong acid)  is added to this mixture, and system returns to equilibrium? (For Ca(OH) 2, Ksp = 6.5 × 10−6)

Accepted Answer

A)  The solubility of Ca(OH) 2 will be unchanged.
B)  The OH − concentration will decrease and the Ca 2+ concentration will increase.
C)  The OH − concentration will increase and the Ca 2+ concentration will decrease.
D)  The concentrations of both Ca 2+ and OH − will increase.
E)  The solubility of Ca(OH) 2 will decrease.F) C) and D)
G) B) and E)

Exam 19: Ionic Equilibria in Aqueous Systems

The end point in a titration is defined as the point when the indicator changes color.

Correct Answer
verified

Calculate the solubility of lead(II) iodide, PbI₂, in 0.025 M KI. K_sp = 7.9 × 10⁻⁹

Correct Answer
verified

A solution is prepared by adding 4.50 mol of sodium hydroxide to 1.00 L of 1.00 M Co(NO₃) ₂. What is the equilibrium concentration of cobalt ions? K_f= 5.0 × 10⁹ for Co(OH) ₄²⁻

Correct Answer
verified
C

A formic acid buffer containing 0.50 M HCOOH and 0.50 M HCOONa has a pH of 3.77. What will the pH be after 0.010 mol of NaOH has been added to 100.0 mL of the buffer?

Correct Answer
verified

A buffer is prepared by adding 1.00 L of 1.0 M HCl to 750 mL of 1.5 M NaHCOO. What is the pH of this buffer? K_a = 1.7 × 10⁻⁴

Correct Answer
verified

The indicator propyl red has K_a = 3.3 × 10⁻⁶. What would be the approximate pH range over which it would change color?

Correct Answer
verified

Calculate the solubility of strontium fluoride, SrF₂, in pure water. K_sp = 2.6 × 10⁻⁹

Correct Answer
verified

Calculate the solubility of zinc hydroxide, Zn(OH) ₂, in 1.00 M NaOH. K_sp = 3.0 × 10⁻¹⁶ for Zn(OH) ₂, Kf = 3.0 × 10¹⁵ for Zn(OH) ₄²⁻

Correct Answer
verified

A 35.0-mL sample of 0.20 M LiOH is titrated with 0.25 M HCl. What is the pH of the solution after 23.0 mL of HCl have been added to the base?

Correct Answer
verified

Buffer solutions with the component concentrations shown below were prepared. Which of them should have the lowest pH?

Correct Answer
verified

What is the maximum mass of KCl that can be added to 1.0 L of a 0.010 M lead(II) chloride solution without causing any precipitation of lead(II) chloride? Assume that addition of KCl does not affect the solution volume. For lead(II) chloride, K_sp = 1.6 × 10⁻⁵.

Correct Answer
verified

A buffer is prepared by adding 100 mL of 0.50 M sodium hydroxide to 100 mL of 0.75 M propanoic acid. Is this a buffer solution, and if so, what is its pH?

Correct Answer
verified

The solubility of salt MX (solubility product constant K_sp) in water will always be greater than that of salt MX₃ (solubility product constant K'_sp) provided that K_sp > K'_sp.

Correct Answer
verified

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

Correct Answer
verified

Correct Answer
verified
D

Consider the dissolution of MnS in water (K_sp = 3.0 × 10⁻¹⁴) . MnS(s) + H₂O(l) ⇄ Mn²⁺(aq) + HS⁻(aq) + OH⁻(aq) How is the solubility of manganese(II) sulfide affected by the addition of aqueous potassium hydroxide to the system?

Correct Answer
verified

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

Correct Answer
verified

An acetic acid buffer containing 0.50 M CH₃COOH and 0.50 M CH₃COONa has a pH of 4.74. What will the pH be after 0.0020 mol of HCl has been added to 100.0 mL of the buffer?

Correct Answer
verified
B

Which one of the following pairs of 0.100 mol L⁻¹ solutions, when mixed, will produce a buffer solution?

Correct Answer
verified

Correct Answer
verified

Exam 19: Ionic Equilibria in Aqueous Systems

The end point in a titration is defined as the point when the indicator changes color.

Correct AnswerverifiedShow Answer

Calculate the solubility of lead(II) iodide, PbI2, in 0.025 M KI. Ksp = 7.9 × 10−9

Correct AnswerverifiedShow Answer

A solution is prepared by adding 4.50 mol of sodium hydroxide to 1.00 L of 1.00 M Co(NO3) 2. What is the equilibrium concentration of cobalt ions? Kf = 5.0 × 109 for Co(OH) 42−

Correct AnswerverifiedC

A formic acid buffer containing 0.50 M HCOOH and 0.50 M HCOONa has a pH of 3.77. What will the pH be after 0.010 mol of NaOH has been added to 100.0 mL of the buffer?

Correct AnswerverifiedShow Answer

A buffer is prepared by adding 1.00 L of 1.0 M HCl to 750 mL of 1.5 M NaHCOO. What is the pH of this buffer? Ka = 1.7 × 10−4

Correct AnswerverifiedShow Answer

The indicator propyl red has Ka = 3.3 × 10−6. What would be the approximate pH range over which it would change color?

Correct AnswerverifiedShow Answer

Calculate the solubility of strontium fluoride, SrF2, in pure water. Ksp = 2.6 × 10−9

Correct AnswerverifiedShow Answer

Calculate the solubility of zinc hydroxide, Zn(OH) 2, in 1.00 M NaOH. Ksp = 3.0 × 10−16 for Zn(OH) 2, Kf = 3.0 × 1015 for Zn(OH) 42−

Correct AnswerverifiedShow Answer

A 35.0-mL sample of 0.20 M LiOH is titrated with 0.25 M HCl. What is the pH of the solution after 23.0 mL of HCl have been added to the base?

Correct AnswerverifiedShow Answer

Buffer solutions with the component concentrations shown below were prepared. Which of them should have the lowest pH?

Correct AnswerverifiedShow Answer

What is the maximum mass of KCl that can be added to 1.0 L of a 0.010 M lead(II) chloride solution without causing any precipitation of lead(II) chloride? Assume that addition of KCl does not affect the solution volume. For lead(II) chloride, Ksp = 1.6 × 10−5.

Correct AnswerverifiedShow Answer

A buffer is prepared by adding 100 mL of 0.50 M sodium hydroxide to 100 mL of 0.75 M propanoic acid. Is this a buffer solution, and if so, what is its pH?

Correct AnswerverifiedShow Answer

The solubility of salt MX (solubility product constant Ksp) in water will always be greater than that of salt MX3 (solubility product constant K'sp) provided that Ksp > K'sp.

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Correct AnswerverifiedD

Consider the dissolution of MnS in water (Ksp = 3.0 × 10−14) . MnS(s) + H2O(l) ⇄ Mn2+(aq) + HS−(aq) + OH−(aq) How is the solubility of manganese(II) sulfide affected by the addition of aqueous potassium hydroxide to the system?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

An acetic acid buffer containing 0.50 M CH3COOH and 0.50 M CH3COONa has a pH of 4.74. What will the pH be after 0.0020 mol of HCl has been added to 100.0 mL of the buffer?

Correct AnswerverifiedB

Which one of the following pairs of 0.100 mol L−1 solutions, when mixed, will produce a buffer solution?

Correct AnswerverifiedShow Answer

A saturated solution of calcium hydroxide, Ca(OH) 2, is in contact with excess solid Ca(OH) 2. Which of the following statements correctly describes what will happen when aqueous HCl (a strong acid) is added to this mixture, and system returns to equilibrium? (For Ca(OH) 2, Ksp = 6.5 × 10−6)

Correct AnswerverifiedShow Answer

Correct Answer
verified

Calculate the solubility of lead(II) iodide, PbI₂, in 0.025 M KI. K_sp = 7.9 × 10⁻⁹

Correct Answer
verified

A solution is prepared by adding 4.50 mol of sodium hydroxide to 1.00 L of 1.00 M Co(NO₃) ₂. What is the equilibrium concentration of cobalt ions? K_f= 5.0 × 10⁹ for Co(OH) ₄²⁻

Correct Answer
verified
C

Correct Answer
verified

A buffer is prepared by adding 1.00 L of 1.0 M HCl to 750 mL of 1.5 M NaHCOO. What is the pH of this buffer? K_a = 1.7 × 10⁻⁴

Correct Answer
verified

The indicator propyl red has K_a = 3.3 × 10⁻⁶. What would be the approximate pH range over which it would change color?

Correct Answer
verified

Calculate the solubility of strontium fluoride, SrF₂, in pure water. K_sp = 2.6 × 10⁻⁹

Correct Answer
verified

Calculate the solubility of zinc hydroxide, Zn(OH) ₂, in 1.00 M NaOH. K_sp = 3.0 × 10⁻¹⁶ for Zn(OH) ₂, Kf = 3.0 × 10¹⁵ for Zn(OH) ₄²⁻

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

What is the maximum mass of KCl that can be added to 1.0 L of a 0.010 M lead(II) chloride solution without causing any precipitation of lead(II) chloride? Assume that addition of KCl does not affect the solution volume. For lead(II) chloride, K_sp = 1.6 × 10⁻⁵.

Correct Answer
verified

Correct Answer
verified

The solubility of salt MX (solubility product constant K_sp) in water will always be greater than that of salt MX₃ (solubility product constant K'_sp) provided that K_sp > K'_sp.

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified
D

Consider the dissolution of MnS in water (K_sp = 3.0 × 10⁻¹⁴) . MnS(s) + H₂O(l) ⇄ Mn²⁺(aq) + HS⁻(aq) + OH⁻(aq) How is the solubility of manganese(II) sulfide affected by the addition of aqueous potassium hydroxide to the system?

Correct Answer
verified

Correct Answer
verified

An acetic acid buffer containing 0.50 M CH₃COOH and 0.50 M CH₃COONa has a pH of 4.74. What will the pH be after 0.0020 mol of HCl has been added to 100.0 mL of the buffer?

Correct Answer
verified
B

Which one of the following pairs of 0.100 mol L⁻¹ solutions, when mixed, will produce a buffer solution?

Correct Answer
verified

Correct Answer
verified