Question 1

A 25.0-mL sample of 0.10 M C2H5NH2 (ethylamine)  is titrated with 0.15 M HCl. What is the pH of the solution after 9.00 mL of acid have been added to the amine? [Kb(C2H5NH2)  = 6.5 × 10-4]

Accepted Answer

A)   11.08
B)   10.74
C)   10.81
D)   10.55
E)   10.49F) A) and B)
G) A) and D)

Question 2

A 20.0-mL sample of 0.25 M HNO3 is titrated with 0.15 M NaOH. What is the pH of the solution after 30.0 mL of NaOH have been added to the acid?

Accepted Answer

A)   2.00
B)   1.60
C)   1.05
D)   1.00
E)   0.00F) C) and D)
G) A) and B)

Question 3

If the pH of a buffer solution is greater than the pKa value of the buffer acid, the buffer will have more capacity to neutralize added base than added acid.

Accepted Answer

A) True 
 B)False

Question 4

A 35.0-mL sample of 0.20 M LiOH is titrated with 0.25 M HCl. What is the pH of the solution after 23.0 mL of HCl have been added to the base?

Accepted Answer

A)   1.26
B)   1.67
C)   12.33
D)   12.74
E)   13.03F) B) and D)
G) B) and C)

Question 5

The ________ is the point in a titration where neutralization is complete.

Accepted Answer

The answer of The ________ is the point in a...

Question 6

The molar solubility of manganese(II)  carbonate is 4.2 × 10-6 M. What is Ksp for this compound?

Accepted Answer

A)   4.2 × 10-6
B)   8.4 × 10-6
C)   3.0 × 10-16
D)   1.8 × 10-11
E)   2.0 × 10-3F) C) and D)
G) All of the above

Question 7

What is the [H3O+] in a buffer that consists of 0.30 M HCOOH and 0.20 M HCOONa? [Ka(HCOOH)  = 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)   1.7 × 10-4 MF) A) and B)
G) A) and C)

Question 8

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)   2.96
C)   2.85
D)   1.49
E)   3.81F) A) and D)
G) A) and C)

Question 9

What happens to the solution if sodium acetate is added to a solution of acetic acid? CH3COOH(aq)  3COOH(aq)    H+(aq)  + CH3COO-(aq)  A)  The equilibrium shifts to the right. B)  There is an increase in percent ionization of acetic acid. C)  Less of hydrogen ion is consumed. D)  There is an increased concentration of acetate ions. E)  Less of the acetate ion is consumed." class="answers-bank-image d-inline" rel="preload" > H+(aq)  + CH3COO-(aq)

Accepted Answer

A)   The equilibrium shifts to the right.
B)   There is an increase in percent ionization of acetic acid.
C)   Less of hydrogen ion is consumed.
D)   There is an increased concentration of acetate ions.
E)   Less of the acetate ion is consumed.F) B) and E)
G) All of the above

Question 10

Calculate the solubility of silver oxalate, Ag2C2O4, in pure water. [Ksp(Ag2C2O4)  = 1.0 × 10-11]

Accepted Answer

A)   1.4 × 10-4 M
B)   8.2 × 10-5 M
C)   5.4 × 10-5 M
D)   3.2 × 10-6 M
E)   2.5 × 10-12 MF) B) and D)
G) B) and E)

Question 11

Calculate the pH of a buffer solution that contains 0.25 M benzoic acid (C6H5CO2H)  and 0.15 M 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) B) and C)
G) All of the above

Question 12

Calculate the NaOH concentration necessary to precipitate Ca(OH) 2 from a solution in which [Ca2+] = 1.0. Ksp of Ca(OH) 2 = 8 x 10-6.

Accepted Answer

A)   6.7 x 10-8 M
B)   2.8 x 10-3 M
C)   1.5 x 10-7 M
D)   0.10 ME) None of the above
F) B) and C)

Question 13

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

Accepted Answer

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

Question 14

Which is more soluble in an acidic solution than in pure water?

Accepted Answer

A)   CH3CH2OH, ethanol
B)   Li2O
C)   C6H12O6, glucose
D)   CCl4
E)   ICl3F) B) and C)
G) C) and D)

Question 15

A mixture made of 100 mL of 0.5 M CH3COOH and 100 mL of 0.5 M CH3COONa is classified as a buffer solution.

Accepted Answer

A) True 
 B)False

Question 16

Which results in a buffered solution?

Accepted Answer

A)   A solution containing a strong acid and its conjugate base
B)   A solution containing a strong base and its conjugate acid
C)   A solution containing a catalyst
D)   A solution containing two organic liquids
E)   A solution containing a weak acid and its conjugate baseF) A) and E)
G) B) and D)

Question 17

A 25.0-mL sample of 1.00 M NH3 is titrated with 0.15 M HCl. What is the pH of the solution after 15.00 mL of acid have been added to the ammonia solution? [Kb(NH3)  = 1.8 × 10-5]

Accepted Answer

A)   10.26
B)   9.30
C)   9.21
D)   8.30
E)   8.21F) A) and D)
G) B) and C)

Question 18

What is the ion product expression for magnesium fluoride, MgF2?

Accepted Answer

A)   2? 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
B)   2? 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
C)   2? 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
D)   2? 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
E)   2? 
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >F) C) and E)
G) B) and E)

Question 19

When sodium acetate is added to a solution of acetic acid, what happens to the pH of the solution? Explain why this effect occurs?
CH3COOH(aq)  H+(aq)CH3COO-(aq)

Accepted Answer

The pH increases because the equilibrium...

Question 20

Which is more soluble in an acidic solution than in pure water?

Accepted Answer

A)   CuI
B)   PbCl2
C)   Ca3(PO4) 2
D)   NaNO3
E)   NaBrF) A) and D)
G) None of the above

Exam 17: Acid-Base Equilibria and Solubility Equilibria

What is the ion product expression for magnesium fluoride, MgF2?

Correct AnswerverifiedShow Answer

Which results in a buffered solution?

Correct AnswerverifiedShow Answer

If the pH of a buffer solution is greater than the pKa value of the buffer acid, the buffer will have more capacity to neutralize added base than added acid.

Correct AnswerverifiedShow Answer

The ________ is the point in a titration where neutralization is complete.

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

What is the [H3O+] in a buffer that consists of 0.30 M HCOOH and 0.20 M HCOONa? [Ka(HCOOH) = 1.7 × 10-4]

Correct AnswerverifiedShow Answer

Which is more soluble in an acidic solution than in pure water?

Correct AnswerverifiedShow Answer

Calculate the NaOH concentration necessary to precipitate Ca(OH) 2 from a solution in which [Ca2+] = 1.0. Ksp of Ca(OH) 2 = 8 x 10-6.

Correct AnswerverifiedShow Answer

A 35.0-mL sample of 0.20 M LiOH is titrated with 0.25 M HCl. What is the pH of the solution after 23.0 mL of HCl have been added to the base?

Correct AnswerverifiedShow Answer

A 25.0-mL sample of 0.10 M C2H5NH2 (ethylamine) is titrated with 0.15 M HCl. What is the pH of the solution after 9.00 mL of acid have been added to the amine? [Kb(C2H5NH2) = 6.5 × 10-4]

Correct AnswerverifiedShow Answer

A mixture made of 100 mL of 0.5 M CH3COOH and 100 mL of 0.5 M CH3COONa is classified as a buffer solution.

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

A 20.0-mL sample of 0.25 M HNO3 is titrated with 0.15 M NaOH. What is the pH of the solution after 30.0 mL of NaOH have been added to the acid?

Correct AnswerverifiedShow Answer

Calculate the solubility of silver oxalate, Ag2C2O4, in pure water. [Ksp(Ag2C2O4) = 1.0 × 10-11]

Correct AnswerverifiedShow Answer

The molar solubility of manganese(II) carbonate is 4.2 × 10-6 M. What is Ksp for this compound?

Correct AnswerverifiedShow Answer

What happens to the solution if sodium acetate is added to a solution of acetic acid? CH3COOH(aq) H+(aq) + CH3COO-(aq)

Correct AnswerverifiedShow Answer

A 25.0-mL sample of 1.00 M NH3 is titrated with 0.15 M HCl. What is the pH of the solution after 15.00 mL of acid have been added to the ammonia solution? [Kb(NH3) = 1.8 × 10-5]

Correct AnswerverifiedShow Answer

When sodium acetate is added to a solution of acetic acid, what happens to the pH of the solution? Explain why this effect occurs? CH3COOH(aq) H+(aq)CH3COO-(aq)

Correct AnswerverifiedThe pH increases because the equilibrium...View AnswerShow Answer

Which is more soluble in an acidic solution than in pure water?

Correct AnswerverifiedShow Answer

What is the ion product expression for magnesium fluoride, MgF₂?

Correct Answer
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If the pH of a buffer solution is greater than the pK_a value of the buffer acid, the buffer will have more capacity to neutralize added base than added acid.

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

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

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? [K_a(HCOOH) = 1.7 × 10^-4]

Correct Answer
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Correct Answer
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Calculate the NaOH concentration necessary to precipitate Ca(OH) ₂ from a solution in which [Ca²⁺] = 1.0. K_sp of Ca(OH) ₂ = 8 x 10^-6.

Correct Answer
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Correct Answer
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A 25.0-mL sample of 0.10 M C₂H₅NH₂ (ethylamine) is titrated with 0.15 M HCl. What is the pH of the solution after 9.00 mL of acid have been added to the amine? [K_b(C₂H₅NH₂) = 6.5 × 10^-4]

Correct Answer
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A mixture made of 100 mL of 0.5 M CH₃COOH and 100 mL of 0.5 M CH₃COONa is classified as a buffer solution.

Correct Answer
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Correct Answer
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A 20.0-mL sample of 0.25 M HNO₃ is titrated with 0.15 M NaOH. What is the pH of the solution after 30.0 mL of NaOH have been added to the acid?

Correct Answer
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Calculate the solubility of silver oxalate, Ag₂C₂O₄, in pure water. [K_sp(Ag₂C₂O₄) = 1.0 × 10^-11]

Correct Answer
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The molar solubility of manganese(II) carbonate is 4.2 × 10^-6^M. What is K_sp for this compound?

Correct Answer
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What happens to the solution if sodium acetate is added to a solution of acetic acid? CH₃COOH(aq) H⁺(aq) + CH₃COO^-(aq)

Correct Answer
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A 25.0-mL sample of 1.00 M NH₃ is titrated with 0.15 M HCl. What is the pH of the solution after 15.00 mL of acid have been added to the ammonia solution? [K_b(NH₃) = 1.8 × 10^-5]

Correct Answer
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When sodium acetate is added to a solution of acetic acid, what happens to the pH of the solution? Explain why this effect occurs? CH₃COOH(aq) H⁺(aq)CH₃COO^-(aq)

Correct Answer
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The pH increases because the equilibrium...
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Correct Answer
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