Question 1

The molar solubility of ZnS is 1.6 × 10-12 mol L-1 in pure water. Calculate the Ksp for ZnS.

Accepted Answer

A)  8.0 × 10-13 
B)  3.2 × 10-12 
C)  1.6 × 10-35 
D)  2.6 × 10-24 
E)  6.8 × 10-5 
A)  8.0 × 10-13 
B)  3.2 × 10-12 
C)  1.6 × 10-35 
D)  2.6 × 10-24 
E)  6.8 × 10-5

Question 2

In which of the following solutions would solid PbBr2 be expected to be the least soluble at 25 °C?

Accepted Answer

A)  0.1 mol L-1 H Br 
B)  0.1 mol L-1 NaBr 
C)  0.1 mol L-1 CaBr2 
D)  0.1 mol L-1 K NO3 
A)  0.1 mol L-1 H Br 
B)  0.1 mol L-1 NaBr 
C)  0.1 mol L-1 CaBr2 
D)  0.1 mol L-1 K NO3

Question 3

The titration of 25.0 mL of an unknown concentration H2SO4 solution requires 83.6 mL of a 0.12 mol L-1 LiOH solution. What is the concentration of the H2SO4 solution (in mol L-1)?

Accepted Answer

A)  0.20 mol L-1 
B)  0.40 mol L-1 
C)  0.10 mol L-1 
D)  0.36 mol L-1 
E)  0.25 mol L-1 
A)  0.20 mol L-1 
B)  0.40 mol L-1 
C)  0.10 mol L-1 
D)  0.36 mol L-1 
E)  0.25 mol L-1

Question 4

Which of the following is the correct equation relating Q to Ksp for a saturated solution?

Accepted Answer

A)  Q > Ksp 
B)  Q sp 
C)  Q = Ksp 
D)  Q ≠ Ksp 
E)  Q ≥ Ksp 
A)  Q > Ksp 
B)  Q sp 
C)  Q = Ksp 
D)  Q ≠ Ksp 
E)  Q ≥ Ksp

Question 5

A 100.0 mL sample of 0.10 mol L-1 Ca(OH)2 is titrated with 0.10 mol L-1 HBr. Determine the pH of the solution before the addition of any HBr.

Accepted Answer

A)  12.86 
B)  13.00 
C)  13.30 
D)  0.70 
E)  1.00 
A)  12.86 
B)  13.00 
C)  13.30 
D)  0.70 
E)  1.00

Question 6

Calculate the pH of a buffer that is 0.058 mol L-1 HF and 0.058 mol L-1 LiF. The Ka for HF is 3.5 × 10-4.

Accepted Answer

A)  2.86 
B)  9.31 
C)  10.54 
D)  3.46 
E)  4.69 
A)  2.86 
B)  9.31 
C)  10.54 
D)  3.46 
E)  4.69

Question 7

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

Accepted Answer

A)  PbCl2 
B)  FeS 
C)  Ca(ClO4)2 
D)  CuI 
E)  AgBr 
A)  PbCl2 
B)  FeS 
C)  Ca(ClO4)2 
D)  CuI 
E)  AgBr

Question 8

Which of the following is TRUE?

Accepted Answer

A)  An effective buffer has a [base]/[acid] ratio in the range of 10-100. 
B)  A buffer is most resistant to pH change when [acid] = [conjugate base]. 
C)  An effective buffer has very small absolute concentrations of acid and conjugate base. 
D)  The capacity of a buffer cannot be exceeded by adding too much strong base. It can only be exceeded by adding too much strong acid. 
E)  A buffer has the best resistance to pH change when the buffer's pH is significantly lower than the pKa of the acid used to make the buffer solution. 
A)  An effective buffer has a [base]/[acid] ratio in the range of 10-100. 
B)  A buffer is most resistant to pH change when [acid] = [conjugate base]. 
C)  An effective buffer has very small absolute concentrations of acid and conjugate base. 
D)  The capacity of a buffer cannot be exceeded by adding too much strong base. It can only be exceeded by adding too much strong acid. 
E)  A buffer has the best resistance to pH change when the buffer's pH is significantly lower than the pKa of the acid used to make the buffer solution.

Question 9

A solution is prepared by dissolving 0.23 mol of formic acid and 0.27 mol of sodium formate in water sufficient to yield 1.00 L of solution. The addition of 0.05 mol of HCl to this buffer solution causes the pH to drop slightly. The pH does not decrease drastically because the HCl reacts with the ________ present in the buffer solution. The   of formic acid is 1.36 × 10-3.

Accepted Answer

A)    O 
B)    
C)  formate ion 
D)  formic acid 
E)  This is a buffer solution: the pH does not change at all upon addition of acid or base. 
A)    O 
B)    
C)  formate ion 
D)  formic acid 
E)  This is a buffer solution: the pH does not change at all upon addition of acid or base.

Question 10

A 100.0 mL sample of 0.10 mol L-1 Ca(OH)2 is titrated with 0.10 mol L-1 HBr. Determine the pH of the solution after the addition of 300.0 mL HBr.

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 11

What is the molar solubility of Mg(OH)2 in a basic solution with a pH of 12.50? Ksp for Mg(OH)2 is

Accepted Answer

A)  1.8 × 10-10 mol L-1 
B)  5.6 × 10-9 mol L-1 
C)  2.4 × 10-6 mol L-1 
D)  1.1 × 10-4 mol L-1 
A)  1.8 × 10-10 mol L-1 
B)  5.6 × 10-9 mol L-1 
C)  2.4 × 10-6 mol L-1 
D)  1.1 × 10-4 mol L-1

Question 12

A 1.00 L buffer solution is 0.250 mol L-1 in HF and 0.250 mol L-1 in NaF. Calculate the pH of the solution after the addition of 100.0 mL of 1.00 mol L-1 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 13

Match the following.
-pH = 7

Accepted Answer

A) equivalence point of a weak acid-strong base titration 
B) halfway to equivalence point of a weak acid-strong base titration 
C) equivalence point of a strong acid-strong base titration 
D) equivalence point of a weak base-strong acid titration 
E) three-quarters of the way to second equivalence point of a diprotic acid-strong base titration 
A) equivalence point of a weak acid-strong base titration 
B) halfway to equivalence point of a weak acid-strong base titration 
C) equivalence point of a strong acid-strong base titration 
D) equivalence point of a weak base-strong acid titration 
E) three-quarters of the way to second equivalence point of a diprotic acid-strong base titration

The molar solubility of ZnS is 1.6 × 10^-12 mol L^-1 in pure water. Calculate the K_sp for ZnS.

In which of the following solutions would solid PbBr₂ be expected to be the least soluble at 25 °C?

The titration of 25.0 mL of an unknown concentration H₂SO₄ solution requires 83.6 mL of a 0.12 mol L^-1 LiOH solution. What is the concentration of the H₂SO₄ solution (in mol L^-1)?

Which of the following is the correct equation relating Q to K_sp for a saturated solution?

A 100.0 mL sample of 0.10 mol L^-1 Ca(OH)₂ is titrated with 0.10 mol L^-1 HBr. Determine the pH of the solution before the addition of any HBr.

Calculate the pH of a buffer that is 0.058 mol L^-1 HF and 0.058 mol L^-1 LiF. The K_a for HF is 3.5 × 10^-4.

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

Which of the following is TRUE?

A 100.0 mL sample of 0.10 mol L^-¹ Ca(OH)₂ is titrated with 0.10 mol L^-1 HBr. Determine the pH of the solution after the addition of 300.0 mL HBr.

What is the molar solubility of Mg(OH)₂ in a basic solution with a pH of 12.50? K_spfor Mg(OH)₂ is

A 1.00 L buffer solution is 0.250 mol L^-1 in HF and 0.250 mol L^-1 in NaF. Calculate the pH of the solution after the addition of 100.0 mL of 1.00 mol L^-1 HCl. The K_a for HF is 3.5 × 10^-4.

Match the following. -pH = 7

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Exam 16: Aqueous Ionic Equilibrium

The molar solubility of ZnS is 1.6 × 10-12 mol L-1 in pure water. Calculate the Ksp for ZnS.

In which of the following solutions would solid PbBr2 be expected to be the least soluble at 25 °C?

The titration of 25.0 mL of an unknown concentration H2SO4 solution requires 83.6 mL of a 0.12 mol L-1 LiOH solution. What is the concentration of the H2SO4 solution (in mol L-1)?

Which of the following is the correct equation relating Q to Ksp for a saturated solution?

A 100.0 mL sample of 0.10 mol L-1 Ca(OH)2 is titrated with 0.10 mol L-1 HBr. Determine the pH of the solution before the addition of any HBr.

Calculate the pH of a buffer that is 0.058 mol L-1 HF and 0.058 mol L-1 LiF. 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?

Which of the following is TRUE?

A 100.0 mL sample of 0.10 mol L-1 Ca(OH)2 is titrated with 0.10 mol L-1 HBr. Determine the pH of the solution after the addition of 300.0 mL HBr.

What is the molar solubility of Mg(OH)2 in a basic solution with a pH of 12.50? Ksp for Mg(OH)2 is

A 1.00 L buffer solution is 0.250 mol L-1 in HF and 0.250 mol L-1 in NaF. Calculate the pH of the solution after the addition of 100.0 mL of 1.00 mol L-1 HCl. The Ka for HF is 3.5 × 10-4.

Match the following. -pH = 7

Units of Measurement for Physical and Chemical Change

Atoms and Elements

Molecules, Compounds, and Nomenclature

Chemical Reactions and Stoichiometry

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, and Molecular Orbital Theory

Liquids, Solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Gibbs Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry I: Structures

Organic Chemistry Ii: Reactions

Biochemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Transition Metals and Coordination Compounds

Filters

The molar solubility of ZnS is 1.6 × 10^-12 mol L^-1 in pure water. Calculate the K_sp for ZnS.

In which of the following solutions would solid PbBr₂ be expected to be the least soluble at 25 °C?

The titration of 25.0 mL of an unknown concentration H₂SO₄ solution requires 83.6 mL of a 0.12 mol L^-1 LiOH solution. What is the concentration of the H₂SO₄ solution (in mol L^-1)?

Which of the following is the correct equation relating Q to K_sp for a saturated solution?

A 100.0 mL sample of 0.10 mol L^-1 Ca(OH)₂ is titrated with 0.10 mol L^-1 HBr. Determine the pH of the solution before the addition of any HBr.

Calculate the pH of a buffer that is 0.058 mol L^-1 HF and 0.058 mol L^-1 LiF. The K_a for HF is 3.5 × 10^-4.

A 100.0 mL sample of 0.10 mol L^-¹ Ca(OH)₂ is titrated with 0.10 mol L^-1 HBr. Determine the pH of the solution after the addition of 300.0 mL HBr.

What is the molar solubility of Mg(OH)₂ in a basic solution with a pH of 12.50? K_spfor Mg(OH)₂ is

A 1.00 L buffer solution is 0.250 mol L^-1 in HF and 0.250 mol L^-1 in NaF. Calculate the pH of the solution after the addition of 100.0 mL of 1.00 mol L^-1 HCl. The K_a for HF is 3.5 × 10^-4.