Question 1

Determine the molar solubility for Pb3(PO4)2 in pure water.Ksp for Pb3(PO4)2 is 1.0 × 10-54.

Accepted Answer

A)  4.1 × 10-28 M 
B)  5.8 × 10-10 M 
C)  1.1 × 10-11 M 
D)  6.2 × 10-12 M 
E)  1.0 × 10-54 M 
A)  4.1 × 10-28 M 
B)  5.8 × 10-10 M 
C)  1.1 × 10-11 M 
D)  6.2 × 10-12 M 
E)  1.0 × 10-54 M

Question 2

A 1.00 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 100.0 mL of 1.00 M HCl.The Ka for HF is 3.5 × 10-4.

Accepted Answer

A)  3.09 
B)  4.11 
C)  3.82 
D)  3.46 
E)  2.78 
A)  3.09 
B)  4.11 
C)  3.82 
D)  3.46 
E)  2.78

Question 3

Calculate the pH of a buffer that is 0.032 M HF and 0.032 M KF.The Ka for HF is 3.5 × 10-4.

Accepted Answer

A)  2.86 
B)  9.31 
C)  10.54 
D)  3.46 
E)  4.89 
A)  2.86 
B)  9.31 
C)  10.54 
D)  3.46 
E)  4.89

Question 4

What is the pH of a buffer solution that is 0.222 M in lactic acid and 0.132 M in sodium lactate? The Ka of lactic acid is 1.4 × 10-4.

Accepted Answer

A)  14.23 
B)  10.38 
C)  5.39 
D)  3.62 
E)  4.08 
A)  14.23 
B)  10.38 
C)  5.39 
D)  3.62 
E)  4.08

Question 5

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M NH4Cl with 100.0 mL of 0.20 M NH3.The Kb for NH3 is 1.8 × 10-5.

Accepted Answer

A)  9.13 
B)  9.25 
C)  9.53 
D)  4.74 
E)  8.98 
A)  9.13 
B)  9.25 
C)  9.53 
D)  4.74 
E)  8.98

Question 6

A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M 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)  1.70 
B)  6.44 
C)  7.56 
D)  12.30 
E)  2.30 
A)  1.70 
B)  6.44 
C)  7.56 
D)  12.30 
E)  2.30

Question 7

Which of the following would be considered a complex ion?

Accepted Answer

A)  F- 
B)  PO33- 
C)  AlF6- 
D)  Fe2+ 
E)  NH4+ 
A)  F- 
B)  PO33- 
C)  AlF6- 
D)  Fe2+ 
E)  NH4+

Question 8

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

Accepted Answer

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

Question 9

What is the pH of a solution prepared by mixing 100.00 mL of 0.020 M Ca(OH)2 with 50.00 mL of 0.100 M NaOH? Assume that the volumes are additive.

Accepted Answer

A)  12.67 
B)  12.78 
C)  12.95 
D)  13.25 
A)  12.67 
B)  12.78 
C)  12.95 
D)  13.25

Question 10

Determine the molar solubility of CuCl in a solution containing 0.040 M KCl.Ksp (CuCl)= 1.0 × 10-6.

Accepted Answer

A)  1.0 × 10-12 M 
B)  4.0 × 10-8 M 
C)  2.5 × 10-5 M 
D)  1.0 × 10-3 M 
E)  0.050 M 
A)  1.0 × 10-12 M 
B)  4.0 × 10-8 M 
C)  2.5 × 10-5 M 
D)  1.0 × 10-3 M 
E)  0.050 M

Question 11

What is the molar solubility of silver carbonate ( Ag2CO3 )in water? The solubility-product constant for Ag2CO3 is 8.1 × 10-12 at 25°C.

Accepted Answer

A)  1.4 × 10-6 
B)  2.0 × 10-4 
C)  4.0 × 10-6 
D)  1.3 × 10-4 
E)  2.7 × 10-12 
A)  1.4 × 10-6 
B)  2.0 × 10-4 
C)  4.0 × 10-6 
D)  1.3 × 10-4 
E)  2.7 × 10-12

Question 12

What is the [CH3CO2-]/[CH3CO2H] ratio necessary to make a buffer solution with a pH of 4.44? Ka = 1.8 × 10-5 for CH3CO2H.

Accepted Answer

A)  0.50:1 
B)  0.94:1 
C)  1.1:1 
D)  2.0:1 
A)  0.50:1 
B)  0.94:1 
C)  1.1:1 
D)  2.0:1

Question 13

Give the equation for an unsaturated solution in comparing Q with Ksp.

Accepted Answer

A)  Q > Ksp 
B)  Q sp 
C)  Q = Ksp 
D)  Q ≠ Ksp 
E)  none of the above 
A)  Q > Ksp 
B)  Q sp 
C)  Q = Ksp 
D)  Q ≠ Ksp 
E)  none of the above

Question 14

Stalactites and stalagmites form as ________ precipitates out of the water evaporating in underground caves.

Accepted Answer

A)  hydrochloric acid 
B)  sodium hydroxide 
C)  sodium chloride 
D)  calcium carbonate 
E)  sodium bicarbonate 
A)  hydrochloric acid 
B)  sodium hydroxide 
C)  sodium chloride 
D)  calcium carbonate 
E)  sodium bicarbonate

Question 15

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

Accepted Answer

A)  pH will be less than 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)  pH will be equal to 7 at the equivalence point. 
E)  titration will require more moles of acid than base to reach the equivalence point. 
A)  pH will be less than 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)  pH will be equal to 7 at the equivalence point. 
E)  titration will require more moles of acid than base to reach the equivalence point.

Question 16

Determine the molar solubility of BiPO4 in a solution containing 0.358 M K3PO4.The Ksp for BiPO4 is 1.3 × 10-23.

Accepted Answer

A)  5.7 × 10-15 
B)  3.6 × 10-23 
C)  1.3 × 10-13 
D)  1.5 × 10-8 
E)  8.3 × 10-18 
A)  5.7 × 10-15 
B)  3.6 × 10-23 
C)  1.3 × 10-13 
D)  1.5 × 10-8 
E)  8.3 × 10-18

Question 17

A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3.Determine the pH of the solution after the addition of 50.0 mL of HNO3.The Kb of NH3 is 1.8 × 10-5.

Accepted Answer

A)  4.74 
B)  7.78 
C)  7.05 
D)  9.26 
E)  10.34 
A)  4.74 
B)  7.78 
C)  7.05 
D)  9.26 
E)  10.34

Question 18

An important buffer in the blood is a mixture of

Accepted Answer

A)  sodium chloride and hydrochloric acid. 
B)  hydrochloric acid and sodium hydroxide. 
C)  carbonic acid and bicarbonate ion. 
D)  acetic acid and bicarbonate ion. 
E)  acetic acid and carbonate ion. 
A)  sodium chloride and hydrochloric acid. 
B)  hydrochloric acid and sodium hydroxide. 
C)  carbonic acid and bicarbonate ion. 
D)  acetic acid and bicarbonate ion. 
E)  acetic acid and carbonate ion.

Question 19

Identify the indicator that can be used at the lowest pH.

Accepted Answer

A)  2,4-dinitrophenol 
B)  thymol blue 
C)  crystal violet 
D)  thymolphthalein 
E)  methyl red 
A)  2,4-dinitrophenol 
B)  thymol blue 
C)  crystal violet 
D)  thymolphthalein 
E)  methyl red

Question 20

Calculate the percent ionization of nitrous acid in a solution that is 0.169 M in nitrous acid.The acid dissociation constant of nitrous acid is 4.50 × 10-4.

Accepted Answer

A)  7.61 × 10-5 
B)  0.0450 
C)  5.16 
D)  0.743 
E)  3.76 
A)  7.61 × 10-5 
B)  0.0450 
C)  5.16 
D)  0.743 
E)  3.76

Exam 18: Aqueous Ionic Equilibrium

Determine the molar solubility for Pb3(PO4)2 in pure water.Ksp for Pb3(PO4)2 is 1.0 × 10-54.

A 1.00 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 100.0 mL of 1.00 M HCl.The Ka for HF is 3.5 × 10-4.

Calculate the pH of a buffer that is 0.032 M HF and 0.032 M KF.The Ka for HF is 3.5 × 10-4.

What is the pH of a buffer solution that is 0.222 M in lactic acid and 0.132 M in sodium lactate? The Ka of lactic acid is 1.4 × 10-4.

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M NH4Cl with 100.0 mL of 0.20 M NH3.The Kb for NH3 is 1.8 × 10-5.

A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M 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.

Which of the following would be considered a complex ion?

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

What is the pH of a solution prepared by mixing 100.00 mL of 0.020 M Ca(OH)2 with 50.00 mL of 0.100 M NaOH? Assume that the volumes are additive.

Determine the molar solubility of CuCl in a solution containing 0.040 M KCl.Ksp (CuCl)= 1.0 × 10-6.

What is the molar solubility of silver carbonate ( Ag2CO3 )in water? The solubility-product constant for Ag2CO3 is 8.1 × 10-12 at 25°C.

What is the [CH3CO2-]/[CH3CO2H] ratio necessary to make a buffer solution with a pH of 4.44? Ka = 1.8 × 10-5 for CH3CO2H.

Give the equation for an unsaturated solution in comparing Q with Ksp.

Stalactites and stalagmites form as ________ precipitates out of the water evaporating in underground caves.

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

Determine the molar solubility of BiPO4 in a solution containing 0.358 M K3PO4.The Ksp for BiPO4 is 1.3 × 10-23.

A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3.Determine the pH of the solution after the addition of 50.0 mL of HNO3.The Kb of NH3 is 1.8 × 10-5.

An important buffer in the blood is a mixture of

Identify the indicator that can be used at the lowest pH.

Calculate the percent ionization of nitrous acid in a solution that is 0.169 M in nitrous acid.The acid dissociation constant of nitrous acid is 4.50 × 10-4.

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

Filters

Determine the molar solubility for Pb₃(PO₄)₂ in pure water.K_sp for Pb₃(PO₄)₂ is 1.0 × 10^-54.

A 1.00 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 100.0 mL of 1.00 M HCl.The K_a for HF is 3.5 × 10^-4.

Calculate the pH of a buffer that is 0.032 M HF and 0.032 M KF.The K_a for HF is 3.5 × 10^-4.

What is the pH of a buffer solution that is 0.222 M in lactic acid and 0.132 M in sodium lactate? The K_a of lactic acid is 1.4 × 10^-4.

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M NH₄Cl with 100.0 mL of 0.20 M NH₃.The K_b for NH₃ is 1.8 × 10^-5.

A 100.0 mL sample of 0.10 M NH₃ is titrated with 0.10 M 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.

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

What is the pH of a solution prepared by mixing 100.00 mL of 0.020 M Ca(OH)₂ with 50.00 mL of 0.100 M NaOH? Assume that the volumes are additive.

Determine the molar solubility of CuCl in a solution containing 0.040 M KCl.K_sp (CuCl)= 1.0 × 10^-6.

What is the molar solubility of silver carbonate ( Ag₂CO₃ )in water? The solubility-product constant for Ag₂CO₃ is 8.1 × 10^-12 at 25°C.

What is the [CH₃CO₂-]/[CH₃CO₂H] ratio necessary to make a buffer solution with a pH of 4.44? K_a = 1.8 × 10^-5for CH₃CO₂H.

Give the equation for an unsaturated solution in comparing Q with K_sp.

Determine the molar solubility of BiPO₄ in a solution containing 0.358 M K₃PO₄.The Ksp for BiPO₄is 1.3 × 10^-23.

A 100.0 mL sample of 0.10 M NH₃ is titrated with 0.10 M HNO₃.Determine the pH of the solution after the addition of 50.0 mL of HNO₃.The K_b of NH₃ is 1.8 × 10^-5.

Calculate the percent ionization of nitrous acid in a solution that is 0.169 M in nitrous acid.The acid dissociation constant of nitrous acid is 4.50 × 10^-4.