Calculate the solubility of silver oxalate, Ag2C2O4, in pure water. Ksp = 1.0 × 10-11

A) 1.4 × 10-4 M B) 8.2 × 10-5 M C) 5.4 × 10-5 M D) 3.2 × 10-6 M E) 2.5 × 10-12 M A) 1.4 × 10-4 M B) 8.2 × 10-5 M C) 5.4 × 10-5 M D) 3.2 × 10-6 M E) 2.5 × 10-12 M

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

A popular buffer solution consists of carbonate (CO32-) and hydrogen carbonate (HCO3-) conjugate acid-base pair. Which, if any, of the following such buffers has the highest buffer capacity?

A) 0.9 M CO32- and 0.1 M HCO3- B) 0.1 M CO32- and 0.9 M HCO3- C) 0.5 M CO32- and 0.5 M HCO3- D) 0.1 M CO32- and 0.1 M HCO3- E) They all have the same buffer capacity. A) 0.9 M CO32- and 0.1 M HCO3- B) 0.1 M CO32- and 0.9 M HCO3- C) 0.5 M CO32- and 0.5 M HCO3- D) 0.1 M CO32- and 0.1 M HCO3- E) They all have the same buffer capacity.

What is the maximum amount of sodium sulfate that can be added to 1.00 L of 0.0020 M Ca(NO3)2 before precipitation of calcium sulfate begins? Ksp = 2.4 × 10-5 for calcium sulfate.

A) 1.2 × 10-2 mol B) 4.9 × 10-3 mol C) 3.5 × 10-3 mol D) 1.2 × 10-5 mol E) 4.8 × 10-8 mol A) 1.2 × 10-2 mol B) 4.9 × 10-3 mol C) 3.5 × 10-3 mol D) 1.2 × 10-5 mol E) 4.8 × 10-8 mol

Exam 19: Ionic Equilibria in Aqueous Systems

Use the following information to calculate the solubility product constant, K_sp, for PbCl₂. A saturated solution of PbCl₂ in water was prepared and filtered. From the filtrate, 1.0 L was measured out into a beaker and evaporated to dryness. The solid PbCl₂ residue recovered in the beaker amounted to 0.0162 moles.

(Multiple Choice)

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Question 61

Calculate the solubility of silver oxalate, Ag₂C₂O₄, in pure water. K_sp = 1.0 × 10^-11

(Multiple Choice)

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Question 62

A popular buffer solution consists of carbonate (CO₃^2-) and hydrogen carbonate (HCO₃^-) conjugate acid-base pair. Which, if any, of the following such buffers can neutralize the greatest amount of added hydrochloric acid, while remaining within its buffer range?

(Multiple Choice)

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Question 63

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 64

What is the pK_a for the acid HA if a solution of 0.65 M HA and 0.85 M NaA has a pH of 4.75?

(Multiple Choice)

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Question 65

Which one of the following aqueous solutions, when mixed with an equal volume of 0.10 mol L^-1 aqueous NH₃, will produce a buffer solution?

(Multiple Choice)

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Question 66

A change in pH will significantly affect the solubility of which, if any, of the following compounds?

(Multiple Choice)

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Question 67

A buffer is prepared by adding 150 mL of 1.0 M NaOH to 250 mL of 1.0 M NaH₂PO₄. How many moles of HCl must be added to this buffer solution to change the pH by 0.18 units? If necessary, assume the total volume remains unchanged at 400 mL.

(Multiple Choice)

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Question 68

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)₄^2-

(Multiple Choice)

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Question 69

The solubility of silver chromate is 0.0287 g/1.0 L of solution. What is the K_sp for Ag₂CrO₄?

(Multiple Choice)

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Question 70

Calculate the solubility of silver phosphate, Ag3PO4, in pure water. K_sp = 2.6 × 10^-18

(Multiple Choice)

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Question 71

A 20.0-mL sample of 0.50 M H₂C₆H₆O₆ (ascorbic acid, a diprotic acid) was titrated with 0.50 M NaOH. The following data were gathered during the titration. mL NaOH added 10.00 20.00 30.00 40.00 PH 4.17 5.21 11.55 12.89 What is K_a2 for ascorbic acid?

(Multiple Choice)

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Question 72

Equal volumes of the following pairs of solutions are mixed. Which pair will produce a buffer solution?

(Multiple Choice)

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Question 73

A popular buffer solution consists of carbonate (CO₃^2-) and hydrogen carbonate (HCO₃^-) conjugate acid-base pair. Which, if any, of the following such buffers has the highest buffer capacity?

(Multiple Choice)

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Question 74

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 75

Use the following information to calculate the solubility product constant, K_sp, for CuCl. A saturated solution of CuCl in water was prepared and filtered. From the filtrate, 1.0 L was measured out into a beaker and evaporated to dryness. The solid CuCl residue recovered in the beaker was found to weigh 0.041g.

(Multiple Choice)

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Question 76

Calculate the molar solubility of silver carbonate in 1.0 M sodium carbonate solution. (K_sp for Ag₂CO₃ = 8.1 x 10^-12)

(Multiple Choice)

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Question 77

What is the maximum amount of sodium sulfate that can be added to 1.00 L of 0.0020 M Ca(NO₃)₂ before precipitation of calcium sulfate begins? K_sp = 2.4 × 10^-5 for calcium sulfate.

(Multiple Choice)

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Question 78

An acetate buffer has a pH of 4.40. Which of the following changes will cause the pH to decrease?

(Multiple Choice)

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Question 79

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 80

Showing 61 - 80 of 114

Exam 19: Ionic Equilibria in Aqueous Systems

Calculate the solubility of silver oxalate, Ag2C2O4, in pure water. Ksp = 1.0 × 10-11

A popular buffer solution consists of carbonate (CO32-) and hydrogen carbonate (HCO3-) conjugate acid-base pair. Which, if any, of the following such buffers can neutralize the greatest amount of added hydrochloric acid, while remaining within its buffer range?

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

What is the pKa for the acid HA if a solution of 0.65 M HA and 0.85 M NaA has a pH of 4.75?

Which one of the following aqueous solutions, when mixed with an equal volume of 0.10 mol L-1 aqueous NH3, will produce a buffer solution?

A change in pH will significantly affect the solubility of which, if any, of the following compounds?

A buffer is prepared by adding 150 mL of 1.0 M NaOH to 250 mL of 1.0 M NaH2PO4. How many moles of HCl must be added to this buffer solution to change the pH by 0.18 units? If necessary, assume the total volume remains unchanged at 400 mL.

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-

The solubility of silver chromate is 0.0287 g/1.0 L of solution. What is the Ksp for Ag2CrO4?

Calculate the solubility of silver phosphate, Ag3PO4, in pure water. Ksp = 2.6 × 10-18

A 20.0-mL sample of 0.50 M H2C6H6O6 (ascorbic acid, a diprotic acid) was titrated with 0.50 M NaOH. The following data were gathered during the titration. mL NaOH added 10.00 20.00 30.00 40.00 PH 4.17 5.21 11.55 12.89 What is Ka2 for ascorbic acid?

Equal volumes of the following pairs of solutions are mixed. Which pair will produce a buffer solution?

A popular buffer solution consists of carbonate (CO32-) and hydrogen carbonate (HCO3-) conjugate acid-base pair. Which, if any, of the following such buffers has the highest buffer capacity?

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.

Calculate the molar solubility of silver carbonate in 1.0 M sodium carbonate solution. (Ksp for Ag2CO3 = 8.1 x 10-12)

What is the maximum amount of sodium sulfate that can be added to 1.00 L of 0.0020 M Ca(NO3)2 before precipitation of calcium sulfate begins? Ksp = 2.4 × 10-5 for calcium sulfate.

An acetate buffer has a pH of 4.40. Which of the following changes will cause the pH to decrease?

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?

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Calculate the solubility of silver oxalate, Ag₂C₂O₄, in pure water. K_sp = 1.0 × 10^-11

A popular buffer solution consists of carbonate (CO₃^2-) and hydrogen carbonate (HCO₃^-) conjugate acid-base pair. Which, if any, of the following such buffers can neutralize the greatest amount of added hydrochloric acid, while remaining within its buffer range?

What is the pK_a for the acid HA if a solution of 0.65 M HA and 0.85 M NaA has a pH of 4.75?

Which one of the following aqueous solutions, when mixed with an equal volume of 0.10 mol L^-1 aqueous NH₃, will produce a buffer solution?

A buffer is prepared by adding 150 mL of 1.0 M NaOH to 250 mL of 1.0 M NaH₂PO₄. How many moles of HCl must be added to this buffer solution to change the pH by 0.18 units? If necessary, assume the total volume remains unchanged at 400 mL.

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)₄^2-

The solubility of silver chromate is 0.0287 g/1.0 L of solution. What is the K_sp for Ag₂CrO₄?

Calculate the solubility of silver phosphate, Ag3PO4, in pure water. K_sp = 2.6 × 10^-18

A 20.0-mL sample of 0.50 M H₂C₆H₆O₆ (ascorbic acid, a diprotic acid) was titrated with 0.50 M NaOH. The following data were gathered during the titration. mL NaOH added 10.00 20.00 30.00 40.00 PH 4.17 5.21 11.55 12.89 What is K_a2 for ascorbic acid?

A popular buffer solution consists of carbonate (CO₃^2-) and hydrogen carbonate (HCO₃^-) conjugate acid-base pair. Which, if any, of the following such buffers has the highest buffer capacity?

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.

Calculate the molar solubility of silver carbonate in 1.0 M sodium carbonate solution. (K_sp for Ag₂CO₃ = 8.1 x 10^-12)

What is the maximum amount of sodium sulfate that can be added to 1.00 L of 0.0020 M Ca(NO₃)₂ before precipitation of calcium sulfate begins? K_sp = 2.4 × 10^-5 for calcium sulfate.