Question 1

You need to prepare a buffer solution with a pH of 4.00, using NaF and HF. What ratio of the ratio of [base]/[acid] should be used in making the buffer? For HF, Ka = 7.2 × 10- 4.

Accepted Answer

A)   [base]/[acid] = 0.14
B)   [base]/[acid] = 0.42
C)   [base]/[acid] = 2.36
D)   [base]/[acid] = 7.20
E)   None of the above ratios is correct.F) A) and E)
G) A) and B)

Question 2

What mass of NaF must be added to 50.0 mL of a 0.500 M HF solution to achieve a pH of 3.25? For HF, Ka = 7.2 × 10-4.

Accepted Answer

A)   1.3 g
B)   0.69 g
C)   6.9 g
D)   23 g
E)   1.5 gF) A) and D)
G) None of the above

Question 3

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 = 1.7 × 10-4

Accepted Answer

A)   2.87
B)   3.72
C)   3.82
D)   3.95
E)   4.66F) A) and D)
G) A) and E)

Question 4

What is the [H3O+] in a solution that consists of 0.15 M C2N2H8 (ethylene diamine)  and 0.35 C2N2H9Cl? Kb = 4.7 × 10-4

Accepted Answer

A)   2.0 × 10-3 M
B)   1.1 × 10-3 M
C)   6.3 × 10-9 M
D)   2.1 × 10-10 M
E)   5.0 × 10-11 MF) A) and D)
G) All of the above

Question 5

Which one of the following is the best representation of the titration curve which will be obtained in the titration of a weak base (0.10 mol L-1)  with HCl of the same concentration?

Accepted Answer

A)  -1)  with HCl of the same concentration?   
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Question 6

A solution is prepared by mixing 50.0 mL of 0.50 M Cu(NO3) 2 with 50.0 mL of 0.50 M Co(NO3) 2. Sodium hydroxide is added to the mixture. Which hydroxide precipitates first and what concentration of hydroxide ions present in solution will accomplish the separation? Ksp = 2.2 × 10-20 for Cu(OH) 2, Ksp = 1.3 × 10-15 for Co(OH) 2

Accepted Answer

A)   Co(OH) 2; [OH-] = 6.9 × 10-6 M
B)   Co(OH) 2; [OH-] = 2.6 × 10-7 M
C)   Cu(OH) 2; [OH-] = 1.8 × 10-7 M
D)   Cu(OH) 2; [OH-] = 1.1 × 10-9 M
E)   Cu(OH) 2; [OH-] = 1.0 × 10-17 MF) A) and B)
G) A) and D)

Question 7

A buffer is prepared by adding 0.5 mol of solid sodium hydroxide to 1.0 L of 1.0 M acetic acid (CH3COOH) . What is the pH of the buffer?

Accepted Answer

A)   The pH will be pKa - 0.30, where pKa is that of acetic acid.
B)   The pH will be greater than the pKa for acetic acid.
C)   The pH will be less than the value in answer a.
D)   The pH will be equal to the pKa for acetic acid.
E)   More information is needed to solve the problem.F) A) and E)
G) B) and C)

Question 8

Calculate the solubility of copper(II) carbonate, CuCO3, in 1.00 mol L-1 NH3.
Ksp = 3.0 × 10-12 for CuCO3, Kf = 5.6 × 1011 for Cu(NH3)42+

Accepted Answer

Question 9

A 10.0-mL sample of 0.75 M CH3CH2COOH is titrated with 0.30 M NaOH. What is the pH of the solution after 22.0 mL of NaOH have been added to the acid? Ka = 1.3 × 10-5

Accepted Answer

A)   5.75
B)   4.94
C)   4.83
D)   4.02
E)   3.95F) B) and C)
G) A) and E)

Question 10

Use the following information to calculate the solubility product constant, Ksp, for CuCl. A saturated solution of CuCl in water was prepared and filtered. From the filtrate, 1.0 L was measured out into a beaker and evaporated to dryness. The solid CuCl residue recovered in the beaker was found to weigh 0.041g.

Accepted Answer

A)   Ksp =1.7 × 10-9
B)   Ksp = 1.7 × 10-7
C)   Ksp = 1.7 × 10-5
D)   Ksp = 4.3 × 10-4
E)   Ksp = 2.1 × 10-2F) B) and C)
G) A) and B)

Question 11

Buffer solutions with the component concentrations shown below were prepared. Which of them should have the highest pH?

Accepted Answer

A)   [H2PO4-] = 0.50 M, [HPO42-] = 0.50 M
B)   [H2PO4-] = 1.0 M, [HPO42-] = 1.0 M
C)   [H2PO4-] = 1.0 M, [HPO42-] = 0.50 M
D)   [H2PO4-] = 0.50 M, [HPO42-] = 1.0 M
E)   [H2PO4-] = 0.75 M, [HPO42-] = 1.0 MF) C) and E)
G) None of the above

Question 12

What is the maximum amount of sodium sulfate that can be added to 1.00 L of 0.0020 M Ca(NO3) 2 before precipitation of calcium sulfate begins? Ksp = 2.4 × 10-5 for calcium sulfate.

Accepted Answer

A)   1.2 × 10-2 mol
B)   4.9 × 10-3 mol
C)   3.5 × 10-3 mol
D)   1.2 × 10-5 mol
E)   4.8 × 10-8 molF) All of the above
G) B) and D)

Question 13

Write the ion product expression for magnesium fluoride, MgF2.

Accepted Answer

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G) All of the above

Question 14

The end point in a titration is defined as the point when the indicator changes color.

Accepted Answer

A) True 
 B)False

Question 15

Increasing the concentrations of the components of a buffer solution will increase the buffer range.

Accepted Answer

A) True 
 B)False

Question 16

Equal volumes of the following pairs of solutions are mixed. Which pair will produce a buffer solution?

Accepted Answer

A)   0.10 mol L-1 HCl and 0.05 mol L-1 NaOH
B)   0.10 mol L-1 HCl and 0.15 mol L-1 NH3
C)   0.10 mol L-1 HCl and 0.05 mol L-1 NH3
D)   0.10 mol L-1 HCl and 0.20 mol L-1 CH3COOH
E)   0.10 mol L-1 HCl and 0.20 mol L-1 NaClF) B) and D)
G) A) and B)

Question 17

What is the pH of a solution that consists of 0.50 M H2C6H6O6 (ascorbic acid)  and 0.75 M NaHC6H6O6 (sodium ascorbate) ? For ascorbic acid, Ka = 6.8 × 10-5

Accepted Answer

A)   3.76
B)   3.99
C)   4.34
D)   4.57
E)   5.66F) A) and C)
G) A) and E)

Question 18

A change in pH will significantly affect the solubility of which, if any, of the following compounds?

Accepted Answer

A)   BaF2
B)   CuCl
C)   CuBr
D)   AgI
E)   None of the solubilities will be significantly affected.F) C) and E)
G) A) and E)

Question 19

A popular buffer solution consists of carbonate (CO32-)  and hydrogen carbonate (HCO3-)  conjugate acid-base pair. Which, if any, of the following such buffers can neutralize the greatest amount of added hydrochloric acid, while remaining within its buffer range?

Accepted Answer

A)   1 L of 0.9 M CO32- and 0.1 M HCO3-
B)   1 L of 0.1 M CO32- and 0.9 M HCO3-
C)   1 L of 0.5 M CO32- and 0.5 M HCO3-
D)   1 L of 0.1 M CO32- and 0.1 M HCO3-
E)   They can all neutralize the same amount of hydrochloric acid.F) B) and D)
G) None of the above

Question 20

Hydrofluoric acid (HF) has a Ka value of 7.2 × 10-4.
a. 0.250 mol of F- ions (in the form of NaF) are added to 1.00 L of 0.100 mol L-1 aqueous HF. Calculate the resulting pH.
b. To the solution produced in (a) is added 10.0 mL of 5.00 mol L-1 NaOH. Calculate the resulting pH.

Accepted Answer

Exam 19: Ionic Equilibria in Aqueous Systems

A 10.0-mL sample of 0.75 M CH₃CH₂COOH is titrated with 0.30 M NaOH. What is the pH of the solution after 22.0 mL of NaOH have been added to the acid? K_a = 1.3 × 10^-5

Correct Answer
verified

Write the ion product expression for magnesium fluoride, MgF₂.

Correct Answer
verified

You need to prepare a buffer solution with a pH of 4.00, using NaF and HF. What ratio of the ratio of [base]/[acid] should be used in making the buffer? For HF, K_a = 7.2 × 10^{- 4}.

Correct Answer
verified

The end point in a titration is defined as the point when the indicator changes color.

Correct Answer
verified

Correct Answer
verified

What is the maximum amount of sodium sulfate that can be added to 1.00 L of 0.0020 M Ca(NO₃) ₂before precipitation of calcium sulfate begins? K_sp = 2.4 × 10^-5 for calcium sulfate.

Correct Answer
verified

Buffer solutions with the component concentrations shown below were prepared. Which of them should have the highest pH?

Correct Answer
verified

What mass of NaF must be added to 50.0 mL of a 0.500 M HF solution to achieve a pH of 3.25? For HF, K_a = 7.2 × 10^-4.

Correct Answer
verified

What is the [H₃O⁺] in a solution that consists of 0.15 M C₂N₂H₈(ethylene diamine) and 0.35 C₂N₂H₉Cl? K_b = 4.7 × 10^-4

Correct Answer
verified

Increasing the concentrations of the components of a buffer solution will increase the buffer range.

Correct Answer
verified

Hydrofluoric acid (HF) has a K_a value of 7.2 × 10^-4. a. 0.250 mol of F^- ions (in the form of NaF) are added to 1.00 L of 0.100 mol L^-1 aqueous HF. Calculate the resulting pH. b. To the solution produced in (a) is added 10.0 mL of 5.00 mol L^-1 NaOH. Calculate the resulting pH.

Correct Answer
verified

A popular buffer solution consists of carbonate (CO₃^2-) and hydrogen carbonate (HCO₃^-) conjugate acid-base pair. Which, if any, of the following such buffers can neutralize the greatest amount of added hydrochloric acid, while remaining within its buffer range?

Correct Answer
verified

A buffer is prepared by adding 0.5 mol of solid sodium hydroxide to 1.0 L of 1.0 M acetic acid (CH₃COOH) . What is the pH of the buffer?

Correct Answer
verified

Which one of the following is the best representation of the titration curve which will be obtained in the titration of a weak base (0.10 mol L^-1) with HCl of the same concentration?

Correct Answer
verified

What is the pH of a solution that consists of 0.50 M H₂C₆H₆O₆(ascorbic acid) and 0.75 M NaHC₆H₆O₆(sodium ascorbate) ? For ascorbic acid, K_a = 6.8 × 10^-5

Correct Answer
verified

Calculate the solubility of copper(II) carbonate, CuCO₃, in 1.00 mol L^-1 NH₃. K_sp = 3.0 × 10^-12 for CuCO₃, K_f = 5.6 × 10¹¹ for Cu(NH₃)₄²⁺

Correct Answer
verified

Correct Answer
verified

A change in pH will significantly affect the solubility of which, if any, of the following compounds?

Correct Answer
verified

Equal volumes of the following pairs of solutions are mixed. Which pair will produce a buffer solution?

Correct Answer
verified

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 = 1.7 × 10^-4

Correct Answer
verified

Exam 19: Ionic Equilibria in Aqueous Systems

A 10.0-mL sample of 0.75 M CH3CH2COOH is titrated with 0.30 M NaOH. What is the pH of the solution after 22.0 mL of NaOH have been added to the acid? Ka = 1.3 × 10-5

Correct AnswerverifiedShow Answer

Write the ion product expression for magnesium fluoride, MgF2.

Correct AnswerverifiedShow Answer

You need to prepare a buffer solution with a pH of 4.00, using NaF and HF. What ratio of the ratio of [base]/[acid] should be used in making the buffer? For HF, Ka = 7.2 × 10- 4.

Correct AnswerverifiedShow Answer

The end point in a titration is defined as the point when the indicator changes color.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

What is the maximum amount of sodium sulfate that can be added to 1.00 L of 0.0020 M Ca(NO3) 2 before precipitation of calcium sulfate begins? Ksp = 2.4 × 10-5 for calcium sulfate.

Correct AnswerverifiedShow Answer

Buffer solutions with the component concentrations shown below were prepared. Which of them should have the highest pH?

Correct AnswerverifiedShow Answer

What mass of NaF must be added to 50.0 mL of a 0.500 M HF solution to achieve a pH of 3.25? For HF, Ka = 7.2 × 10-4.

Correct AnswerverifiedShow Answer

What is the [H3O+] in a solution that consists of 0.15 M C2N2H8 (ethylene diamine) and 0.35 C2N2H9Cl? Kb = 4.7 × 10-4

Correct AnswerverifiedShow Answer

Increasing the concentrations of the components of a buffer solution will increase the buffer range.

Correct AnswerverifiedShow Answer

Hydrofluoric acid (HF) has a Ka value of 7.2 × 10-4. a. 0.250 mol of F- ions (in the form of NaF) are added to 1.00 L of 0.100 mol L-1 aqueous HF. Calculate the resulting pH. b. To the solution produced in (a) is added 10.0 mL of 5.00 mol L-1 NaOH. Calculate the resulting pH.

Correct AnswerverifiedShow Answer

A popular buffer solution consists of carbonate (CO32-) and hydrogen carbonate (HCO3-) conjugate acid-base pair. Which, if any, of the following such buffers can neutralize the greatest amount of added hydrochloric acid, while remaining within its buffer range?

Correct AnswerverifiedShow Answer

A buffer is prepared by adding 0.5 mol of solid sodium hydroxide to 1.0 L of 1.0 M acetic acid (CH3COOH) . What is the pH of the buffer?

Correct AnswerverifiedShow Answer

Which one of the following is the best representation of the titration curve which will be obtained in the titration of a weak base (0.10 mol L-1) with HCl of the same concentration?

Correct AnswerverifiedShow Answer

What is the pH of a solution that consists of 0.50 M H2C6H6O6 (ascorbic acid) and 0.75 M NaHC6H6O6 (sodium ascorbate) ? For ascorbic acid, Ka = 6.8 × 10-5

Correct AnswerverifiedShow Answer

Calculate the solubility of copper(II) carbonate, CuCO3, in 1.00 mol L-1 NH3. Ksp = 3.0 × 10-12 for CuCO3, Kf = 5.6 × 1011 for Cu(NH3)42+

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

A change in pH will significantly affect the solubility of which, if any, of the following compounds?

Correct AnswerverifiedShow Answer

Equal volumes of the following pairs of solutions are mixed. Which pair will produce a buffer solution?

Correct AnswerverifiedShow Answer

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 = 1.7 × 10-4

Correct AnswerverifiedShow Answer

A 10.0-mL sample of 0.75 M CH₃CH₂COOH is titrated with 0.30 M NaOH. What is the pH of the solution after 22.0 mL of NaOH have been added to the acid? K_a = 1.3 × 10^-5

Correct Answer
verified

Write the ion product expression for magnesium fluoride, MgF₂.

Correct Answer
verified

You need to prepare a buffer solution with a pH of 4.00, using NaF and HF. What ratio of the ratio of [base]/[acid] should be used in making the buffer? For HF, K_a = 7.2 × 10^{- 4}.

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

What is the maximum amount of sodium sulfate that can be added to 1.00 L of 0.0020 M Ca(NO₃) ₂before precipitation of calcium sulfate begins? K_sp = 2.4 × 10^-5 for calcium sulfate.

Correct Answer
verified

Correct Answer
verified

What mass of NaF must be added to 50.0 mL of a 0.500 M HF solution to achieve a pH of 3.25? For HF, K_a = 7.2 × 10^-4.

Correct Answer
verified

What is the [H₃O⁺] in a solution that consists of 0.15 M C₂N₂H₈(ethylene diamine) and 0.35 C₂N₂H₉Cl? K_b = 4.7 × 10^-4

Correct Answer
verified

Correct Answer
verified

Hydrofluoric acid (HF) has a K_a value of 7.2 × 10^-4. a. 0.250 mol of F^- ions (in the form of NaF) are added to 1.00 L of 0.100 mol L^-1 aqueous HF. Calculate the resulting pH. b. To the solution produced in (a) is added 10.0 mL of 5.00 mol L^-1 NaOH. Calculate the resulting pH.

Correct Answer
verified

A popular buffer solution consists of carbonate (CO₃^2-) and hydrogen carbonate (HCO₃^-) conjugate acid-base pair. Which, if any, of the following such buffers can neutralize the greatest amount of added hydrochloric acid, while remaining within its buffer range?

Correct Answer
verified

A buffer is prepared by adding 0.5 mol of solid sodium hydroxide to 1.0 L of 1.0 M acetic acid (CH₃COOH) . What is the pH of the buffer?

Correct Answer
verified

Which one of the following is the best representation of the titration curve which will be obtained in the titration of a weak base (0.10 mol L^-1) with HCl of the same concentration?

Correct Answer
verified

What is the pH of a solution that consists of 0.50 M H₂C₆H₆O₆(ascorbic acid) and 0.75 M NaHC₆H₆O₆(sodium ascorbate) ? For ascorbic acid, K_a = 6.8 × 10^-5

Correct Answer
verified

Calculate the solubility of copper(II) carbonate, CuCO₃, in 1.00 mol L^-1 NH₃. K_sp = 3.0 × 10^-12 for CuCO₃, K_f = 5.6 × 10¹¹ for Cu(NH₃)₄²⁺

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

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 = 1.7 × 10^-4

Correct Answer
verified