Question 1

Which will precipitate first when AgNO3 is added to a solution containing equal concentrations of Br-, Cl-, and I- ions?

Accepted Answer

A)  AgBr 
B)  AgCl 
C)  AgI 
D)  AgNO3 
E)  No precipitate will form 
A)  AgBr 
B)  AgCl 
C)  AgI 
D)  AgNO3 
E)  No precipitate will form

Question 2

What molar ratio of CH3COOH to CH3COONa should be used in order to prepare an acetic acid / sodium acetate buffer solution with a pH of 4.00 ± 0.02? [Ka(CH3COOH) = 1.8 × 10-5]

Accepted Answer

A)  0.18 
B)  0.84 
C)  1.2 
D)  5.6 
E)  0.10 
A)  0.18 
B)  0.84 
C)  1.2 
D)  5.6 
E)  0.10

Question 3

The solubility of magnesium phosphate is 2.27 × 10-3 g/1.0 L of solution. What is the Ksp for Mg3(PO4)2?

Accepted Answer

A)  7.46 × 10-11 
B)  2.68 × 10-9 
C)  5.19 × 10-24 
D)  4.80 × 10-26 
E)  1.20 × 10-26 
A)  7.46 × 10-11 
B)  2.68 × 10-9 
C)  5.19 × 10-24 
D)  4.80 × 10-26 
E)  1.20 × 10-26

Question 4

A buffer is prepared by adding 1.00 L of 1.0 M HCl to 750 mL of 1.5 M NaHCOO. What is the pH of this buffer? [Ka(HCOOH) = 1.7 × 10-4]

Accepted Answer

A)  2.87 
B)  3.72 
C)  3.82 
D)  3.95 
E)  4.66 
A)  2.87 
B)  3.72 
C)  3.82 
D)  3.95 
E)  4.66

Question 5

Calculate the minimum concentration of Cr3+ that must be added to 0.095 M NaF in order to initiate a precipitate of chromium(III) fluoride. [Ksp(CrF3) = 6.6 × 10-11]

Accepted Answer

A)  0.023 M 
B)  0.032 M 
C)  7.7 × 10-8 M 
D)  2.9 × 10-9 M 
E)  6.9 × 10-10 M 
A)  0.023 M 
B)  0.032 M 
C)  7.7 × 10-8 M 
D)  2.9 × 10-9 M 
E)  6.9 × 10-10 M

Question 6

A 50.0-mL sample of a 0.100 M solution of a weak acid HA has an equilibrium pH of 4.00. After 1.0 × 10-3mol of a substance X is added to the solution, it is observed that the pH of the solution increases. What might be true about substance X? I. X might be a strong base that partially neutralized some weak acid.
II) X might be a strong acid that made the solution more acidic.
III) X might be a soluble ionic compound containing the anion A-.

Accepted Answer

A)  I only 
B)  II only 
C)  III only 
D)  I or III 
E)  II or III 
A)  I only 
B)  II only 
C)  III only 
D)  I or III 
E)  II or III

Question 7

Which of the following is an exact or approximate value of the pH at the equivalence point of a titration of a strong acid with a strong base?

Accepted Answer

A)  14.0 
B)  7.0 
C)  3.5 
D)  1.0 
E)  0.0 
A)  14.0 
B)  7.0 
C)  3.5 
D)  1.0 
E)  0.0

Question 8

The solubility of lead(II) iodide is 0.064 g/100 mL at 20°C. What is the solubility product for lead(II) iodide?

Accepted Answer

A)  1.1 × 10-8 
B)  2.7 × 10-9 
C)  1.1 × 10-11 
D)  2.7 × 10-12 
E)  1.1 × 10-3 
A)  1.1 × 10-8 
B)  2.7 × 10-9 
C)  1.1 × 10-11 
D)  2.7 × 10-12 
E)  1.1 × 10-3

Question 9

A buffer is prepared by adding 150 mL of 1.0 M NaOH to 250 mL of 1.0 M NaH2PO4. How many moles of HCl must be added to this buffer solution to change the pH by 0.18 units?

Accepted Answer

A)  0.025 mol HCl 
B)  0.063 mol HCl 
C)  0.082 mol HCl 
D)  0.50 mol HCl 
E)  1.0 mol HCl 
A)  0.025 mol HCl 
B)  0.063 mol HCl 
C)  0.082 mol HCl 
D)  0.50 mol HCl 
E)  1.0 mol HCl

Question 10

Which pair of substances is capable of forming a buffer in aqueous solution?

Accepted Answer

A)  H3PO4, Na3PO3 
B)  HNO3, NaNO3 
C)  HCl, NaCl 
D)  H2CO3, NaNO2 
E)  CH3COOH, CH3COONa 
A)  H3PO4, Na3PO3 
B)  HNO3, NaNO3 
C)  HCl, NaCl 
D)  H2CO3, NaNO2 
E)  CH3COOH, CH3COONa

Question 11

Which compound has the highest solubility in pure water?

Accepted Answer

A)  Ag2C2O4, Ksp = 1.0 × 10-11 
B)  PbCl2, Ksp = 1.7 × 10-5 
C)  CaSO4, Ksp = 2.4 × 10-5 
D)  Ca3(PO4)2, Ksp = 1.2 × 10-26 
E)  MgF2, Ksp = 6.9 × 10-9 
A)  Ag2C2O4, Ksp = 1.0 × 10-11 
B)  PbCl2, Ksp = 1.7 × 10-5 
C)  CaSO4, Ksp = 2.4 × 10-5 
D)  Ca3(PO4)2, Ksp = 1.2 × 10-26 
E)  MgF2, Ksp = 6.9 × 10-9

Question 12

The molar solubility of magnesium carbonate is 1.8 × 10-4 mol/L. What is Ksp for this compound?

Accepted Answer

A)  1.8 × 10-4 
B)  3.6 × 10-4 
C)  1.3 × 10-7 
D)  3.2 × 10-8 
E)  2.8 × 10-14 
A)  1.8 × 10-4 
B)  3.6 × 10-4 
C)  1.3 × 10-7 
D)  3.2 × 10-8 
E)  2.8 × 10-14

Question 13

After the equivalence point, the titration curve of a weak acid is identical to that of a ________ ________.

Accepted Answer

The answer of After the equivalence point, the titration curve...

Question 14

A ________ helps maintain a constant pH even after the addition of acid or base.

Accepted Answer

The answer of A ________ helps maintain a constant pH...

Question 15

Which best describes the pH at the equivalence point of a titration of a weak base with a strong acid?

Accepted Answer

A)  Less than zero 
B)  Between 0 and 7 
C)  Close to 7.0 
D)  Between 7 and 14 
E)  Greater than 14 
A)  Less than zero 
B)  Between 0 and 7 
C)  Close to 7.0 
D)  Between 7 and 14 
E)  Greater than 14

Question 16

Which compound has the lowest solubility in pure water?

Accepted Answer

A)  Ag2C2O4, Ksp = 1.0 × 10-11 
B)  PbCl2, Ksp = 1.7 × 10-5 
C)  FePO4, Ksp = 1.3 × 10-22 
D)  Ca3(PO4)2, Ksp = 1.2 × 10-26 
E)  MgF2, Ksp = 6.9 × 10-9 
A)  Ag2C2O4, Ksp = 1.0 × 10-11 
B)  PbCl2, Ksp = 1.7 × 10-5 
C)  FePO4, Ksp = 1.3 × 10-22 
D)  Ca3(PO4)2, Ksp = 1.2 × 10-26 
E)  MgF2, Ksp = 6.9 × 10-9

Question 17

Which is the best choice for preparing a buffer with a pH of 3.5?

Accepted Answer

A)  C5H5O5COOH, Ka = 4.0 × 10-6 
B)  HOC6H4OCOOH, Ka = 1.0 × 10-3 
C)  HBrO, Ka = 2.3 × 10-9 
D)  C6H4(COOH)2, Ka = 2.9 × 10-4 
E)  CH3COOH, Ka = 1.8 ×10-5 
A)  C5H5O5COOH, Ka = 4.0 × 10-6 
B)  HOC6H4OCOOH, Ka = 1.0 × 10-3 
C)  HBrO, Ka = 2.3 × 10-9 
D)  C6H4(COOH)2, Ka = 2.9 × 10-4 
E)  CH3COOH, Ka = 1.8 ×10-5

Question 18

A(n) ________ is a measure of the tendency of a metal ion to form a particular complex ion and is the equilibrium constant for the complex ion formation.

Accepted Answer

formation constant o

Question 19

When a weak acid is titrated with a weak base, the pH at the equivalence point

Accepted Answer

A)  is greater than 7.0. 
B)  is equal to 7.0. 
C)  is less than 7.0. 
D)  is determined by the magnitudes of Ka and Kb. 
E)  depends on the pKa of the indicator. 
A)  is greater than 7.0. 
B)  is equal to 7.0. 
C)  is less than 7.0. 
D)  is determined by the magnitudes of Ka and Kb. 
E)  depends on the pKa of the indicator.

Question 20

Explain the effect on the ionization of the acetic acid when sodium acetate is added to a solution of acetic acid?
CH3COOH(aq)   H+(aq) + CH3COO-(aq)

Accepted Answer

The equilibrium shif

Exam 17: Acid-Base Equilibria and Solubility Equilibria

Which will precipitate first when AgNO3 is added to a solution containing equal concentrations of Br-, Cl-, and I- ions?

What molar ratio of CH3COOH to CH3COONa should be used in order to prepare an acetic acid / sodium acetate buffer solution with a pH of 4.00 ± 0.02? [Ka(CH3COOH) = 1.8 × 10-5]

The solubility of magnesium phosphate is 2.27 × 10-3 g/1.0 L of solution. What is the Ksp for Mg3(PO4)2?

A buffer is prepared by adding 1.00 L of 1.0 M HCl to 750 mL of 1.5 M NaHCOO. What is the pH of this buffer? [Ka(HCOOH) = 1.7 × 10-4]

Calculate the minimum concentration of Cr3+ that must be added to 0.095 M NaF in order to initiate a precipitate of chromium(III) fluoride. [Ksp(CrF3) = 6.6 × 10-11]

Which of the following is an exact or approximate value of the pH at the equivalence point of a titration of a strong acid with a strong base?

The solubility of lead(II) iodide is 0.064 g/100 mL at 20°C. What is the solubility product for lead(II) iodide?

A buffer is prepared by adding 150 mL of 1.0 M NaOH to 250 mL of 1.0 M NaH2PO4. How many moles of HCl must be added to this buffer solution to change the pH by 0.18 units?

Which pair of substances is capable of forming a buffer in aqueous solution?

Which compound has the highest solubility in pure water?

The molar solubility of magnesium carbonate is 1.8 × 10-4 mol/L. What is Ksp for this compound?

After the equivalence point, the titration curve of a weak acid is identical to that of a ________ ________.

A ________ helps maintain a constant pH even after the addition of acid or base.

Which best describes the pH at the equivalence point of a titration of a weak base with a strong acid?

Which compound has the lowest solubility in pure water?

Which is the best choice for preparing a buffer with a pH of 3.5?

A(n) ________ is a measure of the tendency of a metal ion to form a particular complex ion and is the equilibrium constant for the complex ion formation.

When a weak acid is titrated with a weak base, the pH at the equivalence point

Explain the effect on the ionization of the acetic acid when sodium acetate is added to a solution of acetic acid? CH3COOH(aq) H+(aq) + CH3COO-(aq)

Chemistry: the Central Science

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Stoichiometry: Ratios of Combination

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Quantum Theory and the Electronic Structure of Atoms

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Chemical Bonding II: Molecular Geometry and Bonding Theories

Gases

Intermolecular Forces and the Physical Properties of Liquids and Solids

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Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Entropy, Free Energy, and Equilibrium

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Filters

Which will precipitate first when AgNO₃ is added to a solution containing equal concentrations of Br^-, Cl^-, and I^- ions?

What molar ratio of CH₃COOH to CH₃COONa should be used in order to prepare an acetic acid / sodium acetate buffer solution with a pH of 4.00 ± 0.02? [K_a(CH₃COOH) = 1.8 × 10^-5]

The solubility of magnesium phosphate is 2.27 × 10^-3 g/1.0 L of solution. What is the K_sp for Mg₃(PO₄)₂?

A buffer is prepared by adding 1.00 L of 1.0 M HCl to 750 mL of 1.5 M NaHCOO. What is the pH of this buffer? [K_a(HCOOH) = 1.7 × 10^-4]

Calculate the minimum concentration of Cr³⁺ that must be added to 0.095 M NaF in order to initiate a precipitate of chromium(III) fluoride. [K_sp(CrF₃) = 6.6 × 10^-11]

A buffer is prepared by adding 150 mL of 1.0 M NaOH to 250 mL of 1.0 M NaH₂PO₄. How many moles of HCl must be added to this buffer solution to change the pH by 0.18 units?

The molar solubility of magnesium carbonate is 1.8 × 10^-4 mol/L. What is K_sp for this compound?

After the equivalence point, the titration curve of a weak acid is identical to that of a .

Explain the effect on the ionization of the acetic acid when sodium acetate is added to a solution of acetic acid? CH₃COOH(aq) H⁺(aq) + CH₃COO^-(aq)