Question 1

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

A)   10.1
B)   10.3
C)   10.5
D)   10.7
E)   None of the AboveF) C) and E)
G) All of the above

Question 2

What volume of 0.0500 M sodium hydroxide should be added to 250. mL of 0.100 M HCOOH? to obtain a solution with a pH of 4.50 [Ka(HCOOH)  = 1.7 * 10-4]

Accepted Answer

A)   540 mL
B)   420 mL
C)   80. mL
D)   340 mL
E)   500. mLF) A) and D)
G) D) and E)

Question 3

25.0 mL of a 0.100 M solution of NH3 is titrated with 0.150M HCl. After 10.0 mL of the HCl has been added, the resultant solution is:

Accepted Answer

A)   Basic and before the equivalence point
B)   Basic and after the equivalence point
C)   Acidic and before the equivalence point
D)   Acidic and after the equivalence point
E)   Neutral and at the equivalence pointF) B) and D)
G) A) and D)

Question 4

A precipitate of AgCl will form when 0.050 mol NaCl(s) and 0.050 mol AgNO3(s) are dissolved in 500. mL of 3.0 M NH3. [Kf for Ag(NH3)2+ is 1.5 * 107; Ksp(AgCl) = 1.6 * 10-10]

Accepted Answer

A) True 
 B)False

Question 5

An environmental chemist obtained a 200. mL sample of lake water believed to be contaminated with a single monoprotic strong acid. Titrating this sample with a 0.0050 M NaOH(aq)  required 7.3 mL of the NaOH solution to reach the endpoint. What is the concentration of H+ in the lake

Accepted Answer

A)   1.8 * 10-4 M
B)   2.0 * 10-4 M
C)   2.2 * 10-4 M
D)   2.4 * 10-4 M
E)   None of the aboveF) All of the above
G) A) and E)

Question 6

The Ksp for silver(I)  phosphate is 1.8 * 10-18. Calculate the molar solubility of silver(I)  phosphate.

Accepted Answer

A)   1.6 * 10-5 M
B)   2.1 * 10-5 M
C)   3.7 * 10-5 M
D)   7.2 * 10-1 M
E)   1.8 * 10-1 MF) B) and C)
G) A) and C)

Question 7

To 1.00 L of a 0.100 M aqueous solution of benzoic acid (C6H5COOH)  is added 1.00 mL of 12.0 M HCl. What is the percentage ionization of the benzoic acid in the resulting solution [Ka(C6H5COOH)  = 6.5 * 10-5]

Accepted Answer

A)   3.3%
B)   12%
C)   1.3%
D)   0.52%
E)   0.065%F) A) and B)
G) C) and E)

Question 8

Calculate the silver ion concentration in a saturated solution of silver(I)  carbonate (Ksp = 8.1 *10-12) .

Accepted Answer

A)   5.0 * 10-5 M
B)   2.5 * 10-4 M
C)   1.3 * 10-4 M
D)   2.0 * 10-4 M
E)   8.1 * 10-4 MF) A) and E)
G) C) and E)

Question 9

Calculate the pH of a solution that is 0.20M NH3(aq)  and 0.35 M NH4Cl(aq) .(Kb(NH3)  = 1.8 x 10-5)

Accepted Answer

A)   9.01
B)   9.21
C)   9.41
D)   9.61
E)   None of the AboveF) B) and E)
G) A) and E)

Question 10

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 1.0 M HCl
C)   0.1 M CH3COOH plus 0.1 M CH3COONa
D)   0.1 M CH3COOH plus 0.2 M CH3COONaE) A) and B)
F) B) and D)

Question 11

The pH of a solution that is 0.20 M CH3COOH and 0.20 M CH3COONa should be higher than the pH of a 0.20 M CH3COOH solution.

Accepted Answer

A) True 
 B)False

Question 12

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

Accepted Answer

A) True 
 B)False

Question 13

Calculate the molar solubility of lead (II)  fluoride. (Ksp (PbF2 = 4.1 x 10-8) )

Accepted Answer

A)   1.6 x 10-3 M
B)   1.8 x 10-3 M
C)   2.0 x 10-3 M
D)   2.2 x 10-3 M
E)   None of the aboveF) B) and E)
G) A) and B)

Question 14

Calculate the concentration of fluoride ions in a saturated barium fluoride (Ksp = 1.7 * 10-6)  solution.

Accepted Answer

A)   7.6 * 10-3 M
B)   1.5 * 10-2 M
C)   3.4 * 10-5 M
D)   1.7 * 10-6 M
E)   3.4 * 10-6 MF) None of the above
G) A) and E)

Question 15

Calculate the equilibrium constant Kc for the following overall reaction: AgCl(s)  + 2CN-(aq)   ⇋\leftrightharpoons⇋  Ag(CN) 2-(aq)  + Cl-(aq) 
For AgCl, Ksp = 1.6 * 10-10; for Ag(CN) 2-, Kf = 1.0 * 1021.

Accepted Answer

A)   1.2 * 1011
B)   1.4 * 1011
C)   1.6 * 1011
D)   1.8 * 1011
E)   None of the above F) A) and B)
G) A) and D)

Question 16

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 CH3COONaF) A) and D)
G) D) and E)

Question 17

5.0 mL of 12 M NH3 is added to 500. mL of 0.050 M AgNO3. What concentration of silver ion will exist after equilibrium is established [Kf for Ag(NH3) 2+ is 1.5 * 107.]

Accepted Answer

A)   8.2 * 10-6 M
B)   8.4 * 10-6 M
C)   8.6 * 10-6 M
D)   8.8 * 10-6 M
E)   None of the aboveF) A) and E)
G) A) and D)

Question 18

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) C) and D)
G) D) and E)

Question 19

340. mL of a 0.150 M solution of NH3(aq)  is titrated with 0.100 M HCl. Calculate the pH of the solution after 350. mL of HCl has been added. (Ka(NH4+)  = 5.6 x 10-10)

Accepted Answer

A)   8.71
B)   8.91
C)   9.11
D)   9.31
E)   None of the aboveF) A) and D)
G) D) and E)

Question 20

Which of the following compounds is more soluble in a 0.10 M NH3(aq)  solution than in pure neutral water

Accepted Answer

A)   CaF2
B)   MgCO3
C)   AgI
D)   SrSO4
E)   Ba(NO3) 2F) A) and B)
G) All of the above

Exam 16: Acid-Base Equilibria and Solubility Equilibria

5.0 mL of 12 M NH3 is added to 500. mL of 0.050 M AgNO3. What concentration of silver ion will exist after equilibrium is established [Kf for Ag(NH3) 2+ is 1.5 * 107.]

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To 1.00 L of a 0.100 M aqueous solution of benzoic acid (C6H5COOH) is added 1.00 mL of 12.0 M HCl. What is the percentage ionization of the benzoic acid in the resulting solution [Ka(C6H5COOH) = 6.5 * 10-5]

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Calculate the equilibrium constant Kc for the following overall reaction: AgCl(s) + 2CN-(aq) ⇋\leftrightharpoons⇋ Ag(CN) 2-(aq) + Cl-(aq) For AgCl, Ksp = 1.6 * 10-10; for Ag(CN) 2-, Kf = 1.0 * 1021.

Correct AnswerverifiedShow Answer

What volume of 0.0500 M sodium hydroxide should be added to 250. mL of 0.100 M HCOOH? to obtain a solution with a pH of 4.50 [Ka(HCOOH) = 1.7 * 10-4]

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340. mL of a 0.150 M solution of NH3(aq) is titrated with 0.100 M HCl. Calculate the pH of the solution after 350. mL of HCl has been added. (Ka(NH4+) = 5.6 x 10-10)

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Calculate the silver ion concentration in a saturated solution of silver(I) carbonate (Ksp = 8.1 *10-12) .

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A precipitate of AgCl will form when 0.050 mol NaCl(s) and 0.050 mol AgNO3(s) are dissolved in 500. mL of 3.0 M NH3. [Kf for Ag(NH3)2+ is 1.5 * 107; Ksp(AgCl) = 1.6 * 10-10]

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Calculate the molar solubility of lead (II) fluoride. (Ksp (PbF2 = 4.1 x 10-8) )

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Which of the following compounds is more soluble in a 0.10 M NH3(aq) solution than in pure neutral water

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

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

Correct AnswerverifiedShow Answer

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

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]

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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]

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Calculate the concentration of fluoride ions in a saturated barium fluoride (Ksp = 1.7 * 10-6) solution.

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25.0 mL of a 0.100 M solution of NH3 is titrated with 0.150M HCl. After 10.0 mL of the HCl has been added, the resultant solution is:

Correct AnswerverifiedShow Answer

An environmental chemist obtained a 200. mL sample of lake water believed to be contaminated with a single monoprotic strong acid. Titrating this sample with a 0.0050 M NaOH(aq) required 7.3 mL of the NaOH solution to reach the endpoint. What is the concentration of H+ in the lake

Correct AnswerverifiedShow Answer

The pH of a solution that is 0.20 M CH3COOH and 0.20 M CH3COONa should be higher than the pH of a 0.20 M CH3COOH solution.

Correct AnswerverifiedShow Answer

The Ksp for silver(I) phosphate is 1.8 * 10-18. Calculate the molar solubility of silver(I) phosphate.

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Calculate the pH of a solution that is 0.20M NH3(aq) and 0.35 M NH4Cl(aq) .(Kb(NH3) = 1.8 x 10-5)

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5.0 mL of 12 M NH₃ is added to 500. mL of 0.050 M AgNO₃. What concentration of silver ion will exist after equilibrium is established [K_f for Ag(NH₃) ₂⁺ is 1.5 * 10⁷.]

Correct Answer
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To 1.00 L of a 0.100 M aqueous solution of benzoic acid (C₆H₅COOH) is added 1.00 mL of 12.0 M HCl. What is the percentage ionization of the benzoic acid in the resulting solution [K_a(C₆H₅COOH) = 6.5 * 10^-5]

Correct Answer
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Calculate the equilibrium constant K_c for the following overall reaction: AgCl(s) + 2CN^-(aq) $\leftrightharpoons$ Ag(CN) ₂^-(aq) + Cl^-(aq) For AgCl, K_sp = 1.6 * 10^-10; for Ag(CN) ₂^-, K_f = 1.0 * 10²¹.

Correct Answer
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What volume of 0.0500 M sodium hydroxide should be added to 250. mL of 0.100 M HCOOH? to obtain a solution with a pH of 4.50 [K_a(HCOOH) = 1.7 * 10^-4]

Correct Answer
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340. mL of a 0.150 M solution of NH₃(aq) is titrated with 0.100 M HCl. Calculate the pH of the solution after 350. mL of HCl has been added. (K_a(NH₄⁺) = 5.6 x 10^-10)

Correct Answer
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Calculate the silver ion concentration in a saturated solution of silver(I) carbonate (K_sp = 8.1 *10^-12) .

Correct Answer
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A precipitate of AgCl will form when 0.050 mol NaCl(s) and 0.050 mol AgNO₃(s) are dissolved in 500. mL of 3.0 M NH₃. [K_f for Ag(NH₃)₂⁺ is 1.5 * 10⁷; K_sp(AgCl) = 1.6 * 10^-10]

Correct Answer
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Calculate the molar solubility of lead (II) fluoride. (K_sp (PbF₂ = 4.1 x 10^-8) )

Correct Answer
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Which of the following compounds is more soluble in a 0.10 M NH₃(aq) solution than in pure neutral water

Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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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
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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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Calculate the concentration of fluoride ions in a saturated barium fluoride (K_sp = 1.7 * 10^-6) solution.

Correct Answer
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25.0 mL of a 0.100 M solution of NH₃ is titrated with 0.150M HCl. After 10.0 mL of the HCl has been added, the resultant solution is:

Correct Answer
verified

An environmental chemist obtained a 200. mL sample of lake water believed to be contaminated with a single monoprotic strong acid. Titrating this sample with a 0.0050 M NaOH(aq) required 7.3 mL of the NaOH solution to reach the endpoint. What is the concentration of H⁺ in the lake

Correct Answer
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The pH of a solution that is 0.20 M CH₃COOH and 0.20 M CH₃COONa should be higher than the pH of a 0.20 M CH₃COOH solution.

Correct Answer
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The K_sp for silver(I) phosphate is 1.8 * 10^-18. Calculate the molar solubility of silver(I) phosphate.

Correct Answer
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Calculate the pH of a solution that is 0.20M NH₃(aq) and 0.35 M NH₄Cl(aq) .(K_b(NH₃) = 1.8 x 10^-5)

Correct Answer
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