Question 1

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

Accepted Answer

A)  1.74 
B)  1.05 
C)  0.74 
D)  0.57 
E)  1.57 
A)  1.74 
B)  1.05 
C)  0.74 
D)  0.57 
E)  1.57 C

Question 2

Calculate the pH of a solution formed by mixing 200.0 mL of 0.30 M HClO with 300.0 mL of 0.20 M KClO.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 C

Question 3

Calculate the pH of a buffer that is 0.115 M HC2H3O2 and 0.160 M KC2H3O2.The Ka for HC2H3O2 is 1.8 × 10-5.

Accepted Answer

A)  4.89 
B)  8.81 
C)  4.74 
D)  5.15 
E)  4.60 
A)  4.89 
B)  8.81 
C)  4.74 
D)  5.15 
E)  4.60 A

Question 4

What is the molar solubility of zinc oxalate ( ZnC2O4 )in water? The solubility-product constant for ZnC2O4 is 2.7 × 10-8 at 25°C.

Accepted Answer

A)  1.4 × 10-8 
B)  5.4 × 10-8 
C)  7.57 
D)  2.3 × 10-4 
E)  1.6 × 10-4 
A)  1.4 × 10-8 
B)  5.4 × 10-8 
C)  7.57 
D)  2.3 × 10-4 
E)  1.6 × 10-4

Question 5

Determine the molar solubility of MgCO3 in pure water.Ksp (MgCO3)= 6.82 × 10-6.

Accepted Answer

A)  6.82 × 10-6 M 
B)  3.41 × 10-6 M 
C)  4.65 × 10-3 M 
D)  2.61 × 10-3 M 
E)  3.25 × 10-4 M 
A)  6.82 × 10-6 M 
B)  3.41 × 10-6 M 
C)  4.65 × 10-3 M 
D)  2.61 × 10-3 M 
E)  3.25 × 10-4 M

Question 6

The molar solubility of Ag2S is 1.26 × 10-16 M in pure water.Calculate the Ksp for Ag2S.

Accepted Answer

A)  1.59 × 10-32 
B)  1.12 × 10-8 
C)  6.81 × 10-63 
D)  3.78 × 10-12 
E)  8.00 × 10-48 
A)  1.59 × 10-32 
B)  1.12 × 10-8 
C)  6.81 × 10-63 
D)  3.78 × 10-12 
E)  8.00 × 10-48

Question 7

Sketch the titration curve for a monoprotic weak 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 8

Give the equation for a supersaturated 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 9

Determine the molar solubility of CaSO4 in a solution containing 0.14 M Na2SO4.Ksp (CaSO4)= 2.4 × 10-5.

Accepted Answer

A)  3.4 × 10-6 M 
B)  1.7 × 10-4 M 
C)  5.8 × 10-10 M 
D)  4.9 × 10-3 M 
E)  0.10 M 
A)  3.4 × 10-6 M 
B)  1.7 × 10-4 M 
C)  5.8 × 10-10 M 
D)  4.9 × 10-3 M 
E)  0.10 M

Question 10

A 1.00 L buffer solution is 0.150 M in HC7H5O2 and 0.250 M in LiC7H5O2.Calculate the pH of the solution after the addition of 100.0 mL of 1.00 M HCl.The Ka for HC7H5O2 is 6.5 × 10-5.

Accepted Answer

A)  4.19 
B)  5.03 
C)  4.41 
D)  3.34 
E)  3.97 
A)  4.19 
B)  5.03 
C)  4.41 
D)  3.34 
E)  3.97

Question 11

Define a buffer.

Accepted Answer

Buffers contain significant am

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 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 13

What is the pH of a solution made by mixing 20.00 mL of 0.100 M HCl with 40.00 mL of 0.100 M KOH? Assume that the volumes of the solutions are additive.

Accepted Answer

A)  0.48 
B)  1.48 
C)  12.52 
D)  13.52 
A)  0.48 
B)  1.48 
C)  12.52 
D)  13.52

Question 14

Determine the molar solubility for Ag2C2O4 in pure water.The Ksp for Ag2C2O4 is 3.5 × 10-11.

Accepted Answer

A)  1.8 × 10-11 M 
B)  1.4 × 10-6 M 
C)  5.9 × 10-6 M 
D)  2.1 × 10-4 M 
E)  3.5 × 10-6 M 
A)  1.8 × 10-11 M 
B)  1.4 × 10-6 M 
C)  5.9 × 10-6 M 
D)  2.1 × 10-4 M 
E)  3.5 × 10-6 M

Question 15

If the pKa of HCHO2 is 3.74 and the pH of an HCHO2/NaCHO2 solution is 3.89,which of the following is TRUE?

Accepted Answer

A)  [HCHO2] 2] 
B)  [HCHO2] = [NaCHO2] 
C)  [HCHO2] > [NaCHO2] 
D)  [HCHO2] >> [NaCHO2] 
E)  It is not possible to make a buffer of this pH from HCHO2 and NaCHO2. 
A)  [HCHO2] 2] 
B)  [HCHO2] = [NaCHO2] 
C)  [HCHO2] > [NaCHO2] 
D)  [HCHO2] >> [NaCHO2] 
E)  It is not possible to make a buffer of this pH from HCHO2 and NaCHO2.

Question 16

A solution contains 0.021 M Cl⁻ and 0.017 M I⁻.A solution containing copper (I)ions is added to selectively precipitate one of the ions.At what concentration of copper (I)ion will a precipitate begin to form? What is the identity of the precipitate?
Ksp(CuCl)= 1.0 × 10-6,Ksp(CuI)= 5.1 × 10-12.

Accepted Answer

A)  3.0 × 10-10 M, CuI 
B)  3.0 × 10-10 M, CuCl 
C)  4.8 × 10-5 M, CuCl 
D)  4.8 × 10-5 M, CuI 
E)  No precipitate will form at any concentration of copper (I). 
A)  3.0 × 10-10 M, CuI 
B)  3.0 × 10-10 M, CuCl 
C)  4.8 × 10-5 M, CuCl 
D)  4.8 × 10-5 M, CuI 
E)  No precipitate will form at any concentration of copper (I).

Question 17

A solution contains 3.8 × 10-2 M in Al3+ and 0.29 M in NaF.If the Kf for AlF63- is 7 × 1019,how much aluminum ion remains at equilibrium?

Accepted Answer

A)  1.1 × 10-19 M 
B)  3.1 × 10-22 M 
C)  9.1 × 10-19 M 
D)  1.9 × 10-21 M 
E)  4.4 × 10-20 M 
A)  1.1 × 10-19 M 
B)  3.1 × 10-22 M 
C)  9.1 × 10-19 M 
D)  1.9 × 10-21 M 
E)  4.4 × 10-20 M

Question 18

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M NH4Cl with 200.0 mL of 0.12 M 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 19

Gives what happens at neutral pH for aluminum hydroxide.

Accepted Answer

A)  Al(H2O)53+ precipitates 
B)  Al(H2O)4(OH)2- dissolves 
C)  Al(OH)3 precipitates 
D)  Al precipitates 
E)  Al dissolves 
A)  Al(H2O)53+ precipitates 
B)  Al(H2O)4(OH)2- dissolves 
C)  Al(OH)3 precipitates 
D)  Al precipitates 
E)  Al dissolves

Question 20

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 200.0 mL HBr.

Accepted Answer

A)  2.62 
B)  2.00 
C)  1.48 
D)  12.52 
E)  7.00 
A)  2.62 
B)  2.00 
C)  1.48 
D)  12.52 
E)  7.00

Exam 18: Aqueous Ionic Equilibrium

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

Calculate the pH of a solution formed by mixing 200.0 mL of 0.30 M HClO with 300.0 mL of 0.20 M KClO.The Ka for HClO is 2.9 × 10-8.

Calculate the pH of a buffer that is 0.115 M HC2H3O2 and 0.160 M KC2H3O2.The Ka for HC2H3O2 is 1.8 × 10-5.

What is the molar solubility of zinc oxalate ( ZnC2O4 )in water? The solubility-product constant for ZnC2O4 is 2.7 × 10-8 at 25°C.

Determine the molar solubility of MgCO3 in pure water.Ksp (MgCO3)= 6.82 × 10-6.

The molar solubility of Ag2S is 1.26 × 10-16 M in pure water.Calculate the Ksp for Ag2S.

Sketch the titration curve for a monoprotic weak 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.

Give the equation for a supersaturated solution in comparing Q with Ksp.

Determine the molar solubility of CaSO4 in a solution containing 0.14 M Na2SO4.Ksp (CaSO4)= 2.4 × 10-5.

A 1.00 L buffer solution is 0.150 M in HC7H5O2 and 0.250 M in LiC7H5O2.Calculate the pH of the solution after the addition of 100.0 mL of 1.00 M HCl.The Ka for HC7H5O2 is 6.5 × 10-5.

Define a buffer.

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.

What is the pH of a solution made by mixing 20.00 mL of 0.100 M HCl with 40.00 mL of 0.100 M KOH? Assume that the volumes of the solutions are additive.

Determine the molar solubility for Ag2C2O4 in pure water.The Ksp for Ag2C2O4 is 3.5 × 10-11.

If the pKa of HCHO2 is 3.74 and the pH of an HCHO2/NaCHO2 solution is 3.89,which of the following is TRUE?

A solution contains 3.8 × 10-2 M in Al3+ and 0.29 M in NaF.If the Kf for AlF63- is 7 × 1019,how much aluminum ion remains at equilibrium?

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

Gives what happens at neutral pH for aluminum hydroxide.

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 200.0 mL HBr.

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

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

Calculate the pH of a solution formed by mixing 200.0 mL of 0.30 M HClO with 300.0 mL of 0.20 M KClO.The K_a for HClO is 2.9 × 10^-8.

Calculate the pH of a buffer that is 0.115 M HC₂H₃O₂ and 0.160 M KC₂H₃O₂.The K_a for HC₂H₃O₂ is 1.8 × 10^-5.

What is the molar solubility of zinc oxalate ( ZnC₂O₄ )in water? The solubility-product constant for ZnC₂O₄ is 2.7 × 10^-8 at 25°C.

Determine the molar solubility of MgCO₃in pure water.K_sp (MgCO₃)= 6.82 × 10^-6.

The molar solubility of Ag₂S is 1.26 × 10^-16 M in pure water.Calculate the K_sp for Ag₂S.

Give the equation for a supersaturated solution in comparing Q with K_sp.

Determine the molar solubility of CaSO₄ in a solution containing 0.14 M Na₂SO₄.K_sp (CaSO₄)= 2.4 × 10^-5.

A 1.00 L buffer solution is 0.150 M in HC₇H₅O₂ and 0.250 M in LiC₇H₅O₂.Calculate the pH of the solution after the addition of 100.0 mL of 1.00 M HCl.The K_a for HC₇H₅O₂ is 6.5 × 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.

Determine the molar solubility for Ag₂C₂O₄ in pure water.The K_sp for Ag₂C₂O₄ is 3.5 × 10^-11.

If the pKa of HCHO₂ is 3.74 and the pH of an HCHO₂/NaCHO₂solution is 3.89,which of the following is TRUE?

A solution contains 3.8 × 10^-2M in Al³⁺ and 0.29 M in NaF.If the K_f for AlF₆^3- is 7 × 10¹⁹,how much aluminum ion remains at equilibrium?

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

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 200.0 mL HBr.