Question 1

Identify the diprotic acid.

Accepted Answer

A)   HNO3
B)   HBr
C)   CH3COOH
D)   H2SO3
E)   HClO3F) B) and D)
G) B) and E)

Question 2

Determine the pH of a 0.18 M H2CO3 solution.Carbonic acid is a diprotic acid whose Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

Accepted Answer

A)   11.00
B)   10.44
C)   5.50
D)   4.31
E)   3.56F) B) and E)
G) A) and E)

Question 3

Identify the acid that is in vinegar.

Accepted Answer

A)   H2SO4
B)   NaHCO3
C)   Rb2CO3
D)   CH3COOH
E)   HIF) B) and C)
G) A) and B)

Question 4

Calculate the concentration of H3O⁺ in a solution that contains 5.5 × 10-5 M OH⁻ at 25°C.Identify the solution as acidic,basic,or neutral.

Accepted Answer

A)   1.8 × 10-10 M, basic
B)   1.8 × 10-10 M, acidic
C)   5.5 × 10-10 M, neutral
D)   9.2 × 10-1 M, acidic
E)   9.2 × 10-1 M, basicF) A) and D)
G) A) and E)

Question 5

Calculate the hydronium ion concentration in an aqueous solution with a pH of 4.33 at 25°C.

Accepted Answer

A)   2.1 × 10-10 M
B)   9.7 × 10-10 M
C)   4.7 × 10-5 M
D)   3.8 × 10-5 M
E)   6.3 × 10-6 MF) A) and B)
G) D) and E)

Question 6

The acid-dissociation constant of hydrocyanic acid (HCN) at 25.0°C is 4.9 × 10-10.What is the pH of an aqueous solution of 0.080 M sodium cyanide (NaCN) ?

Accepted Answer

A)   11.11
B)   2.89
C)   1.3 × 10-3
D)   7.8 × 10-12
E)   3.9 × 10-11F) D) and E)
G) C) and D)

Question 7

Calculate the hydroxide ion concentration in an aqueous potassium hydroxide solution that contains 3.50 × 10-6 M in hydronium ion.

Accepted Answer

A)   2.86 × 10-1 M
B)   2.86 × 10-8 M
C)   2.86 × 10-9 M
D)   3.50 × 10-9 M
E)   3.50 × 10-6 MF) A) and D)
G) A) and C)

Question 8

Which of the following bases is the weakest? The base is followed by its Kb value.

Accepted Answer

A)   HOCH2CH2NH2, 3.2 × 10-5
B)   NH3, 1.76 × 10-5
C)   C5H5N, 1.7 × 10-9
D)   (CH3CH2) 3N, 5.2 × 10-4
E)   Since these are all weak bases, they have the same strength.F) A) and D)
G) B) and E)

Question 9

The Lewis model describes the transfer of

Accepted Answer

A)   one neutron.
B)   protons.
C)   electron pairs.
D)   neutrons.
E)   one electron.F) B) and D)
G) C) and D)

Question 10

What is the concentration of hydroxide ions in pure water at 30.0∘C,if Kw at this temperature is 1.47 × 10-14?

Accepted Answer

A)   1.00 × 10-7 M
B)   1.30 × 10-7 M
C)   1.47 × 10-7 M
D)   8.93 × 10-8 M
E)   1.21 × 10-7 MF) A) and B)
G) A) and C)

Question 11

Which one of the following salts,when dissolved in water,produces the solution with the highest pH?

Accepted Answer

A)   RbI
B)   RbBr
C)   RbCl
D)   RbFE) All of the above
F) None of the above

Question 12

Identify the strongest acid.

Accepted Answer

A)   1.00 M HCOOH
B)   1.00 M CH3COOH
C)   1.00 M HCl
D)   1.00 M HClO
E)   1.00 M HFF) B) and C)
G) C) and E)

Question 13

What is the conjugate acid of HCO3⁻ ?

Accepted Answer

A)   H3O+
B)   H2O
C)   CO32-
D)   OH⁻
E)   H2CO3F) C) and E)
G) D) and E)

Question 14

If an equal number of moles of the weak acid HF and the strong base NaOH are added to water,is the resulting solution acidic,basic,or neutral?

Accepted Answer

A)   acidic
B)   basic
C)   neutral
D)   There is insufficient information provided to answer this question.E) None of the above
F) A) and C)

Question 15

Identify the acid in citrus fruits.

Accepted Answer

A)   citric acid
B)   hydrochloric acid
C)   carbonic acid
D)   hydrofluoric acid
E)   phosphoric acidF) A) and E)
G) All of the above

Question 16

Which of the following is a polyprotic acid?

Accepted Answer

A)   HBr
B)   H2SO4
C)   KCN
D)   CF4
E)   HC2H3O2F) B) and D)
G) D) and E)

Question 17

Calculate the pH of a 0.800 M NaCH3CO2 solution.Ka for acetic acid,CH3CO2H,is 1.8 × 10-5.

Accepted Answer

A)   2.42
B)   4.68
C)   9.32
D)   11.58E) A) and B)
F) A) and C)

Question 18

Which of the following is a Lewis acid?

Accepted Answer

A)   AlI3
B)   CF4
C)   NH3
D)   CHI3
E)   None of the above is a Lewis acid.F) D) and E)
G) B) and D)

Question 19

Calculate the pH for an aqueous solution of pyridine that contains 2.15 × 10-4 M hydroxide ion.

Accepted Answer

A)   4.65 × 10-11
B)   2.15 × 10-4 
C)   3.67
D)   10.33E) B) and C)
F) All of the above

Question 20

Which of the following is a triprotic acid?

Accepted Answer

A)   HBr
B)   H2SO4
C)   H3PO4
D)   CI4
E)   HC2H3O2F) C) and D)
G) A) and B)

Exam 16: Acids and Bases

Determine the pH of a 0.18 M H2CO3 solution.Carbonic acid is a diprotic acid whose Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

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What is the conjugate acid of HCO3⁻ ?

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Identify the strongest acid.

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The Lewis model describes the transfer of

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Which of the following is a polyprotic acid?

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Which of the following is a Lewis acid?

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Which one of the following salts,when dissolved in water,produces the solution with the highest pH?

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Calculate the pH of a 0.800 M NaCH3CO2 solution.Ka for acetic acid,CH3CO2H,is 1.8 × 10-5.

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Calculate the hydronium ion concentration in an aqueous solution with a pH of 4.33 at 25°C.

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Calculate the hydroxide ion concentration in an aqueous potassium hydroxide solution that contains 3.50 × 10-6 M in hydronium ion.

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What is the concentration of hydroxide ions in pure water at 30.0∘C,if Kw at this temperature is 1.47 × 10-14?

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Identify the acid that is in vinegar.

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Calculate the concentration of H3O⁺ in a solution that contains 5.5 × 10-5 M OH⁻ at 25°C.Identify the solution as acidic,basic,or neutral.

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Identify the acid in citrus fruits.

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Which of the following is a triprotic acid?

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Calculate the pH for an aqueous solution of pyridine that contains 2.15 × 10-4 M hydroxide ion.

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Identify the diprotic acid.

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Which of the following bases is the weakest? The base is followed by its Kb value.

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If an equal number of moles of the weak acid HF and the strong base NaOH are added to water,is the resulting solution acidic,basic,or neutral?

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The acid-dissociation constant of hydrocyanic acid (HCN) at 25.0°C is 4.9 × 10-10.What is the pH of an aqueous solution of 0.080 M sodium cyanide (NaCN) ?

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Determine the pH of a 0.18 M H₂CO₃ solution.Carbonic acid is a diprotic acid whose K_a1 = 4.3 × 10^-7 and K_a2 = 5.6 × 10^-11.

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What is the conjugate acid of HCO₃⁻ ?

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Calculate the pH of a 0.800 M NaCH₃CO₂ solution.K_a for acetic acid,CH₃CO₂H,is 1.8 × 10^-⁵.

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Calculate the hydroxide ion concentration in an aqueous potassium hydroxide solution that contains 3.50 × 10^-6 M in hydronium ion.

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What is the concentration of hydroxide ions in pure water at 30.0^∘C,if K_w at this temperature is 1.47 × 10^-14?

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Calculate the concentration of H₃O⁺ in a solution that contains 5.5 × 10^-5 M OH⁻ at 25°C.Identify the solution as acidic,basic,or neutral.

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Calculate the pH for an aqueous solution of pyridine that contains 2.15 × 10^-⁴M hydroxide ion.

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Which of the following bases is the weakest? The base is followed by its K_b value.

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If an equal number of moles of the weak acid HFand the strong base NaOH are added to water,is the resulting solution acidic,basic,or neutral?

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The acid-dissociation constant of hydrocyanic acid (HCN) at 25.0°C is 4.9 × 10^-1⁰.What is the pH of an aqueous solution of 0.080 M sodium cyanide (NaCN) ?

Correct Answer
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