Question 1

A 100.0 mL sample of 0.10 M Ca(OH)2 is titrated with 0.10 M 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 2

A weak acid is titrated with a strong base to the equivalence point.The pH of the resulting solution is found to be 9.18.The pKa of the acid is

Accepted Answer

A)  9.18. 
B)  7.00. 
C)  4.59. 
D)  2.50. 
E)  6.28. 
A)  9.18. 
B)  7.00. 
C)  4.59. 
D)  2.50. 
E)  6.28.

Question 3

Which of the following compounds solubility will not be affected by a low pH in solution?

Accepted Answer

A)  AgCl 
B)  Ca(OH)2 
C)  SrF2 
D)  CuS 
E)  CaCO3 
A)  AgCl 
B)  Ca(OH)2 
C)  SrF2 
D)  CuS 
E)  CaCO3

Question 4

Determine the molar solubility of AgBr in a solution containing 0.150 M NaBr.Ksp (AgBr)= 7.7 × 10-13.

Accepted Answer

A)  8.8 × 10-7 M 
B)  3.9 × 10-13 M 
C)  5.8 × 10-5 M 
D)  5.1 × 10-12 M 
E)  0.150 M 
A)  8.8 × 10-7 M 
B)  3.9 × 10-13 M 
C)  5.8 × 10-5 M 
D)  5.1 × 10-12 M 
E)  0.150 M

Question 5

Calculate the pH of a buffer that is 0.200 M H3BO3 and 0.122 M KH2BO3.The Ka for H3BO3 is 5.8 × 10-10.

Accepted Answer

A)  8.93 
B)  9.02 
C)  10.77 
D)  9.46 
E)  3.52 
A)  8.93 
B)  9.02 
C)  10.77 
D)  9.46 
E)  3.52

Question 6

Determine the molar solubility of BaF2 in a solution containing 0.0750 M LiF.Ksp (BaF2)= 1.7 × 10-6.

Accepted Answer

A)  2.3 × 10-5 M 
B)  8.5 × 10-7 M 
C)  1.2 × 10-2 M 
D)  0.0750 M 
E)  3.0 × 10-4 M 
A)  2.3 × 10-5 M 
B)  8.5 × 10-7 M 
C)  1.2 × 10-2 M 
D)  0.0750 M 
E)  3.0 × 10-4 M

Question 7

Give the expression for the solubility product constant for BaF2.

Accepted Answer

A)    
B)    
C)  [Ba2+]2[ F⁻] 
D)  [Ba2+][F⁻]2 
E)  [Ba2+][ F⁻] 
A)    
B)    
C)  [Ba2+]2[ F⁻] 
D)  [Ba2+][F⁻]2 
E)  [Ba2+][ F⁻]

Question 8

Calculate the pH of a solution formed by mixing 250.0 mL of 0.900 M NH4Cl with 250.0 mL of 1.60 M NH3.The Kb for NH3 is 1.8 × 10-5.

Accepted Answer

A)  8.25 
B)  9.18 
C)  9.50 
D)  10.12 
E)  10.83 
A)  8.25 
B)  9.18 
C)  9.50 
D)  10.12 
E)  10.83

Question 9

A sample contains Ba3(PO4)2, CdS,AgCl,NH4Cl,and ZnS.Identify the soluble ions after the addition of 6 M HCl; H2S and 0.2 M HCl; OH- to a pH of 8; and (NH4)2HPO4 with NH3.

Accepted Answer

A)  Ba3(PO4)2 
B)  CdS 
C)  AgCl 
D)  NH4Cl 
E)  FeS 
A)  Ba3(PO4)2 
B)  CdS 
C)  AgCl 
D)  NH4Cl 
E)  FeS

Question 10

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 the 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 the 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 11

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M NH3 with 10.00 mL of 0.10 M NH4Cl? Assume that the volume of the solutions are additive and that Kb = 1.8 × 10-5 for NH3.

Accepted Answer

A)  8.56 
B)  9.28 
C)  9.95 
D)  11.13 
A)  8.56 
B)  9.28 
C)  9.95 
D)  11.13

Question 12

A 1.50 L buffer solution is 0.250 M in HF and 0.250 M in NaF.Calculate the pH of the solution after the addition of 0.100 moles of solid NaOH.Assume no volume change upon the addition of base.The Ka for HF is 3.5 × 10-4.

Accepted Answer

A)  3.22 
B)  3.82 
C)  3.69 
D)  3.09 
E)  4.46 
A)  3.22 
B)  3.82 
C)  3.69 
D)  3.09 
E)  4.46

Question 13

Which of the following compounds will be more soluble in acidic solution than in pure water?

Accepted Answer

A)  PbI2 
B)  CuS 
C)  Ca(ClO4)2 
D)  CuCl 
E)  None of the above will be more soluble in acidic solution. 
A)  PbI2 
B)  CuS 
C)  Ca(ClO4)2 
D)  CuCl 
E)  None of the above will be more soluble in acidic solution.

Question 14

If a chemist wishes to prepare a buffer that will be effective at a pH of 3.00 at 25°C,the best choice would be an acid component with a Ka equal to

Accepted Answer

A)  9.10 × 10-2. 
B)  9.10 × 10-4. 
C)  9.10 × 10-6. 
D)  9.10 × 10-8. 
E)  9.10 × 10-10. 
A)  9.10 × 10-2. 
B)  9.10 × 10-4. 
C)  9.10 × 10-6. 
D)  9.10 × 10-8. 
E)  9.10 × 10-10.

Question 15

Sketch the titration curve for a strong acid titrated with a strong base.Make sure to indicate the equivalence point (and whether it is acidic,basic or neutral)and the buffer region.

Accepted Answer

See figure

Question 16

Calculate the solubility (in g/L)of silver chromate in water at 25°C if the Ksp for   is 1.1 ×   .

Accepted Answer

A)  3.5 × 10-4 g/L 
B)  2.2 × 10-2 g/L 
C)  2.7 × 10-2 g/L 
D)  3.4 × 10-2 g/L 
A)  3.5 × 10-4 g/L 
B)  2.2 × 10-2 g/L 
C)  2.7 × 10-2 g/L 
D)  3.4 × 10-2 g/L

Question 17

Calculate the pH of a solution that is 0.210 M in nitrous acid (   )and 0.290 M in potassium nitrite (   ).The acid dissociation constant of nitrous acid is 4.50 ×   .

Accepted Answer

A)  3.487 
B)  3.210 
C)  13.86 
D)  10.51 
E)  4.562 
A)  3.487 
B)  3.210 
C)  13.86 
D)  10.51 
E)  4.562

Question 18

What is the pH at the equivalence point of a weak base-strong acid titration if 20.00 mL of NaOCl requires 28.30 mL of 0.20 M HCl? Ka = 3.0 × 10-8 for HOCl.

Accepted Answer

A)  0.70 
B)  3.39 
C)  3.76 
D)  4.23 
A)  0.70 
B)  3.39 
C)  3.76 
D)  4.23

Question 19

A 100.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M LiOH.Determine the pH of the solution after the addition of 100.0 mL of LiOH.

Accepted Answer

A)  13.13 
B)  12.65 
C)  1.35 
D)  0.87 
E)  12.95 
A)  13.13 
B)  12.65 
C)  1.35 
D)  0.87 
E)  12.95

Question 20

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

Exam 18: Aqueous Ionic Equilibrium

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

A weak acid is titrated with a strong base to the equivalence point.The pH of the resulting solution is found to be 9.18.The pKa of the acid is

Which of the following compounds solubility will not be affected by a low pH in solution?

Determine the molar solubility of AgBr in a solution containing 0.150 M NaBr.Ksp (AgBr)= 7.7 × 10-13.

Calculate the pH of a buffer that is 0.200 M H3BO3 and 0.122 M KH2BO3.The Ka for H3BO3 is 5.8 × 10-10.

Determine the molar solubility of BaF2 in a solution containing 0.0750 M LiF.Ksp (BaF2)= 1.7 × 10-6.

Give the expression for the solubility product constant for BaF2.

Calculate the pH of a solution formed by mixing 250.0 mL of 0.900 M NH4Cl with 250.0 mL of 1.60 M NH3.The Kb for NH3 is 1.8 × 10-5.

A sample contains Ba3(PO4)2, CdS,AgCl,NH4Cl,and ZnS.Identify the soluble ions after the addition of 6 M HCl; H2S and 0.2 M HCl; OH- to a pH of 8; and (NH4)2HPO4 with NH3.

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

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M NH3 with 10.00 mL of 0.10 M NH4Cl? Assume that the volume of the solutions are additive and that Kb = 1.8 × 10-5 for NH3.

A 1.50 L buffer solution is 0.250 M in HF and 0.250 M in NaF.Calculate the pH of the solution after the addition of 0.100 moles of solid NaOH.Assume no volume change upon the addition of base.The Ka for HF is 3.5 × 10-4.

Which of the following compounds will be more soluble in acidic solution than in pure water?

If a chemist wishes to prepare a buffer that will be effective at a pH of 3.00 at 25°C,the best choice would be an acid component with a Ka equal to

Sketch the titration curve for a strong acid titrated with a strong base.Make sure to indicate the equivalence point (and whether it is acidic,basic or neutral)and the buffer region.

Calculate the solubility (in g/L)of silver chromate in water at 25°C if the Ksp for is 1.1 × .

Calculate the pH of a solution that is 0.210 M in nitrous acid ( )and 0.290 M in potassium nitrite ( ).The acid dissociation constant of nitrous acid is 4.50 × .

What is the pH at the equivalence point of a weak base-strong acid titration if 20.00 mL of NaOCl requires 28.30 mL of 0.20 M HCl? Ka = 3.0 × 10-8 for HOCl.

A 100.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M LiOH.Determine the pH of the solution after the addition of 100.0 mL of LiOH.

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

Essentials: Units, Measurements, and Problem Solving

Atoms

The Quantum Mechanical Model of the Atom

Periodic Properties of the Elements

Molecules and Compounds

Chemical Bonding I

Chemical Bonding Ii

Chemical Reactions and Chemical Quantities

Introduction to Solutions and Aqueous Reactions

Thermochemistry

Gases

Liquids, Solids, and Intermolecular Forces

Crystalline Solids and Modern Materials

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Free Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry

Transition Metals and Coordination Compounds

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

A weak acid is titrated with a strong base to the equivalence point.The pH of the resulting solution is found to be 9.18.The pK_a of the acid is

Determine the molar solubility of AgBr in a solution containing 0.150 M NaBr.K_sp (AgBr)= 7.7 × 10^-13.

Calculate the pH of a buffer that is 0.200 M H₃BO₃ and 0.122 M KH₂BO₃.The K_a for H₃BO₃ is 5.8 × 10^-10.

Determine the molar solubility of BaF₂ in a solution containing 0.0750 M LiF.K_sp (BaF₂)= 1.7 × 10^-6.

Give the expression for the solubility product constant for BaF₂.

Calculate the pH of a solution formed by mixing 250.0 mL of 0.900 M NH₄Cl with 250.0 mL of 1.60 M NH₃.The K_b for NH₃ is 1.8 × 10^-5.

A sample contains Ba₃(PO₄)₂,CdS,AgCl,NH₄Cl,and ZnS.Identify the soluble ions after the addition of 6 M HCl; H₂S and 0.2 M HCl; OH^-to a pH of 8; and (NH₄)₂HPO₄ with NH₃.

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M NH₃ with 10.00 mL of 0.10 M NH₄Cl? Assume that the volume of the solutions are additive and that K_b = 1.8 × 10^-5for NH₃.

A 1.50 L buffer solution is 0.250 M in HF and 0.250 M in NaF.Calculate the pH of the solution after the addition of 0.100 moles of solid NaOH.Assume no volume change upon the addition of base.The K_a for HF is 3.5 × 10^-4.

If a chemist wishes to prepare a buffer that will be effective at a pH of 3.00 at 25°C,the best choice would be an acid component with a K_a equal to

Calculate the solubility (in g/L)of silver chromate in water at 25°C if the K_sp for is 1.1 × .

What is the pH at the equivalence point of a weak base-strong acid titration if 20.00 mL of NaOCl requires 28.30 mL of 0.20 M HCl? K_a = 3.0 × 10^-8 for HOCl.

A 100.0 mL sample of 0.18 M HClO₄ is titrated with 0.27 M LiOH.Determine the pH of the solution after the addition of 100.0 mL of LiOH.

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