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?

A) 4.77 B) 4.71 C) 4.68 D) 4.62 E) None of these choices are correct. A) 4.77 B) 4.71 C) 4.68 D) 4.62 E) None of these choices are correct. B

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−

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 M 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 M C

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−

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

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

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 3COONa 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 3COONa

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

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. 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.

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

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 M 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 M

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

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 M 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 M

Exam 19: Ionic Equilibria in Aqueous Systems

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?

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(Multiple Choice)

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Question 1

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⁻

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(Multiple Choice)

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Question 2

Correct Answer:

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A solution is prepared by mixing 50.0 mL of 0.50 M Cu(NO₃)₂with 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? K_sp = 2.2 × 10⁻²⁰ for Cu(OH)₂, K_sp = 1.3 × 10⁻¹⁵for Co(OH)₂

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Question 3

Correct Answer:

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

(Multiple Choice)

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Question 4

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⁻

(Multiple Choice)

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Question 5

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

(True/False)

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Question 6

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

(Multiple Choice)

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Question 7

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

(Multiple Choice)

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Question 8

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.

(Multiple Choice)

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Question 9

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, K_sp = 6.5 × 10⁻⁶)

(Multiple Choice)

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Question 10

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

(Multiple Choice)

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Question 11

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?

(Multiple Choice)

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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?

(Multiple Choice)

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Question 13

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.

(True/False)

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Question 14

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?

(Multiple Choice)

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Question 15

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

(Multiple Choice)

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Question 16

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

(Multiple Choice)

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Question 17

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

(Multiple Choice)

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Question 18

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

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Question 19

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?

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Question 20

Showing 1 - 20 of 114

Exam 19: Ionic Equilibria in Aqueous Systems

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?

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−

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

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−

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

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

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

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.

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)

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

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?

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?

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.

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?

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

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

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

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

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?

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Three Major Classes of Chemical Reactions

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Transition Elements and Their Coordination Compounds

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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?

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⁻

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⁻

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

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

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.

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

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.

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

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

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?