Question 1

Calculate the pH of a solution that has a concentration of 0.190 M H2S and 0.550 M KHS? The Ka of H2S is 1.1 × 10-7.

Accepted Answer

A)  11.02 
B)  7.49 
C)  3.22 
D)  7.42 
A)  11.02 
B)  7.49 
C)  3.22 
D)  7.42

Question 2

Determine the molar solubility of PbSO4 in pure water.Ksp (PbSO4)= 1.82 × 10-8.

Accepted Answer

A)  1.82 × 10-8 M 
B)  1.35 × 10-4 M 
C)  9.1 × 10-9 M 
D)  3.31 × 10-16 M 
E)  4.48 × 10-4 M 
A)  1.82 × 10-8 M 
B)  1.35 × 10-4 M 
C)  9.1 × 10-9 M 
D)  3.31 × 10-16 M 
E)  4.48 × 10-4 M

Question 3

Determine the molar solubility of Pb(IO3)2 in pure water.Ksp for Pb(IO3)2 = 2.60 × 10-13.

Accepted Answer

A)  4.02 × 10-5 M 
B)  9.35 × 10-6 M 
C)  5.08 × 10-7 M 
D)  6.48 × 10-5 M 
E)  2.23 × 10-6 M 
A)  4.02 × 10-5 M 
B)  9.35 × 10-6 M 
C)  5.08 × 10-7 M 
D)  6.48 × 10-5 M 
E)  2.23 × 10-6 M

Question 4

Determine the molar solubility of Ag2CrO4 in a solution containing 0.153 M AgNO3.The Ksp for Ag2CrO4 is 2.0 × 10-12.

Accepted Answer

A)  8.5 × 10-11 M 
B)  4.2 × 10-5 M 
C)  1.9 × 10-2 M 
D)  7.2 × 10-5 M 
E)  1.3 × 10-11 M 
A)  8.5 × 10-11 M 
B)  4.2 × 10-5 M 
C)  1.9 × 10-2 M 
D)  7.2 × 10-5 M 
E)  1.3 × 10-11 M

Question 5

A 1.0 L buffer solution is 0.250 M HC2H3O2 and 0.050 M NaC2H3O2.Which of the following actions will destroy the buffer?

Accepted Answer

A)  adding 0.050 moles of NaC2H3O2 
B)  adding 0.050 moles of HC2H3O2 
C)  adding 0.050 moles of HCl 
D)  adding 0.050 moles of NaOH 
E)  None of the above will destroy the buffer. 
A)  adding 0.050 moles of NaC2H3O2 
B)  adding 0.050 moles of HC2H3O2 
C)  adding 0.050 moles of HCl 
D)  adding 0.050 moles of NaOH 
E)  None of the above will destroy the buffer.

Question 6

Determine the molar solubility of Al(OH)3 in a solution containing 0.0500 M AlCl3.Ksp (Al(OH)3)= 1.3 × 10-33.

Accepted Answer

A)  2.6 × 10-9M 
B)  5.2 × 10-31 M 
C)  9.87 × 10-12 M 
D)  1.04 × 10-29 M 
E)  6.5 × 10-35 M 
A)  2.6 × 10-9M 
B)  5.2 × 10-31 M 
C)  9.87 × 10-12 M 
D)  1.04 × 10-29 M 
E)  6.5 × 10-35 M

Question 7

Describe the solubility of Al(OH)3 with respect to pH.

Accepted Answer

A)  soluble at low pH, insoluble in pH-neutral solution, and soluble at high pH 
B)  soluble at low pH, insoluble in pH-neutral solution, and insoluble at high pH 
C)  insoluble at low pH,insoluble in pH-neutral solution, and soluble at high pH 
D)  soluble at low pH, in pH-neutral solution, and at high pH 
E)  pH has no effect on the solubility. 
A)  soluble at low pH, insoluble in pH-neutral solution, and soluble at high pH 
B)  soluble at low pH, insoluble in pH-neutral solution, and insoluble at high pH 
C)  insoluble at low pH,insoluble in pH-neutral solution, and soluble at high pH 
D)  soluble at low pH, in pH-neutral solution, and at high pH 
E)  pH has no effect on the solubility.

Question 8

A sample contains Ba3(PO4)2, CdS,AgCl,NH4Cl,and ZnS.Identify the precipitate after the addition of 6 M HCl,then H2S and 0.2 M HCl.

Accepted Answer

A)  Ba3(PO4)2 
B)  CuS 
C)  AgCl 
D)  NH4Cl 
E)  CoS 
A)  Ba3(PO4)2 
B)  CuS 
C)  AgCl 
D)  NH4Cl 
E)  CoS

Question 9

What is the pH of a solution made by mixing 40.00 mL of 0.100 M HCl with 25.00 mL of 0.100 M KOH? Assume that the volumes of the solutions are additive.

Accepted Answer

A)  0.64 
B)  1.64 
C)  12.36 
D)  13.36 
E)  10.00 
A)  0.64 
B)  1.64 
C)  12.36 
D)  13.36 
E)  10.00

Question 10

A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH.Determine the pH of the solution after the addition of 200.0 mL of KOH.The Ka of HF is 3.5 × 10-4.

Accepted Answer

A)  9.62 
B)  7.00 
C)  3.46 
D)  10.54 
E)  8.14 
A)  9.62 
B)  7.00 
C)  3.46 
D)  10.54 
E)  8.14

Question 11

A solution of NaF is added dropwise to a solution that is 0.0158 M in Ba2+.When the concentration of F- exceeds ________ M,BaF2 will precipitate.Neglect volume changes.For BaF2,Ksp = 1.7 × 10-6.

Accepted Answer

A)  5.4 × 10-5 
B)  1.0 × 10-2 
C)  2.7 × 10-8 
D)  2.6 × 10-3 
E)  1.1 × 10-4 
A)  5.4 × 10-5 
B)  1.0 × 10-2 
C)  2.7 × 10-8 
D)  2.6 × 10-3 
E)  1.1 × 10-4

Question 12

Identify a good buffer.

Accepted Answer

A)  small amounts of both a weak acid and its conjugate base 
B)  significant amounts of both a strong acid and a strong base 
C)  small amounts of both a strong acid and a strong base 
D)  significant amounts of both a weak acid and a strong acid 
E)  significant amounts of both a weak acid and its conjugate base 
A)  small amounts of both a weak acid and its conjugate base 
B)  significant amounts of both a strong acid and a strong base 
C)  small amounts of both a strong acid and a strong base 
D)  significant amounts of both a weak acid and a strong acid 
E)  significant amounts of both a weak acid and its conjugate base

Question 13

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

Accepted Answer

A)  alizarin 
B)  thymol blue 
C)  methyl red 
D)  thymolphthalein 
E)  alizarin yellow R 
A)  alizarin 
B)  thymol blue 
C)  methyl red 
D)  thymolphthalein 
E)  alizarin yellow R

Question 14

What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M CH3CO2H with 25.00 mL of 0.040 M CH3CO2Na? Assume that the volume of the solutions are additive and that Ka = 1.8 × 10-5 for CH3CO2H.

Accepted Answer

A)  2.87 
B)  4.35 
C)  4.75 
D)  5.14 
A)  2.87 
B)  4.35 
C)  4.75 
D)  5.14

Question 15

A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in LiF.Calculate the pH of the solution after the addition of 0.150 moles of solid LiOH.Assume no volume change upon the addition of base.The Ka for HF is 3.5 × 10-4.

Accepted Answer

A)  3.46 
B)  4.06 
C)  2.85 
D)  3.63 
E)  4.24 
A)  3.46 
B)  4.06 
C)  2.85 
D)  3.63 
E)  4.24

Question 16

How many milliliters of 0.175 M of Ba(OH)2 are required to titrate 78.5 mL of 0.0750M H I to the equivalence point?

Accepted Answer

A)  33.6 mL 
B)  67.3 mL 
C)  135 mL 
D)  78.5 mL 
A)  33.6 mL 
B)  67.3 mL 
C)  135 mL 
D)  78.5 mL

Question 17

Which of the following acids (listed with pKa values)and their conjugate base would form a buffer with a pH of 8.10?

Accepted Answer

A)  HC7H5O2, pKa = 4.19 
B)  H2SO3, pKa = 1.77 
C)  HClO, pKa = 7.54 
D)  HCN, pKa = 9.31 
E)  HNO2, pKa = 3.34 
A)  HC7H5O2, pKa = 4.19 
B)  H2SO3, pKa = 1.77 
C)  HClO, pKa = 7.54 
D)  HCN, pKa = 9.31 
E)  HNO2, pKa = 3.34

Question 18

Calculate the molar solubility of thallium chloride in 0.40 M NaCl at 25°C.Ksp for TlCl is 1.7 × 10-4.

Accepted Answer

A)  6.8 × 10-5 M 
B)  4.2 × 10-4 M 
C)  8.2 × 10-3 M 
D)  1.3 × 10-2 M 
A)  6.8 × 10-5 M 
B)  4.2 × 10-4 M 
C)  8.2 × 10-3 M 
D)  1.3 × 10-2 M

Question 19

A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH.Determine the pH of the solution after the addition of 400.0 mL of KOH.The Ka of HF is 3.5 × 10-4.

Accepted Answer

A)  13.08 
B)  12.60 
C)  13.85 
D)  12.30 
E)  12.78 
A)  13.08 
B)  12.60 
C)  13.85 
D)  12.30 
E)  12.78

Question 20

Describe the information necessary (and why)to chose a good indicator for a weak acid/strong base titration.

Accepted Answer

In order to choose an appropriate indica

Exam 18: Aqueous Ionic Equilibrium

Calculate the pH of a solution that has a concentration of 0.190 M H2S and 0.550 M KHS? The Ka of H2S is 1.1 × 10-7.

Determine the molar solubility of PbSO4 in pure water.Ksp (PbSO4)= 1.82 × 10-8.

Determine the molar solubility of Pb(IO3)2 in pure water.Ksp for Pb(IO3)2 = 2.60 × 10-13.

Determine the molar solubility of Ag2CrO4 in a solution containing 0.153 M AgNO3.The Ksp for Ag2CrO4 is 2.0 × 10-12.

A 1.0 L buffer solution is 0.250 M HC2H3O2 and 0.050 M NaC2H3O2.Which of the following actions will destroy the buffer?

Determine the molar solubility of Al(OH)3 in a solution containing 0.0500 M AlCl3.Ksp (Al(OH)3)= 1.3 × 10-33.

Describe the solubility of Al(OH)3 with respect to pH.

A sample contains Ba3(PO4)2, CdS,AgCl,NH4Cl,and ZnS.Identify the precipitate after the addition of 6 M HCl,then H2S and 0.2 M HCl.

What is the pH of a solution made by mixing 40.00 mL of 0.100 M HCl with 25.00 mL of 0.100 M KOH? Assume that the volumes of the solutions are additive.

A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH.Determine the pH of the solution after the addition of 200.0 mL of KOH.The Ka of HF is 3.5 × 10-4.

A solution of NaF is added dropwise to a solution that is 0.0158 M in Ba2+.When the concentration of F- exceeds ________ M,BaF2 will precipitate.Neglect volume changes.For BaF2,Ksp = 1.7 × 10-6.

Identify a good buffer.

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

What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M CH3CO2H with 25.00 mL of 0.040 M CH3CO2Na? Assume that the volume of the solutions are additive and that Ka = 1.8 × 10-5 for CH3CO2H.

A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in LiF.Calculate the pH of the solution after the addition of 0.150 moles of solid LiOH.Assume no volume change upon the addition of base.The Ka for HF is 3.5 × 10-4.

How many milliliters of 0.175 M of Ba(OH)2 are required to titrate 78.5 mL of 0.0750M H I to the equivalence point?

Which of the following acids (listed with pKa values)and their conjugate base would form a buffer with a pH of 8.10?

Calculate the molar solubility of thallium chloride in 0.40 M NaCl at 25°C.Ksp for TlCl is 1.7 × 10-4.

A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH.Determine the pH of the solution after the addition of 400.0 mL of KOH.The Ka of HF is 3.5 × 10-4.

Describe the information necessary (and why)to chose a good indicator for a weak acid/strong base titration.

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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Calculate the pH of a solution that has a concentration of 0.190 M H₂S and 0.550 M KHS? The K_a of H₂S is 1.1 × 10^-7.

Determine the molar solubility of PbSO₄ in pure water.K_sp (PbSO₄)= 1.82 × 10^-8.

Determine the molar solubility of Pb(IO₃)₂in pure water.K_sp for Pb(IO₃)₂= 2.60 × 10^-13.

Determine the molar solubility of Ag₂CrO₄ in a solution containing 0.153 M AgNO₃.The Ksp for Ag₂CrO₄is 2.0 × 10^-12.

A 1.0 L buffer solution is 0.250 M HC₂H₃O₂ and 0.050 M NaC₂H₃O₂.Which of the following actions will destroy the buffer?

Determine the molar solubility of Al(OH)₃ in a solution containing 0.0500 M AlCl₃.K_sp (Al(OH)₃)= 1.3 × 10^-33.

Describe the solubility of Al(OH)₃ with respect to pH.

A sample contains Ba₃(PO₄)₂,CdS,AgCl,NH₄Cl,and ZnS.Identify the precipitate after the addition of 6 M HCl,then H₂S and 0.2 M HCl.

A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH.Determine the pH of the solution after the addition of 200.0 mL of KOH.The K_a of HF is 3.5 × 10^-4.

A solution of NaF is added dropwise to a solution that is 0.0158 M in Ba²⁺.When the concentration of F^- exceeds ________ M,BaF₂ will precipitate.Neglect volume changes.For BaF₂,K_sp = 1.7 × 10^-6.

What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M CH₃CO₂H with 25.00 mL of 0.040 M CH₃CO₂Na? Assume that the volume of the solutions are additive and that K_a = 1.8 × 10^-5 for CH₃CO₂H.

A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in LiF.Calculate the pH of the solution after the addition of 0.150 moles of solid LiOH.Assume no volume change upon the addition of base.The K_a for HF is 3.5 × 10^-4.

How many milliliters of 0.175 M of Ba(OH)₂ are required to titrate 78.5 mL of 0.0750M H I to the equivalence point?

Which of the following acids (listed with pK_a values)and their conjugate base would form a buffer with a pH of 8.10?

Calculate the molar solubility of thallium chloride in 0.40 M NaCl at 25°C.K_sp for TlCl is 1.7 × 10^-4.

A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH.Determine the pH of the solution after the addition of 400.0 mL of KOH.The K_a of HF is 3.5 × 10^-4.