Question 1

The solubility of La(IO3)3 in a 0.10 M KIO3 solution is 1.0 F1F1F1S1F1F1F10 10-7 mol/L. Calculate Ksp for La(IO3)3.

Accepted Answer

A)  2.7 F1F1F1S1F1F1F10 10-9 
B)  2.7 F1F1F1S1F1F1F10 10-27 
C)  1.0 F1F1F1S1F1F1F10 10-8 
D)  1.0 F1F1F1S1F1F1F10 10-10 
E)  none of these

Question 2

The concentration of Ag+ in a saturated solution of Ag2CrO4 is 1.6 F1F1F1S1F1F1F10 10-4 M. Calculate Ksp for Ag2CrO4.

Accepted Answer

A)  2.6 F1F1F1S1F1F1F10 10-8 
B)  5.1 F1F1F1S1F1F1F10 10-8 
C)  1.6 F1F1F1S1F1F1F10 10-11 
D)  4.1 F1F1F1S1F1F1F10 10-12 
E)  2.0 F1F1F1S1F1F1F10 10-12

Question 3

Which of the following salts shows the lowest solubility in water? Ksp values are as follows: Ag2S = 1.6 F1F1F1S1F1F1F10 10-49; Bi2S3 = 1.0 F1F1F1S1F1F1F10 10-72; HgS = 1.6 F1F1F1S1F1F1F10 10-54; Mg(OH)2 = 8.9 F1F1F1S1F1F1F10 10-12; MnS = 2.3 F1F1F1S1F1F1F10 10-13)

Accepted Answer

A)  HgS 
B)  MnS 
C)  Bi2S3 
D)  Ag2S 
E)  Mg(OH)2

Question 4

What is the molar solubility of AgCl (Ksp = 1.6 F1F1F1S1F1F1F10 10-10) in 0.0020 M sodium chloride at 25°C?

Accepted Answer

A)  8.0 F1F1F1S1F1F1F10 10-8 
B)  0.0020 
C)  1.7 F1F1F1S1F1F1F10 10-10 
D)  1.3 F1F1F1S1F1F1F10 10-5 
E)  none of these

Question 5

Which titration curve would result from the titration of phosphoric acid by a strong base?

Accepted Answer

A)   
B)   
C)   
D)   
E)  None of the above

Question 6

44.4 mL of a 1.42 M NaOH solution is titrated with a 1.90 M HCl solution. What is the final volume of the solution when the NaOH has been completely neutralized by the HCl? (Assume the volumes are additive.)

Accepted Answer

A)  33.2 mL 
B)  77.6 mL 
C)  59.4 mL 
D)  45.1 mL 
E)  104 mL

Question 7

A titration of 100.0 mL of 1.00 M malonic acid (HS1U1B12S1U1B0A) was done with 1.00 M NaOH. For malonic acid, KS1U1B1a1S1U1B0 = 1.49 F1F1F1S1F1F1F10 10S1U1P1-S1S1P0S1U1P12S1S1P0, KS1U1B1a2S1U1B0 = 2.03 F1F1F1S1F1F1F10 10S1U1P1-S1S1P0S1U1P16S1S1P0.
-Calculate the [H+] after 50.00 mL of 1.00 M NaOH has been added.

Accepted Answer

A)  2.00 F1F1F1S1F1F1F10 10-6 M 
B)  1.41 F1F1F1S1F1F1F10 10-10 M 
C)  1.49 F1F1F1S1F1F1F10 10-2 M 
D)  3.87 F1F1F1S1F1F1F10 10-2 M 
E)  none of these

Question 8

You are given 5.00 mL of an H2SO4 solution of unknown concentration. You divide the 5.00-mL sample into five 1.00-mL samples and titrate each separately with 0.1000 M NaOH. In each titration, the H2SO4 is completely neutralized. The average volume of NaOH solution used to reach the endpoint is 15.3 mL. What was the concentration of H2SO4 in the 5.00-mL sample?

Accepted Answer

A)  0.306 M 
B)  0.765 M 
C)  3.06 M 
D)  1.53 F1F1F1S1F1F1F10 10-3 M 
E)  1.53 M

Question 9

A 50.00-mL sample of 0.100 M Ca(NO3)2 is mixed with 50.00 mL of 0.200 M NaF. When the system has come to equilibrium, which of the following sets of conditions will hold? The Ksp for CaF2 is 4.0 F1F1F1S1F1F1F10 10-11.

Accepted Answer

A)  10.0 F1F1F1S1F1F1F10 10-3 1.3 F1F1F1S1F1F1F10 10-5 M 1.3 F1F1F1S1F1F1F10 10-5 M 
B)  5.0 F1F1F1S1F1F1F10 10-3 3.5 F1F1F1S1F1F1F10 10-4 M 7.0 F1F1F1S1F1F1F10 10-4 M 
C)  5.0 F1F1F1S1F1F1F10 10-3 2.2 F1F1F1S1F1F1F10 10-4 M 4.3 F1F1F1S1F1F1F10 10-4 M 
D)  5.0 F1F1F1S1F1F1F10 10-3 3.5 F1F1F1S1F1F1F10 10-4 M 4.3 F1F1F1S1F1F1F10 10-4 M 
E)  5.0 F1F1F1S1F1F1F10 10-3 3.4 F1F1F1S1F1F1F10 10-9 M 5.0 F1F1F1S1F1F1F10 10-2 M

Question 10

Which of the following titration curves schematically represents a diprotic acid being titrated by a strong base?

Accepted Answer

A)   
B)   
C)   
D)   
E)  None of the above

Question 11

The observed solubility of the salt MX in 4.0 M strong acid is 2.30 F1F1F1S1F1F1F10 10-3 M. The Ka value for the acid HX is 1.00 F1F1F1S1F1F1F10 10-9. Calculate the value of Ksp for the salt MX.

Accepted Answer

A)  1.3 F1F1F1S1F1F1F10 103 
B)  1.3 F1F1F1S1F1F1F10 10-15 
C)  5.3 F1F1F1S1F1F1F10 10-6 
D)  1.3 F1F1F1S1F1F1F10 10-6 
E)  5.3 F1F1F1S1F1F1F10 10-15

Question 12

A solution is formed by mixing 50.0 mL of 10.00 M NaCN with 50.0 mL of 2.0 F1F1F1S1F1F1F10 10S1U1P1-3S1S1P0 M CuNOS1U1B13S1U1B0. Cu(I) forms complex ions with cyanide as follows:  Calculate the following concentrations at equilibrium:
-[Cu(CN)32-]

Accepted Answer

A)  3.33 M 
B)  1.67 M 
C)  2.0 F1F1F1S1F1F1F10 10-3 M 
D)  1.0 F1F1F1S1F1F1F10 10-3 M 
E)  none of these

Question 13

Differentiate between a formation constant and a solubility product constant. Provide examples of each.

Accepted Answer

The answer of Differentiate between a formation constant and a...

Question 14

The cation M²⁺ reacts with NH₃ to form a series of complex ions as follows: Consider an experiment in which 1.0 *10^-³ mol of M(NO₃)₂is added to 1.0 L of 15.0 M NH₃. Calculate the equilibrium concentrations of M²⁺, M(NH₃)₂²⁺, and M(NH₃)₃²⁺

Accepted Answer

The answer of The cation M²⁺ reacts with NH₃ to...

Question 15

What is the pH of a solution that results when 0.012 mol HNO3 is added to 670.0 mL of a solution that is 0.26 M in aqueous ammonia and 0.48 M in ammonium nitrate. Assume no volume change. (Kb for NH3 = 1.8 F1F1F1S1F1F1F10 10-5.)

Accepted Answer

A)  8.94 
B)  9.57 
C)  5.06 
D)  8.99 
E)  4.43

Question 16

Which of the following is the net ionic equation for the reaction that occurs during the titration of nitrous acid with potassium hydroxide?

Accepted Answer

A)  HNO2 + KOH F1F1F1S1F1F1F10 K+ + NO2- + H2O 
B)  H+ + OH- F1F1F1S1F1F1F10 H2O 
C)  HNO2 + OH- F1F1F1S1F1F1F10 NO2- + H2O 
D)  HNO2 + H2O F1F1F1S1F1F1F10 NO2- + H3O+ 
E)  HNO2 + K+ + OH- F1F1F1S1F1F1F10 KNO2 + H2O

Question 17

How many moles of Fe(OH)2 [Ksp = 1.8 F1F1F1S1F1F1F10 10-15] will dissolve in 1 L of water buffered at pH = 12.00?

Accepted Answer

A)  1.8 F1F1F1S1F1F1F10 10-11 mol 
B)  1.8 F1F1F1S1F1F1F10 10-9 mol 
C)  5.0 F1F1F1S1F1F1F10 10-12 mol 
D)  8.0 F1F1F1S1F1F1F10 10-6 mol 
E)  4.0 F1F1F1S1F1F1F10 10-8 mol

Question 18

How many moles of CaF2 will dissolve in 3.0 L of 0.050 M NaF solution? (Ksp for CaF2 = 4.0 F1F1F1S1F1F1F10 10-11)

Accepted Answer

A)  4.8 F1F1F1S1F1F1F10 10-8 mol 
B)  8.9 F1F1F1S1F1F1F10 10-9 mol 
C)  8.0 F1F1F1S1F1F1F10 10-8 mol 
D)  2.7 F1F1F1S1F1F1F10 10-8 mol 
E)  none of these

Question 19

Calculate the solubility of Cu(OH)2 in a solution buffered at pH = 8.50. (Ksp = 1.6 F1F1F1S1F1F1F10 10-19)

Accepted Answer

A)  5.7 F1F1F1S1F1F1F10 10-10 M 
B)  1.6 F1F1F1S1F1F1F10 10-2 M 
C)  1.8 F1F1F1S1F1F1F10 10-7 M 
D)  1.6 F1F1F1S1F1F1F10 10-8 M 
E)  none of these

Question 20

Which of the following will not produce a buffered solution?

Accepted Answer

A)  100 mL of 0.1 M Na2CO3 and 50 mL of 0.1 M HCl 
B)  100 mL of 0.1 M NaHCO3 and 25 mL of 0.2 M HCl 
C)  100 mL of 0.1 M Na2CO3 and 75 mL of 0.2 M HCl 
D)  50 mL of 0.2 M Na2CO3 and 5 mL of 1.0 M HCl 
E)  100 mL of 0.1 M Na2CO3 and 50 mL of 0.1 M NaOH

Exam 8: Applications of Aqueous Equilibria

The solubility of La(IO₃) ₃ in a 0.10 M KIO₃ solution is 1.0  10^-⁷ mol/L. Calculate K_sp for La(IO₃) ₃.

The concentration of Ag⁺ in a saturated solution of Ag₂CrO₄ is 1.6  10^-⁴ M. Calculate K_sp for Ag₂CrO₄.

Which of the following salts shows the lowest solubility in water? K_sp values are as follows: Ag₂S = 1.6  10^-⁴⁹; Bi₂S₃ = 1.0  10^-⁷²; HgS = 1.6  10^-⁵⁴; Mg(OH) ₂ = 8.9  10^-¹²; MnS = 2.3  10^-¹³)

What is the molar solubility of AgCl (K_sp = 1.6  10^-¹⁰) in 0.0020 M sodium chloride at 25°C?

Which titration curve would result from the titration of phosphoric acid by a strong base?

44.4 mL of a 1.42 M NaOH solution is titrated with a 1.90 M HCl solution. What is the final volume of the solution when the NaOH has been completely neutralized by the HCl? (Assume the volumes are additive.)

A titration of 100.0 mL of 1.00 M malonic acid (H₂A) was done with 1.00 M NaOH. For malonic acid, K_a1 = 1.49  10^-², K_a2 = 2.03  10^-⁶. -Calculate the [H⁺] after 50.00 mL of 1.00 M NaOH has been added.

A 50.00-mL sample of 0.100 M Ca(NO₃) ₂ is mixed with 50.00 mL of 0.200 M NaF. When the system has come to equilibrium, which of the following sets of conditions will hold? The K_sp for CaF₂ is 4.0  10^-¹¹.

Which of the following titration curves schematically represents a diprotic acid being titrated by a strong base?

The observed solubility of the salt MX in 4.0 M strong acid is 2.30  10^-³ M. The K_a value for the acid HX is 1.00  10^-⁹. Calculate the value of K_sp for the salt MX.

A solution is formed by mixing 50.0 mL of 10.00 M NaCN with 50.0 mL of 2.0  10^-3 M CuNO₃. Cu(I) forms complex ions with cyanide as follows: Calculate the following concentrations at equilibrium: -[Cu(CN) ₃²^-]

Differentiate between a formation constant and a solubility product constant. Provide examples of each.

The cation M²⁺ reacts with NH₃ to form a series of complex ions as follows: Consider an experiment in which 1.0 *10^-³ mol of M(NO₃)₂is added to 1.0 L of 15.0 M NH₃. Calculate the equilibrium concentrations of M²⁺, M(NH₃)₂²⁺, and M(NH₃)₃²⁺

What is the pH of a solution that results when 0.012 mol HNO₃ is added to 670.0 mL of a solution that is 0.26 M in aqueous ammonia and 0.48 M in ammonium nitrate. Assume no volume change. (K_b for NH₃ = 1.8  10^-⁵.)

Which of the following is the net ionic equation for the reaction that occurs during the titration of nitrous acid with potassium hydroxide?

How many moles of Fe(OH) ₂ [K_sp = 1.8  10^-¹⁵] will dissolve in 1 L of water buffered at pH = 12.00?

How many moles of CaF₂ will dissolve in 3.0 L of 0.050 M NaF solution? (K_sp for CaF₂ = 4.0  10^-¹¹)

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

Which of the following will not produce a buffered solution?

Exam 8: Applications of Aqueous Equilibria

The solubility of La(IO3) 3 in a 0.10 M KIO3 solution is 1.0  10-7 mol/L. Calculate Ksp for La(IO3) 3.

The concentration of Ag+ in a saturated solution of Ag2CrO4 is 1.6  10-4 M. Calculate Ksp for Ag2CrO4.

Which of the following salts shows the lowest solubility in water? Ksp values are as follows: Ag2S = 1.6  10-49; Bi2S3 = 1.0  10-72; HgS = 1.6  10-54; Mg(OH) 2 = 8.9  10-12; MnS = 2.3  10-13)

What is the molar solubility of AgCl (Ksp = 1.6  10-10) in 0.0020 M sodium chloride at 25°C?

Which titration curve would result from the titration of phosphoric acid by a strong base?

44.4 mL of a 1.42 M NaOH solution is titrated with a 1.90 M HCl solution. What is the final volume of the solution when the NaOH has been completely neutralized by the HCl? (Assume the volumes are additive.)

A titration of 100.0 mL of 1.00 M malonic acid (H2A) was done with 1.00 M NaOH. For malonic acid, Ka1 = 1.49  10-2, Ka2 = 2.03  10-6. -Calculate the [H+] after 50.00 mL of 1.00 M NaOH has been added.

A 50.00-mL sample of 0.100 M Ca(NO3) 2 is mixed with 50.00 mL of 0.200 M NaF. When the system has come to equilibrium, which of the following sets of conditions will hold? The Ksp for CaF2 is 4.0  10-11.

Which of the following titration curves schematically represents a diprotic acid being titrated by a strong base?

The observed solubility of the salt MX in 4.0 M strong acid is 2.30  10-3 M. The Ka value for the acid HX is 1.00  10-9. Calculate the value of Ksp for the salt MX.

A solution is formed by mixing 50.0 mL of 10.00 M NaCN with 50.0 mL of 2.0  10-3 M CuNO3. Cu(I) forms complex ions with cyanide as follows: Calculate the following concentrations at equilibrium: -[Cu(CN) 32-]

Differentiate between a formation constant and a solubility product constant. Provide examples of each.

The cation M2+ reacts with NH3 to form a series of complex ions as follows: Consider an experiment in which 1.0 *10-3 mol of M(NO3)2 is added to 1.0 L of 15.0 M NH3. Calculate the equilibrium concentrations of M2+, M(NH3)22+, and M(NH3)32+

What is the pH of a solution that results when 0.012 mol HNO3 is added to 670.0 mL of a solution that is 0.26 M in aqueous ammonia and 0.48 M in ammonium nitrate. Assume no volume change. (Kb for NH3 = 1.8  10-5.)

Which of the following is the net ionic equation for the reaction that occurs during the titration of nitrous acid with potassium hydroxide?

How many moles of Fe(OH) 2 [Ksp = 1.8  10-15] will dissolve in 1 L of water buffered at pH = 12.00?

How many moles of CaF2 will dissolve in 3.0 L of 0.050 M NaF solution? (Ksp for CaF2 = 4.0  10-11)

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

Which of the following will not produce a buffered solution?

The solubility of La(IO₃) ₃ in a 0.10 M KIO₃ solution is 1.0  10^-⁷ mol/L. Calculate K_sp for La(IO₃) ₃.

The concentration of Ag⁺ in a saturated solution of Ag₂CrO₄ is 1.6  10^-⁴ M. Calculate K_sp for Ag₂CrO₄.

Which of the following salts shows the lowest solubility in water? K_sp values are as follows: Ag₂S = 1.6  10^-⁴⁹; Bi₂S₃ = 1.0  10^-⁷²; HgS = 1.6  10^-⁵⁴; Mg(OH) ₂ = 8.9  10^-¹²; MnS = 2.3  10^-¹³)

What is the molar solubility of AgCl (K_sp = 1.6  10^-¹⁰) in 0.0020 M sodium chloride at 25°C?

A titration of 100.0 mL of 1.00 M malonic acid (H₂A) was done with 1.00 M NaOH. For malonic acid, K_a1 = 1.49  10^-², K_a2 = 2.03  10^-⁶. -Calculate the [H⁺] after 50.00 mL of 1.00 M NaOH has been added.

A 50.00-mL sample of 0.100 M Ca(NO₃) ₂ is mixed with 50.00 mL of 0.200 M NaF. When the system has come to equilibrium, which of the following sets of conditions will hold? The K_sp for CaF₂ is 4.0  10^-¹¹.

The observed solubility of the salt MX in 4.0 M strong acid is 2.30  10^-³ M. The K_a value for the acid HX is 1.00  10^-⁹. Calculate the value of K_sp for the salt MX.

A solution is formed by mixing 50.0 mL of 10.00 M NaCN with 50.0 mL of 2.0  10^-3 M CuNO₃. Cu(I) forms complex ions with cyanide as follows: Calculate the following concentrations at equilibrium: -[Cu(CN) ₃²^-]

The cation M²⁺ reacts with NH₃ to form a series of complex ions as follows: Consider an experiment in which 1.0 *10^-³ mol of M(NO₃)₂is added to 1.0 L of 15.0 M NH₃. Calculate the equilibrium concentrations of M²⁺, M(NH₃)₂²⁺, and M(NH₃)₃²⁺

What is the pH of a solution that results when 0.012 mol HNO₃ is added to 670.0 mL of a solution that is 0.26 M in aqueous ammonia and 0.48 M in ammonium nitrate. Assume no volume change. (K_b for NH₃ = 1.8  10^-⁵.)

How many moles of Fe(OH) ₂ [K_sp = 1.8  10^-¹⁵] will dissolve in 1 L of water buffered at pH = 12.00?

How many moles of CaF₂ will dissolve in 3.0 L of 0.050 M NaF solution? (K_sp for CaF₂ = 4.0  10^-¹¹)

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