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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?


A) 6.8 × 10-5
B) 6.2 × 10-6
C) 6.2 × 10-7
D) 6.2 × 10-8
E) 2.8 × 10-12

F) A) and B)
G) None of the above

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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

F) A) and B)
G) B) and E)

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Use the following information to calculate the solubility product constant, Ksp, 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.


A) Ksp = 1.7 × 10y9
B) Ksp = 1.7 × 10y7
C) Ksp = 1.7 × 10-5
D) Ksp = 4.3 × 10-4
E) Ksp = 2.1 × 10-2

F) None of the above
G) A) and E)

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


A) dissolving a small amount of solid sodium acetate
B) adding a small amount of dilute hydrochloric acid
C) adding a small amount of dilute sodium hydroxide
D) dissolving a small amount of solid sodium chloride
E) diluting the buffer solution with water

F) D) and E)
G) C) and D)

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


A) BaF2
B) CuCl
C) CuBr
D) AgI
E) None of these choices are correct.

F) A) and E)
G) A) and D)

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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) True
B) False

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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?


A) 1 L of 0.9 M CO32- and 0.1 M HCO3-
B) 1 L of 0.1 M CO32- and 0.9 M HCO3-
C) 1 L of 0.5 M CO32- and 0.5 M HCO3-
D) 1 L of 0.1 M CO32- and 0.1 M HCO3-
E) They can all neutralize the same amount of hydrochloric acid.

F) B) and D)
G) C) and E)

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


A) [CH3COOH] = 0.25 M, [CH3COO-] = 0.25 M
B) [CH3COOH] = 0.75 M, [CH3COO-] = 0.75 M
C) [CH3COOH] = 0.75 M, [CH3COO-] = 0.25 M
D) [CH3COOH] = 0.25 M, [CH3COO-] = 0.75 M
E) [CH3COOH] = 1.00 M, [CH3COO-] = 1.00 M

F) A) and B)
G) B) and D)

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


A) 8.1 x 10-12 M
B) 2.8 x 10-6 M
C) 1.4 x 10-6 M
D) 1.4 x 10-8 M
E) 2.0 x 10-4 M

F) A) and D)
G) D) and E)

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


A) 9.5 × 10-5
B) 2.4 × 10-5
C) 2.6 × 10-12
D) 6.5 × 10-13
E) < 1.0 × 10-13

F) B) and D)
G) A) and B)

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Use the following information to calculate the solubility product constant, Ksp, 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.


A) Ksp = 6.9 × 10-8
B) Ksp = 4.3 × 10-6
C) Ksp = 1.7 × 10-5
D) Ksp = 2.6 × 10-4
E) Ksp = 3.2 × 10-2

F) A) and E)
G) A) and C)

Correct Answer

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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) 0.025 mol HCl
B) 0.063 mol HCl
C) 0.082 mol HCl
D) 0.50 mol HCl
E) 1.0 mol HCl

F) B) and E)
G) A) and E)

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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) 0.10 mol L-1 HCl
B) 0.20 mol L-1 HCl
C) 0.10 mol L-1 CH3COOH
D) 0.050 mol L-1 NaOH
E) 0.20 mol L-1 NH4Cl

F) All of the above
G) A) and E)

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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.

F) A) and C)
G) C) and E)

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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?


A) < 4.00
B) 4.63
C) 4.87
D) 5.02
E) > 5.50

F) A) and B)
G) B) and E)

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


A) 4.0 × 10-5 M
B) 1.8 × 10-5 M
C) 4.0 × 10-6 M
D) 1.5 × 10-5 M
E) < 1.0 × 10-5 M

F) A) and B)
G) A) and D)

Correct Answer

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


A) 0.10 mol L-1 HCl and 0.05 mol L-1 NaOH
B) 0.10 mol L-1 HCl and 0.15 mol L-1 NH3
C) 0.10 mol L-1 HCl and 0.05 mol L-1 NH3
D) 0.10 mol L-1 HCl and 0.20 mol L-1 CH3COOH
E) 0.10 mol L-1 HCl and 0.20 mol L-1 NaCl

F) All of the above
G) A) and E)

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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) 1.26
B) 1.67
C) 12.33
D) 12.74
E) 13.03

F) B) and D)
G) B) and C)

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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

F) C) and D)
G) A) and D)

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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

F) A) and B)
G) C) and E)

Correct Answer

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