Question 1

Calculate the hydronium ion concentration in an aqueous solution with a pOH of 9.85 at 25°C.

Accepted Answer

A)   7.1 × 10-5 M
B)   4.2 × 10-10 M
C)   8.7 × 10-10 M
D)   6.5 × 10-5 M
E)   1.4 × 10-10 M

Question 2

Identify the acid that is used to preserve soft drinks.

Accepted Answer

A)   citric acid
B)   hydrochloric acid
C)   carbonic acid
D)   hydrofluoric acid
E)   phosphoric acid

Question 3

Determine the pH of a 0.461 M C6H5CO2H M solution if the Ka of C6H5CO2H is 6.5 × 10-5.

Accepted Answer

A)   2.26
B)   4.52
C)   11.74
D)   9.48
E)   5.48

Question 4

Identify the acid that is in car batteries.

Accepted Answer

A)   H2SO4
B)   HNO3
C)   Na2CO3
D)   CH3COOH
E)   HCl A

Question 5

Identify the substance that is NOT acidic.

Accepted Answer

A)   soft drink
B)   apple
C)   household ammonia
D)   lemon
E)   plum

Question 6

Which Br∅nsted-Lowry acid is NOT considered to be a strong acid in water?

Accepted Answer

A)   HBr
B)   HBr 
C)   HNO2
D)   HNO3

Question 7

Calculate the concentration of bicarbonate ion,HCO3-,in a 0.010 M H2CO3 solution that has the stepwise dissociation constants Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

Accepted Answer

A)   6.6 × 10-5 M
B)   4.3 × 10-7 M
C)   4.3 × 10-9 M
D)   5.6 × 10-11 M

Question 8

What is the pH of a 0.30 M pyridine solution that has Kb = 1.9 × 10-9? The equation for the dissociation of pyridine is: C5H5N(aq) + H2O(l) ⇌ C5H5NH+(aq) + OH-(aq)

Accepted Answer

A)   4.62
B)   8.72
C)   9.38
D)   10.38

Question 9

What is the pH of pure water at 40.0°C if the Kw at this temperature is 2.92 × 10-14?

Accepted Answer

A)   6.767
B)   0.465
C)   7.000
D)   7.233
E)   8.446

Question 10

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

Accepted Answer

A)   (CH3CH2) 2NH, 8.6 × 10-4
B)   CH3NH2, 4.4 × 10-4
C)   C6H5NH2, 4.0 × 10-10
D)   NH3, 1.76 × 10-5
E)   C5H5N, 1.7 × 10-9

Question 11

Carbon dioxide combines with rainwater to form

Accepted Answer

A)   phosphoric acid.
B)   carbonic acid.
C)   nitric acid.
D)   sulfuric acid.
E)   nitrous acid. B

Question 12

Which of the following is an Arrhenius base?

Accepted Answer

A)   CH3CO2H
B)   RbOH
C)   CH3OH
D)   KBr
E)   More than one of these compounds is an Arrhenius base. B

Question 13

Determine the concentration of CO32- ions in 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)   2.8 × 10-4 M
B)   3.2 × 10-6 M
C)   5.6 × 10-11 M
D)   4.3 × 10-7 M
E)   6.9 × 10-8 M

Question 14

Calculate the pH of a 1.60 M KBrO solution.Ka for hypobromous acid,HBrO,is a for hypobromous acid,HBrO,is   A)  2.55 B)  4.25 C)  9.75 D)  11.45" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   2.55
B)   4.25
C)   9.75
D)   11.45

Question 15

Which one of the following will form an acidic solution in water?

Accepted Answer

A)   NH4Cl
B)   LiF
C)   NaI
D)   LiNO3
E)   None of the above solutions will be acidic.

Question 16

Find the percent ionization of a 0.337 M HF solution.The Ka for HF is 3.5 × 10-4.

Accepted Answer

A)   1.1%
B)   1.2 × 10-2%
C)   3.2%
D)   3.5 × 10-2%
E)   4.7%

Question 17

The stronger the acid,then which of the following is TRUE?

Accepted Answer

A)   the stronger the conjugate acid
B)   the stronger the conjugate base
C)   the weaker the conjugate base
D)   the weaker the conjugate acid
E)   none of the above

Question 18

Determine the [H3O⁺] in a 0.265 M HClO solution.The Ka of HClO is 2.9 × 10-8.

Accepted Answer

A)   1.1 × 10-10 M
B)   7.7 × 10-9 M
C)   1.3 × 10-6 M
D)   4.9 × 10-4 M
E)   8.8 × 10-5 M

Question 19

A solution with a hydrogen ion concentration of 3.25 × 10-6 M is ________ and has a hydroxide ion concentration of ________.

Accepted Answer

A)   acidic, 3.08 × 10-8 M
B)   acidic, 3.08 × 10-9 M
C)   basic, 3.08 × 10-8 M
D)   basic, 3.08 × 10-9 M

Question 20

Which of the following solutions would have the highest pH? Assume that they are all 0.10 M in acid at 25∘C.The acid is followed by its Ka value.

Accepted Answer

A)   HF, 3.5 × 10-4
B)   HCN, 4.9 × 10-10
C)   HNO2, 4.6 × 10-4
D)   HCHO2, 1.8 × 10-4
E)   HClO2, 1.1 × 10-2

Exam 16: Acids and Bases

Calculate the hydronium ion concentration in an aqueous solution with a pOH of 9.85 at 25°C.

Correct AnswerverifiedShow Answer

Identify the acid that is used to preserve soft drinks.

Correct AnswerverifiedShow Answer

Determine the pH of a 0.461 M C6H5CO2H M solution if the Ka of C6H5CO2H is 6.5 × 10-5.

Correct AnswerverifiedShow Answer

Identify the acid that is in car batteries.

Correct AnswerverifiedA

Identify the substance that is NOT acidic.

Correct AnswerverifiedShow Answer

Which Br∅nsted-Lowry acid is NOT considered to be a strong acid in water?

Correct AnswerverifiedShow Answer

Calculate the concentration of bicarbonate ion,HCO3-,in a 0.010 M H2CO3 solution that has the stepwise dissociation constants Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

Correct AnswerverifiedShow Answer

What is the pH of a 0.30 M pyridine solution that has Kb = 1.9 × 10-9? The equation for the dissociation of pyridine is: C5H5N(aq) + H2O(l) ⇌ C5H5NH+(aq) + OH-(aq)

Correct AnswerverifiedShow Answer

What is the pH of pure water at 40.0°C if the Kw at this temperature is 2.92 × 10-14?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Carbon dioxide combines with rainwater to form

Correct AnswerverifiedB

Which of the following is an Arrhenius base?

Correct AnswerverifiedB

Determine the concentration of CO32- ions in a 0.18 M H2CO3 solution.Carbonic acid is a diprotic acid whose Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

Correct AnswerverifiedShow Answer

Calculate the pH of a 1.60 M KBrO solution.Ka for hypobromous acid,HBrO,is

Correct AnswerverifiedShow Answer

Which one of the following will form an acidic solution in water?

Correct AnswerverifiedShow Answer

Find the percent ionization of a 0.337 M HF solution.The Ka for HF is 3.5 × 10-4.

Correct AnswerverifiedShow Answer

The stronger the acid,then which of the following is TRUE?

Correct AnswerverifiedShow Answer

Determine the [H3O⁺] in a 0.265 M HClO solution.The Ka of HClO is 2.9 × 10-8.

Correct AnswerverifiedShow Answer

A solution with a hydrogen ion concentration of 3.25 × 10-6 M is ________ and has a hydroxide ion concentration of ________.

Correct AnswerverifiedShow Answer

Which of the following solutions would have the highest pH? Assume that they are all 0.10 M in acid at 25∘C.The acid is followed by its Ka value.

Correct AnswerverifiedShow Answer

Correct Answer
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Determine the pH of a 0.461 M C₆H₅CO₂H M solution if the K_a of C₆H₅CO₂H is 6.5 × 10^-5.

Correct Answer
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A

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Calculate the concentration of bicarbonate ion,HCO₃^-,in a 0.010 M H₂CO₃ solution that has the stepwise dissociation constants K_a1 = 4.3 × 10^-7 and K_a2 = 5.6 × 10^-11.

Correct Answer
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What is the pH of a 0.30 M pyridine solution that has K_b = 1.9 × 10^-9? The equation for the dissociation of pyridine is: C₅H₅N(aq) + H₂O(l) ⇌ C₅H₅NH⁺(aq) + OH^-(aq)

Correct Answer
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What is the pH of pure water at 40.0°C if the K_w at this temperature is 2.92 × 10^-14?

Correct Answer
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Which of the following bases is the strongest? The base is followed by its K_bvalue.

Correct Answer
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B

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B

Determine the concentration of CO₃^2- ions in 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.

Correct Answer
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Calculate the pH of a 1.60 M KBrO solution.K_a for hypobromous acid,HBrO,is

Correct Answer
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Correct Answer
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Find the percent ionization of a 0.337 M HF solution.The K_a for HF is 3.5 × 10^-4.

Correct Answer
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Determine the [H₃O⁺] in a 0.265 M HClO solution.The K_a of HClO is 2.9 × 10^-8.

Correct Answer
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A solution with a hydrogen ion concentration of 3.25 × 10^-6 M is and has a hydroxide ion concentration of .

Correct Answer
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Which of the following solutions would have the highest pH? Assume that they are all 0.10 M in acid at 25^∘C.The acid is followed by its K_a value.

Correct Answer
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