Question 1

You wish to prepare a buffer containing CH3COOH with a pH of 5.44. If the pKa of acetic acid is 4.74, what ratio of [CH3COO⁻]/[CH3COOH] must you use?

Accepted Answer

A)  0.70 
B)  0.20 
C)  1.4 
D)  5.0 
E)  1.1 
A)  0.70 
B)  0.20 
C)  1.4 
D)  5.0 
E)  1.1

Question 2

Match the following.
-pH = pKa2

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 3

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 after the addition of 150.0 mL of HNO3. The Kb of NH3 is 1.8 × 10-5.

Accepted Answer

A)  1.7 
B)  6.4 
C)  7.6 
D)  12.3 
E)  2.3 
A)  1.7 
B)  6.4 
C)  7.6 
D)  12.3 
E)  2.3

Question 4

Calculate the pH of a buffer that is 0.225 mol L-1 CH3COOH and 0.162 mol L-1 CH3COOK. The Ka for CH3COOH is 1.8 × 10-5.

Accepted Answer

A)  4.89 
B)  9.11 
C)  4.74 
D)  9.26 
E)  4.60 
A)  4.89 
B)  9.11 
C)  4.74 
D)  9.26 
E)  4.60

Question 5

What is the molar solubility of calcium hydroxide ( Ca(OH)2) in water? The solubility-product constant for CaOH2 is 4.5 × 10-6 at

Accepted Answer

A)  1.5 × 10-6 mol L-1 
B)  3.0 × 10-3 mol L-1 
C)  1.1 × 10-3 mol L-1 
D)  1.7 × 10-2 mol L-1 
E)  1.0 × 10-2 mol L-1 
A)  1.5 × 10-6 mol L-1 
B)  3.0 × 10-3 mol L-1 
C)  1.1 × 10-3 mol L-1 
D)  1.7 × 10-2 mol L-1 
E)  1.0 × 10-2 mol L-1

Question 6

Explain the common ion effect with respect to molar solubility.

Accepted Answer

The common ion effect occurs when a solu

Question 7

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 mol L-1 NH4Cl with 200.0 mL of 0.12 mol L-1 NH3. The Kb for NH3 is 1.8 × 10-5.

Accepted Answer

A)  9.06 
B)  9.45 
C)  4.55 
D)  4.74 
E)  9.26 
A)  9.06 
B)  9.45 
C)  4.55 
D)  4.74 
E)  9.26

Question 8

Identify the compound that is acid-insoluble.

Accepted Answer

A)  PbCl2 
B)  As2S3 
C)  CoS 
D)  Ca3(PO4)2 
E)  NaCl 
A)  PbCl2 
B)  As2S3 
C)  CoS 
D)  Ca3(PO4)2 
E)  NaCl

Question 9

A 1.0 L buffer solution is 0.050 mol L-1 CH3COOH and 0.250 mol L-1 CH3COOLi. Which of the following actions will destroy the buffer?

Accepted Answer

A)  adding 0.050 moles of NaOH 
B)  adding 0.050 moles of HCl 
C)  adding 0.050 moles of CH3COOH 
D)  adding 0.050 moles of CH3COOLi 
E)  adding 0.050 moles of NH4Cl. 
A)  adding 0.050 moles of NaOH 
B)  adding 0.050 moles of HCl 
C)  adding 0.050 moles of CH3COOH 
D)  adding 0.050 moles of CH3COOLi 
E)  adding 0.050 moles of NH4Cl.

Question 10

Predict the number of equivalence point(s) in the titration for a diprotic acid with a strong base.

Accepted Answer

The answer of Predict the number of equivalence point(s) in...

Question 11

Determine the molar solubility of CuCl in a solution containing 0.050 mol L-1 KCl. Ksp (CuCl) = 1.0 × 10-6.

Accepted Answer

A)  1.0 × 10-12 mol L-1 
B)  5.0 × 10-7 mol L-1 
C)  2.0 × 10-5 mol L-1 
D)  1.0 × 10-3 mol L-1 
E)  0.050 mol L-1 
A)  1.0 × 10-12 mol L-1 
B)  5.0 × 10-7 mol L-1 
C)  2.0 × 10-5 mol L-1 
D)  1.0 × 10-3 mol L-1 
E)  0.050 mol L-1

Question 12

What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous hydrofluoric acid requires 30.00 mL of 0. 400 mol L-1 NaOH? Ka = 6.76 × 10-4 for HF.

Accepted Answer

A)  1.74 
B)  5.75 
C)  8.25 
D)  12.26 
A)  1.74 
B)  5.75 
C)  8.25 
D)  12.26

Question 13

Name the chemical compound that forms stalactites and stalagmites.

Accepted Answer

The answer of Name the chemical compound that forms stalactites...

Question 14

What is the pH of a solution made by mixing 30.00 mL of 0.10 mol L-1 acetic acid (CH3COOH) with 50.00 mL of 0. 100 mol L-1 KOH? Assume that the volumes of the solutions are additive. Ka = 1.8 × 10-5 for

Accepted Answer

A)  8.26 
B)  9.26 
C)  11.13 
D)  12. 40 
A)  8.26 
B)  9.26 
C)  11.13 
D)  12. 40

Question 15

A 1.50 L buffer solution is 0.250 mol L-1 in HF and 0.250 mol L-1 in NaF. Calculate the pH of the solution after the addition of 0.0500 moles of solid NaOH. Assume no volume change upon the addition of the base. The Ka for HF is 3.5 × 10-4.

Accepted Answer

A)  3.34 
B)  3.46 
C)  3.57 
D)  3.63 
E)  2.89 
A)  3.34 
B)  3.46 
C)  3.57 
D)  3.63 
E)  2.89

Question 16

What is the pH of a solution prepared by mixing 100.00 mL of 0.020 mol L-1 Ca(OH)2 with 50.00 mL of 0. 300 mol L-1 NaOH? Assume that the volumes are additive.

Accepted Answer

A)  13.05 
B)  13.10 
C)  13.28 
D)  13.58 
A)  13.05 
B)  13.10 
C)  13.28 
D)  13.58

Question 17

Solid potassium chromate (K2CrO4) is slowly added to a solution containing 0. 50 mol L-1 AgNO3 and 0. 50 mol L-1 Ba(NO3)2. What is the Ag+ concentration when BaCrO4 just starts to precipitate? The Ksp for Ag2CrO4 and BaCrO4 are 1.1 × 10-12 and   respectively.

Accepted Answer

A)  6.5 × 10-5 mol L-1 
B)  1.3 × 10-4 mol L-1 
C)  3.2 × 10-4 mol L-1 
D)  6.8 × 10-2 mol L-1 
A)  6.5 × 10-5 mol L-1 
B)  1.3 × 10-4 mol L-1 
C)  3.2 × 10-4 mol L-1 
D)  6.8 × 10-2 mol L-1

Question 18

Calculate the pH of a buffer that is 0.158 mol L-1 HClO and 0.099 mol L-1 NaClO. The Ka for HClO is 2.9 × 10-8.

Accepted Answer

A)  7.54 
B)  6.67 
C)  3.77 
D)  6.46 
E)  7.33 
A)  7.54 
B)  6.67 
C)  3.77 
D)  6.46 
E)  7.33

Question 19

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 mol L-1 HCOOH with 100.0 mL of 0.20 mol L-1 HCOOLi. The Ka for HCHO2 is 1.8 × 10-4.

Accepted Answer

A)  3.87 
B)  3.74 
C)  10.53 
D)  3.47 
E)  10.13 
A)  3.87 
B)  3.74 
C)  10.53 
D)  3.47 
E)  10.13

Question 20

What is the molar solubility of silver iodide ( AgI ) in water? The solubility-product constant for AgI  is 8.5 × 10-17 at 25 °C.

Accepted Answer

A)  16 mol L-1 
B)  1.3 × 10-8 mol L-1 
C)  1.7 × 10-16 mol L-1 
D)  4.3 × 10-17 mol L-1 
E)  9.2 × 10-9 mol L-1 
A)  16 mol L-1 
B)  1.3 × 10-8 mol L-1 
C)  1.7 × 10-16 mol L-1 
D)  4.3 × 10-17 mol L-1 
E)  9.2 × 10-9 mol L-1

Exam 16: Aqueous Ionic Equilibrium

You wish to prepare a buffer containing CH3COOH with a pH of 5.44. If the pKa of acetic acid is 4.74, what ratio of [CH3COO⁻]/[CH3COOH] must you use?

Match the following. -pH = pKa2

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 after the addition of 150.0 mL of HNO3. The Kb of NH3 is 1.8 × 10-5.

Calculate the pH of a buffer that is 0.225 mol L-1 CH3COOH and 0.162 mol L-1 CH3COOK. The Ka for CH3COOH is 1.8 × 10-5.

What is the molar solubility of calcium hydroxide ( Ca(OH)2) in water? The solubility-product constant for CaOH2 is 4.5 × 10-6 at

Explain the common ion effect with respect to molar solubility.

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 mol L-1 NH4Cl with 200.0 mL of 0.12 mol L-1 NH3. The Kb for NH3 is 1.8 × 10-5.

Identify the compound that is acid-insoluble.

A 1.0 L buffer solution is 0.050 mol L-1 CH3COOH and 0.250 mol L-1 CH3COOLi. Which of the following actions will destroy the buffer?

Predict the number of equivalence point(s) in the titration for a diprotic acid with a strong base.

Determine the molar solubility of CuCl in a solution containing 0.050 mol L-1 KCl. Ksp (CuCl) = 1.0 × 10-6.

What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous hydrofluoric acid requires 30.00 mL of 0. 400 mol L-1 NaOH? Ka = 6.76 × 10-4 for HF.

Name the chemical compound that forms stalactites and stalagmites.

What is the pH of a solution made by mixing 30.00 mL of 0.10 mol L-1 acetic acid (CH3COOH) with 50.00 mL of 0. 100 mol L-1 KOH? Assume that the volumes of the solutions are additive. Ka = 1.8 × 10-5 for

A 1.50 L buffer solution is 0.250 mol L-1 in HF and 0.250 mol L-1 in NaF. Calculate the pH of the solution after the addition of 0.0500 moles of solid NaOH. Assume no volume change upon the addition of the base. The Ka for HF is 3.5 × 10-4.

What is the pH of a solution prepared by mixing 100.00 mL of 0.020 mol L-1 Ca(OH)2 with 50.00 mL of 0. 300 mol L-1 NaOH? Assume that the volumes are additive.

Solid potassium chromate (K2CrO4) is slowly added to a solution containing 0. 50 mol L-1 AgNO3 and 0. 50 mol L-1 Ba(NO3)2. What is the Ag+ concentration when BaCrO4 just starts to precipitate? The Ksp for Ag2CrO4 and BaCrO4 are 1.1 × 10-12 and respectively.

Calculate the pH of a buffer that is 0.158 mol L-1 HClO and 0.099 mol L-1 NaClO. The Ka for HClO is 2.9 × 10-8.

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 mol L-1 HCOOH with 100.0 mL of 0.20 mol L-1 HCOOLi. The Ka for HCHO2 is 1.8 × 10-4.

What is the molar solubility of silver iodide ( AgI ) in water? The solubility-product constant for AgI is 8.5 × 10-17 at 25 °C.

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You wish to prepare a buffer containing CH₃COOH with a pH of 5.44. If the pK_a of acetic acid is 4.74, what ratio of [CH₃COO⁻]/[CH₃COOH] must you use?

Match the following. -pH = pK_a2

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 after the addition of 150.0 mL of HNO₃. The K_b of NH₃ is 1.8 × 10^-5.

Calculate the pH of a buffer that is 0.225 mol L^-1 CH₃COOH and 0.162 mol L^-1 CH₃COOK. The K_a for CH₃COOH is 1.8 × 10^-5.

What is the molar solubility of calcium hydroxide ( Ca(OH)₂) in water? The solubility-product constant for CaOH₂ is 4.5 × 10^-6 at

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 mol L^-1 NH₄Cl with 200.0 mL of 0.12 mol L^-1 NH₃. The K_b for NH₃ is 1.8 × 10^-5.

A 1.0 L buffer solution is 0.050 mol L^-1 CH₃COOH and 0.250 mol L^-1 CH₃COOLi. Which of the following actions will destroy the buffer?

Determine the molar solubility of CuCl in a solution containing 0.050 mol L^-1 KCl. K_sp (CuCl) = 1.0 × 10^-6.

What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous hydrofluoric acid requires 30.00 mL of 0. 400 mol L^-1 NaOH? K_a = 6.76 × 10^-4 for HF.

What is the pH of a solution made by mixing 30.00 mL of 0.10 mol L^-1 acetic acid (CH₃COOH) with 50.00 mL of 0. 100 mol L^-1 KOH? Assume that the volumes of the solutions are additive. K_a = 1.8 × 10^-5for

A 1.50 L buffer solution is 0.250 mol L^-1 in HF and 0.250 mol L^-1 in NaF. Calculate the pH of the solution after the addition of 0.0500 moles of solid NaOH. Assume no volume change upon the addition of the base. The K_a for HF is 3.5 × 10^-4.

What is the pH of a solution prepared by mixing 100.00 mL of 0.020 mol L^-1 Ca(OH)₂ with 50.00 mL of 0. 300 mol L^-1 NaOH? Assume that the volumes are additive.

Solid potassium chromate (K₂CrO₄) is slowly added to a solution containing 0. 50 mol L^-1 AgNO₃ and 0. 50 mol L^-1 Ba(NO₃)₂. What is the Ag⁺ concentration when BaCrO₄ just starts to precipitate? The K_sp for Ag₂CrO₄ and BaCrO₄ are 1.1 × 10^-12 and respectively.

Calculate the pH of a buffer that is 0.158 mol L^-1 HClO and 0.099 mol L^-1 NaClO. The K_a for HClO is 2.9 × 10^-8.

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 mol L^-1 HCOOH with 100.0 mL of 0.20 mol L^-1 HCOOLi. The K_a for HCHO₂ is 1.8 × 10^-4.

What is the molar solubility of silver iodide ( AgI) in water? The solubility-product constant for AgI is 8.5 × 10^-17 at 25 °C.