Question 1

Which of the following acids (listed with Ka values) and their conjugate base would be the best choice to make a buffer with a pH of 10.40?

Accepted Answer

A)  C6H5COOH, Ka = 6.5 × 10-5 
B)  HF, Ka = 3.5 × 10-4 
C)  HClO, Ka = 2.9 × 10-8 
D)  HCN, Ka = 4.9 × 10-10 
E)  HClO2, Ka = 1.1 × 10-2 
A)  C6H5COOH, Ka = 6.5 × 10-5 
B)  HF, Ka = 3.5 × 10-4 
C)  HClO, Ka = 2.9 × 10-8 
D)  HCN, Ka = 4.9 × 10-10 
E)  HClO2, Ka = 1.1 × 10-2

Question 2

A 100.0 mL sample of 0.18 mol L-1 HClO4 is titrated with 0.27 mol L-1 NaOH. Determine the pH of the solution after the addition of 30.0 mL of NaOH.

Accepted Answer

A)  0.86 
B)  1.21 
C)  2.00 
D)  1.12 
E)  2.86 
A)  0.86 
B)  1.21 
C)  2.00 
D)  1.12 
E)  2.86

Question 3

Determine the molar solubility of Fe(OH)2 in pure water. Ksp for Fe(OH)2 = 4.87 × 10-17.

Accepted Answer

A)  2.44 × 10-17 mol L-1 
B)  1.62 × 10-17 mol L-1 
C)  4.03 × 10-9 mol L-1 
D)  3.65 × 10-6 mol L-1 
E)  2.30 × 10-6 mol L-1 
A)  2.44 × 10-17 mol L-1 
B)  1.62 × 10-17 mol L-1 
C)  4.03 × 10-9 mol L-1 
D)  3.65 × 10-6 mol L-1 
E)  2.30 × 10-6 mol L-1

Question 4

For a monoprotic weak acid titrated with a strong base, is the equivalence point acidic, basic, or neutral?

Accepted Answer

The answer of For a monoprotic weak acid titrated with...

Question 5

A 100.0 mL sample of 0.10 mol L-1 Ca(OH)2 is titrated with 0.10 mol L-1 HBr. Determine the pH of the solution after the addition of 100.0 mL HBr.

Accepted Answer

A)  2.00 
B)  12.00 
C)  1.30 
D)  12.70 
E)  7.00 
A)  2.00 
B)  12.00 
C)  1.30 
D)  12.70 
E)  7.00

Question 6

A 100.0 mL sample of 0.20 mol L-1 HF is titrated with 0.10 mol L-1 KOH. Determine the pH of the solution after the addition of 100.0 mL of KOH. The Ka of HF is 3.5 × 10-4.

Accepted Answer

A)  2.08 
B)  3.15 
C)  4.33 
D)  3.46 
E)  4.15 
A)  2.08 
B)  3.15 
C)  4.33 
D)  3.46 
E)  4.15

Question 7

Determine the molar solubility of AgI in pure water. Ksp (AgI) = 8.51 × 10-17.

Accepted Answer

A)  9.22 × 10-9 mol L-1 
B)  4.26 × 10-17 mol L-1 
C)  8.51 × 10-17 mol L-1 
D)  2.77 × 10-6 mol L-1 
E)  4.40 × 10-6 mol L-1 
A)  9.22 × 10-9 mol L-1 
B)  4.26 × 10-17 mol L-1 
C)  8.51 × 10-17 mol L-1 
D)  2.77 × 10-6 mol L-1 
E)  4.40 × 10-6 mol L-1

Question 8

Calculate the pH of a solution that is 0.445 mol L-1 in sodium formate (HCOONa) and 0.265   in formic acid (HCOOH). The   of formic acid is 1.77 ×   .

Accepted Answer

A)  4.860 
B)  3.527 
C)  10.023 
D)  3.977 
E)  3.752 
A)  4.860 
B)  3.527 
C)  10.023 
D)  3.977 
E)  3.752

Question 9

What is the pH of a buffer solution that is 0.251 mol L-1 in lactic acid and 0.151 mol L-1 in sodium lactate? The   of lactic acid is 1.4 ×   .

Accepted Answer

A)  12.58 
B)  5.28 
C)  4.08 
D)  10.37 
E)  3.63 
A)  12.58 
B)  5.28 
C)  4.08 
D)  10.37 
E)  3.63

Question 10

What is the pH of a solution made by mixing 25.00 mL of 0. 100 mol L-1 HCl with 40.00 mL of 0. 100 mol L-1 KOH? Assume that the volumes of the solutions are additive.

Accepted Answer

A)  0.64 
B)  1.64 
C)  12.36 
D)  13.36 
A)  0.64 
B)  1.64 
C)  12.36 
D)  13.36

Question 11

Match the following.
-pH < 7

Accepted Answer

A) equivalence point of a weak acid-strong base titration 
B) halfway to equivalence point of a weak acid-strong base titration 
C) equivalence point of a strong acid-strong base titration 
D) equivalence point of a weak base-strong acid titration 
E) three-quarters of the way to second equivalence point of a diprotic acid-strong base titration 
A) equivalence point of a weak acid-strong base titration 
B) halfway to equivalence point of a weak acid-strong base titration 
C) equivalence point of a strong acid-strong base titration 
D) equivalence point of a weak base-strong acid titration 
E) three-quarters of the way to second equivalence point of a diprotic acid-strong base titration

Question 12

What is the pH of a solution made by mixing 10.00 mL of 0.10 mol L-1 acetic acid with 10.00 mL of 0.10 mol L-1 KOH? Assume that the volumes of the solutions are additive. Ka =   for CH3COOH.

Accepted Answer

A)  5.28 
B)  7.00 
C)  8.72 
D)  10.02 
A)  5.28 
B)  7.00 
C)  8.72 
D)  10.02

Question 13

Which of the following acids (listed with pKa values) and its conjugate would be the best choice to make a buffer with a pH of 5.20?

Accepted Answer

A)  HC7H5O2, pKa = 4.19 
B)  HF, pKa = 3.46 
C)  HClO, pKa = 7.54 
D)  HCN, pKa = 9.31 
E)  HClO2, pKa = 1.96 
A)  HC7H5O2, pKa = 4.19 
B)  HF, pKa = 3.46 
C)  HClO, pKa = 7.54 
D)  HCN, pKa = 9.31 
E)  HClO2, pKa = 1.96

Question 14

Which of the following compounds will have the highest molar solubility in pure water?

Accepted Answer

A)  PbSO4, Ksp = 1.82 × 10-8 
B)  MgCO3, Ksp = 6.82 × 10-6 
C)  AgI, Ksp = 8.51 × 10-17 
D)  PbS, Ksp = 9.04 × 10-29 
E)  FeS, Ksp = 3.72 × 10-19 
A)  PbSO4, Ksp = 1.82 × 10-8 
B)  MgCO3, Ksp = 6.82 × 10-6 
C)  AgI, Ksp = 8.51 × 10-17 
D)  PbS, Ksp = 9.04 × 10-29 
E)  FeS, Ksp = 3.72 × 10-19

Question 15

A 25.0 mL sample of 0.150 mol L-1 hydrofluoric acid is titrated with a 0.150 mol L-1 NaOH solution. What is the pH before any base is added? Hydrofluoric acid is monoprotic. The   of hydrofluoric acid is 3.5 × 10-4.

Accepted Answer

A)  2.33 × 10-3 
B)  2.63 
C)  3.46 
D)  7.07 × 10-3 
E)  2.15 
A)  2.33 × 10-3 
B)  2.63 
C)  3.46 
D)  7.07 × 10-3 
E)  2.15

Question 16

A 100.0 mL sample of 0.10 mol L-1 NH3 is titrated with 0.10 mol L-1 HNO3. Determine the pH of the solution before the addition of any HNO3. The Kb of NH3 is 1.8 × 10-5.

Accepted Answer

A)  4.74 
B)  9.26 
C)  11.13 
D)  13.00 
E)  12.55 
A)  4.74 
B)  9.26 
C)  11.13 
D)  13.00 
E)  12.55

Question 17

Calculate the pH of a solution that is 0.240 mol L-1 in nitrous acid (   ) and 0.320 mol L-1 in potassium nitrite (   ). The acid dissociation constant of nitrous acid is 4.50 ×   .

Accepted Answer

A)  12.885 
B)  4.461 
C)  3.222 
D)  10.528 
E)  3.472 
A)  12.885 
B)  4.461 
C)  3.222 
D)  10.528 
E)  3.472

Question 18

When titrating a monoprotic strong acid with a weak base at 25 °C, the ________.

Accepted Answer

A)  pH will be 7 at the equivalence point 
B)  pH will be greater than 7 at the equivalence point 
C)  titration will require more moles of base than acid to reach the equivalence point 
D)  titration will require more moles of acid than base to reach the equivalence point 
E)  pH will be less than 7 at the equivalence point 
A)  pH will be 7 at the equivalence point 
B)  pH will be greater than 7 at the equivalence point 
C)  titration will require more moles of base than acid to reach the equivalence point 
D)  titration will require more moles of acid than base to reach the equivalence point 
E)  pH will be less than 7 at the equivalence point

Question 19

Identify the expression for the solubility product constant for Ca3(PO4)2.

Accepted Answer

A)    
B)    
C)    
D)  [Ca2+]2[PO43-]3 
E)  [Ca2+]3[PO43-]2 
A)    
B)    
C)    
D)  [Ca2+]2[PO43-]3 
E)  [Ca2+]3[PO43-]2

Question 20

Calculate the pH of a solution formed by mixing 200.0 mL of 0.30 mol L-1 HClO with 300.0 mL of 0.20 mol L-1 KClO. The Ka for HClO is 2.9 × 10-8.

Accepted Answer

A)  5.99 
B)  8.01 
C)  7.54 
D)  7.06 
E)  6.46 
A)  5.99 
B)  8.01 
C)  7.54 
D)  7.06 
E)  6.46

Exam 16: Aqueous Ionic Equilibrium

Which of the following acids (listed with Ka values) and their conjugate base would be the best choice to make a buffer with a pH of 10.40?

A 100.0 mL sample of 0.18 mol L-1 HClO4 is titrated with 0.27 mol L-1 NaOH. Determine the pH of the solution after the addition of 30.0 mL of NaOH.

Determine the molar solubility of Fe(OH)2 in pure water. Ksp for Fe(OH)2 = 4.87 × 10-17.

For a monoprotic weak acid titrated with a strong base, is the equivalence point acidic, basic, or neutral?

A 100.0 mL sample of 0.10 mol L-1 Ca(OH)2 is titrated with 0.10 mol L-1 HBr. Determine the pH of the solution after the addition of 100.0 mL HBr.

A 100.0 mL sample of 0.20 mol L-1 HF is titrated with 0.10 mol L-1 KOH. Determine the pH of the solution after the addition of 100.0 mL of KOH. The Ka of HF is 3.5 × 10-4.

Determine the molar solubility of AgI in pure water. Ksp (AgI) = 8.51 × 10-17.

Calculate the pH of a solution that is 0.445 mol L-1 in sodium formate (HCOONa) and 0.265 in formic acid (HCOOH). The of formic acid is 1.77 × .

What is the pH of a buffer solution that is 0.251 mol L-1 in lactic acid and 0.151 mol L-1 in sodium lactate? The of lactic acid is 1.4 × .

What is the pH of a solution made by mixing 25.00 mL of 0. 100 mol L-1 HCl with 40.00 mL of 0. 100 mol L-1 KOH? Assume that the volumes of the solutions are additive.

Match the following. -pH < 7

What is the pH of a solution made by mixing 10.00 mL of 0.10 mol L-1 acetic acid with 10.00 mL of 0.10 mol L-1 KOH? Assume that the volumes of the solutions are additive. Ka = for CH3COOH.

Which of the following acids (listed with pKa values) and its conjugate would be the best choice to make a buffer with a pH of 5.20?

Which of the following compounds will have the highest molar solubility in pure water?

A 25.0 mL sample of 0.150 mol L-1 hydrofluoric acid is titrated with a 0.150 mol L-1 NaOH solution. What is the pH before any base is added? Hydrofluoric acid is monoprotic. The of hydrofluoric acid is 3.5 × 10-4.

A 100.0 mL sample of 0.10 mol L-1 NH3 is titrated with 0.10 mol L-1 HNO3. Determine the pH of the solution before the addition of any HNO3. The Kb of NH3 is 1.8 × 10-5.

Calculate the pH of a solution that is 0.240 mol L-1 in nitrous acid ( ) and 0.320 mol L-1 in potassium nitrite ( ). The acid dissociation constant of nitrous acid is 4.50 × .

When titrating a monoprotic strong acid with a weak base at 25 °C, the ________.

Identify the expression for the solubility product constant for Ca3(PO4)2.

Calculate the pH of a solution formed by mixing 200.0 mL of 0.30 mol L-1 HClO with 300.0 mL of 0.20 mol L-1 KClO. The Ka for HClO is 2.9 × 10-8.

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Which of the following acids (listed with K_a values) and their conjugate base would be the best choice to make a buffer with a pH of 10.40?

A 100.0 mL sample of 0.18 mol L^-1 HClO₄ is titrated with 0.27 mol L^-1 NaOH. Determine the pH of the solution after the addition of 30.0 mL of NaOH.

Determine the molar solubility of Fe(OH)₂in pure water. K_sp for Fe(OH)₂ = 4.87 × 10^-17.

A 100.0 mL sample of 0.10 mol L^-1 Ca(OH)₂ is titrated with 0.10 mol L^-1 HBr. Determine the pH of the solution after the addition of 100.0 mL HBr.

A 100.0 mL sample of 0.20 mol L^-1 HF is titrated with 0.10 mol L^-1 KOH. Determine the pH of the solution after the addition of 100.0 mL of KOH. The K_a of HF is 3.5 × 10^-4.

Determine the molar solubility of AgI in pure water. K_sp (AgI) = 8.51 × 10^-¹⁷.

Calculate the pH of a solution that is 0.445 mol L^-1 in sodium formate (HCOONa) and 0.265 in formic acid (HCOOH). The of formic acid is 1.77 × .

What is the pH of a buffer solution that is 0.251 mol L^-1 in lactic acid and 0.151 mol L^-1 in sodium lactate? The of lactic acid is 1.4 × .

What is the pH of a solution made by mixing 25.00 mL of 0. 100 mol L^-1 HCl with 40.00 mL of 0. 100 mol L^-1 KOH? Assume that the volumes of the solutions are additive.

What is the pH of a solution made by mixing 10.00 mL of 0.10 mol L^-1 acetic acid with 10.00 mL of 0.10 mol L^-1 KOH? Assume that the volumes of the solutions are additive. K_a = for CH₃COOH.

Which of the following acids (listed with pK_a values) and its conjugate would be the best choice to make a buffer with a pH of 5.20?

A 25.0 mL sample of 0.150 mol L^-1 hydrofluoric acid is titrated with a 0.150 mol L^-1 NaOH solution. What is the pH before any base is added? Hydrofluoric acid is monoprotic. The of hydrofluoric acid is 3.5 × 10^-4.

A 100.0 mL sample of 0.10 mol L^-1 NH₃ is titrated with 0.10 mol L^-1 HNO₃. Determine the pH of the solution before the addition of any HNO₃. The K_b of NH₃ is 1.8 × 10^-5.

Calculate the pH of a solution that is 0.240 mol L^-1 in nitrous acid ( ) and 0.320 mol L^-1 in potassium nitrite ( ). The acid dissociation constant of nitrous acid is 4.50 × .

Identify the expression for the solubility product constant for Ca₃(PO₄)₂.

Calculate the pH of a solution formed by mixing 200.0 mL of 0.30 mol L^-1 HClO with 300.0 mL of 0.20 mol L^-1 KClO. The K_a for HClO is 2.9 × 10^-8.