Question 1

Which of the following statements is/are true of HCl solution?​
1)  A 1.0 M HCl solution contains H+ and Cl− ions rather than HCl molecules.2. A 1.0 M HCl solution contains 6.02 × 10−23 HCl molecules and no ions.3. In 1.0 M HCl, water produces less than 10−7 M H+ ions.

Accepted Answer

A)   1 only
B)   2 only
C)   3 only
D)   1 and 2
E)   1 and 3F) C) and D)
G) B) and E)

Question 2

Find the pH of a solution at 25°C in which [OH-] = 2.5 × 10-9 M.

Accepted Answer

A)   6.50
B)   8.60
C)   7.40
D)   2.50
E)   5.40F) A) and D)
G) D) and E)

Question 3

Given that the Ka for HOCl is 3.5 × 10-8, calculate the K value for the reaction of HOCl with OH-.

Accepted Answer

A)   3.5 × 10-22
B)   3.5 × 10-8
C)   2.9 × 10-7
D)   3.5 × 106
E)   none of theseF) A) and C)
G) B) and C)

Question 4

Calculate the pH of a 0.50 M NH3 (Kb = 1.8 × 10-5)  solution.

Accepted Answer

A)   4.78
B)   2.52
C)   7.00
D)   13.72
E)   none of theseF) A) and E)
G) None of the above

Question 5

Which of the following species is not amphoteric?

Accepted Answer

A)   H2PO4-
B)   HPO42-
C)   H2O
D)   HSO4-
E)   All of these are amphoteric.F) B) and E)
G) None of the above

Question 6

What is the pH in a solution of 1.0 M H2A (Ka1 = 1.0 × 10-6; Ka2 = 1.0 × 10-10) ?

Accepted Answer

A)   8.00
B)   3.00
C)   2.00
D)   13.00
E)   5.00F) A) and B)
G) A) and E)

Question 7

Calculate the pH of a 2.0 × 10-8 M solution of HNO3.

Accepted Answer

A)   7.70
B)   6.96
C)   7.00
D)   6.30
E)   7.04F) A) and B)
G) C) and D)

Question 8

The pH of a strong acid solution is always lower than the pH of a weak acid solution. If this is true, explain why and include an example with calculations. If it is false, explain why and include a counterexample with calculations.

Accepted Answer

A) True 
 B)False

Question 9

Calculate the pH of the following aqueous solutions. Choose your answer from the given pH ranges.
-0.5 M NH4F (pKb for NH3 = 4.74, pKa for HF = 3.14)

Accepted Answer

A)   pH 11.00-14.00
B)   pH 0.00-2.99
C)   pH 3.00-5.99
D)   pH 6.00-8.99
E)   pH 9.00-10.99F) A) and D)
G) A) and C)

Question 10

Which of the following represents a conjugate acid-base pair?

Accepted Answer

A)   H2PO4- and PO43-
B)   HNO3 and NO3-
C)   HCl and NaOH
D)   HSO4- and SO32-
E)   none of theseF) A) and B)
G) A) and C)

Question 11

Calculate the pH of 0.10 M NH4CN. (Kb for NH3 = 1.8 × 10-5; Ka for HCN = 6.2 × 10-10)

Accepted Answer

A)   5.79
B)   8.21
C)   8.87
D)   5.13
E)   9.23F) B) and C)
G) A) and C)

Question 12

A 2.98-g sample of NaOH(s)  is added to enough water to make 300.0 mL of solution at 25°C. What is the pH of this solution?

Accepted Answer

A)   10.40
B)   0.60
C)   13.40
D)   15.00
E)   12.35F) B) and E)
G) A) and D)

Question 13

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid potassium chloride (KCl)

Accepted Answer

A)   acidic
B)   neutral
C)   basicD) None of the above
E) B) and C)

Question 14

A solution is made by mixing equal volumes of 0.20 M HCN (Ka = 6.2 × 10-10) and 0.20 M NH3 (Kb = 1.8 × 10-5). Determine the pH of the solution.

Accepted Answer

Question 15

The conjugate base of a weak acid is

Accepted Answer

A)   a strong base.
B)   a strong acid.
C)   a weak base.
D)   a weak acid.
E)   none of theseF) D) and E)
G) None of the above

Question 16

Which of the following species is present in the greatest concentration in a 0.100 M H2SO4 solution in H2O?

Accepted Answer

A)   H2SO4
B)   H3O+
C)   All species are in equilibrium and therefore have the same concentration.
D)   HSO4-
E)   SO42-F) A) and D)
G) A) and B)

Question 17

Which of the species below, when dissolved in H2O, will not produce a basic solution?

Accepted Answer

A)   Ba(OH) 2
B)   NH3
C)   SO2
D)   BaO
E)   none of these; that is, they all will produce a basic solutionF) A) and C)
G) A) and B)

Question 18

Calculate the percentage of pyridine (C5H5N)  that forms pyridinium ion, C5H5NH+, in a 0.10 M aqueous solution of pyridine (Kb = 1.7 × 10-9) .

Accepted Answer

A)   0.77%
B)   0.060%
C)   0.0060%
D)   1.6%
E)   0.013%F) B) and E)
G) None of the above

Question 19

Calculate [OH-] in a 4.0 × 10-8 M solution of NaOH.

Accepted Answer

A)   8.2 × 10-8 M
B)   6.7 × 10-6 M
C)   2.5 × 10-7 M
D)   4.0 × 10-8 M
E)   1.2 × 10-7 MF) C) and D)
G) B) and D)

Question 20

The acids HC2H3O2 and HF are both weak, but HF is a stronger acid than HC2H3O2. HCl is a strong acid. Order the following according to base strength.

Accepted Answer

A)   Cl- > F- > C2H3O2- > H2O
B)   C2H3O2- > F- > H2O > Cl-
C)   C2H3O2- > F- > Cl- > H2O
D)   F- > C2H3O2- > H2O > Cl-
E)   none of theseF) C) and E)
G) B) and C)

Exam 7: Acids and Bases

If the following substance is dissolved in pure water, will the solution be acidic, neutral, or basic? solid potassium chloride (KCl)

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Calculate the percentage of pyridine (C5H5N) that forms pyridinium ion, C5H5NH+, in a 0.10 M aqueous solution of pyridine (Kb = 1.7 × 10-9) .

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The acids HC2H3O2 and HF are both weak, but HF is a stronger acid than HC2H3O2. HCl is a strong acid. Order the following according to base strength.

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Given that the Ka for HOCl is 3.5 × 10-8, calculate the K value for the reaction of HOCl with OH-.

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The pH of a strong acid solution is always lower than the pH of a weak acid solution. If this is true, explain why and include an example with calculations. If it is false, explain why and include a counterexample with calculations.

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Find the pH of a solution at 25°C in which [OH-] = 2.5 × 10-9 M.

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Calculate [OH-] in a 4.0 × 10-8 M solution of NaOH.

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Which of the species below, when dissolved in H2O, will not produce a basic solution?

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Calculate the pH of the following aqueous solutions. Choose your answer from the given pH ranges. -0.5 M NH4F (pKb for NH3 = 4.74, pKa for HF = 3.14)

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Which of the following species is not amphoteric?

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Which of the following statements is/are true of HCl solution?​ 1) A 1.0 M HCl solution contains H+ and Cl− ions rather than HCl molecules.2. A 1.0 M HCl solution contains 6.02 × 10−23 HCl molecules and no ions.3. In 1.0 M HCl, water produces less than 10−7 M H+ ions.

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A solution is made by mixing equal volumes of 0.20 M HCN (Ka = 6.2 × 10-10) and 0.20 M NH3 (Kb = 1.8 × 10-5). Determine the pH of the solution.

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Calculate the pH of a 2.0 × 10-8 M solution of HNO3.

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A 2.98-g sample of NaOH(s) is added to enough water to make 300.0 mL of solution at 25°C. What is the pH of this solution?

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Which of the following species is present in the greatest concentration in a 0.100 M H2SO4 solution in H2O?

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What is the pH in a solution of 1.0 M H2A (Ka1 = 1.0 × 10-6; Ka2 = 1.0 × 10-10) ?

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Calculate the pH of 0.10 M NH4CN. (Kb for NH3 = 1.8 × 10-5; Ka for HCN = 6.2 × 10-10)

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Calculate the pH of a 0.50 M NH3 (Kb = 1.8 × 10-5) solution.

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Which of the following represents a conjugate acid-base pair?

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The conjugate base of a weak acid is

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Calculate the percentage of pyridine (C₅H₅N) that forms pyridinium ion, C₅H₅NH⁺, in a 0.10 M aqueous solution of pyridine (K_b = 1.7 × 10^-9) .

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The acids HC₂H₃O₂ and HF are both weak, but HF is a stronger acid than HC₂H₃O₂. HCl is a strong acid. Order the following according to base strength.

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Given that the K_a for HOCl is 3.5 × 10^-8, calculate the K value for the reaction of HOCl with OH^-.

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Find the pH of a solution at 25°C in which [OH^-] = 2.5 × 10^-9 M.

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Calculate [OH^-] in a 4.0 × 10^-8 M solution of NaOH.

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Which of the species below, when dissolved in H₂O, will not produce a basic solution?

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Calculate the pH of the following aqueous solutions. Choose your answer from the given pH ranges. -0.5 M NH₄F (pK_b for NH₃ = 4.74, pK_a for HF = 3.14)

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Which of the following statements is/are true of HCl solution? 1) A 1.0 M HCl solution contains H⁺ and Cl⁻ ions rather than HCl molecules.2. A 1.0 M HCl solution contains 6.02 × 10⁻²³ HCl molecules and no ions.3. In 1.0 M HCl, water produces less than 10⁻⁷ M H⁺ ions.

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A solution is made by mixing equal volumes of 0.20 M HCN (K_a = 6.2 × 10^-10) and 0.20 M NH₃ (K_b = 1.8 × 10^-5). Determine the pH of the solution.

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Calculate the pH of a 2.0 × 10^-8 M solution of HNO₃.

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Which of the following species is present in the greatest concentration in a 0.100 M H₂SO₄ solution in H₂O?

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What is the pH in a solution of 1.0 M H₂A (K_a1 = 1.0 × 10^-6; K_a2 = 1.0 × 10^-10) ?

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Calculate the pH of 0.10 M NH₄CN. (K_b for NH₃ = 1.8 × 10^-5; K_a for HCN = 6.2 × 10^-10)

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Calculate the pH of a 0.50 M NH₃ (K_b = 1.8 × 10^-5) solution.

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