Question 1

Calculate the molar solubility of BaCO3 in a 0.10 M solution of Na2CO3(aq) .(Ksp (BaCO3) = 8.1 x 10-9)

Accepted Answer

A)  8.1 x 10-9 M
B)  9.0 x 10-5 M
C)  8.1 x 10-8 M
D)  2.8 x 10-4 M
E)  0.10 M

Question 2

At 25 °C, the base ionization constant for NH3 is 1.8 × 10-5.Determine the pH of a solution prepared by adding 0.0500 mol of solid ammonium chloride to 100.mL of 0.150 M ammonia.

Accepted Answer

Question 3

Write a net ionic equation for the reaction that occurs when a small amount of nitric acid is added to a NaNO2/HNO2 buffer.

Accepted Answer

Question 4

What molar ratio of benzoate ion to benzoic acid would be required to prepare a buffer with a pH of 5.20? [Ka(C6H5COOH)= 6.5 × 10-5]

Accepted Answer

Question 5

Which of the following yields a buffer solution when equal volumes of the two solutions are mixed?

Accepted Answer

A)  0.10M H2CO3 and 0.050M HCl
B)  0.10M H2CO3 and 0.10M KOH
C)  0.10M H2CO3 and 0.10M HCl
D)  0.10M H2CO3 and 0.050M KOH
E)  0.10M K2CO3 and 0.050M KOH

Question 6

Find the concentration of calcium ions in a solution made by adding 3.50 g of calcium fluoride to 750.mL of 0.125 M NaF.[For CaF2, Ksp = 3.95 × 10-11.]

Accepted Answer

A)  3.16 × 10-10 M
B)  2.53 × 10-9 M
C)  4.29 × 10-4 M
D)  6.32 × 10-10 M
E)  2.15 × 10-4 M

Question 7

Find the concentration of Pb2+ ions in a solution made by adding 5.00 g of lead(II) iodide to 500.mL of 0.150 M KI.[For PbI2, Ksp = 1.39 × 10-8.]

Accepted Answer

A)  3.04 × 10-4 M
B)  1.54 × 10-7 M
C)  6.18 × 10-7 M
D)  1.52 × 10-4 M
E)  9.27 × 10-8 M

Question 8

Which response has both answers correct? Will a precipitate form when 250 mL of 0.33 M Na2CrO4 are added to 250 mL of 0.12 M AgNO3? [Ksp(Ag2CrO4) = 1.1 × 10-12] What is the concentration of the silver ion remaining in solution?

Accepted Answer

A)  Yes, [Ag+] = 2.9 × 10-6 M.
B)  Yes, [Ag+] = 0.060 M.
C)  Yes, [Ag+] = 1.3 × 10-4 M.
D)  No, [Ag+] = 0.060 M.
E)  No, [Ag+] = 0.105 M.

Question 9

The molar solubility of lead(II) iodate in water is 4.0 × 10-5 mol/L.Calculate Ksp for lead(II) iodate.

Accepted Answer

A)  1.6 × 10-9
B)  6.4 × 10-14
C)  2.6 × 10-13
D)  4.0 × 10-5
E)  4.0 × 10-15

Question 10

A mixture made from 10 mL of 1 M HCl and 20 mL of 1 M CH3COONa would be classified as a buffer solution.

Accepted Answer

A) True 
 B)False

Question 11

The solubility product for calcium phosphate is Ksp = 1.3 × 10-26.What is the molar solubility of calcium phosphate?

Accepted Answer

A)  1.3 × 10-26 M
B)  1.5 × 10-7 M
C)  2.6 × 10-6 M
D)  4.6 × 10-6 M
E)  6.6 × 10-6 M

Question 12

In which one of the following solutions will acetic acid have the greatest percent ionization?

Accepted Answer

A)  0.1 M CH3COOH
B)  0.1 M CH3COOH dissolved in 0.1 M HCl
C)  0.1 M CH3COOH dissolved in 0.2 M HCl
D)  0.1 M CH3COOH plus 0.1 M CH3COONa
E)  0.1 M CH3COOH plus 0.2 M CH3COONa

Question 13

What is the pH at the equivalence point in the titration of 100 mL of 0.10 M HCl with 0.10 M NaOH?

Accepted Answer

A)  1.0
B)  6.0
C)  7.0
D)  8.0
E)  13.0

Question 14

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

Question 15

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.(For CrF3 , Ksp = 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

Question 16

Calculate the percent ionization of cyanic acid, Ka = 2.0 × 10-4, in a buffer solution that is 0.50 M HCNO and 0.10 M NaCNO.

Accepted Answer

A)  0.02%
B)  0.10%
C)  0.20%
D)  2.0%
E)  20% C

Question 17

All indicators are weak acids that are one color in acidic solution and another color in basic solution.

Accepted Answer

A) True 
 B)False  False

Question 18

Solid sodium iodide is slowly added to a solution that is 0.0050 M Pb2+ and 0.0050 M Ag+.[Ksp (PbI2)= 1.4 × 10-8; Ksp (AgI)= 8.3 × 10-17] Calculate the Ag+ concentration when PbI2 just begins to precipitate.

Accepted Answer

Question 19

The Ksp value for lead(II) chloride is 2.4 × 10-4.What is the molar solubility of lead(II) chloride?

Accepted Answer

A)  2.4 × 10-4 mol/L
B)  6.2 × 10-2 mol/L
C)  7.7 × 10-3 mol/L
D)  3.9 × 10-2 mol/L
E)  6.0 × 10-5 mol/L

Question 20

Which of the following would decrease the Ksp for PbI2?

Accepted Answer

A)  Lowering the pH of the solution
B)  Adding a solution of Pb(NO3) 2
C)  Adding a solution of KI
D)  None of the above-the Ksp of a compound is constant at constant temperature. D

Exam 16: Acid-Base Equilibria and Solubility Equilibria

Calculate the molar solubility of BaCO3 in a 0.10 M solution of Na2CO3(aq) .(Ksp (BaCO3) = 8.1 x 10-9)

Correct AnswerverifiedShow Answer

At 25 °C, the base ionization constant for NH3 is 1.8 × 10-5.Determine the pH of a solution prepared by adding 0.0500 mol of solid ammonium chloride to 100.mL of 0.150 M ammonia.

Correct AnswerverifiedShow Answer

Write a net ionic equation for the reaction that occurs when a small amount of nitric acid is added to a NaNO2/HNO2 buffer.

Correct AnswerverifiedShow Answer

What molar ratio of benzoate ion to benzoic acid would be required to prepare a buffer with a pH of 5.20? [Ka(C6H5COOH)= 6.5 × 10-5]

Correct AnswerverifiedShow Answer

Which of the following yields a buffer solution when equal volumes of the two solutions are mixed?

Correct AnswerverifiedShow Answer

Find the concentration of calcium ions in a solution made by adding 3.50 g of calcium fluoride to 750.mL of 0.125 M NaF.[For CaF2, Ksp = 3.95 × 10-11.]

Correct AnswerverifiedShow Answer

Find the concentration of Pb2+ ions in a solution made by adding 5.00 g of lead(II) iodide to 500.mL of 0.150 M KI.[For PbI2, Ksp = 1.39 × 10-8.]

Correct AnswerverifiedShow Answer

Which response has both answers correct? Will a precipitate form when 250 mL of 0.33 M Na2CrO4 are added to 250 mL of 0.12 M AgNO3? [Ksp(Ag2CrO4) = 1.1 × 10-12] What is the concentration of the silver ion remaining in solution?

Correct AnswerverifiedShow Answer

The molar solubility of lead(II) iodate in water is 4.0 × 10-5 mol/L.Calculate Ksp for lead(II) iodate.

Correct AnswerverifiedShow Answer

A mixture made from 10 mL of 1 M HCl and 20 mL of 1 M CH3COONa would be classified as a buffer solution.

Correct AnswerverifiedShow Answer

The solubility product for calcium phosphate is Ksp = 1.3 × 10-26.What is the molar solubility of calcium phosphate?

Correct AnswerverifiedShow Answer

In which one of the following solutions will acetic acid have the greatest percent ionization?

Correct AnswerverifiedShow Answer

What is the pH at the equivalence point in the titration of 100 mL of 0.10 M HCl with 0.10 M NaOH?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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.(For CrF3 , Ksp = 6.6 × 10-11.)

Correct AnswerverifiedShow Answer

Calculate the percent ionization of cyanic acid, Ka = 2.0 × 10-4, in a buffer solution that is 0.50 M HCNO and 0.10 M NaCNO.

Correct AnswerverifiedC

All indicators are weak acids that are one color in acidic solution and another color in basic solution.

Correct AnswerverifiedFalse

Solid sodium iodide is slowly added to a solution that is 0.0050 M Pb2+ and 0.0050 M Ag+.[Ksp (PbI2)= 1.4 × 10-8; Ksp (AgI)= 8.3 × 10-17] Calculate the Ag+ concentration when PbI2 just begins to precipitate.

Correct AnswerverifiedShow Answer

The Ksp value for lead(II) chloride is 2.4 × 10-4.What is the molar solubility of lead(II) chloride?

Correct AnswerverifiedShow Answer

Which of the following would decrease the Ksp for PbI2?

Correct AnswerverifiedD

Calculate the molar solubility of BaCO₃ in a 0.10 M solution of Na₂CO₃(aq) .(K_sp (BaCO₃) = 8.1 x 10^-9)

Correct Answer
verified

At 25 °C, the base ionization constant for NH₃ is 1.8 × 10^-5.Determine the pH of a solution prepared by adding 0.0500 mol of solid ammonium chloride to 100.mL of 0.150 M ammonia.

Correct Answer
verified

Write a net ionic equation for the reaction that occurs when a small amount of nitric acid is added to a NaNO₂/HNO₂ buffer.

Correct Answer
verified

What molar ratio of benzoate ion to benzoic acid would be required to prepare a buffer with a pH of 5.20? [K_a(C₆H₅COOH)= 6.5 × 10^-5]

Correct Answer
verified

Correct Answer
verified

Find the concentration of calcium ions in a solution made by adding 3.50 g of calcium fluoride to 750.mL of 0.125 M NaF.[For CaF₂, K_sp = 3.95 × 10^-11.]

Correct Answer
verified

Find the concentration of Pb²⁺ ions in a solution made by adding 5.00 g of lead(II) iodide to 500.mL of 0.150 M KI.[For PbI₂, K_sp = 1.39 × 10^-8.]

Correct Answer
verified

Which response has both answers correct? Will a precipitate form when 250 mL of 0.33 M Na₂CrO₄ are added to 250 mL of 0.12 M AgNO₃? [K_sp(Ag₂CrO₄) = 1.1 × 10^-12] What is the concentration of the silver ion remaining in solution?

Correct Answer
verified

The molar solubility of lead(II) iodate in water is 4.0 × 10^-5 mol/L.Calculate K_sp for lead(II) iodate.

Correct Answer
verified

A mixture made from 10 mL of 1 M HCl and 20 mL of 1 M CH₃COONa would be classified as a buffer solution.

Correct Answer
verified

The solubility product for calcium phosphate is K_sp = 1.3 × 10^-26.What is the molar solubility of calcium phosphate?

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

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

Correct Answer
verified

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.(For CrF₃, K_sp = 6.6 × 10^-11.)

Correct Answer
verified

Calculate the percent ionization of cyanic acid, K_a = 2.0 × 10^-4, in a buffer solution that is 0.50 M HCNO and 0.10 M NaCNO.

Correct Answer
verified
C

Correct Answer
verified
False

Solid sodium iodide is slowly added to a solution that is 0.0050 M Pb²⁺ and 0.0050 M Ag⁺.[K_sp (PbI₂)= 1.4 × 10^-8; K_sp (AgI)= 8.3 × 10^-17] Calculate the Ag⁺ concentration when PbI₂ just begins to precipitate.

Correct Answer
verified

The K_sp value for lead(II) chloride is 2.4 × 10^-4.What is the molar solubility of lead(II) chloride?

Correct Answer
verified

Which of the following would decrease the K_sp for PbI₂?

Correct Answer
verified
D