Question 1

The solubility of silver chloride _______________ 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) D) and E)
G) A) and E)

Question 2

When 0.300 g of a diprotic acid was titrated with 0.100 M LiOH, 40.0 mL of the LiOH solution was needed to reach the second equivalence point. Identify the formula of the diprotic acid.

Accepted Answer

A)   H2S
B)   H2C2O4
C)   H2C4H4O6
D)   H2Se
E)   H2TeF) C) and D)
G) B) and E)

Question 3

You need to use KH2PO4 and K2HPO4 to prepare a buffer with a pH of 7.45. Which of the following ratios of [base]/[acid] is required? For phosphoric acid, (H3PO4) , Ka2 = 6.2 × 10-8.

Accepted Answer

A)   [base]/[acid] = 1.75
B)   [base]/[acid] = 1.27
C)   [base]/[acid] = 1.24
D)   [base]/[acid] = 0.79
E)   [base]/[acid] = 0.57F) A) and B)
G) B) and C)

Question 4

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) C) and E)
G) A) and E)

Question 5

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) B) and E)
G) All of the above

Question 6

Calculate the solubility of lead(II)  iodide, PbI2, in 0.025 M KI. Ksp = 7.9 × 10-9

Accepted Answer

A)   4.5 × 10-2 M
B)   2.8 × 10-2 M
C)   8.9 × 10-5 M
D)   5.0 × 10-5 M
E)   1.3 × 10-5 MF) All of the above
G) A) and C)

Question 7

Which of the following substances has the greatest solubility in water?

Accepted Answer

A)   Ba(IO3) 2, Ksp = 1.5 × 10-9
B)   PbF2, Ksp = 3.6 × 10-8
C)   SrSO4, Ksp = 3.2 × 10-7
D)   CuCl, Ksp = 1.9 × 10-7
E)   CdS, Ksp = 1.0 × 10-24F) B) and D)
G) A) and E)

Question 8

A buffer is prepared by adding 300.0 mL of 2.0 M NaOH to 500.0 mL of 2.0 M CH3COOH. What is the pH of this buffer? Ka = 1.8 × 10-5

Accepted Answer

A)   4.57
B)   4.52
C)   4.87
D)   4.92
E)   4.97F) A) and C)
G) B) and E)

Question 9

A phosphate buffer (H2PO4-/HPO42-)  has a pH of 8.3. Which of the following changes will cause the pH to increase?

Accepted Answer

A)   dissolving a small amount of Na2HPO4
B)   dissolving a small amount of NaH2PO4
C)   adding a small amount of dilute hydrochloric acid
D)   adding a small amount of dilute phosphoric acid
E)   making the buffer more concentrated by removing some waterF) B) and C)
G) A) and E)

Question 10

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) A) and E)

Question 11

The solubility of lead(II)  chloride is 0.45 g/100 mL of solution. What is the Ksp of PbCl2?

Accepted Answer

A)   4.9 × 10-2
B)   1.7 × 10-5
C)   8.5 × 10-6
D)   4.2 × 10-6
E)   -6F) All of the above
G) B) and E)

Question 12

A buffer is to be prepared by adding solid sodium acetate to 0.10 M CH3COOH. Which of the following concentrations of sodium acetate will produce the most effective buffer?

Accepted Answer

A)   3.0 M CH3COONa
B)   2.5 M CH3COONa
C)   2.0 M CH3COONa
D)   1.5 M CH3COONa
E)   0.30 M CH3COONaF) All of the above
G) A) and E)

Question 13

At the equivalence point in an acid-base titration

Accepted Answer

A)   the [H3O+] equals the Ka of the acid.
B)   the [H3O+] equals the Ka of the indicator.
C)   the amounts of acid and base which have been combined are in their stoichiometric ratio.
D)   the pH is 7.0.
E)   the pH has reached a maximum.F) B) and E)
G) C) and D)

Question 14

Write the ion product expression for magnesium fluoride, MgF2.

Accepted Answer

A)   2. 
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G) C) and E)

Question 15

If 10.0 g of NaF and 20.0 g of HF are dissolved in water to make one liter of solution, what will the pH be? For HF, Ka = 6.8 × 10-4.

Accepted Answer

A)   7.13
B)   2.54
C)   1.57
D)   3.17
E)   4.86F) A) and C)
G) B) and E)

Question 16

The indicator propyl red has Ka = 3.3 × 10-6. What would be the approximate pH range over which it would change color?

Accepted Answer

A)   3.5-5.5
B)   4.5-6.5
C)   5.5-7.5
D)   6.5-8.5
E)   None of these choices are correct.F) C) and E)
G) B) and E)

Question 17

The salts X(NO3) 2 and Y(NO3) 2 (where X+ and Y+ are metal ions)  are dissolved in water to give a solution which is 0.1 M in each of them. Using the Ksp values listed below, decide which aqueous reagent, if any, will definitely precipitate X+ before precipitating Y+ from solution. Given Ksp values:
XCl2, 1 × 10-5 YCl2, 1 × 10-10 X(OH) 2, 1 × 10-10 Y(OH) 2, 1 × 10-5

Accepted Answer

A)   1 M NaNO3
B)   1 M HCl
C)   1 M HNO3
D)   1 M NaCl
E)   None of these choices are correct.F) All of the above
G) A) and E)

Question 18

When 20.0 mL of 0.15 M hydrochloric acid is mixed with 20.0 mL of 0.10 M sodium hydroxide, the pH of the resulting solution is

Accepted Answer

A)   0.00.
B)   12.40.
C)   1.60.
D)   0.82.
E)   7.00.F) B) and E)
G) B) and D)

Question 19

When a weak acid is titrated with a weak base, the pH at the equivalence point

Accepted Answer

A)   is greater than 7.0.
B)   is equal to 7.0.
C)   is less than 7.0.
D)   is determined by the sizes of Ka and Kb.
E)   is no longer affected by addition of base.F) D) and E)
G) B) and E)

Question 20

The salts X(NO3) 2 and Y(NO3) 2 (where X+ and Y+ are metal ions)  are dissolved in water to give a solution which is 0.1 M in each of them. Which of the answers gives the concentration of chloride ions will precipitate the most YCl2 without precipitating any XCl2? Given Ksp values: XCl2, 2 × 10-5 YCl2, 1 × 10-10

Accepted Answer

A)   1 M Cl-
B)   0.1 M Cl-
C)   0.01 M Cl-
D)   0.001 M Cl-
E)   0.0001 M Cl-F) B) and D)
G) C) and D)

Exam 19: Ionic Equilibria in Aqueous Systems

A buffer is to be prepared by adding solid sodium acetate to 0.10 M CH₃COOH. Which of the following concentrations of sodium acetate will produce the most effective buffer?

Correct Answer
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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
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When 20.0 mL of 0.15 M hydrochloric acid is mixed with 20.0 mL of 0.10 M sodium hydroxide, the pH of the resulting solution is

Correct Answer
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When a weak acid is titrated with a weak base, the pH at the equivalence point

Correct Answer
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The solubility of silver chloride _______________ when dilute nitric acid is added to it.

Correct Answer
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Calculate the solubility of lead(II) iodide, PbI₂, in 0.025 M KI. K_sp = 7.9 × 10^-9

Correct Answer
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A buffer is prepared by adding 300.0 mL of 2.0 M NaOH to 500.0 mL of 2.0 M CH₃COOH. What is the pH of this buffer? K_a = 1.8 × 10^-5

Correct Answer
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At the equivalence point in an acid-base titration

Correct Answer
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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
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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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If 10.0 g of NaF and 20.0 g of HF are dissolved in water to make one liter of solution, what will the pH be? For HF, K_a = 6.8 × 10^-4.

Correct Answer
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Write the ion product expression for magnesium fluoride, MgF₂.

Correct Answer
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You need to use KH₂PO₄ and K₂HPO₄ to prepare a buffer with a pH of 7.45. Which of the following ratios of [base]/[acid] is required? For phosphoric acid, (H₃PO₄) , K_a2 = 6.2 × 10^-8.

Correct Answer
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The solubility of lead(II) chloride is 0.45 g/100 mL of solution. What is the K_sp of PbCl₂?

Correct Answer
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The indicator propyl red has K_a = 3.3 × 10^-6. What would be the approximate pH range over which it would change color?

Correct Answer
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Correct Answer
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A phosphate buffer (H₂PO₄^-/HPO₄^2-) has a pH of 8.3. Which of the following changes will cause the pH to increase?

Correct Answer
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When 0.300 g of a diprotic acid was titrated with 0.100 M LiOH, 40.0 mL of the LiOH solution was needed to reach the second equivalence point. Identify the formula of the diprotic acid.

Correct Answer
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Which of the following substances has the greatest solubility in water?

Correct Answer
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Exam 19: Ionic Equilibria in Aqueous Systems

A buffer is to be prepared by adding solid sodium acetate to 0.10 M CH3COOH. Which of the following concentrations of sodium acetate will produce the most effective buffer?

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

When 20.0 mL of 0.15 M hydrochloric acid is mixed with 20.0 mL of 0.10 M sodium hydroxide, the pH of the resulting solution is

Correct AnswerverifiedShow Answer

When a weak acid is titrated with a weak base, the pH at the equivalence point

Correct AnswerverifiedShow Answer

The solubility of silver chloride _______________ when dilute nitric acid is added to it.

Correct AnswerverifiedShow Answer

Calculate the solubility of lead(II) iodide, PbI2, in 0.025 M KI. Ksp = 7.9 × 10-9

Correct AnswerverifiedShow Answer

A buffer is prepared by adding 300.0 mL of 2.0 M NaOH to 500.0 mL of 2.0 M CH3COOH. What is the pH of this buffer? Ka = 1.8 × 10-5

Correct AnswerverifiedShow Answer

At the equivalence point in an acid-base titration

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

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

If 10.0 g of NaF and 20.0 g of HF are dissolved in water to make one liter of solution, what will the pH be? For HF, Ka = 6.8 × 10-4.

Correct AnswerverifiedShow Answer

Write the ion product expression for magnesium fluoride, MgF2.

Correct AnswerverifiedShow Answer

You need to use KH2PO4 and K2HPO4 to prepare a buffer with a pH of 7.45. Which of the following ratios of [base]/[acid] is required? For phosphoric acid, (H3PO4) , Ka2 = 6.2 × 10-8.

Correct AnswerverifiedShow Answer

The solubility of lead(II) chloride is 0.45 g/100 mL of solution. What is the Ksp of PbCl2?

Correct AnswerverifiedShow Answer

The indicator propyl red has Ka = 3.3 × 10-6. What would be the approximate pH range over which it would change color?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

A phosphate buffer (H2PO4-/HPO42-) has a pH of 8.3. Which of the following changes will cause the pH to increase?

Correct AnswerverifiedShow Answer

When 0.300 g of a diprotic acid was titrated with 0.100 M LiOH, 40.0 mL of the LiOH solution was needed to reach the second equivalence point. Identify the formula of the diprotic acid.

Correct AnswerverifiedShow Answer

Which of the following substances has the greatest solubility in water?

Correct AnswerverifiedShow Answer

A buffer is to be prepared by adding solid sodium acetate to 0.10 M CH₃COOH. Which of the following concentrations of sodium acetate will produce the most effective buffer?

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
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Correct Answer
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Correct Answer
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Correct Answer
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Calculate the solubility of lead(II) iodide, PbI₂, in 0.025 M KI. K_sp = 7.9 × 10^-9

Correct Answer
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A buffer is prepared by adding 300.0 mL of 2.0 M NaOH to 500.0 mL of 2.0 M CH₃COOH. What is the pH of this buffer? K_a = 1.8 × 10^-5

Correct Answer
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Correct Answer
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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
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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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If 10.0 g of NaF and 20.0 g of HF are dissolved in water to make one liter of solution, what will the pH be? For HF, K_a = 6.8 × 10^-4.

Correct Answer
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Write the ion product expression for magnesium fluoride, MgF₂.

Correct Answer
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You need to use KH₂PO₄ and K₂HPO₄ to prepare a buffer with a pH of 7.45. Which of the following ratios of [base]/[acid] is required? For phosphoric acid, (H₃PO₄) , K_a2 = 6.2 × 10^-8.

Correct Answer
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The solubility of lead(II) chloride is 0.45 g/100 mL of solution. What is the K_sp of PbCl₂?

Correct Answer
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The indicator propyl red has K_a = 3.3 × 10^-6. What would be the approximate pH range over which it would change color?

Correct Answer
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Correct Answer
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A phosphate buffer (H₂PO₄^-/HPO₄^2-) has a pH of 8.3. Which of the following changes will cause the pH to increase?

Correct Answer
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Correct Answer
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Correct Answer
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