Question 1

Citric acid has an acid dissociation constant of 8.4 *10¯4. It would be most effective for preparation of a buffer with a pH of:

Accepted Answer

A)   2
B)   3
C)   4
D)   5
E)   6F) B) and E)
G) None of the above

Question 2

A solution is prepared by adding 500 mL of 0.3 M NaClO to 500 mL of 0.4 M HClO. What is the pH of this solution?

Accepted Answer

A)   The pH will be greater than the pKa of hypochlorous acid.
B)   The pH will be less than the pKa of hypochlorous acid.
C)   The pH will be equal to the pKa of hypochlorous acid.
D)   The pH will equal the pKb of sodium hypochlorite.
E)   None of these choices is correct.F) C) and D)
G) A) and D)

Question 3

The solubility of aluminum hydroxide in water ______________ when dilute nitric acid is added to it.

Accepted Answer

A)   increases
B)   decreases
C)   does not change
D)   first increases, then decreases
E)   first decreases, then increasesF) A) and B)
G) C) and D)

Question 4

The concentration of the complex ion in each of following solutions is 1.00 M. In which of the solutions will the concentration of the uncomplexed metal ion be the greatest? 2+ B)  Be2+ C)  Zn2+ D)  Cu2+ E)  Cd2+" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   Hg2+
B)   Be2+
C)   Zn2+
D)   Cu2+
E)   Cd2+F) B) and D)
G) B) and E)

Question 5

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

Accepted Answer

A) True 
 B)False

Question 6

Calculate the solubility of zinc hydroxide, Zn(OH) 2, in 1.00 M NaOH. 2, in 1.00 M NaOH.   A)  0.60 M B)  0.52 M C)  0.37 M D)  0.32 M E)  0.24 M" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   0.60 M
B)   0.52 M
C)   0.37 M
D)   0.32 M
E)   0.24 MF) B) and E)
G) C) and D)

Question 7

A 50.0-mL sample of 0.50 M HCl is titrated with 0.50 M NaOH. What is the pH of the solution after 28.0 mL of NaOH have been added to the acid?

Accepted Answer

A)   0.85
B)   0.75
C)   0.66
D)   0.49
E)   3.8F) A) and B)
G) C) and D)

Question 8

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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B)     
C)     
D)     
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B)   1)  with HCl of the same concentration? 
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B)     
C)     
D)     
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C)   1)  with HCl of the same concentration? 
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D)     
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D)   1)  with HCl of the same concentration? 
A)     
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D)     
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E)   1)  with HCl of the same concentration? 
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D)     
E)    " class="answers-bank-image d-inline" rel="preload" >F) A) and B)
G) A) and C)

Question 9

The solubility of silver chromate is 0.0287 g/1.0 L of solution. What is the Ksp for Ag2CrO4?

Accepted Answer

A)   9.5 * 10¯5
B)   2.4 * 10¯5
C)   2.6 * 10¯12
D)   6.5 * 10¯13
E)   13F) A) and B)
G) All of the above

Question 10

An acetate buffer has a pH of 4.40. Which of the following changes will cause the pH to decrease?

Accepted Answer

A)   dissolving a small amount of solid sodium acetate
B)   adding a small amount of dilute hydrochloric acid
C)   adding a small amount of dilute sodium hydroxide
D)   dissolving a small amount of solid sodium chloride
E)   diluting the buffer solution with waterF) A) and B)
G) C) and E)

Question 11

What is the pH of a buffer that consists of 0.20 M NaH2PO4 and 0.40 M Na2HPO4? For NaH2PO4, Ka = 6.2*10¯8

Accepted Answer

A)   6.51
B)   6.91
C)   7.51
D)   7.90
E)   8.13F) A) and B)
G) B) and E)

Question 12

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) All of the above
G) A) and D)

Question 13

A 25.0-mL sample of 0.35 M HCOOH is titrated with 0.20 M KOH. What is the pH of the solution after 25.0 mL of KOH has been added to the acid? Ka = 1.77 * 10¯4

Accepted Answer

A)   4.00
B)   3.88
C)   3.63
D)   3.51
E)   3.47F) All of the above
G) A) and B)

Question 14

A buffer is prepared by adding 100 mL of 0.50 M sodium hydroxide to 100 mL of 0.75 M propanoic acid. Is this a buffer solution, and if so, what is its pH?

Accepted Answer

A)   It is a buffer, pH > pKa of propanoic acid.
B)   It is a buffer, pH a of propanoic acid.
C)   It is a buffer, pH = pKa of propanoic acid.
D)   It is a buffer, pH = pKb of sodium propanoate.
E)   Since sodium hydroxide is a strong base, this is not a buffer.F) A) and B)
G) A) and C)

Question 15

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

Accepted Answer

A) True 
 B)False

Question 16

Calculate the solubility of magnesium sulfate, MgSO4, when placed into a 0.10 M MgCl2 solution. Ksp = 5.9 *10¯3

Accepted Answer

A)   4.2 * 10¯2 M
B)   5.9 *10¯2 M
C)   7.7 *10¯2 M
D)   3.5 * 10¯5 M
E)   3.5 * 10¯6 MF) A) and D)
G) None of the above

Question 17

What is the [H3O+] in a buffer that consists of 0.30 M HCOOH and 0.20 M HCOONa? For HCOOH, Ka = 1.7 * 10¯4

Accepted Answer

A)   1.1 * 10¯4 M
B)   2.6 *10¯4 M
C)   4.3* 10¯4 M
D)   6.7 *10¯5 M
E)   None of these choices is correct.F) A) and E)
G) A) and D)

Question 18

What will be the effect of adding 0.5 mL of 0.1 M NaOH to 100 mL of an acetate buffer in which [CH3COOH] = [CH3COO¯] = 0.5 M?

Accepted Answer

A)   The pH will increase slightly.
B)   The pH will increase significantly.
C)   The pH will decrease slightly.
D)   The pH will decrease significantly.
E)   Since it is a buffer solution, the pH will not be affected.F) C) and D)
G) C) and E)

Question 19

What volume of 0.500 M H2SO4 is needed to react completely with 20.0 mL of 0.400 M LiOH?

Accepted Answer

A)   4.00 mL
B)   8.00 mL
C)   12.5 mL
D)   16.0 mL
E)   32.0 mLF) D) and E)
G) None of the above

Question 20

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 E)
G) B) and D)

Exam 19: Ionic Equilibria in Aqueous Systems

An acetate buffer has a pH of 4.40. Which of the following changes will cause the pH to decrease?

Correct Answer
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The solubility of aluminum hydroxide in water ______________ when dilute nitric acid is added to it.

Correct Answer
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What is the [H₃O⁺] in a buffer that consists of 0.30 M HCOOH and 0.20 M HCOONa? For HCOOH, K_a = 1.7 * 10¯⁴

Correct Answer
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What will be the effect of adding 0.5 mL of 0.1 M NaOH to 100 mL of an acetate buffer in which [CH₃COOH] = [CH₃COO¯] = 0.5 M?

Correct Answer
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What volume of 0.500 M H₂SO₄ is needed to react completely with 20.0 mL of 0.400 M LiOH?

Correct Answer
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Calculate the solubility of magnesium sulfate, MgSO₄, when placed into a 0.10 M MgCl₂ solution. K_sp = 5.9 *10¯³

Correct Answer
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The concentration of the complex ion in each of following solutions is 1.00 M. In which of the solutions will the concentration of the uncomplexed metal ion be the greatest?

Correct Answer
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A buffer is prepared by adding 100 mL of 0.50 M sodium hydroxide to 100 mL of 0.75 M propanoic acid. Is this a buffer solution, and if so, what is its pH?

Correct Answer
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What is the pH of a buffer that consists of 0.20 M NaH₂PO₄ and 0.40 M Na₂HPO₄? For NaH₂PO₄, K_a = 6.2*10¯⁸

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

Correct Answer
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The solubility of silver chromate is 0.0287 g/1.0 L of solution. What is the K_sp for Ag₂CrO₄?

Correct Answer
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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
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A solution is prepared by adding 500 mL of 0.3 M NaClO to 500 mL of 0.4 M HClO. What is the pH of this solution?

Correct Answer
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Citric acid has an acid dissociation constant of 8.4 *10¯⁴. It would be most effective for preparation of a buffer with a pH of:

Correct Answer
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A 25.0-mL sample of 0.35 M HCOOH is titrated with 0.20 M KOH. What is the pH of the solution after 25.0 mL of KOH has been added to the acid? K_a = 1.77 * 10¯⁴

Correct Answer
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Correct Answer
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Increasing the concentrations of the components of a buffer solution will increase the buffer capacity.

Correct Answer
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Calculate the solubility of zinc hydroxide, Zn(OH) ₂, in 1.00 M NaOH.

Correct Answer
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A 50.0-mL sample of 0.50 M HCl is titrated with 0.50 M NaOH. What is the pH of the solution after 28.0 mL of NaOH have been added to the acid?

Correct Answer
verified

Exam 19: Ionic Equilibria in Aqueous Systems

An acetate buffer has a pH of 4.40. Which of the following changes will cause the pH to decrease?

Correct AnswerverifiedShow Answer

The solubility of aluminum hydroxide in water ______________ when dilute nitric acid is added to it.

Correct AnswerverifiedShow Answer

What is the [H3O+] in a buffer that consists of 0.30 M HCOOH and 0.20 M HCOONa? For HCOOH, Ka = 1.7 * 10¯4

Correct AnswerverifiedShow Answer

What will be the effect of adding 0.5 mL of 0.1 M NaOH to 100 mL of an acetate buffer in which [CH3COOH] = [CH3COO¯] = 0.5 M?

Correct AnswerverifiedShow Answer

What volume of 0.500 M H2SO4 is needed to react completely with 20.0 mL of 0.400 M LiOH?

Correct AnswerverifiedShow Answer

Calculate the solubility of magnesium sulfate, MgSO4, when placed into a 0.10 M MgCl2 solution. Ksp = 5.9 *10¯3

Correct AnswerverifiedShow Answer

The concentration of the complex ion in each of following solutions is 1.00 M. In which of the solutions will the concentration of the uncomplexed metal ion be the greatest?

Correct AnswerverifiedShow Answer

A buffer is prepared by adding 100 mL of 0.50 M sodium hydroxide to 100 mL of 0.75 M propanoic acid. Is this a buffer solution, and if so, what is its pH?

Correct AnswerverifiedShow Answer

What is the pH of a buffer that consists of 0.20 M NaH2PO4 and 0.40 M Na2HPO4? For NaH2PO4, Ka = 6.2*10¯8

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

The solubility of silver chromate is 0.0287 g/1.0 L of solution. What is the Ksp for Ag2CrO4?

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

A solution is prepared by adding 500 mL of 0.3 M NaClO to 500 mL of 0.4 M HClO. What is the pH of this solution?

Correct AnswerverifiedShow Answer

Citric acid has an acid dissociation constant of 8.4 *10¯4. It would be most effective for preparation of a buffer with a pH of:

Correct AnswerverifiedShow Answer

A 25.0-mL sample of 0.35 M HCOOH is titrated with 0.20 M KOH. What is the pH of the solution after 25.0 mL of KOH has been added to the acid? Ka = 1.77 * 10¯4

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Calculate the solubility of zinc hydroxide, Zn(OH) 2, in 1.00 M NaOH.

Correct AnswerverifiedShow Answer

A 50.0-mL sample of 0.50 M HCl is titrated with 0.50 M NaOH. What is the pH of the solution after 28.0 mL of NaOH have been added to the acid?

Correct AnswerverifiedShow Answer

Correct Answer
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Correct Answer
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What is the [H₃O⁺] in a buffer that consists of 0.30 M HCOOH and 0.20 M HCOONa? For HCOOH, K_a = 1.7 * 10¯⁴

Correct Answer
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What will be the effect of adding 0.5 mL of 0.1 M NaOH to 100 mL of an acetate buffer in which [CH₃COOH] = [CH₃COO¯] = 0.5 M?

Correct Answer
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What volume of 0.500 M H₂SO₄ is needed to react completely with 20.0 mL of 0.400 M LiOH?

Correct Answer
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Calculate the solubility of magnesium sulfate, MgSO₄, when placed into a 0.10 M MgCl₂ solution. K_sp = 5.9 *10¯³

Correct Answer
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Correct Answer
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Correct Answer
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What is the pH of a buffer that consists of 0.20 M NaH₂PO₄ and 0.40 M Na₂HPO₄? For NaH₂PO₄, K_a = 6.2*10¯⁸

Correct Answer
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Correct Answer
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Correct Answer
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The solubility of silver chromate is 0.0287 g/1.0 L of solution. What is the K_sp for Ag₂CrO₄?

Correct Answer
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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

Correct Answer
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Citric acid has an acid dissociation constant of 8.4 *10¯⁴. It would be most effective for preparation of a buffer with a pH of:

Correct Answer
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A 25.0-mL sample of 0.35 M HCOOH is titrated with 0.20 M KOH. What is the pH of the solution after 25.0 mL of KOH has been added to the acid? K_a = 1.77 * 10¯⁴

Correct Answer
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Correct Answer
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Correct Answer
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Calculate the solubility of zinc hydroxide, Zn(OH) ₂, in 1.00 M NaOH.

Correct Answer
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Correct Answer
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