Question 1

What is the pH of a 0.375 M solution of benzoic acid? Ka = 6.3 × 10-5

Accepted Answer

A)   8.9
B)   5.1
C)   2.3
D)   0.43
E)   11.7F) A) and E)
G) B) and D)

Question 2

Which of the following statements concerning aqueous solutions of salts is FALSE?

Accepted Answer

A)   For any salt of a strong acid and a strong base, the pH will be about 7.
B)   For any salt of a strong acid and a weak base, the pH will be 
C)   For any salt of a weak acid and a strong base, the pH will be >7.
D)   For any salt of a weak acid and a weak base, the pH will be about 7.E) None of the above
F) All of the above

Question 3

What is the [HPO4-2] of a solution labeled "0.10 M Phosphoric Acid"? [Ka1 = 7.1 × 10-3; Ka2 = 6.3 × 10-8; Ka3 = 4.2 × 10-13]

Accepted Answer

A)   4.2 × 10-13 M
B)   6.3 × 10-8 M
C)   7.1 × 10-3 M
D)   1.6 × 10-9 M
E)   1.6 × 10-16 MF) A) and E)
G) None of the above

Question 4

What is the concentration of free sulfate ion in a solution labeled "3.6M H2SO4"? [Ka2 = 1.1 × 10-2]

Accepted Answer

A)   0.011 M
B)   0.040 M
C)   0.20 M
D)   0.60 M
E)   1.8 MF) A) and C)
G) A) and B)

Question 5

For which of the following polyprotic acids is the first ionization step approximately 100%?

Accepted Answer

A)   H2S
B)   H2SO3
C)   H2CO3
D)   H2SO4
E)   H3PO4F) A) and D)
G) C) and D)

Question 6

For the following compound, predict whether the solution is acidic, basic or neutral and why: Na2CO3.

Accepted Answer

A)   acidic because Na2CO3 is a strong acid
B)   basic because Na2CO3 is a weak base
C)   neutral because there is no hydrolysis
D)   basic because Na2CO3 is the salt of a weak acid
E)   acidic because Na2CO3 is the salt of a weak baseF) C) and E)
G) C) and D)

Question 7

A solution has pOH of -0.47. This means that:

Accepted Answer

A)   the solution has a pH of 13.53
B)   the solution has an [OH-] = 0.34 M
C)   the solution has an [OH-] greater than 10.0 M
D)   the solution has an [OH-] = 2.95 M
E)   The solution has an [H+] = 2.95 MF) A) and D)
G) None of the above

Question 8

A 0.632 M solution of a monoprotic base has a pH of 11.53. What is the ionization constant of this base?

Accepted Answer

A)   1.8 × 10-5
B)   2.1 × 10-3
C)   1.6 × 10-23
D)   5.0 × 10-12
E)   5.3 × 10-3F) D) and E)
G) A) and D)

Question 9

What is the pH of a 0.240 M solution of potassium cyanide? Ka (HCN)  = 6.2 × 10-10

Accepted Answer

A)   11.3
B)   2.7
C)   4.9
D)   9.1
E)   9.4F) None of the above
G) B) and E)

Question 10

A 0.505 g sample of a monoprotic base (mm = 45.09 g/mol)  was dissolved in water to produce 100.0 mL of solution with a pH = 11.84. What is the ionization constant of this base?

Accepted Answer

A)   4.3 × 10-5
B)   1.9 × 10-23
C)   4.3 × 10-4
D)   3.4 × 10-1
E)   1.3 × 10-11F) B) and D)
G) A) and B)

Question 11

List the following acids in order of increasing strength: 
HClO2   &emsp;HClO3   &emsp;HClO4

Accepted Answer

A)   HClO2 4 3
B)   HClO4 3 2
C)   HClO4 2 3
D)   HClO3 2 4E) A) and B)
F) B) and D)

Question 12

Which of the following are Br∅nsted-Lowry acid? 
I. CH3COOH
II. [Cu(H2O) 4]2+
III. H2O
IV. CH3NH2
V. H3O+

Accepted Answer

A)   I) , II)  and III) 
B)   II) , III) , and IV) 
C)   I) , II) , III)  and IV) 
D)   I) , II) , III) , and V) 
E)   II) , III)  and V) F) A) and B)
G) C) and E)

Question 13

A 0.0925 g sample of a monoprotic base (mm = 17.03 g/mol)  was dissolved in water to produce 100 mL of solution with a pH = 11.00. What is the ionization constant of this base?

Accepted Answer

A)   1.8 × 10-6
B)   1.8 × 10-11
C)   1.8 × 10-21
D)   1.9 × 10-5
E)   1.1 × 10-6F) B) and E)
G) C) and E)

Question 14

In the following reversible reaction the Br∅nsted acids are ________. HCO3-(aq)  + OH-(aq)  ⇌ CO32-(aq)  + H2O

Accepted Answer

A)   HCO3- and H2O
B)   HCO3- and CO32-
C)   OH- and CO32-
D)   OH- and H2O
E)   H2O and CO32-F) A) and D)
G) C) and D)

Question 15

At 25°C, the pH of pure water is:

Accepted Answer

A)   0
B)   >0, 
C)   7
D)   >7, 
E)   14F) A) and E)
G) B) and D)

Question 16

What is the [AsO43-] for a solution labeled 0.10 M arsenic acid (H3AsO4) ? [Ka1 = 6 × 10-3, Ka2 = 1 × 10-7, Ka3 = 3 × 10-12]

Accepted Answer

A)   1 × 10-7 M
B)   1 × 10-17 M
C)   3 × 10-12 M
D)   3 × 10-19 M
E)   6 × 10-10 MF) B) and E)
G) A) and B)

Question 17

Choose the INCORRECT statement.

Accepted Answer

A)   H2SO4, HCl, and HNO3 all form H3O+ when reacted with H2O.
B)   Neutralization takes place when the hydronium ion reacts with the hydroxide ion to form water.
C)   Br nsted and Lowry suggested that bases be defined as proton acceptors.
D)   The odor that is noticeable when the stopper is removed from a bottle of aqueous ammonia is good evidence of the strength of the substance as a base.
E)   Br nsted and Lowry suggested that acids be defined as proton donors.F) A) and B)
G) B) and D)

Question 18

What is the [H2PO4-] of a solution labeled "0.10 M Phosphoric Acid"? [Ka1 = 7.1 × 10-3; Ka2 = 6.3 × 10-8; Ka3 = 4.2 × 10-13]

Accepted Answer

A)   0.023 M
B)   6.3 × 10-8 M
C)   7.1 × 10-3 M
D)   4.2 × 10-13 M
E)   0.013 MF) All of the above
G) A) and E)

Question 19

Choose the Br∅nsted-Lowry acids and bases in the following equation: NH4+ + OH- ⇌ H2O + NH3

Accepted Answer

A)   acids NH4+, OH- bases H2O, NH3
B)   acids OH-, H2O bases NH3, NH4+
C)   acids NH4+, OH- bases NH4+, H2O
D)   acids NH4+, H2O bases OH-, NH3
E)   acids NH4+, NH3 bases OH-, H2OF) None of the above
G) A) and B)

Question 20

The pH of a solution of NH4C2H3O2 is approximately 7. The best explanation is:

Accepted Answer

A)   This salt does not react with water.
B)   Ammonium acetate is a weak electrolyte.
C)   All salts of weak acids and weak bases are neutral.
D)   Aqueous ammonia and acetic acid have approximately equal ionization constants.
E)   The salt is a product of a strong acid and a strong base.F) A) and C)
G) B) and C)

Exam 16: Acids and Bases

What is the pH of a 0.375 M solution of benzoic acid? Ka = 6.3 × 10-5

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Which of the following statements concerning aqueous solutions of salts is FALSE?

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Choose the Br∅nsted-Lowry acids and bases in the following equation: NH4+ + OH- ⇌ H2O + NH3

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What is the concentration of free sulfate ion in a solution labeled "3.6M H2SO4"? [Ka2 = 1.1 × 10-2]

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At 25°C, the pH of pure water is:

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A 0.505 g sample of a monoprotic base (mm = 45.09 g/mol) was dissolved in water to produce 100.0 mL of solution with a pH = 11.84. What is the ionization constant of this base?

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A 0.0925 g sample of a monoprotic base (mm = 17.03 g/mol) was dissolved in water to produce 100 mL of solution with a pH = 11.00. What is the ionization constant of this base?

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Choose the INCORRECT statement.

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In the following reversible reaction the Br∅nsted acids are ________. HCO3-(aq) + OH-(aq) ⇌ CO32-(aq) + H2O

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A solution has pOH of -0.47. This means that:

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What is the [HPO4-2] of a solution labeled "0.10 M Phosphoric Acid"? [Ka1 = 7.1 × 10-3; Ka2 = 6.3 × 10-8; Ka3 = 4.2 × 10-13]

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What is the [AsO43-] for a solution labeled 0.10 M arsenic acid (H3AsO4) ? [Ka1 = 6 × 10-3, Ka2 = 1 × 10-7, Ka3 = 3 × 10-12]

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List the following acids in order of increasing strength: HClO2 HClO3 HClO4

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The pH of a solution of NH4C2H3O2 is approximately 7. The best explanation is:

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What is the [H2PO4-] of a solution labeled "0.10 M Phosphoric Acid"? [Ka1 = 7.1 × 10-3; Ka2 = 6.3 × 10-8; Ka3 = 4.2 × 10-13]

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For which of the following polyprotic acids is the first ionization step approximately 100%?

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For the following compound, predict whether the solution is acidic, basic or neutral and why: Na2CO3.

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What is the pH of a 0.240 M solution of potassium cyanide? Ka (HCN) = 6.2 × 10-10

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Which of the following are Br∅nsted-Lowry acid? I. CH3COOH II. [Cu(H2O) 4]2+ III. H2O IV. CH3NH2 V. H3O+

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A 0.632 M solution of a monoprotic base has a pH of 11.53. What is the ionization constant of this base?

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What is the pH of a 0.375 M solution of benzoic acid? Ka = 6.3 × 10^-5

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Choose the Br∅nsted-Lowry acids and bases in the following equation: NH₄⁺ + OH- ⇌ H₂O + NH₃

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What is the concentration of free sulfate ion in a solution labeled "3.6M H₂SO₄"? [Ka2 = 1.1 × 10^-2]

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In the following reversible reaction the Br∅nsted acids are ________. HCO₃^-(aq) + OH-(aq) ⇌ CO₃^2-(aq) + H₂O

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What is the [HPO₄^-2] of a solution labeled "0.10 M Phosphoric Acid"? [Ka1 = 7.1 × 10^-3; Ka₂ = 6.3 × 10^-8; Ka₃ = 4.2 × 10^-13]

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What is the [AsO₄^3-] for a solution labeled 0.10 M arsenic acid (H₃AsO₄) ? [Ka1 = 6 × 10^-3, Ka₂ = 1 × 10^-7, Ka₃= 3 × 10^-12]

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List the following acids in order of increasing strength: HClO₂ HClO₃ HClO₄

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The pH of a solution of NH₄C₂H₃O₂ is approximately 7. The best explanation is:

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What is the [H₂PO₄^-] of a solution labeled "0.10 M Phosphoric Acid"? [Ka1 = 7.1 × 10^-3; Ka2 = 6.3 × 10^-8; Ka3 = 4.2 × 10^-13]

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For the following compound, predict whether the solution is acidic, basic or neutral and why: Na₂CO₃.

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What is the pH of a 0.240 M solution of potassium cyanide? Ka (HCN) = 6.2 × 10^-10

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Which of the following are Br∅nsted-Lowry acid? I. CH₃COOH II. [Cu(H₂O) ₄]²⁺ III. H₂O IV. CH₃NH₂ V. H₃O+

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