Question 1

What is the hydronium ion concentration of pure water at 25°C?

Accepted Answer

A)  7.0 × 107 M
B)  7.0 × 10-7 M
C)  1.0 × 107 M
D)  1.0 × 10-7 M
E)  1.0 × 10-14 MF) A) and B)
G) None of the above

Question 2

What is the pH of a 1.0 × 10−4 M solution of KOH?

Accepted Answer

A)  4.00
B)  6.00
C)  7.00
D)  10.00
E)  14.00F) A) and C)
G) A) and E)

Question 3

The combination of a weak acid and a strong acid form a buffer solution.

Accepted Answer

A) True 
 B)False

Question 4

For the reaction shown below, which of the following correctly represents a conjugate acid-base pair? HCO2H(aq)  + H2O(l)  2H(aq)  + H2O(l)    H3O+(aq)  + HCO2−(aq)  A) HCO2H/H3O+ B) HCO2H/H2O C) H2O/HCO2- D) H3O+/HCO2- E) HCO2H/HCO2−" class="answers-bank-image d-inline" rel="preload" > H3O+(aq)  + HCO2−(aq)

Accepted Answer

A)  HCO2H/H3O+
B)  HCO2H/H2O
C)  H2O/HCO2-
D)  H3O+/HCO2-
E)  HCO2H/HCO2−F) A) and B)
G) A) and E)

Question 5

The concentration of a weak acid or base affects its degree of dissociation in water.

Accepted Answer

A) True 
 B)False

Question 6

A buffer solution contains carbonic acid (H2CO3)  and sodium bicarbonate (NaHCO3) , each at a concentration of 0.100 M.The relevant equilibrium is shown below.What is the pH of this buffer solution? H2CO3(aq)  + H2O(l)  2CO3)  and sodium bicarbonate (NaHCO3) , each at a concentration of 0.100 M.The relevant equilibrium is shown below.What is the pH of this buffer solution? H2CO3(aq)  + H2O(l)    H3O+(aq)  + HCO3−(aq)  Ka = 4.5 × 10−7 A) 4.50 B) 7.00 C) 6.35 D) 7.65 E) 2.16" class="answers-bank-image d-inline" rel="preload" > H3O+(aq)  + HCO3−(aq)  Ka = 4.5 × 10−7

Accepted Answer

A)  4.50
B)  7.00
C)  6.35
D)  7.65
E)  2.16F) A) and D)
G) All of the above

Question 7

What is the pH of a 0.035 M HCl solution?

Accepted Answer

A)  3.50
B)  1.46
C)  2.27
D)  5.59
E)  12.54F) A) and C)
G) B) and E)

Question 8

Which of the following is an example of a diprotic acid?

Accepted Answer

A)  NH2−
B)  H2SO4
C)  HCl
D)  CH4
E)  NH2− and H2SO4 are correct.F) A) and D)
G) A) and C)

Question 9

Consider the following generalized buffer solution equilibrium: BH+(aq)  + H2O(l)  +(aq)  + H2O(l)    H3O+(aq)  + B(aq)  When a small amount of a strong base such as sodium hydroxide is added to the solution, which of the four species shown would experience an increase in concentration? (Hint: Use LeChatelier's principle.)  A) BH+ B) H2O C) H3O+ D) B E) None of the species would increase in concentration." class="answers-bank-image d-inline" rel="preload" > H3O+(aq)  + B(aq) 
When a small amount of a strong base such as sodium hydroxide is added to the solution, which of the four species shown would experience an increase in concentration? (Hint: Use LeChatelier's principle.)

Accepted Answer

A)  BH+
B)  H2O
C)  H3O+
D)  B
E)  None of the species would increase in concentration.F) A) and B)
G) C) and D)

Question 10

A buffer solution contains acetic acid (HC2H3O2)  at a concentration of 0.225 M and sodium acetate (NaC2H3O2)  at a concentration of 0.164 M.The value of Ka for acetic acid is 1.75 × 10-5.What is the pH of this buffer solution?

Accepted Answer

A)  0.137
B)  0.862
C)  2.40
D)  4.62
E)  4.76F) B) and E)
G) A) and D)

Question 11

A sample of black coffee was measured to have [H3O+] = 7.94 × 10−6.What is TRUE about this solution?

Accepted Answer

A)  The solution is acidic.
B)  The solution contains less hydronium ions than pure water itself.
C)  The solution does not contain any OH−ions.
D)  The solution has [OH−] = 7.94 × 10−6.
E)  The pH of the solution is 7.94.F) A) and B)
G) B) and D)

Question 12

Which of the following best represents the autoionization, or self-ionization, of water?

Accepted Answer

A)  H2O(l)  → H+(aq)  + OH-(aq) 
B)  2H2O(l)  2O(l)  → H+(aq)  + OH-(aq)  
B)  2H2O(l)    2H2(aq)  + O2(aq)  
C)  2H2O(l)    H3O+(aq)  + OH-(aq)  
D)  H2O(l)  → H2(aq)  + O2-(aq)  
E)  H+(aq)  + OH-(aq)  → H2O(l) " class="answers-bank-image d-inline" rel="preload" > 2H2(aq)  + O2(aq) 
C)  2H2O(l)  2O(l)  → H+(aq)  + OH-(aq)  
B)  2H2O(l)    2H2(aq)  + O2(aq)  
C)  2H2O(l)    H3O+(aq)  + OH-(aq)  
D)  H2O(l)  → H2(aq)  + O2-(aq)  
E)  H+(aq)  + OH-(aq)  → H2O(l) " class="answers-bank-image d-inline" rel="preload" > H3O+(aq)  + OH-(aq) 
D)  H2O(l)  → H2(aq)  + O2-(aq) 
E)  H+(aq)  + OH-(aq)  → H2O(l) F) D) and E)
G) A) and D)

Question 13

A particular buffer solution consists of a weak acid and its conjugate base.How could this buffer solution be modified so as to increase its buffer capacity against added base?

Accepted Answer

A)  Increase the concentration of the weak acid.
B)  Increase the concentration of its conjugate base.
C)  Use a strong base and its conjugate acid instead.
D)  Use a strong acid and its conjugate base instead.
E)  Make the concentrations of the weak acid and its conjugate base equal.F) A) and C)
G) A) and B)

Question 14

Calculate the molar concentration of a sodium hydroxide solution if 60.00 mL of this solution were required to neutralize 30.00 mL of a 0.150 M hydrochloric acid solution.NaOH(aq)  + HCl(aq)  → NaCl(aq)  + H2O(l)

Accepted Answer

A)  3.00 M
B)  6.00 M
C)  0.0750 M
D)  0.150 M
E)  2.25 MF) D) and E)
G) A) and C)

Question 15

A solution containing a buffer has an initial pH of 8.78.If a student adds 5 drops of HCl(aq)  to this solution, what would be a reasonable pH for the resulting solution?

Accepted Answer

A)  5.22
B)  7.00
C)  8.64
D)  8.78
E)  8.89F) B) and C)
G) All of the above

Question 16

If the hydronium ion concentration of an aqueous solution at 25°C is 5 × 10-6 M, what is the hydroxide ion concentration?

Accepted Answer

A)  2 × 10-10 M
B)  2 × 10-9 M
C)  2 × 10-8 M
D)  2 × 107 M
E)  2 × 1019 MF) All of the above
G) A) and B)

Question 17

According to Arrhenius' theory of acids and bases, acids increase the hydrogen ion concentration in water.

Accepted Answer

A) True 
 B)False

Question 18

Which of the following correctly describes what is meant by the term neutralization?

Accepted Answer

A)  the reaction between hydroxide (OH−)  and water to form a base
B)  the reaction between a proton (H+)  and water to form a hydronium ion (H3O+) 
C)  the reaction between an acid and a base to form a salt and water
D)  the reaction between two molecules of water, one acting as an acid and the other acting as a base
E)  the reaction between an oxidizing agent and a reducing agentF) D) and E)
G) B) and E)

Question 19

What is always a characteristic of a solution that contains a buffer?

Accepted Answer

A)  The solution is neutral and has a pH of 7.
B)  The solution contains a small amount of solute dissolved in a large volume of solvent.
C)  The solution has been diluted by the addition of solvent.
D)  The solution resists large changes in pH when small amounts of acids or bases are added.
E)  The solution maintains a constant pH value; no amount of added acid or base can change the pH.F) A) and B)
G) A) and C)

Exam 8: Acids and Bases

A buffer solution contains carbonic acid (H₂CO₃) and sodium bicarbonate (NaHCO₃) , each at a concentration of 0.100 M.The relevant equilibrium is shown below.What is the pH of this buffer solution? H₂CO₃(aq) + H₂O(l) H₃O⁺(aq) + HCO₃−(aq) K_a = 4.5 × 10⁻⁷

Correct Answer
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A solution containing a buffer has an initial pH of 8.78.If a student adds 5 drops of HCl(aq) to this solution, what would be a reasonable pH for the resulting solution?

Correct Answer
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What is the pH of a 1.0 × 10⁻⁴ M solution of KOH?

Correct Answer
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Which of the following best represents the autoionization, or self-ionization, of water?

Correct Answer
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What is the hydronium ion concentration of pure water at 25°C?

Correct Answer
verified

Which of the following is an example of a diprotic acid?

Correct Answer
verified

A particular buffer solution consists of a weak acid and its conjugate base.How could this buffer solution be modified so as to increase its buffer capacity against added base?

Correct Answer
verified

The combination of a weak acid and a strong acid form a buffer solution.

Correct Answer
verified

The concentration of a weak acid or base affects its degree of dissociation in water.

Correct Answer
verified

For the reaction shown below, which of the following correctly represents a conjugate acid-base pair? HCO₂H(aq) + H₂O(l) H₃O⁺(aq) + HCO₂−(aq)

Correct Answer
verified

Calculate the molar concentration of a sodium hydroxide solution if 60.00 mL of this solution were required to neutralize 30.00 mL of a 0.150 M hydrochloric acid solution.NaOH(aq) + HCl(aq) → NaCl(aq) + H₂O(l)

Correct Answer
verified

According to Arrhenius' theory of acids and bases, acids increase the hydrogen ion concentration in water.

Correct Answer
verified

If the hydronium ion concentration of an aqueous solution at 25°C is 5 × 10^-6 M, what is the hydroxide ion concentration?

Correct Answer
verified

What is the pH of a 0.035 M HCl solution?

Correct Answer
verified

Correct Answer
verified

Which of the following correctly describes what is meant by the term neutralization?

Correct Answer
verified

A sample of black coffee was measured to have [H₃O⁺] = 7.94 × 10⁻⁶.What is TRUE about this solution?

Correct Answer
verified

What is always a characteristic of a solution that contains a buffer?

Correct Answer
verified

A buffer solution contains acetic acid (HC₂H₃O₂) at a concentration of 0.225 M and sodium acetate (NaC₂H₃O₂) at a concentration of 0.164 M.The value of K_a for acetic acid is 1.75 × 10^-5.What is the pH of this buffer solution?

Correct Answer
verified

Exam 8: Acids and Bases

A buffer solution contains carbonic acid (H2CO3) and sodium bicarbonate (NaHCO3) , each at a concentration of 0.100 M.The relevant equilibrium is shown below.What is the pH of this buffer solution? H2CO3(aq) + H2O(l) H3O+(aq) + HCO3−(aq) Ka = 4.5 × 10−7

Correct AnswerverifiedShow Answer

A solution containing a buffer has an initial pH of 8.78.If a student adds 5 drops of HCl(aq) to this solution, what would be a reasonable pH for the resulting solution?

Correct AnswerverifiedShow Answer

What is the pH of a 1.0 × 10−4 M solution of KOH?

Correct AnswerverifiedShow Answer

Which of the following best represents the autoionization, or self-ionization, of water?

Correct AnswerverifiedShow Answer

What is the hydronium ion concentration of pure water at 25°C?

Correct AnswerverifiedShow Answer

Which of the following is an example of a diprotic acid?

Correct AnswerverifiedShow Answer

A particular buffer solution consists of a weak acid and its conjugate base.How could this buffer solution be modified so as to increase its buffer capacity against added base?

Correct AnswerverifiedShow Answer

The combination of a weak acid and a strong acid form a buffer solution.

Correct AnswerverifiedShow Answer

The concentration of a weak acid or base affects its degree of dissociation in water.

Correct AnswerverifiedShow Answer

For the reaction shown below, which of the following correctly represents a conjugate acid-base pair? HCO2H(aq) + H2O(l) H3O+(aq) + HCO2−(aq)

Correct AnswerverifiedShow Answer

Calculate the molar concentration of a sodium hydroxide solution if 60.00 mL of this solution were required to neutralize 30.00 mL of a 0.150 M hydrochloric acid solution.NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l)

Correct AnswerverifiedShow Answer

According to Arrhenius' theory of acids and bases, acids increase the hydrogen ion concentration in water.

Correct AnswerverifiedShow Answer

If the hydronium ion concentration of an aqueous solution at 25°C is 5 × 10-6 M, what is the hydroxide ion concentration?

Correct AnswerverifiedShow Answer

What is the pH of a 0.035 M HCl solution?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Which of the following correctly describes what is meant by the term neutralization?

Correct AnswerverifiedShow Answer

A sample of black coffee was measured to have [H3O+] = 7.94 × 10−6.What is TRUE about this solution?

Correct AnswerverifiedShow Answer

What is always a characteristic of a solution that contains a buffer?

Correct AnswerverifiedShow Answer

A buffer solution contains acetic acid (HC2H3O2) at a concentration of 0.225 M and sodium acetate (NaC2H3O2) at a concentration of 0.164 M.The value of Ka for acetic acid is 1.75 × 10-5.What is the pH of this buffer solution?

Correct AnswerverifiedShow Answer

A buffer solution contains carbonic acid (H₂CO₃) and sodium bicarbonate (NaHCO₃) , each at a concentration of 0.100 M.The relevant equilibrium is shown below.What is the pH of this buffer solution? H₂CO₃(aq) + H₂O(l) H₃O⁺(aq) + HCO₃−(aq) K_a = 4.5 × 10⁻⁷

Correct Answer
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Correct Answer
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What is the pH of a 1.0 × 10⁻⁴ M solution of KOH?

Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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For the reaction shown below, which of the following correctly represents a conjugate acid-base pair? HCO₂H(aq) + H₂O(l) H₃O⁺(aq) + HCO₂−(aq)

Correct Answer
verified

Calculate the molar concentration of a sodium hydroxide solution if 60.00 mL of this solution were required to neutralize 30.00 mL of a 0.150 M hydrochloric acid solution.NaOH(aq) + HCl(aq) → NaCl(aq) + H₂O(l)

Correct Answer
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Correct Answer
verified

If the hydronium ion concentration of an aqueous solution at 25°C is 5 × 10^-6 M, what is the hydroxide ion concentration?

Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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A sample of black coffee was measured to have [H₃O⁺] = 7.94 × 10⁻⁶.What is TRUE about this solution?

Correct Answer
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Correct Answer
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A buffer solution contains acetic acid (HC₂H₃O₂) at a concentration of 0.225 M and sodium acetate (NaC₂H₃O₂) at a concentration of 0.164 M.The value of K_a for acetic acid is 1.75 × 10^-5.What is the pH of this buffer solution?

Correct Answer
verified