Calculate the minimum concentration of 100.0 mL of sodium sulfate that is required to form a precipitate with 100.0 mL of 1.00 F1F1F1S1F1F1F10 10-2 M calcium nitrate. Ksp for CaSO4 is 6.1 F1F1F1S1F1F1F10 10-5.

A) 6.10 F1F1F1S1F1F1F10 10-5 B) 3.10 F1F1F1S1F1F1F10 10-3 C) 1.22 F1F1F1S1F1F1F10 10-2 D) 6.20 F1F1F1S1F1F1F10 10-3 E) 2.44 F1F1F1S1F1F1F10 10-2 A) 6.10 F1F1F1S1F1F1F10 10-5 B) 3.10 F1F1F1S1F1F1F10 10-3 C) 1.22 F1F1F1S1F1F1F10 10-2 D) 6.20 F1F1F1S1F1F1F10 10-3 E) 2.44 F1F1F1S1F1F1F10 10-2

Determine the pH of a solution prepared by mixing the following: 25.0 mL of 0.200 M HCl 75)0 mL of 0.100 M NaOH 50)0 mL of 0.200 M NaH2PO4 For H3PO4 Ka1 = 7.5 F1F1F1S1F1F1F10 10-3, Ka2 = 6.2 F1F1F1S1F1F1F10 10-8, and Ka3 = 4.8 F1F1F1S1F1F1F10 10-13.

A) 6.73 B) 5.18 C) 1.65 D) 4.32 E) 4.25 A) 6.73 B) 5.18 C) 1.65 D) 4.32 E) 4.25

Calculate the molar concentration of uncomplexed Zn2+ in a solution that contains 0.20 mol of Zn(NH3)42+ per liter. The overall Kf for Zn(NH3)42+ is 3.8 F1F1F1S1F1F1F10 109.

A) 6.7 F1F1F1S1F1F1F10 10-4 M B) 2.9 F1F1F1S1F1F1F10 10-3 M C) 2.0 F1F1F1S1F1F1F10 10-13 M D) 8.8 F1F1F1S1F1F1F10 10-3 M E) none of these A) 6.7 F1F1F1S1F1F1F10 10-4 M B) 2.9 F1F1F1S1F1F1F10 10-3 M C) 2.0 F1F1F1S1F1F1F10 10-13 M D) 8.8 F1F1F1S1F1F1F10 10-3 M E) none of these

Calculate [H+] in a solution that is 0.24 M in NaF and 0.46 M in HF. (Ka = 7.2 F1F1F1S1F1F1F10 10-4)

A) 1.1 F1F1F1S1F1F1F10 10-4 M B) 1.4 F1F1F1S1F1F1F10 10-3 M C) 1.8 F1F1F1S1F1F1F10 10-2 M D) 3.8 F1F1F1S1F1F1F10 10-4 M E) 0.46 M A) 1.1 F1F1F1S1F1F1F10 10-4 M B) 1.4 F1F1F1S1F1F1F10 10-3 M C) 1.8 F1F1F1S1F1F1F10 10-2 M D) 3.8 F1F1F1S1F1F1F10 10-4 M E) 0.46 M

The solubility of Fe(OH)2 in water is 7.9 F1F1F1S1F1F1F10 10-6 mol/L at 25° C. What is Ksp for Fe(OH)2 at 25° C?

A) 4.9 F1F1F1S1F1F1F10 10-16 B) 6.2 F1F1F1S1F1F1F10 10-11 C) 2.5 F1F1F1S1F1F1F10 10-10 D) 2.0 F1F1F1S1F1F1F10 10-15 E) none of these A) 4.9 F1F1F1S1F1F1F10 10-16 B) 6.2 F1F1F1S1F1F1F10 10-11 C) 2.5 F1F1F1S1F1F1F10 10-10 D) 2.0 F1F1F1S1F1F1F10 10-15 E) none of these

2.42 F1F1F1S1F1F1F10 10-3 g of BaSO4 can dissolve in 1.00 L of water. Calculate Ksp for this salt.

A) 1.08 F1F1F1S1F1F1F10 10-10 B) 2.42 F1F1F1S1F1F1F10 10-3 C) 5.86 F1F1F1S1F1F1F10 10-6 D) 1.05 F1F1F1S1F1F1F10 10-5 E) None of these A) 1.08 F1F1F1S1F1F1F10 10-10 B) 2.42 F1F1F1S1F1F1F10 10-3 C) 5.86 F1F1F1S1F1F1F10 10-6 D) 1.05 F1F1F1S1F1F1F10 10-5 E) None of these

A 50.00-mL sample of 0.100 M KOH is titrated with 0.100 M HNO3. Calculate the pH of the solution after the 52.00 mL of HNO3 is added.

A) 6.50 B) 3.01 C) 2.41 D) 2.71 E) none of these A) 6.50 B) 3.01 C) 2.41 D) 2.71 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 total volume of HCl must be added to reach the second equivalence point?

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

Exam 8: Applications of Aqueous Equilibria

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 81

A 135.0-mL sample of a 0.25 M solution of H₃PO₄ is titrated with 0.12 M NaOH. What volume of base must be added to reach the third equivalence point?

(Multiple Choice)

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Question 82

You dissolve 1.24 g of an unknown diprotic acid in 220.0 mL of H₂O. This solution is just neutralized by 6.44 mL of a 1.25 M NaOH solution. What is the molar mass of the unknown acid?

(Multiple Choice)

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Question 83

Calculate the minimum concentration of 100.0 mL of sodium sulfate that is required to form a precipitate with 100.0 mL of 1.00  10^-² M calcium nitrate. K_sp for CaSO₄ is 6.1  10^-⁵.

(Multiple Choice)

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Question 84

Consider a 100.0-mL sample of a 0.10 M H₂A (K_a1 = 1.3 10^-³ , K_a2 = 3.1 10^-⁶) with 0.10 M NaOH. Determine the pH when 0 mL, 50.0 mL, 100.0 mL, and 150.0 mL of 0.10 M NaOH are added.

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Question 85

Determine the pH of a solution prepared by mixing the following: 25.0 mL of 0.200 M HCl 75)0 mL of 0.100 M NaOH 50)0 mL of 0.200 M NaH₂PO₄ 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 86

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 200.0 mL of 0.200 M NaOH is added

(Multiple Choice)

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Question 87

Consider the titration of 200.0 mL of a 0.100 M solution of the weak acid H₂A with 0.200 M NaOH. The first equivalence point is reached after 100.0 mL of 0.200 M NaOH has been added, and the pH is 6.27. The pH after 65.0 mL of 0.200 M NaOH has been added, the pH is 4.95. Calculate the value of K_a2 for H₂A.

(Multiple Choice)

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Question 88

Calculate the molar concentration of uncomplexed Zn²⁺ in a solution that contains 0.20 mol of Zn(NH₃)₄²⁺ per liter. The overall K_f for Zn(NH₃)₄²⁺ is 3.8  10⁹.

(Multiple Choice)

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Question 89

For 110.0 mL of a buffer that is 0.40 M in HOCl and 0.52 M in NaOCl, what is the pH after 11.2 mL of 1.1 M NaOH is added? K_a for HOCl = 3.5  10^-⁸. (Assume the volumes are additive.)

(Multiple Choice)

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Question 90

The solubility of AgCl in water is _____ the solubility of AgCl in strong acid at the same temperature.

(Multiple Choice)

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Question 91

Calculate [H⁺] in a solution that is 0.24 M in NaF and 0.46 M in HF. (K_a = 7.2  10^-⁴)

(Multiple Choice)

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Question 92

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: -Which of the following is a major species present at point IV?

(Multiple Choice)

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Question 93

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 94

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 95

In the titration of a weak acid HA with 0.100 M NaOH, the stoichiometric point is known to occur at a pH value of approximately 11. Which of the following indicators would be best to use to mark the endpoint of this titration?

(Multiple Choice)

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Question 96

2.42  10^-³ g of BaSO₄ can dissolve in 1.00 L of water. Calculate K_sp for this salt.

(Multiple Choice)

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Question 97

A 50.00-mL sample of 0.100 M KOH is titrated with 0.100 M HNO₃. Calculate the pH of the solution after the 52.00 mL of HNO₃ is added.

(Multiple Choice)

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Question 98

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?

(Multiple Choice)

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Question 99

A student titrates an unknown weak acid, HA, to a pale pink phenolphthalein endpoint with 25.0 mL of 0.100 M NaOH. The student then adds 13.0 mL of 0.100 M HCl. The pH of the resulting solution is 4.7. Which of the following statements is true?

(Multiple Choice)

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Question 100

Showing 81 - 100 of 171

A 135.0-mL sample of a 0.25 M solution of H₃PO₄ is titrated with 0.12 M NaOH. What volume of base must be added to reach the third equivalence point?

You dissolve 1.24 g of an unknown diprotic acid in 220.0 mL of H₂O. This solution is just neutralized by 6.44 mL of a 1.25 M NaOH solution. What is the molar mass of the unknown acid?

Calculate the minimum concentration of 100.0 mL of sodium sulfate that is required to form a precipitate with 100.0 mL of 1.00  10^-² M calcium nitrate. K_sp for CaSO₄ is 6.1  10^-⁵.

Consider a 100.0-mL sample of a 0.10 M H₂A (K_a1 = 1.3 10^-³ , K_a2 = 3.1 10^-⁶) with 0.10 M NaOH. Determine the pH when 0 mL, 50.0 mL, 100.0 mL, and 150.0 mL of 0.10 M NaOH are added.

Determine the pH of a solution prepared by mixing the following: 25.0 mL of 0.200 M HCl 75)0 mL of 0.100 M NaOH 50)0 mL of 0.200 M NaH₂PO₄ For H₃PO₄ K_a1 = 7.5  10^-³, K_a2 = 6.2  10^-⁸, and K_a3 = 4.8  10^-¹³.

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 200.0 mL of 0.200 M NaOH is added

Calculate the molar concentration of uncomplexed Zn²⁺ in a solution that contains 0.20 mol of Zn(NH₃)₄²⁺ per liter. The overall K_f for Zn(NH₃)₄²⁺ is 3.8  10⁹.

For 110.0 mL of a buffer that is 0.40 M in HOCl and 0.52 M in NaOCl, what is the pH after 11.2 mL of 1.1 M NaOH is added? K_a for HOCl = 3.5  10^-⁸. (Assume the volumes are additive.)

The solubility of AgCl in water is _____ the solubility of AgCl in strong acid at the same temperature.

Calculate [H⁺] in a solution that is 0.24 M in NaF and 0.46 M in HF. (K_a = 7.2  10^-⁴)

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: -Which of the following is a major species present at point IV?

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.

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?

In the titration of a weak acid HA with 0.100 M NaOH, the stoichiometric point is known to occur at a pH value of approximately 11. Which of the following indicators would be best to use to mark the endpoint of this titration?

2.42  10^-³ g of BaSO₄ can dissolve in 1.00 L of water. Calculate K_sp for this salt.

A 50.00-mL sample of 0.100 M KOH is titrated with 0.100 M HNO₃. Calculate the pH of the solution after the 52.00 mL of HNO₃ is added.

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 student titrates an unknown weak acid, HA, to a pale pink phenolphthalein endpoint with 25.0 mL of 0.100 M NaOH. The student then adds 13.0 mL of 0.100 M HCl. The pH of the resulting solution is 4.7. Which of the following statements is true?

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Exam 8: Applications of Aqueous Equilibria

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.

A 135.0-mL sample of a 0.25 M solution of H3PO4 is titrated with 0.12 M NaOH. What volume of base must be added to reach the third equivalence point?

You dissolve 1.24 g of an unknown diprotic acid in 220.0 mL of H2O. This solution is just neutralized by 6.44 mL of a 1.25 M NaOH solution. What is the molar mass of the unknown acid?

Calculate the minimum concentration of 100.0 mL of sodium sulfate that is required to form a precipitate with 100.0 mL of 1.00  10-2 M calcium nitrate. Ksp for CaSO4 is 6.1  10-5.

Consider a 100.0-mL sample of a 0.10 M H2A (Ka1 = 1.3 *10-3 , Ka2 = 3.1 * 10-6) with 0.10 M NaOH. Determine the pH when 0 mL, 50.0 mL, 100.0 mL, and 150.0 mL of 0.10 M NaOH are added.

Determine the pH of a solution prepared by mixing the following: 25.0 mL of 0.200 M HCl 75)0 mL of 0.100 M NaOH 50)0 mL of 0.200 M NaH2PO4 For H3PO4 Ka1 = 7.5  10-3, Ka2 = 6.2  10-8, and Ka3 = 4.8  10-13.

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 200.0 mL of 0.200 M NaOH is added

Calculate the molar concentration of uncomplexed Zn2+ in a solution that contains 0.20 mol of Zn(NH3)42+ per liter. The overall Kf for Zn(NH3)42+ is 3.8  109.

For 110.0 mL of a buffer that is 0.40 M in HOCl and 0.52 M in NaOCl, what is the pH after 11.2 mL of 1.1 M NaOH is added? Ka for HOCl = 3.5  10-8. (Assume the volumes are additive.)

The solubility of AgCl in water is _____ the solubility of AgCl in strong acid at the same temperature.

Calculate [H+] in a solution that is 0.24 M in NaF and 0.46 M in HF. (Ka = 7.2  10-4)

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: -Which of the following is a major species present at point IV?

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.

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?

In the titration of a weak acid HA with 0.100 M NaOH, the stoichiometric point is known to occur at a pH value of approximately 11. Which of the following indicators would be best to use to mark the endpoint of this titration?

2.42  10-3 g of BaSO4 can dissolve in 1.00 L of water. Calculate Ksp for this salt.

A 50.00-mL sample of 0.100 M KOH is titrated with 0.100 M HNO3. Calculate the pH of the solution after the 52.00 mL of HNO3 is added.

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 student titrates an unknown weak acid, HA, to a pale pink phenolphthalein endpoint with 25.0 mL of 0.100 M NaOH. The student then adds 13.0 mL of 0.100 M HCl. The pH of the resulting solution is 4.7. Which of the following statements is true?

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A 135.0-mL sample of a 0.25 M solution of H₃PO₄ is titrated with 0.12 M NaOH. What volume of base must be added to reach the third equivalence point?

You dissolve 1.24 g of an unknown diprotic acid in 220.0 mL of H₂O. This solution is just neutralized by 6.44 mL of a 1.25 M NaOH solution. What is the molar mass of the unknown acid?

Calculate the minimum concentration of 100.0 mL of sodium sulfate that is required to form a precipitate with 100.0 mL of 1.00  10^-² M calcium nitrate. K_sp for CaSO₄ is 6.1  10^-⁵.

Consider a 100.0-mL sample of a 0.10 M H₂A (K_a1 = 1.3 10^-³ , K_a2 = 3.1 10^-⁶) with 0.10 M NaOH. Determine the pH when 0 mL, 50.0 mL, 100.0 mL, and 150.0 mL of 0.10 M NaOH are added.

Determine the pH of a solution prepared by mixing the following: 25.0 mL of 0.200 M HCl 75)0 mL of 0.100 M NaOH 50)0 mL of 0.200 M NaH₂PO₄ For H₃PO₄ K_a1 = 7.5  10^-³, K_a2 = 6.2  10^-⁸, and K_a3 = 4.8  10^-¹³.

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 200.0 mL of 0.200 M NaOH is added

Calculate the molar concentration of uncomplexed Zn²⁺ in a solution that contains 0.20 mol of Zn(NH₃)₄²⁺ per liter. The overall K_f for Zn(NH₃)₄²⁺ is 3.8  10⁹.

For 110.0 mL of a buffer that is 0.40 M in HOCl and 0.52 M in NaOCl, what is the pH after 11.2 mL of 1.1 M NaOH is added? K_a for HOCl = 3.5  10^-⁸. (Assume the volumes are additive.)

Calculate [H⁺] in a solution that is 0.24 M in NaF and 0.46 M in HF. (K_a = 7.2  10^-⁴)

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: -Which of the following is a major species present at point IV?

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.

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?

2.42  10^-³ g of BaSO₄ can dissolve in 1.00 L of water. Calculate K_sp for this salt.

A 50.00-mL sample of 0.100 M KOH is titrated with 0.100 M HNO₃. Calculate the pH of the solution after the 52.00 mL of HNO₃ is added.

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?