Q: What is the correct equilibrium expression for the ion-product constant of water ($$K_w) at 25$$°C?

$$K_w = [H^+][OH^-] = 1.0 \times 10$$^{-14}$$

Q: A solution has a pH of 4.70. What is the concentration of $$[H_3O^+] in $$this solution?

$$[H_3O^+] = 2.0 \times 10$$^{-5}$$ \text{ M}$$

Q: What is the correct formula for calculating % ionization of a weak acid?

$$\text{% ionization} = \frac{[H_3O^+]_{eq}}{[HA]_i} \times 100$$

Q: If $$K_w = 1.0 \times 10$$^{-14}$$ at 25°C, what is the concentration of $$[OH^-]$$ in a neutral solution?

$$[OH^-] = 1.0 \times 10$$^{-7}$$ M

Question 1

Which of the following best describes an Arrhenius acid?

Accepted Answer

A substance that produces H+ ions when dissolved in water.

Question 2

What is the correct equilibrium expression for the ion-product constant of water ($$K_w) at 25$$°C?

Accepted Answer

$$K_w = [H^+][OH^-] = 1.0 	imes 10$$^{-14}$$

Question 3

A solution has a pH of 4.70. What is the concentration of $$[H_3O^+] in $$this solution?

Accepted Answer

$$[H_3O^+] = 2.0 	imes 10$$^{-5}$$ 	ext{ M}$$

Question 4

Which of the following statements about the pH scale is correct?

Accepted Answer

A pH less than 7.00 indicates an acidic solution.

Question 5

Which of the following is a Lewis acid?

Accepted Answer

A substance that accepts an electron pair.

Question 6

What is the relationship between $$K_a$$ and acid strength for a weak acid?

Accepted Answer

A larger $$K_a$$ means a stronger acid.

Question 7

Calculate the pH of a solution with $$[OH^-] = 2.9 	imes 10$$^{-4}$$ M.

Accepted Answer

pH = 10.46

Question 8

Which of the following is true about the effect of dilution on % ionization of a weak acid?

Accepted Answer

Dilution increases % ionization.

Question 9

What is the correct formula for calculating % ionization of a weak acid?

Accepted Answer

$$	ext{% ionization} = \frac{[H_3O^+]_{eq}}{[HA]_i} 	imes 100$$

Question 10

Which of the following is NOT a strong acid?

Accepted Answer

HC2H3O2

Question 11

A 0.15 M solution of acetic acid ($$K_a = 1.8 	imes 10$$^{-5}$$) has an equilibrium $$[H_3O^+]$$ of 1.6$$ 	imes $$10^{-3} M. $$What is the % ionization?

Accepted Answer

1.1%

Question 12

Which of the following best describes a Brønsted-Lowry base?

Accepted Answer

A proton acceptor.

Question 13

If $$K_w = 1.0 	imes 10$$^{-14}$$ at 25°C, what is the concentration of $$[OH^-]$$ in a neutral solution?

Accepted Answer

$$[OH^-] = 1.0 	imes 10$$^{-7}$$ M

Question 14

Which of the following is an amphoteric substance?

Accepted Answer

H2O

Question 15

What is the relationship between pH and $$[H_3O^+]$$?

Accepted Answer

pH decreases as $$[H_3O^+]$$ increases.

Question 16

Which equation correctly relates pH, pOH, and pKw at 25°C?

Accepted Answer

$$pKw = pH + pOH = 14.00$$

Question 17

Which of the following is a real-life application of the pH concept?

Accepted Answer

Determining the acidity of rainwater to assess environmental pollution.

Question 18

A pH meter uses a glass membrane electrode. What does the potential of this electrode depend on?

Accepted Answer

The concentration of $$[H_3O^+] in $$the solution.

Question 19

Which of the following statements about conjugate acid-base pairs is correct?

Accepted Answer

A conjugate acid is formed when a base accepts a proton.

Acids and Bases: Definitions, Properties, and Calculations

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