Question 1

A solution containing a buffer has an initial pH of 8.78.If a student adds 5 drops of NaCl(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)  8.89

Question 2

A buffer solution is prepared by placing twice the concentration of propanoic acid (C2H5COOH, Ka=1.34 ×10-5)  as the concentration of its conjugate base sodium propanoate into a flask.The pH of the resulting buffer solution is best described as which of the following?

Accepted Answer

A)  less than 4.87
B)  4.87
C)  between 4.87 and 9.00
D)  greater than 11.00
E)  Undeterminable; the concentrations of the acid and conjugate base must be given.

Question 3

Titration of 25.0 mL of an HCl solution of unknown concentration requires 14.8 mL of 0.100 M NaOH.What is the molar concentration of the HCl solution? NaOH(aq)  + HCl(aq)  → NaCl(aq)  + H2O(l)

Accepted Answer

A)  0.592 M
B)  5.87 M
C)  0.0592 M
D)  0.0692 M
E)  1.25 M

Question 4

A patient's urine sample gave a reading of 8.2.What is the value of [H3O+] in this solution?

Accepted Answer

A)  6.0 × 10-9 M
B)  0.91 M
C)  1.6 × 10-8 M
D)  1.6 × 108 M
E)  2.7 × 10-4 M

Question 5

A pH of 0 is considered neutral.

Accepted Answer

A) True 
 B)False

Question 6

What is the pH of a solution that has [H3O+] = 6.0 × 10-3 M?

Accepted Answer

A)  1.7 × 10-12
B)  2.22
C)  3.60
D)  5.12
E)  11.78

Question 7

Butyric acid is a weak acid.Which reaction equation properly represents the dissociation of butyric acid in water?

Accepted Answer

A)  CH3CH2CH2COOH(aq)  + H2O(l)  → CH3CH2CH2COO- (aq)  + H3O+(aq) 
B)  CH3CH2CH2COOH(aq)  + H2O(l)  3CH2CH2COOH(aq)  + H2O(l)  → CH3CH2CH2COO- (aq)  + H3O+(aq)  
B)  CH3CH2CH2COOH(aq)  + H2O(l)    CH3CH2CH2COO-(aq)  + H3O+(aq)  
C)  CH3CH2CH2COOH(aq)  + H2O(l)  → CH3CH2CH2COOH2+(aq)  + OH-(aq)  
D)  CH3CH2CH2COOH(aq)  + H2O(l)    CH2CH2CH2COOH(aq)  + H3O+(aq) " class="answers-bank-image d-inline" rel="preload" > CH3CH2CH2COO-(aq)  + H3O+(aq) 
C)  CH3CH2CH2COOH(aq)  + H2O(l)  → CH3CH2CH2COOH2+(aq)  + OH-(aq) 
D)  CH3CH2CH2COOH(aq)  + H2O(l)  3CH2CH2COOH(aq)  + H2O(l)  → CH3CH2CH2COO- (aq)  + H3O+(aq)  
B)  CH3CH2CH2COOH(aq)  + H2O(l)    CH3CH2CH2COO-(aq)  + H3O+(aq)  
C)  CH3CH2CH2COOH(aq)  + H2O(l)  → CH3CH2CH2COOH2+(aq)  + OH-(aq)  
D)  CH3CH2CH2COOH(aq)  + H2O(l)    CH2CH2CH2COOH(aq)  + H3O+(aq) " class="answers-bank-image d-inline" rel="preload" > CH2CH2CH2COOH(aq)  + H3O+(aq)

Question 8

The species that remains after an acid donates a proton is called its conjugate base.What is the conjugate base of the hydronium ion, H3O+?

Accepted Answer

A)  OH-
B)  H2O-
C)  H2O
D)  H2O+
E)  H3O+ has no conjugate base.

Question 9

Which of the following compounds is NOT considered a polyprotic acid?

Accepted Answer

A)  H2SO4
B)  H3PO4
C)  H2CO3
D)  H2SO3
E)  CH3COOH

Question 10

Consider two beakers, one containing 1.0 M HCl and the other containing 1.0 M CH3COOH.Which solution would have the lowest pH?

Accepted Answer

A)  1.0 M CH3COOH because its solution contains a lower hydronium ion concentration than 1.0 M HCl
B)  1.0 M HCl because its solution contains a higher hydronium ion concentration than 1.0 M CH3COOH
C)  1.0 M HCl because its solution contains a lower hydronium ion concentration than 1.0 M CH3COOH
D)  1.0 M CH3COOH because its solution contains a higher hydronium ion concentration than 1.0 M HCl
E)  Both solutions would have the same pH because they have the same concentration.

Question 11

Sodium hydroxide (NaOH)  can react with phosphoric acid (H3PO4)  in a neutralization reaction.What is the reacting ratio of NaOH to H3PO4?

Accepted Answer

A)  1:1
B)  1:3
C)  3:8
D)  2:7
E)  3:1

Question 12

What is the hydronium ion concentration of a solution with a pH of 6.0?

Accepted Answer

A)  1 × 106 M
B)  1 × 10-6 M
C)  6 × 101 M
D)  6 × 10-1 M
E)  6 × 10-14 M

Question 13

What is the conjugate acid of NH2−?

Accepted Answer

A)  NH2−
B)  NH3
C)  NH4+
D)  NH2+
E)  NH4−

Question 14

The pH of a 12.0 M solution of HCl is -1.1.

Accepted Answer

A) True 
 B)False

Question 15

All Brønsted-Lowry bases contain hydroxide.

Accepted Answer

A) True 
 B)False

Question 16

For the reaction shown below, which of the following is a conjugate acid-base pair? C5H5N(aq)  + H2O(l)  5H5N(aq)  + H2O(l)    C5H5NH+(aq)  + OH−(aq)  A) C5H5N, H2O B) C5H5N, C5H5NH+ C) C5H5NH+, OH− D) H2O, OH− E) C5H5N, C5H5NH+ and H2O, OH−" class="answers-bank-image d-inline" rel="preload" > C5H5NH+(aq)  + OH−(aq)

Accepted Answer

A)  C5H5N, H2O
B)  C5H5N, C5H5NH+
C)  C5H5NH+, OH−
D)  H2O, OH−
E)  C5H5N, C5H5NH+ and H2O, OH−

Question 17

The ion-product of water is affected by a change in temperature.

Accepted Answer

A) True 
 B)False

Question 18

Which statement concerning the relative strength of acids is FALSE?

Accepted Answer

A)  Strong and weak acids differ in their extent of proton transfer to water.
B)  Strong acids are good proton donors; weak acids are poor proton donors.
C)  A strong acid completely transfers its protons to water; a weak acid only partially transfers its protons to water.
D)  Strong acids produce strong conjugate bases; weak acids produce weak conjugate bases.
E)  A strong acid produces more hydronium ions in water than a weak acid of the same concentration.

Question 19

Which statement correctly describes conjugate acids and bases according to the Brønsted-Lowry theory?

Accepted Answer

A)  A conjugate base is the species formed when an acid donates a proton; a conjugate acid is the species formed when a base accepts a proton.
B)  A conjugate base is the species formed when an acid accepts a proton; a conjugate acid is the species formed when a base donates a proton.
C)  A conjugate acid is the species formed when an acid donates a proton; a conjugate base is the species formed when a base accepts a proton.
D)  A conjugate acid is an acid that does not completely transfer a proton to water; a conjugate base is a base that does not completely accept a proton from water.
E)  A conjugate acid is the solution formed when an acid is added to water; a conjugate base is the solution formed when a base is added to water.

Question 20

HCl is a strong electrolyte.A bottle of HCl contains the label 0.015 M HCl(aq) .Which statement concerning this HCl solution is FALSE?

Accepted Answer

A)  The solution is acidic.
B)  The pH of the solution is 1.5.
C)  The hydronium ion concentration in this solution is 0.015 M.
D)  The solution has a higher concentration of hydronium ions than hydroxide ions.
E)  The solution contains dissolved H3O+ and Cl− ions only; no HCl molecules are present.

Exam 8: Acids and Bases

A pH of 0 is considered neutral.

Correct AnswerverifiedShow Answer

For the reaction shown below, which of the following is a conjugate acid-base pair? C5H5N(aq) + H2O(l) C5H5NH+(aq) + OH−(aq)

Correct AnswerverifiedShow Answer

Butyric acid is a weak acid.Which reaction equation properly represents the dissociation of butyric acid in water?

Correct AnswerverifiedShow Answer

What is the pH of a solution that has [H3O+] = 6.0 × 10-3 M?

Correct AnswerverifiedShow Answer

Sodium hydroxide (NaOH) can react with phosphoric acid (H3PO4) in a neutralization reaction.What is the reacting ratio of NaOH to H3PO4?

Correct AnswerverifiedShow Answer

Which statement concerning the relative strength of acids is FALSE?

Correct AnswerverifiedShow Answer

A buffer solution is prepared by placing twice the concentration of propanoic acid (C2H5COOH, Ka=1.34 ×10-5) as the concentration of its conjugate base sodium propanoate into a flask.The pH of the resulting buffer solution is best described as which of the following?

Correct AnswerverifiedShow Answer

Which of the following compounds is NOT considered a polyprotic acid?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

HCl is a strong electrolyte.A bottle of HCl contains the label 0.015 M HCl(aq) .Which statement concerning this HCl solution is FALSE?

Correct AnswerverifiedShow Answer

A patient's urine sample gave a reading of 8.2.What is the value of [H3O+] in this solution?

Correct AnswerverifiedShow Answer

Titration of 25.0 mL of an HCl solution of unknown concentration requires 14.8 mL of 0.100 M NaOH.What is the molar concentration of the HCl solution? NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l)

Correct AnswerverifiedShow Answer

Consider two beakers, one containing 1.0 M HCl and the other containing 1.0 M CH3COOH.Which solution would have the lowest pH?

Correct AnswerverifiedShow Answer

The species that remains after an acid donates a proton is called its conjugate base.What is the conjugate base of the hydronium ion, H3O+?

Correct AnswerverifiedShow Answer

The pH of a 12.0 M solution of HCl is -1.1.

Correct AnswerverifiedShow Answer

All Brønsted-Lowry bases contain hydroxide.

Correct AnswerverifiedShow Answer

What is the conjugate acid of NH2−?

Correct AnswerverifiedShow Answer

The ion-product of water is affected by a change in temperature.

Correct AnswerverifiedShow Answer

Which statement correctly describes conjugate acids and bases according to the Brønsted-Lowry theory?

Correct AnswerverifiedShow Answer

What is the hydronium ion concentration of a solution with a pH of 6.0?

Correct AnswerverifiedShow Answer

Correct Answer
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For the reaction shown below, which of the following is a conjugate acid-base pair? C₅H₅N(aq) + H₂O(l) C₅H₅NH⁺(aq) + OH⁻(aq)

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What is the pH of a solution that has [H₃O⁺] = 6.0 × 10^-3 M?

Correct Answer
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Sodium hydroxide (NaOH) can react with phosphoric acid (H₃PO₄) in a neutralization reaction.What is the reacting ratio of NaOH to H₃PO₄?

Correct Answer
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A buffer solution is prepared by placing twice the concentration of propanoic acid (C₂H₅COOH, K_a=1.34 ×10^-5) as the concentration of its conjugate base sodium propanoate into a flask.The pH of the resulting buffer solution is best described as which of the following?

Correct Answer
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A patient's urine sample gave a reading of 8.2.What is the value of [H₃O⁺] in this solution?

Correct Answer
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Titration of 25.0 mL of an HCl solution of unknown concentration requires 14.8 mL of 0.100 M NaOH.What is the molar concentration of the HCl solution? NaOH(aq) + HCl(aq) → NaCl(aq) + H₂O(l)

Correct Answer
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Consider two beakers, one containing 1.0 M HCl and the other containing 1.0 M CH₃COOH.Which solution would have the lowest pH?

Correct Answer
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The species that remains after an acid donates a proton is called its conjugate base.What is the conjugate base of the hydronium ion, H₃O⁺?

Correct Answer
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What is the conjugate acid of NH₂⁻_?

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