A solution containing 10. mmol of CO32- and 5.0 mmol of HCO3- is titrated with 1)0 M HCl.What total volume of HCl must be added to reach the second equivalence point?

A) 20ml B) 5.0 mL C) 30. mL D) 10. mL E) 25 mL A) 20ml B) 5.0 mL C) 30. mL D) 10. mL E) 25 mL

Equal volumes of 0.1 M HCl and 0.1 M HC2H3O2 are titrated with 0.1 M NaOH. Which of the following would be equal for both titrations?

A) the pH at the equivalence point B) the volume of NaOH added to reach the equivalence point C) the initial pH D) the pH at the halfway point E) two of the above A) the pH at the equivalence point B) the volume of NaOH added to reach the equivalence point C) the initial pH D) the pH at the halfway point E) two of the above

For carbonic acid (H2CO3), Ka1 = 4.30 × 10-7 and Ka2 = 5.62 × 10-11. Calculate the pH of a 0.50 M solution of Na2CO3.

A) 11.97 B) 8.31 C) 10.67 D) 2.03 E) 3.33 A) 11.97 B) 8.31 C) 10.67 D) 2.03 E) 3.33

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

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

A solution is formed by mixing 50.0 mL of 10.00 M NaCN with 50.0 mL of 2.0 × 10S1U1P1-3S1S1P0 M CuNOS1U1B13S1U1B0. Cu(I) forms complex ions with cyanide as follows: Calculate the following concentrations at equilibrium: -[Cu(CN)2-]

A) 1.0 × 10-3 M B) 4.0 × 10-12 M C) 2.0 × 10-7 M D) 2.0 × 10-3 M E) none of these A) 1.0 × 10-3 M B) 4.0 × 10-12 M C) 2.0 × 10-7 M D) 2.0 × 10-3 M E) none of these

The overall Kf for the complex ion Ag(NH3)2+ is 1.7 × 107. Ksp for AgI is 1.5 × 10-16. What is the molar solubility of AgI in a solution that is 2.0 M in NH3?

A) 1.3 × 10-3 B) 1.5 × 10-9 C) 1.0 × 10-4 D) 8.4 × 10-5 E) 5.8 × 10-12 A) 1.3 × 10-3 B) 1.5 × 10-9 C) 1.0 × 10-4 D) 8.4 × 10-5 E) 5.8 × 10-12

How many moles of CaF2 will dissolve in 3.0 L of 0.050 M NaF solution? (Ksp for CaF2 = 4.0 × 10-11)

A) 4.8 × 10-8 mol B) 8.9 × 10-9 mol C) 8.0 × 10-8 mol D) 2.7 × 10-8 mol E) none of these A) 4.8 × 10-8 mol B) 8.9 × 10-9 mol C) 8.0 × 10-8 mol D) 2.7 × 10-8 mol E) none of these

The concentration of Mg2+ in seawater is 0.052 M. At what pH will 99% of the Mg2+ be precipitated as the hydroxide? (Ksp for Mg(OH)2 = 8.9 × 10-12)

A) 6.50 B) 9.22 C) 10.12 D) 8.35 E) 4.86 A) 6.50 B) 9.22 C) 10.12 D) 8.35 E) 4.86

The solubility of Fe(OH)2 in water is 7.9 × 10-6 mol/L at 25° C. What is Ksp for Fe(OH)2 at 25° C?

A) 4.9 × 10-16 B) 6.2 × 10-11 C) 2.5 × 10-10 D) 2.0 × 10-15 E) none of these A) 4.9 × 10-16 B) 6.2 × 10-11 C) 2.5 × 10-10 D) 2.0 × 10-15 E) none of these

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.100.0 mL of 1.00 M NaOH

A) 3.35 B) 8.00 C) 3.00 D) 6.00 E) none of these A) 3.35 B) 8.00 C) 3.00 D) 6.00 E) none of these

Exam 8: Applications of Aqueous Equilibria

Consider the following information about the diprotic acid ascorbic acid (H₂As for short, molar mass = 176.1). The titration curve for disodium ascorbate, Na₂As, with standard HCl is shown below: -What major species is(are) present at point III?

(Multiple Choice)

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Question 21

You have two salts, AgX and AgY, with very similar K_sp values. You know that K_a for HX is much greater than K_a for HY. Which salt is more soluble in acidic solution?

(Multiple Choice)

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Question 22

Given the following values of equilibrium constants: What is the value of the equilibrium constant for the following reaction? Cu(OH)₂(s) + 4NH₃(aq) Cu(NH₃)₄²⁺(aq) + 2OH^-(aq)

(Multiple Choice)

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Question 23

Sodium chloride is added slowly to a solution that is 0.010 M in Cu⁺, Ag⁺, and Au⁺. The K_sp values for the chloride salts are 1.9 × 10^-7, 1.6 × 10^-10, and 2.0 × 10^-13, respectively. Which compound will precipitate first?

(Multiple Choice)

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Question 24

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.)

(Multiple Choice)

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Question 25

Methyl orange is an indicator with a K_a of 1 × 10^-4. Its acid form, HIn, is red, while its base form, In^-, is yellow. At pH 6.0, the indicator will be

(Multiple Choice)

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Question 26

A solution containing 10. mmol of CO₃^2- and 5.0 mmol of HCO₃^- is titrated with 1)0 M HCl.What total volume of HCl must be added to reach the second equivalence point?

(Multiple Choice)

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Question 27

Equal volumes of 0.1 M HCl and 0.1 M HC₂H₃O₂ are titrated with 0.1 M NaOH. Which of the following would be equal for both titrations?

(Multiple Choice)

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Question 28

For carbonic acid (H₂CO₃), K_a1 = 4.30 × 10^-7 and K_a2 = 5.62 × 10^-11. Calculate the pH of a 0.50 M solution of Na₂CO₃.

(Multiple Choice)

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Question 29

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⁺]

(Multiple Choice)

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Question 30

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 350.0 mL of 0.200 M NaOH is added

(Multiple Choice)

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Question 31

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(CN)₂^-]

(Multiple Choice)

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Question 32

In the titration of 250.0 mL of 0.20 M H₃PO₄ with 0.10 M NaOH, the pH of the solution after the addition of some NaOH is 4.66. Which of the following phosphate-containing species is present in the largest amount? For H₃PO₄, K_a1 = 7.5 × 10^-3, K_a2 = 6.2 × 10^-8, and K_a3 = 4.8 × 10^-13.

(Multiple Choice)

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Question 33

The overall K_f for the complex ion Ag(NH₃)₂⁺ is 1.7 × 10⁷. K_sp for AgI is 1.5 × 10^-16. What is the molar solubility of AgI in a solution that is 2.0 M in NH₃?

(Multiple Choice)

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Question 34

How many moles of CaF₂ will dissolve in 3.0 L of 0.050 M NaF solution? (K_sp for CaF₂ = 4.0 × 10^-11)

(Multiple Choice)

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Question 35

The concentration of Mg²⁺ in seawater is 0.052 M. At what pH will 99% of the Mg²⁺ be precipitated as the hydroxide? (K_sp for Mg(OH)₂ = 8.9 × 10^-12)

(Multiple Choice)

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Question 36

The solubility of Fe(OH)₂ in water is 7.9 × 10^-6 mol/L at 25° C. What is K_sp for Fe(OH)₂ at 25° C?

(Multiple Choice)

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Question 37

The two salts AgX and AgY have very similar solubilities in water. The salt AgX is much more soluble in acid than is AgY. What can be said about the relative strengths of the acids HX and HY?

(Multiple Choice)

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Question 38

How much solid NaCN must be added to 1.0 L of a 0.5 M HCN solution to produce a solution with pH 7.0? K_a = 6.2 × 10^-10 for HCN.

(Multiple Choice)

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Question 39

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.100.0 mL of 1.00 M NaOH

(Multiple Choice)

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Question 40

Showing 21 - 40 of 177

Consider the following information about the diprotic acid ascorbic acid (H₂As for short, molar mass = 176.1). The titration curve for disodium ascorbate, Na₂As, with standard HCl is shown below: -What major species is(are) present at point III?

You have two salts, AgX and AgY, with very similar K_sp values. You know that K_a for HX is much greater than K_a for HY. Which salt is more soluble in acidic solution?

Given the following values of equilibrium constants: What is the value of the equilibrium constant for the following reaction? Cu(OH)₂(s) + 4NH₃(aq) Cu(NH₃)₄²⁺(aq) + 2OH^-(aq)

Sodium chloride is added slowly to a solution that is 0.010 M in Cu⁺, Ag⁺, and Au⁺. The K_sp values for the chloride salts are 1.9 × 10^-7, 1.6 × 10^-10, and 2.0 × 10^-13, respectively. Which compound will precipitate first?

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.)

Methyl orange is an indicator with a K_a of 1 × 10^-4. Its acid form, HIn, is red, while its base form, In^-, is yellow. At pH 6.0, the indicator will be

A solution containing 10. mmol of CO₃^2- and 5.0 mmol of HCO₃^- is titrated with 1)0 M HCl.What total volume of HCl must be added to reach the second equivalence point?

Equal volumes of 0.1 M HCl and 0.1 M HC₂H₃O₂ are titrated with 0.1 M NaOH. Which of the following would be equal for both titrations?

For carbonic acid (H₂CO₃), K_a1 = 4.30 × 10^-7 and K_a2 = 5.62 × 10^-11. Calculate the pH of a 0.50 M solution of Na₂CO₃.

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 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 350.0 mL of 0.200 M NaOH is added

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(CN)₂^-]

In the titration of 250.0 mL of 0.20 M H₃PO₄ with 0.10 M NaOH, the pH of the solution after the addition of some NaOH is 4.66. Which of the following phosphate-containing species is present in the largest amount? For H₃PO₄, K_a1 = 7.5 × 10^-3, K_a2 = 6.2 × 10^-8, and K_a3 = 4.8 × 10^-13.

The overall K_f for the complex ion Ag(NH₃)₂⁺ is 1.7 × 10⁷. K_sp for AgI is 1.5 × 10^-16. What is the molar solubility of AgI in a solution that is 2.0 M in NH₃?

How many moles of CaF₂ will dissolve in 3.0 L of 0.050 M NaF solution? (K_sp for CaF₂ = 4.0 × 10^-11)

The concentration of Mg²⁺ in seawater is 0.052 M. At what pH will 99% of the Mg²⁺ be precipitated as the hydroxide? (K_sp for Mg(OH)₂ = 8.9 × 10^-12)

The solubility of Fe(OH)₂ in water is 7.9 × 10^-6 mol/L at 25° C. What is K_sp for Fe(OH)₂ at 25° C?

The two salts AgX and AgY have very similar solubilities in water. The salt AgX is much more soluble in acid than is AgY. What can be said about the relative strengths of the acids HX and HY?

How much solid NaCN must be added to 1.0 L of a 0.5 M HCN solution to produce a solution with pH 7.0? K_a = 6.2 × 10^-10 for HCN.

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.100.0 mL of 1.00 M NaOH

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Exam 8: Applications of Aqueous Equilibria

Consider the following information about the diprotic acid ascorbic acid (H2As for short, molar mass = 176.1). The titration curve for disodium ascorbate, Na2As, with standard HCl is shown below: -What major species is(are) present at point III?

You have two salts, AgX and AgY, with very similar Ksp values. You know that Ka for HX is much greater than Ka for HY. Which salt is more soluble in acidic solution?

Given the following values of equilibrium constants: What is the value of the equilibrium constant for the following reaction? Cu(OH)2(s) + 4NH3(aq) Cu(NH3)42+(aq) + 2OH-(aq)

Sodium chloride is added slowly to a solution that is 0.010 M in Cu+, Ag+, and Au+. The Ksp values for the chloride salts are 1.9 × 10-7, 1.6 × 10-10, and 2.0 × 10-13, respectively. Which compound will precipitate first?

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.)

Methyl orange is an indicator with a Ka of 1 × 10-4. Its acid form, HIn, is red, while its base form, In-, is yellow. At pH 6.0, the indicator will be

A solution containing 10. mmol of CO32- and 5.0 mmol of HCO3- is titrated with 1)0 M HCl.What total volume of HCl must be added to reach the second equivalence point?

Equal volumes of 0.1 M HCl and 0.1 M HC2H3O2 are titrated with 0.1 M NaOH. Which of the following would be equal for both titrations?

For carbonic acid (H2CO3), Ka1 = 4.30 × 10-7 and Ka2 = 5.62 × 10-11. Calculate the pH of a 0.50 M solution of Na2CO3.

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 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 350.0 mL of 0.200 M NaOH is added

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(CN)2-]

In the titration of 250.0 mL of 0.20 M H3PO4 with 0.10 M NaOH, the pH of the solution after the addition of some NaOH is 4.66. Which of the following phosphate-containing species is present in the largest amount? For H3PO4, Ka1 = 7.5 × 10-3, Ka2 = 6.2 × 10-8, and Ka3 = 4.8 × 10-13.

The overall Kf for the complex ion Ag(NH3)2+ is 1.7 × 107. Ksp for AgI is 1.5 × 10-16. What is the molar solubility of AgI in a solution that is 2.0 M in NH3?

How many moles of CaF2 will dissolve in 3.0 L of 0.050 M NaF solution? (Ksp for CaF2 = 4.0 × 10-11)

The concentration of Mg2+ in seawater is 0.052 M. At what pH will 99% of the Mg2+ be precipitated as the hydroxide? (Ksp for Mg(OH)2 = 8.9 × 10-12)

The solubility of Fe(OH)2 in water is 7.9 × 10-6 mol/L at 25° C. What is Ksp for Fe(OH)2 at 25° C?

The two salts AgX and AgY have very similar solubilities in water. The salt AgX is much more soluble in acid than is AgY. What can be said about the relative strengths of the acids HX and HY?

How much solid NaCN must be added to 1.0 L of a 0.5 M HCN solution to produce a solution with pH 7.0? Ka = 6.2 × 10-10 for HCN.

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.100.0 mL of 1.00 M NaOH

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Consider the following information about the diprotic acid ascorbic acid (H₂As for short, molar mass = 176.1). The titration curve for disodium ascorbate, Na₂As, with standard HCl is shown below: -What major species is(are) present at point III?

You have two salts, AgX and AgY, with very similar K_sp values. You know that K_a for HX is much greater than K_a for HY. Which salt is more soluble in acidic solution?

Given the following values of equilibrium constants: What is the value of the equilibrium constant for the following reaction? Cu(OH)₂(s) + 4NH₃(aq) Cu(NH₃)₄²⁺(aq) + 2OH^-(aq)

Sodium chloride is added slowly to a solution that is 0.010 M in Cu⁺, Ag⁺, and Au⁺. The K_sp values for the chloride salts are 1.9 × 10^-7, 1.6 × 10^-10, and 2.0 × 10^-13, respectively. Which compound will precipitate first?

Methyl orange is an indicator with a K_a of 1 × 10^-4. Its acid form, HIn, is red, while its base form, In^-, is yellow. At pH 6.0, the indicator will be

A solution containing 10. mmol of CO₃^2- and 5.0 mmol of HCO₃^- is titrated with 1)0 M HCl.What total volume of HCl must be added to reach the second equivalence point?

Equal volumes of 0.1 M HCl and 0.1 M HC₂H₃O₂ are titrated with 0.1 M NaOH. Which of the following would be equal for both titrations?

For carbonic acid (H₂CO₃), K_a1 = 4.30 × 10^-7 and K_a2 = 5.62 × 10^-11. Calculate the pH of a 0.50 M solution of Na₂CO₃.

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 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 350.0 mL of 0.200 M NaOH is added

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(CN)₂^-]

In the titration of 250.0 mL of 0.20 M H₃PO₄ with 0.10 M NaOH, the pH of the solution after the addition of some NaOH is 4.66. Which of the following phosphate-containing species is present in the largest amount? For H₃PO₄, K_a1 = 7.5 × 10^-3, K_a2 = 6.2 × 10^-8, and K_a3 = 4.8 × 10^-13.

The overall K_f for the complex ion Ag(NH₃)₂⁺ is 1.7 × 10⁷. K_sp for AgI is 1.5 × 10^-16. What is the molar solubility of AgI in a solution that is 2.0 M in NH₃?

How many moles of CaF₂ will dissolve in 3.0 L of 0.050 M NaF solution? (K_sp for CaF₂ = 4.0 × 10^-11)

The concentration of Mg²⁺ in seawater is 0.052 M. At what pH will 99% of the Mg²⁺ be precipitated as the hydroxide? (K_sp for Mg(OH)₂ = 8.9 × 10^-12)

The solubility of Fe(OH)₂ in water is 7.9 × 10^-6 mol/L at 25° C. What is K_sp for Fe(OH)₂ at 25° C?

How much solid NaCN must be added to 1.0 L of a 0.5 M HCN solution to produce a solution with pH 7.0? K_a = 6.2 × 10^-10 for HCN.

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.100.0 mL of 1.00 M NaOH