A solution is formed by mixing 50.0 mL of 10.00 M NaCN with 50.0 mL of 2.0 F1F1F1S1F1F1F10 10S1U1P1-3S1S1P0 M CuNOS1U1B13S1U1B0. Cu(I) forms complex ions with cyanide as follows: Calculate the following concentrations at equilibrium: -[Cu+]

A) 2.0 F1F1F1S1F1F1F10 10-13 M B) 8.0 F1F1F1S1F1F1F10 10-15 M C) 1.6 F1F1F1S1F1F1F10 10-13 M D) 4.0 F1F1F1S1F1F1F10 10-13 M E) none of these A) 2.0 F1F1F1S1F1F1F10 10-13 M B) 8.0 F1F1F1S1F1F1F10 10-15 M C) 1.6 F1F1F1S1F1F1F10 10-13 M D) 4.0 F1F1F1S1F1F1F10 10-13 M E) none of these B

Consider the titration of 100.0 mL of 0.250 M aniline (Kb = 3.8 F1F1F1S1F1F1F10 10-10) with 0.500 M HCl. Calculate the pH of the solution at the stoichiometric point.

A) 8.70 B) 2.68 C) 11.62 D) -0.85 E) none of these A) 8.70 B) 2.68 C) 11.62 D) -0.85 E) none of these B

A 100.0-mL sample of 0.2 M (CH3)3N (Kb = 5.3 F1F1F1S1F1F1F10 10-5) is titrated with 0.2 M HCl. What is the pH at the equivalence point?

A) 5.4 B) 7.0 C) 10.3 D) 3.1 E) 9.9 A) 5.4 B) 7.0 C) 10.3 D) 3.1 E) 9.9

The value of Kf for the complex ion Ag(NH3)2+ is 1.7 F1F1F1S1F1F1F10 107. Ksp for AgCl is 1.6 F1F1F1S1F1F1F10 10-10. Calculate the molar solubility of AgCl in 1.0 M NH3.

A) 1.7 F1F1F1S1F1F1F10 10-10 B) 2.9 F1F1F1S1F1F1F10 10-3 C) 4.7 F1F1F1S1F1F1F10 10-2 D) 1.3 F1F1F1S1F1F1F10 10-5 E) 5.2 F1F1F1S1F1F1F10 10-2 A) 1.7 F1F1F1S1F1F1F10 10-10 B) 2.9 F1F1F1S1F1F1F10 10-3 C) 4.7 F1F1F1S1F1F1F10 10-2 D) 1.3 F1F1F1S1F1F1F10 10-5 E) 5.2 F1F1F1S1F1F1F10 10-2

A 75.0-mL sample of 0.0500 M HCN (Ka = 6.2 F1F1F1S1F1F1F10 10-10) is titrated with 0.500 M NaOH. What is [H+] in the solution after 3.0 mL of 0.500 M NaOH has been added?

A) 9.3 F1F1F1S1F1F1F10 10-10 M B) 5.2 F1F1F1S1F1F1F10 10-13 M C) 1.0 F1F1F1S1F1F1F10 10-7 M D) 4.1 F1F1F1S1F1F1F10 10-10 M E) none of these A) 9.3 F1F1F1S1F1F1F10 10-10 M B) 5.2 F1F1F1S1F1F1F10 10-13 M C) 1.0 F1F1F1S1F1F1F10 10-7 M D) 4.1 F1F1F1S1F1F1F10 10-10 M E) none of these

Calculate the concentration of Ag+ in a saturated aqueous solution of Ag2CrO4. Ksp for Ag2CrO4 is 9.0 F1F1F1S1F1F1F10 10-12.

A) 9.0 F1F1F1S1F1F1F10 10-12 B) 2.6 F1F1F1S1F1F1F10 10-4 C) 2.1 F1F1F1S1F1F1F10 10-4 D) 1.3 F1F1F1S1F1F1F10 10-4 E) 6.5 F1F1F1S1F1F1F10 10-5 A) 9.0 F1F1F1S1F1F1F10 10-12 B) 2.6 F1F1F1S1F1F1F10 10-4 C) 2.1 F1F1F1S1F1F1F10 10-4 D) 1.3 F1F1F1S1F1F1F10 10-4 E) 6.5 F1F1F1S1F1F1F10 10-5

A 59.00-mL sample of 0.0650 M HCN (Ka = 6.2 F1F1F1S1F1F1F10 10-10) is titrated with 0.670 M NaOH. What volume of 0.670 M NaOH is required to reach the stoichiometric point?

A) 5.72 mL B) 59.0 mL C) 608 mL D) 0.00164 mL E) 3.84 mL A) 5.72 mL B) 59.0 mL C) 608 mL D) 0.00164 mL E) 3.84 mL

Consider a solution made by mixing 500.0 mL of 4.0 M NH3 and 500.0 mL of 0.40 M AgNO3. Ag+ reacts with NH3 to form AgNH3+ and Ag(NH3)2+: The concentration of Ag(NH3)2+ at equilibrium is

A) 0.20 M. B) 2.0 M. C) 0.40 M. D) 1.0 F1F1F1S1F1F1F10 10-3 M. E) none of these A) 0.20 M. B) 2.0 M. C) 0.40 M. D) 1.0 F1F1F1S1F1F1F10 10-3 M. E) none of these

The solubility of M(OH)2 in 0.010 M KOH is 1.0 F1F1F1S1F1F1F10 10-5 mol/L. What is Ksp for M(OH)2?

A) 1.0 F1F1F1S1F1F1F10 10-10 B) 4.0 F1F1F1S1F1F1F10 10-15 C) 1.0 F1F1F1S1F1F1F10 10-2 D) 1.0 F1F1F1S1F1F1F10 10-12 E) 1.0 F1F1F1S1F1F1F10 10-9 A) 1.0 F1F1F1S1F1F1F10 10-10 B) 4.0 F1F1F1S1F1F1F10 10-15 C) 1.0 F1F1F1S1F1F1F10 10-2 D) 1.0 F1F1F1S1F1F1F10 10-12 E) 1.0 F1F1F1S1F1F1F10 10-9

Calculate the pH of a solution that contains 3.25 M HCN (Ka = 6.2 F1F1F1S1F1F1F10 10-10), 1.00 M NaOH and 1.50 M NaCN.

A) 8.28 B) 7.46 C) 9.25 D) 8.86 E) none of these A) 8.28 B) 7.46 C) 9.25 D) 8.86 E) none of these

The solubility of Cd(OH)2 in water is 1.7 F1F1F1S1F1F1F10 10-5 mol/L at 25°C. What is Ksp for Cd(OH)2?

A) 5.8 F1F1F1S1F1F1F10F1F1F1S1F1F1F1010-10 B) 2.9 F1F1F1S1F1F1F10 10-10 C) 4.9 F1F1F1S1F1F1F10 10-15 D) 2.0 F1F1F1S1F1F1F10 10-14 E) none of these A) 5.8 F1F1F1S1F1F1F10F1F1F1S1F1F1F1010-10 B) 2.9 F1F1F1S1F1F1F10 10-10 C) 4.9 F1F1F1S1F1F1F10 10-15 D) 2.0 F1F1F1S1F1F1F10 10-14 E) none of these

A solution containing 10. mmol of CO32- and 5.0 mmol of HCO3- is titrated with 1.0 M HCl. What volume of HCl must be added to reach the first equivalence point?

A) 5.0 mL B) 15 mL C) 10. Ml D) 25 mL E) 20. mL A) 5.0 mL B) 15 mL C) 10. Ml D) 25 mL E) 20. mL

Calculate the pH when 200.0 mL of a 1.00 M solution of HS1U1B12S1U1B0A (KS1U1B1a1S1U1B0 = 1.0 F1F1F1S1F1F1F10 10S1U1P1-S1S1P0S1U1P16S1S1P0, KS1U1B1a2S1U1B0 = 1.0 F1F1F1S1F1F1F10 10S1U1P1-S1S1P0S1U1P110S1S1P0) is titrated with the following volumes of 1.00 M NaOH. -600.0 mL of 1.00 M NaOH

A) 11.70 B) 10.00 C) 14.00 D) 13.40 E) None of these A) 11.70 B) 10.00 C) 14.00 D) 13.40 E) None of these

Consider a solution of 2.0 M HCN and 1.0 M NaCN (Ka for HCN = 6.2 F1F1F1S1F1F1F10 10-10). Which of the following statements is true?

A) The solution is not a buffer because [HCN] is not equal to [CN-]. B) [OH-] > [H+] C) The pH will be below 7.00 because the concentration of the acid is greater than that of the base. D) The buffer will be more resistant to pH changes from addition of strong acid than to pH changes from addition of strong base. E) All of these statements are false. A) The solution is not a buffer because [HCN] is not equal to [CN-]. B) [OH-] > [H+] C) The pH will be below 7.00 because the concentration of the acid is greater than that of the base. D) The buffer will be more resistant to pH changes from addition of strong acid than to pH changes from addition of strong base. E) All of these statements are false.

A 50.0-mL sample of 2.0 F1F1F1S1F1F1F10 10-4 M CuNO3 is added to 50.0 mL of 4.0 M NaCN. Cu+ reacts with CN- to form the complex ion Cu(CN)32-: Calculate the solubility of CuBr(s) (Ksp = 1.0 F1F1F1S1F1F1F10 10-5) in 1.0 L of 1.0 M NaCN.

A) 0.33 mol/L B) 1.0 F1F1F1S1F1F1F10 10-6 mol/L C) 1.0 F1F1F1S1F1F1F10 103 mol/L D) 1.0 mol/L E) none of these A) 0.33 mol/L B) 1.0 F1F1F1S1F1F1F10 10-6 mol/L C) 1.0 F1F1F1S1F1F1F10 103 mol/L D) 1.0 mol/L E) none of these

Exam 8: Applications of Aqueous Equilibria

A solution is formed by mixing 50.0 mL of 10.00 M NaCN with 50.0 mL of 2.0  10^-3 M CuNO₃. Cu(I) forms complex ions with cyanide as follows: Calculate the following concentrations at equilibrium: -[Cu⁺]

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Question 1

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A 0.210-g sample of an acid (molar mass = 192 g/mol) is titrated with 30.5 mL of 0.108 M NaOH to a phenolphthalein endpoint. The formula of the acid is

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Question 2

Correct Answer:

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Consider the titration of 100.0 mL of 0.250 M aniline (K_b = 3.8  10^-¹⁰) with 0.500 M HCl. Calculate the pH of the solution at the stoichiometric point.

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Question 3

Correct Answer:

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A 100.0-mL sample of 0.2 M (CH₃)₃N (K_b = 5.3  10^-⁵) is titrated with 0.2 M HCl. What is the pH at the equivalence point?

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Question 4

The value of K_f for the complex ion Ag(NH₃)₂⁺ is 1.7  10⁷. K_sp for AgCl is 1.6  10^-¹⁰. Calculate the molar solubility of AgCl in 1.0 M NH₃.

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Question 5

A 75.0-mL sample of 0.0500 M HCN (K_a = 6.2  10^-¹⁰) is titrated with 0.500 M NaOH. What is [H⁺] in the solution after 3.0 mL of 0.500 M NaOH has been added?

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Question 6

Derive the equation describing the relationship between the pH at the first equivalence point and the K_a values of the diprotic weak acid being titrated with NaOH.

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Question 7

Calculate the concentration of Ag⁺ in a saturated aqueous solution of Ag₂CrO₄. K_sp for Ag₂CrO₄ is 9.0  10^-¹².

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Question 8

A 59.00-mL sample of 0.0650 M HCN (K_a = 6.2  10^-¹⁰) is titrated with 0.670 M NaOH. What volume of 0.670 M NaOH is required to reach the stoichiometric point?

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Question 9

Consider a solution made by mixing 500.0 mL of 4.0 M NH₃ and 500.0 mL of 0.40 M AgNO₃. Ag⁺ reacts with NH₃ to form AgNH₃⁺ and Ag(NH₃)₂⁺: The concentration of Ag(NH₃)₂⁺ at equilibrium is

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Question 10

A solution contains 10. mmol of H₃PO₄ and 5.0 mmol of NaH₂PO₄. How many milliliters of 0.10 M NaOH must be added to reach the second equivalence point of the titration of the H₃PO₄ with NaOH?

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Question 11

The solubility of M(OH)₂ in 0.010 M KOH is 1.0  10^-⁵ mol/L. What is K_sp for M(OH)₂?

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Question 12

Calculate the pH of a solution that contains 3.25 M HCN (K_a = 6.2  10^-¹⁰), 1.00 M NaOH and 1.50 M NaCN.

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Question 13

The solubility of Cd(OH)₂ in water is 1.7  10^-⁵ mol/L at 25°C. What is K_sp for Cd(OH)₂?

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Question 14

A 200.0-mL sample of the weak acid H₃A (0.100 M) is titrated with 0.200 M NaOH. What are the major species at each of the following points in the titration? (Water is always assumed to be a major species.) -After 75.0 mL of 0.200 M NaOH is added

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Question 15

A solution containing 10. mmol of CO₃²^- and 5.0 mmol of HCO₃^- is titrated with 1.0 M HCl. What volume of HCl must be added to reach the first equivalence point?

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Question 16

Calculate the pH when 200.0 mL of a 1.00 M solution of H₂A (K_a1 = 1.0  10^-⁶, K_a2 = 1.0  10^-¹⁰) is titrated with the following volumes of 1.00 M NaOH. -600.0 mL of 1.00 M NaOH

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Question 17

Consider a solution of 2.0 M HCN and 1.0 M NaCN (K_a for HCN = 6.2  10^-¹⁰). Which of the following statements is true?

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Question 18

A 50.0-mL sample of 2.0  10^-⁴ M CuNO₃ is added to 50.0 mL of 4.0 M NaCN. Cu⁺ reacts with CN^- to form the complex ion Cu(CN)₃²^-: Calculate the solubility of CuBr(s) (K_sp = 1.0  10^-⁵) in 1.0 L of 1.0 M NaCN.

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Question 19

What quantity of NaOH(s) must be added to 1.00 L of 0.200 M HCl to achieve a pH of 12.00? (Assume no volume change.)

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Question 20

Showing 1 - 20 of 171

A solution is formed by mixing 50.0 mL of 10.00 M NaCN with 50.0 mL of 2.0  10^-3 M CuNO₃. Cu(I) forms complex ions with cyanide as follows: Calculate the following concentrations at equilibrium: -[Cu⁺]

A 0.210-g sample of an acid (molar mass = 192 g/mol) is titrated with 30.5 mL of 0.108 M NaOH to a phenolphthalein endpoint. The formula of the acid is

Consider the titration of 100.0 mL of 0.250 M aniline (K_b = 3.8  10^-¹⁰) with 0.500 M HCl. Calculate the pH of the solution at the stoichiometric point.

A 100.0-mL sample of 0.2 M (CH₃)₃N (K_b = 5.3  10^-⁵) is titrated with 0.2 M HCl. What is the pH at the equivalence point?

The value of K_f for the complex ion Ag(NH₃)₂⁺ is 1.7  10⁷. K_sp for AgCl is 1.6  10^-¹⁰. Calculate the molar solubility of AgCl in 1.0 M NH₃.

A 75.0-mL sample of 0.0500 M HCN (K_a = 6.2  10^-¹⁰) is titrated with 0.500 M NaOH. What is [H⁺] in the solution after 3.0 mL of 0.500 M NaOH has been added?

Derive the equation describing the relationship between the pH at the first equivalence point and the K_a values of the diprotic weak acid being titrated with NaOH.

Calculate the concentration of Ag⁺ in a saturated aqueous solution of Ag₂CrO₄. K_sp for Ag₂CrO₄ is 9.0  10^-¹².

A 59.00-mL sample of 0.0650 M HCN (K_a = 6.2  10^-¹⁰) is titrated with 0.670 M NaOH. What volume of 0.670 M NaOH is required to reach the stoichiometric point?

Consider a solution made by mixing 500.0 mL of 4.0 M NH₃ and 500.0 mL of 0.40 M AgNO₃. Ag⁺ reacts with NH₃ to form AgNH₃⁺ and Ag(NH₃)₂⁺: The concentration of Ag(NH₃)₂⁺ at equilibrium is

A solution contains 10. mmol of H₃PO₄ and 5.0 mmol of NaH₂PO₄. How many milliliters of 0.10 M NaOH must be added to reach the second equivalence point of the titration of the H₃PO₄ with NaOH?

The solubility of M(OH)₂ in 0.010 M KOH is 1.0  10^-⁵ mol/L. What is K_sp for M(OH)₂?

Calculate the pH of a solution that contains 3.25 M HCN (K_a = 6.2  10^-¹⁰), 1.00 M NaOH and 1.50 M NaCN.

The solubility of Cd(OH)₂ in water is 1.7  10^-⁵ mol/L at 25°C. What is K_sp for Cd(OH)₂?

A 200.0-mL sample of the weak acid H₃A (0.100 M) is titrated with 0.200 M NaOH. What are the major species at each of the following points in the titration? (Water is always assumed to be a major species.) -After 75.0 mL of 0.200 M NaOH is added

A solution containing 10. mmol of CO₃²^- and 5.0 mmol of HCO₃^- is titrated with 1.0 M HCl. What volume of HCl must be added to reach the first equivalence point?

Calculate the pH when 200.0 mL of a 1.00 M solution of H₂A (K_a1 = 1.0  10^-⁶, K_a2 = 1.0  10^-¹⁰) is titrated with the following volumes of 1.00 M NaOH. -600.0 mL of 1.00 M NaOH

Consider a solution of 2.0 M HCN and 1.0 M NaCN (K_a for HCN = 6.2  10^-¹⁰). Which of the following statements is true?

A 50.0-mL sample of 2.0  10^-⁴ M CuNO₃ is added to 50.0 mL of 4.0 M NaCN. Cu⁺ reacts with CN^- to form the complex ion Cu(CN)₃²^-: Calculate the solubility of CuBr(s) (K_sp = 1.0  10^-⁵) in 1.0 L of 1.0 M NaCN.

What quantity of NaOH(s) must be added to 1.00 L of 0.200 M HCl to achieve a pH of 12.00? (Assume no volume change.)

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Exam 8: Applications of Aqueous Equilibria

A solution is formed by mixing 50.0 mL of 10.00 M NaCN with 50.0 mL of 2.0  10-3 M CuNO3. Cu(I) forms complex ions with cyanide as follows: Calculate the following concentrations at equilibrium: -[Cu+]

A 0.210-g sample of an acid (molar mass = 192 g/mol) is titrated with 30.5 mL of 0.108 M NaOH to a phenolphthalein endpoint. The formula of the acid is

Consider the titration of 100.0 mL of 0.250 M aniline (Kb = 3.8  10-10) with 0.500 M HCl. Calculate the pH of the solution at the stoichiometric point.

A 100.0-mL sample of 0.2 M (CH3)3N (Kb = 5.3  10-5) is titrated with 0.2 M HCl. What is the pH at the equivalence point?

The value of Kf for the complex ion Ag(NH3)2+ is 1.7  107. Ksp for AgCl is 1.6  10-10. Calculate the molar solubility of AgCl in 1.0 M NH3.

A 75.0-mL sample of 0.0500 M HCN (Ka = 6.2  10-10) is titrated with 0.500 M NaOH. What is [H+] in the solution after 3.0 mL of 0.500 M NaOH has been added?

Derive the equation describing the relationship between the pH at the first equivalence point and the Ka values of the diprotic weak acid being titrated with NaOH.

Calculate the concentration of Ag+ in a saturated aqueous solution of Ag2CrO4. Ksp for Ag2CrO4 is 9.0  10-12.

A 59.00-mL sample of 0.0650 M HCN (Ka = 6.2  10-10) is titrated with 0.670 M NaOH. What volume of 0.670 M NaOH is required to reach the stoichiometric point?

Consider a solution made by mixing 500.0 mL of 4.0 M NH3 and 500.0 mL of 0.40 M AgNO3. Ag+ reacts with NH3 to form AgNH3+ and Ag(NH3)2+: The concentration of Ag(NH3)2+ at equilibrium is

A solution contains 10. mmol of H3PO4 and 5.0 mmol of NaH2PO4. How many milliliters of 0.10 M NaOH must be added to reach the second equivalence point of the titration of the H3PO4 with NaOH?

The solubility of M(OH)2 in 0.010 M KOH is 1.0  10-5 mol/L. What is Ksp for M(OH)2?

Calculate the pH of a solution that contains 3.25 M HCN (Ka = 6.2  10-10), 1.00 M NaOH and 1.50 M NaCN.

The solubility of Cd(OH)2 in water is 1.7  10-5 mol/L at 25°C. What is Ksp for Cd(OH)2?

A 200.0-mL sample of the weak acid H3A (0.100 M) is titrated with 0.200 M NaOH. What are the major species at each of the following points in the titration? (Water is always assumed to be a major species.) -After 75.0 mL of 0.200 M NaOH is added

A solution containing 10. mmol of CO32- and 5.0 mmol of HCO3- is titrated with 1.0 M HCl. What volume of HCl must be added to reach the first equivalence point?

Calculate the pH when 200.0 mL of a 1.00 M solution of H2A (Ka1 = 1.0  10-6, Ka2 = 1.0  10-10) is titrated with the following volumes of 1.00 M NaOH. -600.0 mL of 1.00 M NaOH

Consider a solution of 2.0 M HCN and 1.0 M NaCN (Ka for HCN = 6.2  10-10). Which of the following statements is true?

A 50.0-mL sample of 2.0  10-4 M CuNO3 is added to 50.0 mL of 4.0 M NaCN. Cu+ reacts with CN- to form the complex ion Cu(CN)32-: Calculate the solubility of CuBr(s) (Ksp = 1.0  10-5) in 1.0 L of 1.0 M NaCN.

What quantity of NaOH(s) must be added to 1.00 L of 0.200 M HCl to achieve a pH of 12.00? (Assume no volume change.)

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A solution is formed by mixing 50.0 mL of 10.00 M NaCN with 50.0 mL of 2.0  10^-3 M CuNO₃. Cu(I) forms complex ions with cyanide as follows: Calculate the following concentrations at equilibrium: -[Cu⁺]

Consider the titration of 100.0 mL of 0.250 M aniline (K_b = 3.8  10^-¹⁰) with 0.500 M HCl. Calculate the pH of the solution at the stoichiometric point.

A 100.0-mL sample of 0.2 M (CH₃)₃N (K_b = 5.3  10^-⁵) is titrated with 0.2 M HCl. What is the pH at the equivalence point?

The value of K_f for the complex ion Ag(NH₃)₂⁺ is 1.7  10⁷. K_sp for AgCl is 1.6  10^-¹⁰. Calculate the molar solubility of AgCl in 1.0 M NH₃.

A 75.0-mL sample of 0.0500 M HCN (K_a = 6.2  10^-¹⁰) is titrated with 0.500 M NaOH. What is [H⁺] in the solution after 3.0 mL of 0.500 M NaOH has been added?

Derive the equation describing the relationship between the pH at the first equivalence point and the K_a values of the diprotic weak acid being titrated with NaOH.

Calculate the concentration of Ag⁺ in a saturated aqueous solution of Ag₂CrO₄. K_sp for Ag₂CrO₄ is 9.0  10^-¹².

A 59.00-mL sample of 0.0650 M HCN (K_a = 6.2  10^-¹⁰) is titrated with 0.670 M NaOH. What volume of 0.670 M NaOH is required to reach the stoichiometric point?

Consider a solution made by mixing 500.0 mL of 4.0 M NH₃ and 500.0 mL of 0.40 M AgNO₃. Ag⁺ reacts with NH₃ to form AgNH₃⁺ and Ag(NH₃)₂⁺: The concentration of Ag(NH₃)₂⁺ at equilibrium is

A solution contains 10. mmol of H₃PO₄ and 5.0 mmol of NaH₂PO₄. How many milliliters of 0.10 M NaOH must be added to reach the second equivalence point of the titration of the H₃PO₄ with NaOH?

The solubility of M(OH)₂ in 0.010 M KOH is 1.0  10^-⁵ mol/L. What is K_sp for M(OH)₂?

Calculate the pH of a solution that contains 3.25 M HCN (K_a = 6.2  10^-¹⁰), 1.00 M NaOH and 1.50 M NaCN.

The solubility of Cd(OH)₂ in water is 1.7  10^-⁵ mol/L at 25°C. What is K_sp for Cd(OH)₂?

A 200.0-mL sample of the weak acid H₃A (0.100 M) is titrated with 0.200 M NaOH. What are the major species at each of the following points in the titration? (Water is always assumed to be a major species.) -After 75.0 mL of 0.200 M NaOH is added

A solution containing 10. mmol of CO₃²^- and 5.0 mmol of HCO₃^- is titrated with 1.0 M HCl. What volume of HCl must be added to reach the first equivalence point?

Calculate the pH when 200.0 mL of a 1.00 M solution of H₂A (K_a1 = 1.0  10^-⁶, K_a2 = 1.0  10^-¹⁰) is titrated with the following volumes of 1.00 M NaOH. -600.0 mL of 1.00 M NaOH

Consider a solution of 2.0 M HCN and 1.0 M NaCN (K_a for HCN = 6.2  10^-¹⁰). Which of the following statements is true?

A 50.0-mL sample of 2.0  10^-⁴ M CuNO₃ is added to 50.0 mL of 4.0 M NaCN. Cu⁺ reacts with CN^- to form the complex ion Cu(CN)₃²^-: Calculate the solubility of CuBr(s) (K_sp = 1.0  10^-⁵) in 1.0 L of 1.0 M NaCN.