Question 1

The solubility product for barium sulfate is 1.1 * 10-10. Calculate the molar solubility of barium sulfate.

Accepted Answer

A)  5.5 * 10-11 mol/L
B)  1.1 * 10-5 mol/L
C)  2.1 * 10-5 mol/L
D)  1.1 * 10-10 mol/L
E)  2.2 * 10-10 mol/LF) D) and E)
G) A) and C)

Question 2

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] What percent of Ag+ remains in solution at this point?

Accepted Answer

1.0 * 10<s...

Question 3

Calculate the percent ionization of formic acid in a 0.010 M HCOOH solution.
(Ka = 1.7 *10-4)

Accepted Answer

The answer of Calculate the percent ionization of formic acid...

Question 4

To 1.00 L of a 0.100 M aqueous solution of the week base pyridine (C5H5N) is added 1.00 mL of 14.0 M NaOH. What fraction of the pyridine molecules in the resulting solution react with water to release hydroxide ions? [Kb(C5H5N) = 1.7 * 10-9]

Accepted Answer

A)  1.2 * 10-7
B)  4.1 * 10-5
C)  0.14
D)  2.4 * 10-10
E)  1.3 * 10-5F) A) and B)
G) A) and D)

Question 5

Calculate the pH of a buffer solution prepared by dissolving 0.20 mole of cyanic acid (HCNO) and 0.80 mole of sodium cyanate (NaCNO) in enough water to make 1.0 liter of solution. [Ka(HCNO) = 2.0 * 10-4]

Accepted Answer

A)  0.97
B)  3.10
C)  4.40
D)  3.70
E)  4.30F) None of the above
G) A) and E)

Question 6

Calculate the pH of the solution resulting from the addition of 10.0 mL of 0.10 M NaOH to 50.0 mL of 0.10 M HCN (Ka = 4.9 * 10-10) solution.

Accepted Answer

A)  5.15
B)  8.71
C)  5.85
D)  9.91
E)  13.0F) A) and B)
G) B) and C)

Question 7

Calculate the percent ionization of formic acid in a solution that is 0.010 M HCOOH and 0.050 M HCOONa.(Ka = 1.7 * 10-4)

Accepted Answer

The answer of Calculate the percent ionization of formic acid...

Question 8

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

Accepted Answer

A)  1.1 * 10-8
B)  3.9 * 10-6
C)  1.1 * 10-11
D)  2.7 * 10-12
E)  1.4 * 10-3F) B) and C)
G) A) and E)

Question 9

A solution is prepared by mixing 500.mL of 0.10 M NaOCl and 500.mL of 0.20 M HOCl.What is the pH of this solution? [Ka(HOCl) = 3.2 * 10-8]

Accepted Answer

A)  4.10
B)  7.00
C)  7.19
D)  7.49
E)  7.80F) B) and D)
G) B) and E)

Question 10

The pH at the equivalence point of a titration may differ from 7.0 due to

Accepted Answer

A)  the initial concentration of the standard solution.
B)  the indicator used.
C)  the self-ionization of H2O.
D)  the initial pH of the unknown.
E)  hydrolysis of the salt formed.F) A) and B)
G) A) and C)

Question 11

Calculate the pH at the equivalence point for the titration of 0.20 M HCl with 0.20 M NH3 (Kb = 1.8 * 10-5) .

Accepted Answer

A)  2.87
B)  4.98
C)  5.12
D)  7.00
E)  11.12F) B) and D)
G) All of the above

Question 12

You have 500.0 mL of a buffer solution containing 0.20 M acetic acid (CH3COOH) and 0.30 M sodium acetate (CH3COONa) . What will the pH of this solution be after the addition of 20.0 mL of 1.00 M NaOH solution? [Ka = 1.8 * 10-5]

Accepted Answer

A)  4.41
B)  4.74
C)  4.56
D)  4.92
E)  5.07F) B) and D)
G) A) and C)

Question 13

Which one of the following is a buffer solution?

Accepted Answer

A)  0.40 M HCN and 0.10 KCN
B)  0.20 M CH3COOH
C)  1.0 M HNO3 and 1.0 M NaNO3
D)  0.10 M KCN
E)  0.50 M HCl and 0.10 NaClF) B) and E)
G) A) and D)

Question 14

Write a net ionic equation for the reaction occurring when a small amount of sodium hydroxide solution is added to a buffer solution containing NH4Cl and NH3.

Accepted Answer

OH^- + NH<...

Question 15

Calculate the percent ionization of formic acid in a solution that is 0.010 M HCOOH and 0.005 M HCOONa and compare your answer to the percent ionization you would calculate if the sodium formate were not present. Explain the difference, if any.(Ka = 1.7 * 10-4)

Accepted Answer

3.4%; the addition of formate ...

Question 16

Write a net ionic equation for the reaction occurring when a small amount of sodium hydroxide is added to a NaNO2/HNO2 buffer.

Accepted Answer

OH^- + HNO...

Question 17

The solubility of strontium carbonate is 0.0011 g/100 mL at 20ºC. Calculate the Ksp value for this compound.

Accepted Answer

A)  7.5 * 10-5
B)  1.5 * 10-4
C)  5.6 * 10-9
D)  7.5 * 10-6
E)  1.5 * 10-3F) A) and B)
G) None of the above

Question 18

Calculate the pH of a buffer solution that contains 0.25 M benzoic acid (C6H5CO2H) and 0.15M sodium benzoate (C6H5COONa) . [Ka = 6.5 * 10-5 for benzoic acid]

Accepted Answer

A)  3.97
B)  4.83
C)  4.19
D)  3.40
E)  4.41F) All of the above
G) A) and B)

Question 19

Calculate the pH at the equivalence point for the titration of 0.22 M HCN with 0.22 M NaOH. (Ka = 4.9 * 10-10 for HCN)

Accepted Answer

The answer of Calculate the pH at the equivalence point...

Question 20

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 MF) C) and D)
G) B) and E)

Exam 16: Acid-Base Equilibria and Solubility Equilibria

Calculate the pH of the solution resulting from the addition of 10.0 mL of 0.10 M NaOH to 50.0 mL of 0.10 M HCN (Ka = 4.9 * 10-10) solution.

Correct AnswerverifiedShow Answer

Which one of the following is a buffer solution?

Correct AnswerverifiedShow Answer

To 1.00 L of a 0.100 M aqueous solution of the week base pyridine (C5H5N) is added 1.00 mL of 14.0 M NaOH. What fraction of the pyridine molecules in the resulting solution react with water to release hydroxide ions? [Kb(C5H5N) = 1.7 * 10-9]

Correct AnswerverifiedShow Answer

Write a net ionic equation for the reaction occurring when a small amount of sodium hydroxide solution is added to a buffer solution containing NH4Cl and NH3.

Correct AnswerverifiedOH- + NH<...View AnswerShow Answer

Calculate the pH at the equivalence point for the titration of 0.22 M HCN with 0.22 M NaOH. (Ka = 4.9 * 10-10 for HCN)

Correct AnswerverifiedShow Answer

Calculate the pH of a buffer solution prepared by dissolving 0.20 mole of cyanic acid (HCNO) and 0.80 mole of sodium cyanate (NaCNO) in enough water to make 1.0 liter of solution. [Ka(HCNO) = 2.0 * 10-4]

Correct AnswerverifiedShow Answer

You have 500.0 mL of a buffer solution containing 0.20 M acetic acid (CH3COOH) and 0.30 M sodium acetate (CH3COONa) . What will the pH of this solution be after the addition of 20.0 mL of 1.00 M NaOH solution? [Ka = 1.8 * 10-5]

Correct AnswerverifiedShow Answer

Calculate the percent ionization of formic acid in a 0.010 M HCOOH solution. (Ka = 1.7 *10-4)

Correct AnswerverifiedShow Answer

The pH at the equivalence point of a titration may differ from 7.0 due to

Correct AnswerverifiedShow Answer

The solubility product for barium sulfate is 1.1 * 10-10. Calculate the molar solubility of barium sulfate.

Correct AnswerverifiedShow Answer

The solubility of strontium carbonate is 0.0011 g/100 mL at 20ºC. Calculate the Ksp value for this compound.

Correct AnswerverifiedShow Answer

Calculate the pH of a buffer solution that contains 0.25 M benzoic acid (C6H5CO2H) and 0.15M sodium benzoate (C6H5COONa) . [Ka = 6.5 * 10-5 for benzoic acid]

Correct AnswerverifiedShow Answer

Write a net ionic equation for the reaction occurring when a small amount of sodium hydroxide is added to a NaNO2/HNO2 buffer.

Correct AnswerverifiedOH- + HNO...View AnswerShow Answer

Calculate the pH at the equivalence point for the titration of 0.20 M HCl with 0.20 M NH3 (Kb = 1.8 * 10-5) .

Correct AnswerverifiedShow Answer

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] What percent of Ag+ remains in solution at this point?

Correct Answerverified1.0 * 10View AnswerShow Answer

Calculate the percent ionization of formic acid in a solution that is 0.010 M HCOOH and 0.050 M HCOONa.(Ka = 1.7 * 10-4)

Correct AnswerverifiedShow Answer

Calculate the percent ionization of formic acid in a solution that is 0.010 M HCOOH and 0.005 M HCOONa and compare your answer to the percent ionization you would calculate if the sodium formate were not present. Explain the difference, if any.(Ka = 1.7 * 10-4)

Correct Answerverified3.4%; the addition of formate ...View AnswerShow 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

A solution is prepared by mixing 500.mL of 0.10 M NaOCl and 500.mL of 0.20 M HOCl.What is the pH of this solution? [Ka(HOCl) = 3.2 * 10-8]

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Calculate the pH of the solution resulting from the addition of 10.0 mL of 0.10 M NaOH to 50.0 mL of 0.10 M HCN (K_a = 4.9 * 10^-10) solution.

Correct Answer
verified

Correct Answer
verified

To 1.00 L of a 0.100 M aqueous solution of the week base pyridine (C₅H₅N) is added 1.00 mL of 14.0 M NaOH. What fraction of the pyridine molecules in the resulting solution react with water to release hydroxide ions? [K_b(C₅H₅N) = 1.7 * 10^-9]

Correct Answer
verified

Write a net ionic equation for the reaction occurring when a small amount of sodium hydroxide solution is added to a buffer solution containing NH₄Cl and NH₃.

Correct Answer
verified
OH^- + NH<...
View Answer

Calculate the pH at the equivalence point for the titration of 0.22 M HCN with 0.22 M NaOH. (K_a = 4.9 * 10^-10 for HCN)

Correct Answer
verified

Calculate the pH of a buffer solution prepared by dissolving 0.20 mole of cyanic acid (HCNO) and 0.80 mole of sodium cyanate (NaCNO) in enough water to make 1.0 liter of solution. [K_a(HCNO) = 2.0 * 10^-4]

Correct Answer
verified

You have 500.0 mL of a buffer solution containing 0.20 M acetic acid (CH₃COOH) and 0.30 M sodium acetate (CH₃COONa) . What will the pH of this solution be after the addition of 20.0 mL of 1.00 M NaOH solution? [K_a = 1.8 * 10^-5]

Correct Answer
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Calculate the percent ionization of formic acid in a 0.010 M HCOOH solution. (K_a = 1.7 *10^-4)

Correct Answer
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Correct Answer
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The solubility product for barium sulfate is 1.1 * 10^-10. Calculate the molar solubility of barium sulfate.

Correct Answer
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The solubility of strontium carbonate is 0.0011 g/100 mL at 20ºC. Calculate the K_sp value for this compound.

Correct Answer
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Calculate the pH of a buffer solution that contains 0.25 M benzoic acid (C₆H₅CO₂H) and 0.15M sodium benzoate (C₆H₅COONa) . [K_a = 6.5 * 10^-5 for benzoic acid]

Correct Answer
verified

Write a net ionic equation for the reaction occurring when a small amount of sodium hydroxide is added to a NaNO₂/HNO₂ buffer.

Correct Answer
verified
OH^- + HNO...
View Answer

Calculate the pH at the equivalence point for the titration of 0.20 M HCl with 0.20 M NH₃ (K_b = 1.8 * 10^-5) .

Correct Answer
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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] What percent of Ag⁺ remains in solution at this point?

Correct Answer
verified
1.0 * 10
View Answer

Calculate the percent ionization of formic acid in a solution that is 0.010 M HCOOH and 0.050 M HCOONa.(K_a = 1.7 * 10^-4)

Correct Answer
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Calculate the percent ionization of formic acid in a solution that is 0.010 M HCOOH and 0.005 M HCOONa and compare your answer to the percent ionization you would calculate if the sodium formate were not present. Explain the difference, if any.(K_a = 1.7 * 10^-4)

Correct Answer
verified
3.4%; the addition of formate ...
View 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, K_sp = 3.95 * 10^-11.]

Correct Answer
verified

A solution is prepared by mixing 500.mL of 0.10 M NaOCl and 500.mL of 0.20 M HOCl.What is the pH of this solution? [K_a(HOCl) = 3.2 * 10^-8]

Correct Answer
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Correct Answer
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