Question 1

Determine the molar solubility for Al(OH)3 in pure water.Ksp for Al(OH)3 = 1.3 × 10-33.

Accepted Answer

A)  3.6 × 10-12 M 
B)  2.2 × 10-10 M 
C)  4.8 × 10-35 M 
D)  2.6 × 10-9 M 
E)  6.0 × 10-19 M 
A)  3.6 × 10-12 M 
B)  2.2 × 10-10 M 
C)  4.8 × 10-35 M 
D)  2.6 × 10-9 M 
E)  6.0 × 10-19 M

Question 2

What volume of 5.00 × 10-3 M HNO3 is needed to titrate 20.00 mL of 5.00 × 10-3 M Ca(OH)2 to the equivalence point?

Accepted Answer

A)  2.50 mL 
B)  10.0 mL 
C)  20.0 mL 
D)  40.0 mL 
E)  180. mL 
A)  2.50 mL 
B)  10.0 mL 
C)  20.0 mL 
D)  40.0 mL 
E)  180. mL

Question 3

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

Accepted Answer

A)  hydrochloric acid 
B)  potassium hydroxide 
C)  lithium bromide 
D)  calcium carbonate 
E)  sodium bicarbonate 
A)  hydrochloric acid 
B)  potassium hydroxide 
C)  lithium bromide 
D)  calcium carbonate 
E)  sodium bicarbonate

Question 4

What is the approximate pH at the equivalence point of a weak acid-strong base titration if 50.00 mL of aqueous hydrofluoric acid requires 60.00 mL of 0.200 M LiOH to reach the equivalence point? Ka = 6.76 × 10-4 for HF.

Accepted Answer

A)  1.89 
B)  5.90 
C)  8.10 
D)  12.10 
A)  1.89 
B)  5.90 
C)  8.10 
D)  12.10

Question 5

A 150.0 mL sample of 0.10 M Ba(OH)2 is titrated with 0.10 M HI.Determine the pH of the solution after the addition of 450.0 mL HI.

Accepted Answer

A)  1.60 
B)  1.30 
C)  1.00 
D)  12.40 
E)  1.12 
A)  1.60 
B)  1.30 
C)  1.00 
D)  12.40 
E)  1.12

Question 6

Calculate the pH of a solution formed by mixing 100.0 mL of 0.20 M HClO with 200.0 mL of 0.30 M NaClO.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

Question 7

Determine the molar solubility of BaF2 in pure water.Ksp for BaF2 = 2.45 × 10-5.

Accepted Answer

A)  1.83 × 10-2 M 
B)  1.23 × 10-5 M 
C)  2.90 × 10-2 M 
D)  4.95 × 10-3 M 
E)  6.13 × 10-6 M 
A)  1.83 × 10-2 M 
B)  1.23 × 10-5 M 
C)  2.90 × 10-2 M 
D)  4.95 × 10-3 M 
E)  6.13 × 10-6 M

Question 8

A 25.0-mL sample of 0.150 M butanoic acid is titrated with a 0.150 M NaOH solution.What is the pH before any base is added? The Ka of butanoic acid is 1.5 × 10-5.

Accepted Answer

A)  2.83 
B)  1.5 × 10-3 
C)  4.82 
D)  4.00 
E)  1.0 × 104 
A)  2.83 
B)  1.5 × 10-3 
C)  4.82 
D)  4.00 
E)  1.0 × 104

Question 9

Which of the following solutions is a good buffer system?

Accepted Answer

A)  a solution that is 0.10 M HC2H3O2 and 0.10 M LiC2H3O2 
B)  a solution that is 0.10 M HBr and 0.10 M KC2H3O2 
C)  a solution that is 0.10 M HI and 0.10 M NH4+ 
D)  a solution that is 0.10 M NaOH and 0.10 M KOH 
E)  None of the above is a buffer system. 
A)  a solution that is 0.10 M HC2H3O2 and 0.10 M LiC2H3O2 
B)  a solution that is 0.10 M HBr and 0.10 M KC2H3O2 
C)  a solution that is 0.10 M HI and 0.10 M NH4+ 
D)  a solution that is 0.10 M NaOH and 0.10 M KOH 
E)  None of the above is a buffer system.

Question 10

Identify the cation that is NOT amphoteric.

Accepted Answer

A)  Fe2+ 
B)  Cr3+ 
C)  Zn2+ 
D)  Pb2+ 
E)  Sn2+ 
A)  Fe2+ 
B)  Cr3+ 
C)  Zn2+ 
D)  Pb2+ 
E)  Sn2+

Question 11

A sample contains Ca3(PO4)2, PbS,AgCl,NH4Br,and ZnS.Identify the precipitate after the addition of 6 M HCl.

Accepted Answer

A)  Ca3(PO4)2 
B)  PbS 
C)  AgCl 
D)  NH4Br 
E)  ZnS 
A)  Ca3(PO4)2 
B)  PbS 
C)  AgCl 
D)  NH4Br 
E)  ZnS

Question 12

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 13

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 100.0 mL of HNO3.The Kb of NH3 is 1.8 × 10-5.

Accepted Answer

A)  6.58 
B)  10.56 
C)  8.72 
D)  3.44 
E)  5.28 
A)  6.58 
B)  10.56 
C)  8.72 
D)  3.44 
E)  5.28

Question 14

A 900.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M LiOH.Determine the pH of the solution after the addition of 300.0 mL of LiOH (this is the equivalence point).

Accepted Answer

A)  0.97 
B)  13.03 
C)  2.76 
D)  11.24 
E)  7.00 
A)  0.97 
B)  13.03 
C)  2.76 
D)  11.24 
E)  7.00

Question 15

A 200.0 mL sample of 0.20 M HF is titrated with 0.10 M NaOH.Determine the pH of the solution before the addition of any NaOH.The Ka of HF is 3.5 × 10-4.

Accepted Answer

A)  4.15 
B)  0.70 
C)  2.08 
D)  3.46 
E)  1.25 
A)  4.15 
B)  0.70 
C)  2.08 
D)  3.46 
E)  1.25

Question 16

Calculate the pH of a buffer that is 0.94 M HClO and 0.059 M NaClO.The Ka for HClO is 2.9 × 10-8.

Accepted Answer

A)  7.54 
B)  6.87 
C)  7.74 
D)  7.36 
E)  6.34 
A)  7.54 
B)  6.87 
C)  7.74 
D)  7.36 
E)  6.34

Question 17

When titrating a strong monoprotic acid and 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 18

Determine the solubility of the ions that is calculated from the Ksp for Mg2CO3.

Accepted Answer

A)  2S3 
B)  S3 
C)  4S3 
D)  S2 
E)  2S2 
A)  2S3 
B)  S3 
C)  4S3 
D)  S2 
E)  2S2

Question 19

The difference between Q and Ksp is

Accepted Answer

A)  Q is greater than Ksp. 
B)  no difference. 
C)  Ksp is the value of the product at equilibrium and Q is the value of the product under any condition. 
D)  Ksp is greater than Q. 
E)  Q is the value of the product at equilibrium and Ksp is the value of the product under any condition. 
A)  Q is greater than Ksp. 
B)  no difference. 
C)  Ksp is the value of the product at equilibrium and Q is the value of the product under any condition. 
D)  Ksp is greater than Q. 
E)  Q is the value of the product at equilibrium and Ksp is the value of the product under any condition.

Question 20

What is the pH of a solution prepared by mixing 100.00 mL of 0.020 M Ba(OH)2 with 50.00 mL of 0.300 M LiOH? 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

Exam 17: Aqueous Ionic Equilibrium

Determine the molar solubility for Al(OH)3 in pure water.Ksp for Al(OH)3 = 1.3 × 10-33.

What volume of 5.00 × 10-3 M HNO3 is needed to titrate 20.00 mL of 5.00 × 10-3 M Ca(OH)2 to the equivalence point?

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

What is the approximate pH at the equivalence point of a weak acid-strong base titration if 50.00 mL of aqueous hydrofluoric acid requires 60.00 mL of 0.200 M LiOH to reach the equivalence point? Ka = 6.76 × 10-4 for HF.

A 150.0 mL sample of 0.10 M Ba(OH)2 is titrated with 0.10 M HI.Determine the pH of the solution after the addition of 450.0 mL HI.

Calculate the pH of a solution formed by mixing 100.0 mL of 0.20 M HClO with 200.0 mL of 0.30 M NaClO.The Ka for HClO is 2.9 × 10-8.

Determine the molar solubility of BaF2 in pure water.Ksp for BaF2 = 2.45 × 10-5.

A 25.0-mL sample of 0.150 M butanoic acid is titrated with a 0.150 M NaOH solution.What is the pH before any base is added? The Ka of butanoic acid is 1.5 × 10-5.

Which of the following solutions is a good buffer system?

Identify the cation that is NOT amphoteric.

A sample contains Ca3(PO4)2, PbS,AgCl,NH4Br,and ZnS.Identify the precipitate after the addition of 6 M HCl.

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.

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 100.0 mL of HNO3.The Kb of NH3 is 1.8 × 10-5.

A 900.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M LiOH.Determine the pH of the solution after the addition of 300.0 mL of LiOH (this is the equivalence point).

A 200.0 mL sample of 0.20 M HF is titrated with 0.10 M NaOH.Determine the pH of the solution before the addition of any NaOH.The Ka of HF is 3.5 × 10-4.

Calculate the pH of a buffer that is 0.94 M HClO and 0.059 M NaClO.The Ka for HClO is 2.9 × 10-8.

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

Determine the solubility of the ions that is calculated from the Ksp for Mg2CO3.

The difference between Q and Ksp is

What is the pH of a solution prepared by mixing 100.00 mL of 0.020 M Ba(OH)2 with 50.00 mL of 0.300 M LiOH? Assume that the volumes are additive.

Matter, measurement, and Problem Solving

Atoms and Elements

Molecules,compounds,and Chemical Equations

Chemical Quantities and Aqueous Reactions

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding Ii: Molecular Shapes,valence Bond Theory,

Liquids,solids,and Intermolecular Forces

Solids and Modern Materials

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Free Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry

Biochemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Transition Metals and Coordination Compounds

Filters

Determine the molar solubility for Al(OH)₃ in pure water.K_sp for Al(OH)₃ = 1.3 × 10^-33.

What volume of 5.00 × 10^-3 M HNO₃ is needed to titrate 20.00 mL of 5.00 × 10^-3 M Ca(OH)₂ to the equivalence point?

What is the approximate pH at the equivalence point of a weak acid-strong base titration if 50.00 mL of aqueous hydrofluoric acid requires 60.00 mL of 0.200 M LiOH to reach the equivalence point? K_a = 6.76 × 10^-4 for HF.

A 150.0 mL sample of 0.10 M Ba(OH)₂ is titrated with 0.10 M HI.Determine the pH of the solution after the addition of 450.0 mL HI.

Calculate the pH of a solution formed by mixing 100.0 mL of 0.20 M HClO with 200.0 mL of 0.30 M NaClO.The K_a for HClO is 2.9 × 10^-8.

Determine the molar solubility of BaF₂in pure water.K_sp for BaF₂ = 2.45 × 10^-5.

A 25.0-mL sample of 0.150 M butanoic acid is titrated with a 0.150 M NaOH solution.What is the pH before any base is added? The K_a of butanoic acid is 1.5 × 10^-5.

A sample contains Ca₃(PO₄)₂,PbS,AgCl,NH₄Br,and ZnS.Identify the precipitate after the addition of 6 M HCl.

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.

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 100.0 mL of HNO₃.The K_b of NH₃ is 1.8 × 10^-5.

A 900.0 mL sample of 0.18 M HClO₄ is titrated with 0.27 M LiOH.Determine the pH of the solution after the addition of 300.0 mL of LiOH (this is the equivalence point).

A 200.0 mL sample of 0.20 M HF is titrated with 0.10 M NaOH.Determine the pH of the solution before the addition of any NaOH.The K_a of HF is 3.5 × 10^-4.

Calculate the pH of a buffer that is 0.94 M HClO and 0.059 M NaClO.The K_a for HClO is 2.9 × 10^-8.

Determine the solubility of the ions that is calculated from the Ksp for Mg₂CO₃.

What is the pH of a solution prepared by mixing 100.00 mL of 0.020 M Ba(OH)₂ with 50.00 mL of 0.300 M LiOH? Assume that the volumes are additive.