Question 1

Calculate the solubility of Cu(OH)2 in a solution buffered at pH = 8.50. (Ksp = 1.6 × 10-19)

Accepted Answer

A)  5.7 × 10-10 M 
B)  1.6 × 10-2 M 
C)  1.8 × 10-7 M 
D)  1.6 × 10-8 M 
E)  none of these 
A)  5.7 × 10-10 M 
B)  1.6 × 10-2 M 
C)  1.8 × 10-7 M 
D)  1.6 × 10-8 M 
E)  none of these

Question 2

Calculate the pH of a solution prepared by mixing 50 mL of a 0.10 M solution of HF with 25 mL of a 0.20 M solution of NaF. pKa of HF is 3.14.

Accepted Answer

A)  5.83 
B)  12.00 
C)  3.14 
D)  7.35 
E)  10.80 
A)  5.83 
B)  12.00 
C)  3.14 
D)  7.35 
E)  10.80

Question 3

Calculate the pH when 200.0 mL of a 1.00 M solution of HS1U1B12S1U1B0A (KS1U1B1a1S1U1B0 = 1.0 × 10S1U1P1-6S1S1P0, KS1U1B1a2S1U1B0 = 1.0 × 10S1U1P1-10S1S1P0) is titrated with the following volumes of 1.00 M NaOH.
-150.0 mL of 1.00 M NaOH

Accepted Answer

A)  6.00 
B)  6.48 
C)  8.00 
D)  8.50 
E)  none of these 
A)  6.00 
B)  6.48 
C)  8.00 
D)  8.50 
E)  none of these

Question 4

A 200.0-mL sample of the weak acid HS1U1B13S1U1B0A (0.100 M) is titrated with 0.200 M NaOH. What are the major species at each of the following points in the titration? (Water is always assumed to be a major species.)
-After 200.0 mL of 0.200 M NaOH is added

Accepted Answer

A)  HA2-, A3- 
B)  HA2- 
C)  H2A- 
D)  H2A-, HA2- 
E)  A3- 
A)  HA2-, A3- 
B)  HA2- 
C)  H2A- 
D)  H2A-, HA2- 
E)  A3-

Question 5

A solution of hydrochloric acid of unknown concentration was titrated with 0.12 M NaOH. If a 250-mL sample of the HCl solution required exactly 24 mL of the NaOH solution to reach the equivalence point, what was the pH of the HCl solution?

Accepted Answer

A)  12.06 
B)  1.98 
C)  0.12 
D)  1.94 
E)  -0.10 
A)  12.06 
B)  1.98 
C)  0.12 
D)  1.94 
E)  -0.10

Question 6

A 75.0-mL sample of 0.0500 M HCN (Ka = 6.2 × 10-10) is titrated with 0.500 M NaOH. What is [H+] in the solution after 3.0 mL of 0.500 M NaOH has been added?

Accepted Answer

A)  9.3 × 10-10 M 
B)  5.2 × 10-13 M 
C)  1.0 × 10-7 M 
D)  4.1 × 10-10 M 
E)  none of these 
A)  9.3 × 10-10 M 
B)  5.2 × 10-13 M 
C)  1.0 × 10-7 M 
D)  4.1 × 10-10 M 
E)  none of these

Question 7

Consider the titration of 100.0 mL of 0.250 M aniline (Kb = 3.8 × 10-10) with 0.500 M HCl. For calculating the volume of HCl required to reach a pH of 8.0, which of the following expressions is correct? (x = volume, in milliliters, of HCl required to reach a pH of 8.0)

Accepted Answer

A)    
B)    
C)    
D)  [H+] = x 
E)  none of these 
A)    
B)    
C)    
D)  [H+] = x 
E)  none of these

Question 8

Explain why we cannot directly compare Ksp values in comparing solubilities of ionic solids with different numbers of ions.

Accepted Answer

See Sectio

Question 9

What volume of 0.0100 M NaOH must be added to 1.00 L of 0.0500 M HOCl to achieve a pH of 8.00? Ka for HOCl is 3.5 × 10-8.

Accepted Answer

A)  1.2 L 
B)  1.0 L 
C)  3.9 L 
D)  5.0 L 
E)  none of these 
A)  1.2 L 
B)  1.0 L 
C)  3.9 L 
D)  5.0 L 
E)  none of these

Question 10

A 200.0-mL sample of the weak acid HS1U1B13S1U1B0A (0.100 M) is titrated with 0.200 M NaOH. What are the major species at each of the following points in the titration? (Water is always assumed to be a major species.)
-After 0 mL of 0.200 M NaOH is added

Accepted Answer

A)  H3A, H2A-, HA2-, A3- 
B)  H3A, H2A- 
C)  H3A 
D)  H2A-, HA2- 
E)  H2A- 
A)  H3A, H2A-, HA2-, A3- 
B)  H3A, H2A- 
C)  H3A 
D)  H2A-, HA2- 
E)  H2A-

Question 11

A solution contains 0.50 (Ka = 2.0 × 10-8) and 0.22 M NaA. Calculate the pH after 0.05mol of NaOH is added to 1.00 L of this solution.

Accepted Answer

A)  7.48 
B)  7.70 
C)  7.34 
D)  7.92 
E)  7.19 
A)  7.48 
B)  7.70 
C)  7.34 
D)  7.92 
E)  7.19

Question 12

The value of Kf for the complex ion Ag(NH3)2+ is 1.7 × 107. Ksp for AgCl is 1.6 × 10-10. Calculate the molar solubility of AgCl in 1.0 M NH3.

Accepted Answer

A)  1.7 × 10-10 
B)  2.9 × 10-3 
C)  4.7 × 10-2 
D)  1.3 × 10-5 
E)  5.2 × 10-2 
A)  1.7 × 10-10 
B)  2.9 × 10-3 
C)  4.7 × 10-2 
D)  1.3 × 10-5 
E)  5.2 × 10-2

Question 13

Silver chromate, Ag2CrO4, has a Ksp of 9.0 × 10-12. Calculate the solubility, in moles per liter, of silver chromate.

Accepted Answer

A)  7.8 × 10-5 M 
B)  9.5 × 10-7 M 
C)  9.8 × 10-5 M 
D)  1.9 × 10-12 M 
E)  1.3 × 10-4 M 
A)  7.8 × 10-5 M 
B)  9.5 × 10-7 M 
C)  9.8 × 10-5 M 
D)  1.9 × 10-12 M 
E)  1.3 × 10-4 M

Question 14

A student titrates an unknown weak acid, HA, to a pale pink phenolphthalein endpoint with 25.0 mL of 0.100 M NaOH. The student then adds 13.0 mL of 0.100 M HCl. The pH of the resulting solution is 4.7. Which of the following statements is true?

Accepted Answer

A)  At pH 4.7, half of the conjugate base, A-, has been converted to HA. 
B)  The pKa of the acid is 4.7. 
C)  The pKa of the acid is less than 4.7. 
D)  The pKa of the acid is greater than 4.7. 
E)  More than one of the above statements are correct. 
A)  At pH 4.7, half of the conjugate base, A-, has been converted to HA. 
B)  The pKa of the acid is 4.7. 
C)  The pKa of the acid is less than 4.7. 
D)  The pKa of the acid is greater than 4.7. 
E)  More than one of the above statements are correct.

Question 15

Consider the following information about the diprotic acid ascorbic acid (HS1U1B12S1U1B0As for short, molar mass = 176.1).   The titration curve for disodium ascorbate, NaS1U1B12S1U1B0As, with standard HCl is shown below:  
-What is the pH at point III?

Accepted Answer

A)  7.95 
B)  11.79 
C)  12.39 
D)  4.10 
E)  none of these 
A)  7.95 
B)  11.79 
C)  12.39 
D)  4.10 
E)  none of these

Question 16

The Ksp value for PbSO4(s) is 1.3 × 10-8. Calculate the solubility, in moles per liter, of PbSO4(s) in a 0.0010 M solution of Na2SO4.

Accepted Answer

A)  4.5 × 10-6 M 
B)  1.3 × 10-11 M 
C)  1.3 × 10-5 M 
D)  1.3 × 10-8 M 
E)  1.4 × 10-4 M 
A)  4.5 × 10-6 M 
B)  1.3 × 10-11 M 
C)  1.3 × 10-5 M 
D)  1.3 × 10-8 M 
E)  1.4 × 10-4 M

Question 17

The Ksp of Al(OH)3 is 2.0 × 10-32. At what pH will a 0.2 M Al3+ solution begin to show precipitation of Al(OH)3?

Accepted Answer

A)  8.4 
B)  5.6 
C)  3.7 
D)  10.3 
E)  1.0 
A)  8.4 
B)  5.6 
C)  3.7 
D)  10.3 
E)  1.0

Question 18

Consider a 100.0-mL sample of a 0.10 M H2A (Ka1 = 1.3 × 10-3 , Ka2 = 3.1 × 10-6) with 0.10 M NaOH. Determine the pH when 0 mL, 50.0 mL, 100.0 mL, and 150.0 mL of 0.10 M NaOH are added.

Accepted Answer

0 mL, pH = 1.94; 50.

Question 19

Calculate the solubility of Ag2SO4 [Ksp = 1.2 × 10-5] in a 2.0 M AgNO3 solution.

Accepted Answer

A)  6.0 × 10-6 mol/L 
B)  1.2 × 10-5 mol/L 
C)  3.0 × 10-6 mol/L 
D)  1.4 × 10-2 mol/L 
E)  none of these 
A)  6.0 × 10-6 mol/L 
B)  1.2 × 10-5 mol/L 
C)  3.0 × 10-6 mol/L 
D)  1.4 × 10-2 mol/L 
E)  none of these

Question 20

A solution contains 10. mmol of H3PO4 and 5.0 mmol of NaH2PO4. How many milliliters of 0.10 M NaOH must be added to reach the second equivalence point of the titration of the H3PO4 with NaOH?

Accepted Answer

A)  2.0 × 102 mL 
B)  150 mL 
C)  250 mL 
D)  1.0 × 102 mL 
E)  50 mL 
A)  2.0 × 102 mL 
B)  150 mL 
C)  250 mL 
D)  1.0 × 102 mL 
E)  50 mL

Calculate the solubility of Cu(OH)₂ in a solution buffered at pH = 8.50. (K_sp = 1.6 × 10^-19)

Calculate the pH of a solution prepared by mixing 50 mL of a 0.10 M solution of HF with 25 mL of a 0.20 M solution of NaF. pK_a of HF is 3.14.

Calculate the pH when 200.0 mL of a 1.00 M solution of H₂A (K_a1 = 1.0 × 10^-6, K_a2 = 1.0 × 10^-10) is titrated with the following volumes of 1.00 M NaOH. -150.0 mL of 1.00 M NaOH

A 200.0-mL sample of the weak acid H₃A (0.100 M) is titrated with 0.200 M NaOH. What are the major species at each of the following points in the titration? (Water is always assumed to be a major species.) -After 200.0 mL of 0.200 M NaOH is added

A solution of hydrochloric acid of unknown concentration was titrated with 0.12 M NaOH. If a 250-mL sample of the HCl solution required exactly 24 mL of the NaOH solution to reach the equivalence point, what was the pH of the HCl solution?

A 75.0-mL sample of 0.0500 M HCN (K_a = 6.2 × 10^-10) is titrated with 0.500 M NaOH. What is [H⁺] in the solution after 3.0 mL of 0.500 M NaOH has been added?

Consider the titration of 100.0 mL of 0.250 M aniline (K_b = 3.8 × 10^-10) with 0.500 M HCl. For calculating the volume of HCl required to reach a pH of 8.0, which of the following expressions is correct? (x = volume, in milliliters, of HCl required to reach a pH of 8.0)

Explain why we cannot directly compare K_sp values in comparing solubilities of ionic solids with different numbers of ions.

What volume of 0.0100 M NaOH must be added to 1.00 L of 0.0500 M HOCl to achieve a pH of 8.00? K_a for HOCl is 3.5 × 10^-8.

A 200.0-mL sample of the weak acid H₃A (0.100 M) is titrated with 0.200 M NaOH. What are the major species at each of the following points in the titration? (Water is always assumed to be a major species.) -After 0 mL of 0.200 M NaOH is added

A solution contains 0.50 (K_a = 2.0 × 10^-8) and 0.22 M NaA. Calculate the pH after 0.05mol of NaOH is added to 1.00 L of this solution.

The value of K_f for the complex ion Ag(NH₃)₂⁺ is 1.7 × 10⁷. K_sp for AgCl is 1.6 × 10^-10. Calculate the molar solubility of AgCl in 1.0 M NH₃.

Silver chromate, Ag₂CrO₄, has a K_sp of 9.0 × 10^-12. Calculate the solubility, in moles per liter, of silver chromate.

A student titrates an unknown weak acid, HA, to a pale pink phenolphthalein endpoint with 25.0 mL of 0.100 M NaOH. The student then adds 13.0 mL of 0.100 M HCl. The pH of the resulting solution is 4.7. Which of the following statements is true?

Consider the following information about the diprotic acid ascorbic acid (H₂As for short, molar mass = 176.1). The titration curve for disodium ascorbate, Na₂As, with standard HCl is shown below: -What is the pH at point III?

The K_sp value for PbSO₄(s) is 1.3 × 10^-8. Calculate the solubility, in moles per liter, of PbSO₄(s) in a 0.0010 M solution of Na₂SO₄.

The K_sp of Al(OH)₃ is 2.0 × 10^-32. At what pH will a 0.2 M Al³⁺ solution begin to show precipitation of Al(OH)₃?

Consider a 100.0-mL sample of a 0.10 M H₂A (K_a1 = 1.3 × 10^-3 , K_a2 = 3.1 × 10^-6) with 0.10 M NaOH. Determine the pH when 0 mL, 50.0 mL, 100.0 mL, and 150.0 mL of 0.10 M NaOH are added.

Calculate the solubility of Ag₂SO₄ [K_sp = 1.2 × 10^-5] in a 2.0 M AgNO₃ solution.

A solution contains 10. mmol of H₃PO₄ and 5.0 mmol of NaH₂PO₄. How many milliliters of 0.10 M NaOH must be added to reach the second equivalence point of the titration of the H₃PO₄ with NaOH?

Atoms, Molecules, and Ions

Stoichiometry

Types of Chemical Reactions and Solution Stoichiometry

Gases

Chemical Equilibrium

Acids and Bases

Energy, Enthalpy, and Thermochemistry

Spontaneity, Entropy, and Free Energy

Electrochemistry

Quantum Mechanics and Atomic Theory

Bonding: General Concepts

Covalent Bonding: Orbitals

Chemical Kinetics

Liquids and Solids

Properties of Solutions

The Representative Elements

Transition Metals and Coordination Chemistry

The Nucleus: a Chemists View

Organic and Biochemical Molecules

Filters

Exam 8: Applications of Aqueous Equilibria

Calculate the solubility of Cu(OH)2 in a solution buffered at pH = 8.50. (Ksp = 1.6 × 10-19)

Calculate the pH of a solution prepared by mixing 50 mL of a 0.10 M solution of HF with 25 mL of a 0.20 M solution of NaF. pKa of HF is 3.14.

Calculate the pH when 200.0 mL of a 1.00 M solution of H2A (Ka1 = 1.0 × 10-6, Ka2 = 1.0 × 10-10) is titrated with the following volumes of 1.00 M NaOH. -150.0 mL of 1.00 M NaOH

A 200.0-mL sample of the weak acid H3A (0.100 M) is titrated with 0.200 M NaOH. What are the major species at each of the following points in the titration? (Water is always assumed to be a major species.) -After 200.0 mL of 0.200 M NaOH is added

A solution of hydrochloric acid of unknown concentration was titrated with 0.12 M NaOH. If a 250-mL sample of the HCl solution required exactly 24 mL of the NaOH solution to reach the equivalence point, what was the pH of the HCl solution?

A 75.0-mL sample of 0.0500 M HCN (Ka = 6.2 × 10-10) is titrated with 0.500 M NaOH. What is [H+] in the solution after 3.0 mL of 0.500 M NaOH has been added?

Consider the titration of 100.0 mL of 0.250 M aniline (Kb = 3.8 × 10-10) with 0.500 M HCl. For calculating the volume of HCl required to reach a pH of 8.0, which of the following expressions is correct? (x = volume, in milliliters, of HCl required to reach a pH of 8.0)

Explain why we cannot directly compare Ksp values in comparing solubilities of ionic solids with different numbers of ions.

What volume of 0.0100 M NaOH must be added to 1.00 L of 0.0500 M HOCl to achieve a pH of 8.00? Ka for HOCl is 3.5 × 10-8.

A 200.0-mL sample of the weak acid H3A (0.100 M) is titrated with 0.200 M NaOH. What are the major species at each of the following points in the titration? (Water is always assumed to be a major species.) -After 0 mL of 0.200 M NaOH is added

A solution contains 0.50 (Ka = 2.0 × 10-8) and 0.22 M NaA. Calculate the pH after 0.05mol of NaOH is added to 1.00 L of this solution.

The value of Kf for the complex ion Ag(NH3)2+ is 1.7 × 107. Ksp for AgCl is 1.6 × 10-10. Calculate the molar solubility of AgCl in 1.0 M NH3.

Silver chromate, Ag2CrO4, has a Ksp of 9.0 × 10-12. Calculate the solubility, in moles per liter, of silver chromate.

A student titrates an unknown weak acid, HA, to a pale pink phenolphthalein endpoint with 25.0 mL of 0.100 M NaOH. The student then adds 13.0 mL of 0.100 M HCl. The pH of the resulting solution is 4.7. Which of the following statements is true?

Consider the following information about the diprotic acid ascorbic acid (H2As for short, molar mass = 176.1). The titration curve for disodium ascorbate, Na2As, with standard HCl is shown below: -What is the pH at point III?

The Ksp value for PbSO4(s) is 1.3 × 10-8. Calculate the solubility, in moles per liter, of PbSO4(s) in a 0.0010 M solution of Na2SO4.

The Ksp of Al(OH)3 is 2.0 × 10-32. At what pH will a 0.2 M Al3+ solution begin to show precipitation of Al(OH)3?

Consider a 100.0-mL sample of a 0.10 M H2A (Ka1 = 1.3 × 10-3 , Ka2 = 3.1 × 10-6) with 0.10 M NaOH. Determine the pH when 0 mL, 50.0 mL, 100.0 mL, and 150.0 mL of 0.10 M NaOH are added.

Calculate the solubility of Ag2SO4 [Ksp = 1.2 × 10-5] in a 2.0 M AgNO3 solution.

A solution contains 10. mmol of H3PO4 and 5.0 mmol of NaH2PO4. How many milliliters of 0.10 M NaOH must be added to reach the second equivalence point of the titration of the H3PO4 with NaOH?

Atoms, Molecules, and Ions

Stoichiometry

Types of Chemical Reactions and Solution Stoichiometry

Gases

Chemical Equilibrium

Acids and Bases

Energy, Enthalpy, and Thermochemistry

Spontaneity, Entropy, and Free Energy

Electrochemistry

Quantum Mechanics and Atomic Theory

Bonding: General Concepts

Covalent Bonding: Orbitals

Chemical Kinetics

Liquids and Solids

Properties of Solutions

The Representative Elements

Transition Metals and Coordination Chemistry

The Nucleus: a Chemists View

Organic and Biochemical Molecules

Filters

Calculate the solubility of Cu(OH)₂ in a solution buffered at pH = 8.50. (K_sp = 1.6 × 10^-19)

Calculate the pH of a solution prepared by mixing 50 mL of a 0.10 M solution of HF with 25 mL of a 0.20 M solution of NaF. pK_a of HF is 3.14.

Calculate the pH when 200.0 mL of a 1.00 M solution of H₂A (K_a1 = 1.0 × 10^-6, K_a2 = 1.0 × 10^-10) is titrated with the following volumes of 1.00 M NaOH. -150.0 mL of 1.00 M NaOH

A 200.0-mL sample of the weak acid H₃A (0.100 M) is titrated with 0.200 M NaOH. What are the major species at each of the following points in the titration? (Water is always assumed to be a major species.) -After 200.0 mL of 0.200 M NaOH is added

A 75.0-mL sample of 0.0500 M HCN (K_a = 6.2 × 10^-10) is titrated with 0.500 M NaOH. What is [H⁺] in the solution after 3.0 mL of 0.500 M NaOH has been added?

Consider the titration of 100.0 mL of 0.250 M aniline (K_b = 3.8 × 10^-10) with 0.500 M HCl. For calculating the volume of HCl required to reach a pH of 8.0, which of the following expressions is correct? (x = volume, in milliliters, of HCl required to reach a pH of 8.0)

Explain why we cannot directly compare K_sp values in comparing solubilities of ionic solids with different numbers of ions.

What volume of 0.0100 M NaOH must be added to 1.00 L of 0.0500 M HOCl to achieve a pH of 8.00? K_a for HOCl is 3.5 × 10^-8.

A 200.0-mL sample of the weak acid H₃A (0.100 M) is titrated with 0.200 M NaOH. What are the major species at each of the following points in the titration? (Water is always assumed to be a major species.) -After 0 mL of 0.200 M NaOH is added

A solution contains 0.50 (K_a = 2.0 × 10^-8) and 0.22 M NaA. Calculate the pH after 0.05mol of NaOH is added to 1.00 L of this solution.

The value of K_f for the complex ion Ag(NH₃)₂⁺ is 1.7 × 10⁷. K_sp for AgCl is 1.6 × 10^-10. Calculate the molar solubility of AgCl in 1.0 M NH₃.

Silver chromate, Ag₂CrO₄, has a K_sp of 9.0 × 10^-12. Calculate the solubility, in moles per liter, of silver chromate.

Consider the following information about the diprotic acid ascorbic acid (H₂As for short, molar mass = 176.1). The titration curve for disodium ascorbate, Na₂As, with standard HCl is shown below: -What is the pH at point III?

The K_sp value for PbSO₄(s) is 1.3 × 10^-8. Calculate the solubility, in moles per liter, of PbSO₄(s) in a 0.0010 M solution of Na₂SO₄.

The K_sp of Al(OH)₃ is 2.0 × 10^-32. At what pH will a 0.2 M Al³⁺ solution begin to show precipitation of Al(OH)₃?

Consider a 100.0-mL sample of a 0.10 M H₂A (K_a1 = 1.3 × 10^-3 , K_a2 = 3.1 × 10^-6) with 0.10 M NaOH. Determine the pH when 0 mL, 50.0 mL, 100.0 mL, and 150.0 mL of 0.10 M NaOH are added.

Calculate the solubility of Ag₂SO₄ [K_sp = 1.2 × 10^-5] in a 2.0 M AgNO₃ solution.

A solution contains 10. mmol of H₃PO₄ and 5.0 mmol of NaH₂PO₄. How many milliliters of 0.10 M NaOH must be added to reach the second equivalence point of the titration of the H₃PO₄ with NaOH?