Question 1

Consider the following Bronsted-Lowry acid-base reaction:
C6H5NH2 + HCOOH→C6H5NH3+ + HCOO -  Which of the following is a conjugate acid-base pair?

Accepted Answer

A)   C6H5NH2 and HCO2H
B)   HCOOH and C6H5NH3+
C)   HCOO -  and C6H5NH2
D)   C6H5NH3+ and C6H5NH2
E)   C6H5NH3+ and HCOO - F) None of the above
G) B) and C) D

Question 2

What is the acid ionization constant , K a, for Chlorous acid, HClO2, if a 0.25 M aqueous solution of chlorous acid has a pH equal to 1.33?
You may want to complete the ICE table before getting started. HClO2 H3O+ ClO21 -  Initial Change @ equilibrium

Accepted Answer

A)   K a = 2.2×10 - 3
B)   K a = 7.4×10 - 3
C)   K a = 8.8×10 - 3
D)   K a = 1.1×10 - 2
E)   K a = 4.7×10 - 2F) None of the above
G) B) and D)

Question 3

In the reaction:
N₂H4 (aq)  + H₂ O 4 (aq)  + H₂ O   N₂H5 + (aq)  + OH - (aq)  A)  N2H4 and N2H5+ act as acids. B)  H2O and N2H5+ act as acids. C)  N2H5+ and OH -  act as acids. D)  only OH -  acts as a base. E)  none of these." class="answers-bank-image d-inline" rel="preload" > N₂H5 + (aq)  + OH - (aq)

Accepted Answer

A)   N2H4 and N2H5+ act as acids.
B)   H2O and N2H5+ act as acids.
C)   N2H5+ and OH -  act as acids.
D)   only OH -  acts as a base.
E)   none of these.F) All of the above
G) C) and D)

Question 4

Regarding acid strength, which of the following is not correctly assigned?

Accepted Answer

A)   (weaker acid)  NH3 2O (stronger acid) 
B)   (weaker acid)  HSO31 -  2SO3 (stronger acid) 
C)   (weaker acid)  HBrO2 3 (stronger acid) 
D)   (weaker acid)  HBr 
E)   (weaker acid)  HClO3 3 (stronger acid) F) D) and E)
G) A) and C) E

Question 5

Which aqueous solution(s)  below is(are)  considered basic ?
I. A solution with a pH = 6
II. A solution with [OH - ] = 1×10 - 7
III. A solution with [H3O+] = 1×10 - 9

Accepted Answer

A)   I only
B)   II only
C)   III only
D)   I and II
E)   I and IIIF) None of the above
G) A) and E)

Question 6

What is the pOH of a 1.0×10 - 4 M solution of HI?

Accepted Answer

A)   10.00
B)   4.00
C)   18.00
D)   - 4.00
E)   2.00F) A) and D)
G) B) and C)

Question 7

If the reaction below proceeds, which of the following is true?
NH3 + C2H5OH→NH2 -  + C2H5OH2+

Accepted Answer

A)   C2H5OH is an acid.
B)   NH2 -  is the conjugate base of NH3.
C)   NH3 is a base.
D)   C2H5OH2+ is a base.
E)   none of theseF) B) and C)
G) C) and D)

Question 8

K b for ammonia is 1.8×10 - 5. Calculate K a for the ammonium ion.

Accepted Answer

A)   5.6×104
B)   4.2×10 - 3
C)   1.8×10 - 5
D)   1.0×10 - 7
E)   5.6×10 - 10F) All of the above
G) A) and E)

Question 9

Consider adding NaClO4 to a basic solution. Which statement below is true?

Accepted Answer

A)   NaClO4 is an acidic salt and the pH of the resulting solution rises.
B)   NaClO4 is an acidic salt and the pH of the resulting solution lowers.
C)   NaClO4 is a basic salt and the pH of the resulting solution rises.
D)   NaClO4 is a basic salt and the pH of the resulting solution lowers.
E)   NaClO4 is a neutral salt and the pH of the resulting solution does not change.F) A) and B)
G) B) and D)

Question 10

What is the pH of an aqueous 0.036 M NaF solution?
K a(HF)  = 6.8×10 - 4

Accepted Answer

A)   pH = 1.44
B)   pH = 2.31
C)   pH = 6.14
D)   pH = 7.86
E)   pH = 11.69F) A) and B)
G) D) and E)

Question 11

At 37 ° C the autoionization constant of water is K w = 2.4×10 - 14. What is the pH of pure water at 37 ° C?

Accepted Answer

A)   6.81
B)   7.00
C)   7.19
D)   2.39
E)   11.61F) A) and B)
G) A) and C)

Question 12

What is the pH of a 0.025 M solution of HSCN ( K a = 4.0×10 - 6) ?

Accepted Answer

A)   1.60
B)   3.50
C)   4.21
D)   5.39
E)   7.00F) All of the above
G) None of the above

Question 13

Aniline, C6 H5 NH₂ , is commonly used as a precursor for making dyes. Aniline is a base when dissolved in water. It ionizes as shown below. What is the base ionization constant, K b , of aniline if an aqueous 0.20 M C6 H5 NH₂ solution has a pOH value equal tO5 .05?
C6 H5 NH₂ + H₂ O 6 H5 NH₂ , is commonly used as a precursor for making dyes. Aniline is a base when dissolved in water. It ionizes as shown below. What is the base ionization constant, K b , of aniline if an aqueous 0.20 M C6 H5 NH₂ solution has a pOH value equal tO5 .05? C6 H5 NH₂ + H₂ O   C6 H5 NH₃+ + OH - A)  K b = 6.3×10 - 18 B)  K b = 4.0×10 - 10 C)  K b = 4.5×10 - 5 D)  K b = 1.5×10 - 2 E)  K b = 6.3×1010" class="answers-bank-image d-inline" rel="preload" > C6 H5 NH₃+ + OH -

Accepted Answer

A)   K b = 6.3×10 - 18
B)   K b = 4.0×10 - 10
C)   K b = 4.5×10 - 5
D)   K b = 1.5×10 - 2
E)   K b = 6.3×1010F) B) and C)
G) A) and C)

Question 14

50 mL of 0.50 M NaOH is added to enough water to make 1.0 liter of solution. Calculate the pH.

Accepted Answer

A)   0.3
B)   1.6
C)   12.4
D)   12.7
E)   13.7F) A) and B)
G) C) and E)

Question 15

An acid HB+ has a K a of 1.0×10 - 9. What is the p K b of the base B?

Accepted Answer

A)   9.0
B)   7.0
C)   5.0
D)   1.0×10 - 5
E)   1.0×10 - 9F) D) and E)
G) B) and C)

Question 16

Which anionic base listed below would be the strongest given the corresponding acid ionization constants for their conjugate acids?

Accepted Answer

A)   F - ; K a(HF)  = 6.8×10 - 4
B)   CH3COO - ; K a(CH3COOH)  = 1.8×10 - 5
C)   IO31 - ; K a(HIO3)  = 1.6×10 - 1
D)   NO21 - ; K a(HNO2)  = 7.1×10 - 4E) B) and D)
F) A) and D)

Question 17

A nitric acid (HNO3)  solution is 16.2 M. Which of the following is correct?

Accepted Answer

A)   pH = 1.21
B)   pH = 2.78
C)   pOH = 15.21
D)   [OH - ] = 1.62×1015
E)   must know K aF) A) and E)
G) All of the above

Question 18

After completing the following unfinished table, what is the order of increasing base strength ?
Base K b p K b Fluoride ion, F -  1.5×10 - 11 Ammonia, NH3 4.75 Acetate ion, CH3COO -  5.7×10 - 10

Accepted Answer

A)   (weakest)  Fluoride ion 
B)   (weakest)  Fluoride ion 
C)   (weakest)  Ammonia 
D)   (weakest)  Acetate ion 
E)   (weakest)  Acetate ion < Fluoride ion < Ammonia (strongest) F) A) and C)
G) C) and D)

Question 19

A 0.250 M aqueous solution of p -toluic acid has a pH of 2.49. What is K a for this weak acid?

Accepted Answer

A)   4.2×10 - 5
B)   3.2×10 - 3
C)   1.3×10 - 2
D)   2.4×10 - 10
E)   1.0×10 - 5F) D) and E)
G) B) and D)

Question 20

When 20.0 grams of a water soluble salt dissolves in 1.0 L of pure water the pH was found to be less than seven. Which of the following statements about the salt is most probable?

Accepted Answer

A)   The salt contained the conjugate acid of a strong base.
B)   The salt contained the conjugate base of a strong acid.
C)   The salt contained the conjugate base of a weak acid.
D)   The salt contained the conjugate acid of a weak base.
E)   The salt was impure and contained some NH4Cl.F) B) and E)
G) A) and E) D

Exam 15: Solutions of Acids and Bases

Consider the following Bronsted-Lowry acid-base reaction: C₆H₅NH₂ + HCOOH→C₆H₅NH₃⁺ + HCOO^- Which of the following is a conjugate acid-base pair?

Correct Answer
verified
D

What is the acid ionization constant , K _a, for Chlorous acid, HClO₂, if a 0.25 M aqueous solution of chlorous acid has a pH equal to 1.33? You may want to complete the ICE table before getting started. HClO₂ H₃O⁺ ClO₂^{1 -} Initial Change @ equilibrium

Correct Answer
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In the reaction: N₂H₄ (aq) + H₂ O N₂H₅ + (aq) + OH - (aq)

Correct Answer
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Regarding acid strength, which of the following is not correctly assigned?

Correct Answer
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E

Which aqueous solution(s) below is(are) considered basic ? I. A solution with a pH = 6 II. A solution with [OH^-] = 1×10^{- 7} III. A solution with [H₃O⁺] = 1×10^{- 9}

Correct Answer
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What is the pOH of a 1.0×10^{- 4} M solution of HI?

Correct Answer
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If the reaction below proceeds, which of the following is true? NH₃ + C₂H₅OH→NH₂^- + C₂H₅OH₂⁺

Correct Answer
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K _b for ammonia is 1.8×10^{- 5}. Calculate K _a for the ammonium ion.

Correct Answer
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Consider adding NaClO₄ to a basic solution. Which statement below is true?

Correct Answer
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What is the pH of an aqueous 0.036 M NaF solution? K _a(HF) = 6.8×10^{- 4}

Correct Answer
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At 37 ° C the autoionization constant of water is K _w = 2.4×10^{- 14}. What is the pH of pure water at 37 ° C?

Correct Answer
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What is the pH of a 0.025 M solution of HSCN ( K _a = 4.0×10^{- 6}) ?

Correct Answer
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Correct Answer
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50 mL of 0.50 M NaOH is added to enough water to make 1.0 liter of solution. Calculate the pH.

Correct Answer
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An acid HB⁺ has a K _a of 1.0×10^{- 9}. What is the p K _b of the base B?

Correct Answer
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Which anionic base listed below would be the strongest given the corresponding acid ionization constants for their conjugate acids?

Correct Answer
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A nitric acid (HNO₃) solution is 16.2 M. Which of the following is correct?

Correct Answer
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After completing the following unfinished table, what is the order of increasing base strength ? Base K _b p K _b Fluoride ion, F^- 1.5×10^{- 11} Ammonia, NH₃ 4.75 Acetate ion, CH₃COO^- 5.7×10^{- 10}

Correct Answer
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A 0.250 M aqueous solution of p -toluic acid has a pH of 2.49. What is K _a for this weak acid?

Correct Answer
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When 20.0 grams of a water soluble salt dissolves in 1.0 L of pure water the pH was found to be less than seven. Which of the following statements about the salt is most probable?

Correct Answer
verified
D

Exam 15: Solutions of Acids and Bases

Consider the following Bronsted-Lowry acid-base reaction: C6H5NH2 + HCOOH→C6H5NH3+ + HCOO - Which of the following is a conjugate acid-base pair?

Correct AnswerverifiedD

What is the acid ionization constant , K a, for Chlorous acid, HClO2, if a 0.25 M aqueous solution of chlorous acid has a pH equal to 1.33? You may want to complete the ICE table before getting started. HClO2 H3O+ ClO21 - Initial Change @ equilibrium

Correct AnswerverifiedShow Answer

In the reaction: N₂H4 (aq) + H₂ O N₂H5 + (aq) + OH - (aq)

Correct AnswerverifiedShow Answer

Regarding acid strength, which of the following is not correctly assigned?

Correct AnswerverifiedE

Which aqueous solution(s) below is(are) considered basic ? I. A solution with a pH = 6 II. A solution with [OH - ] = 1×10 - 7 III. A solution with [H3O+] = 1×10 - 9

Correct AnswerverifiedShow Answer

What is the pOH of a 1.0×10 - 4 M solution of HI?

Correct AnswerverifiedShow Answer

If the reaction below proceeds, which of the following is true? NH3 + C2H5OH→NH2 - + C2H5OH2+

Correct AnswerverifiedShow Answer

K b for ammonia is 1.8×10 - 5. Calculate K a for the ammonium ion.

Correct AnswerverifiedShow Answer

Consider adding NaClO4 to a basic solution. Which statement below is true?

Correct AnswerverifiedShow Answer

What is the pH of an aqueous 0.036 M NaF solution? K a(HF) = 6.8×10 - 4

Correct AnswerverifiedShow Answer

At 37 ° C the autoionization constant of water is K w = 2.4×10 - 14. What is the pH of pure water at 37 ° C?

Correct AnswerverifiedShow Answer

What is the pH of a 0.025 M solution of HSCN ( K a = 4.0×10 - 6) ?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

50 mL of 0.50 M NaOH is added to enough water to make 1.0 liter of solution. Calculate the pH.

Correct AnswerverifiedShow Answer

An acid HB+ has a K a of 1.0×10 - 9. What is the p K b of the base B?

Correct AnswerverifiedShow Answer

Which anionic base listed below would be the strongest given the corresponding acid ionization constants for their conjugate acids?

Correct AnswerverifiedShow Answer

A nitric acid (HNO3) solution is 16.2 M. Which of the following is correct?

Correct AnswerverifiedShow Answer

After completing the following unfinished table, what is the order of increasing base strength ? Base K b p K b Fluoride ion, F - 1.5×10 - 11 Ammonia, NH3 4.75 Acetate ion, CH3COO - 5.7×10 - 10

Correct AnswerverifiedShow Answer

A 0.250 M aqueous solution of p -toluic acid has a pH of 2.49. What is K a for this weak acid?

Correct AnswerverifiedShow Answer

When 20.0 grams of a water soluble salt dissolves in 1.0 L of pure water the pH was found to be less than seven. Which of the following statements about the salt is most probable?

Correct AnswerverifiedD

Consider the following Bronsted-Lowry acid-base reaction: C₆H₅NH₂ + HCOOH→C₆H₅NH₃⁺ + HCOO^- Which of the following is a conjugate acid-base pair?

Correct Answer
verified
D

What is the acid ionization constant , K _a, for Chlorous acid, HClO₂, if a 0.25 M aqueous solution of chlorous acid has a pH equal to 1.33? You may want to complete the ICE table before getting started. HClO₂ H₃O⁺ ClO₂^{1 -} Initial Change @ equilibrium

Correct Answer
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In the reaction: N₂H₄ (aq) + H₂ O N₂H₅ + (aq) + OH - (aq)

Correct Answer
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Correct Answer
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E

Which aqueous solution(s) below is(are) considered basic ? I. A solution with a pH = 6 II. A solution with [OH^-] = 1×10^{- 7} III. A solution with [H₃O⁺] = 1×10^{- 9}

Correct Answer
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What is the pOH of a 1.0×10^{- 4} M solution of HI?

Correct Answer
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If the reaction below proceeds, which of the following is true? NH₃ + C₂H₅OH→NH₂^- + C₂H₅OH₂⁺

Correct Answer
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K _b for ammonia is 1.8×10^{- 5}. Calculate K _a for the ammonium ion.

Correct Answer
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Consider adding NaClO₄ to a basic solution. Which statement below is true?

Correct Answer
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What is the pH of an aqueous 0.036 M NaF solution? K _a(HF) = 6.8×10^{- 4}

Correct Answer
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At 37 ° C the autoionization constant of water is K _w = 2.4×10^{- 14}. What is the pH of pure water at 37 ° C?

Correct Answer
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What is the pH of a 0.025 M solution of HSCN ( K _a = 4.0×10^{- 6}) ?

Correct Answer
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Correct Answer
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Correct Answer
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An acid HB⁺ has a K _a of 1.0×10^{- 9}. What is the p K _b of the base B?

Correct Answer
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Correct Answer
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A nitric acid (HNO₃) solution is 16.2 M. Which of the following is correct?

Correct Answer
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After completing the following unfinished table, what is the order of increasing base strength ? Base K _b p K _b Fluoride ion, F^- 1.5×10^{- 11} Ammonia, NH₃ 4.75 Acetate ion, CH₃COO^- 5.7×10^{- 10}

Correct Answer
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A 0.250 M aqueous solution of p -toluic acid has a pH of 2.49. What is K _a for this weak acid?

Correct Answer
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Correct Answer
verified
D