$$[H^+] = 3.6 \times 10$$^{-3}$$\ \mathrm{M}$$

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

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

Question 1

Which of the following best describes the Brønsted–Lowry definition of an acid?

Accepted Answer

A substance that donates a proton (H$$^+) to $$another substance.

Question 2

Given the reaction: $$\mathrm{$$HNO_2$$(aq) + H_2O(l) \rightleftharpoons NO_2$^-(aq) + H_3O^+(aq)}$$, which species is the conjugate base?

Accepted Answer

$$\mathrm{NO_2$^-}$$

Question 3

Which of the following is an example of an amphiprotic substance?

Accepted Answer

$$\mathrm{H_2O}$$

Question 4

What is the pH of a solution with $$[H^+] = 1.5 	imes 10$$^{-3}$$\ \mathrm{M}$$?

Accepted Answer

$$\mathrm{pH} = 2.82$$

Question 5

Which of the following statements is true regarding the relationship between acid and conjugate base strength?

Accepted Answer

The stronger the acid, the weaker its conjugate base.

Question 6

A 0.125 M solution of $$\mathrm{$$HNO_3$$} is $$prepared. What is the pH of the solution?

Accepted Answer

$$\mathrm{pH} = 0.90$$

Question 7

Which of the following is a Lewis acid in the reaction $$\mathrm{NH_3$ + BF_3$ \rightarrow F_3B-NH_3$}$$?

Accepted Answer

$$\mathrm{BF_3$}$$

Question 8

If the $$[OH^-] = 4.75 	imes 10$$^{-5}$$\ \mathrm{M}$$, what is the pH of the solution at 25$$^\circC$$?

Accepted Answer

$$\mathrm{pH} = 4.32$$

Question 9

Which of the following best describes the autoionization of water?

Accepted Answer

$$\mathrm{H_2O(l) + H_2O(l) \rightleftharpoons OH^-(aq) + H_3O^+(aq)}$$

Question 10

A solution has a pH of 2.44. What is the $$[H^+]$$ concentration?

Accepted Answer

$$[H^+] = 3.6 	imes 10$$^{-3}$$\ \mathrm{M}$$

Question 11

Which of the following is NOT a strong acid?

Accepted Answer

$$\mathrm{HF}$$

Question 12

What is the pOH of a solution with $$[OH^-] = 2.0 	imes 10$$^{-4}$$\ \mathrm{M}$$?

Accepted Answer

$$\mathrm{pOH} = 3.70$$

Question 13

Which of the following best explains why $$\mathrm{H_2SO_4} is a $$strong acid?

Accepted Answer

It completely dissociates in water to produce $$\mathrm{H_3O^+}$$ and $$\mathrm{$$HSO_4$$^-}.$$

Question 14

A 0.15 M solution of $$\mathrm{NH_2OH} (Kb$$ = $$1.1 	imes 10$$^{-8}$$) is prepared. Which of the following is closest to the pH of the solution?

Accepted Answer

$$\mathrm{pH} = 10.2$$

Question 15

Which of the following is the correct expression for the ion product constant for water ($$K_w) at 25$^\circC$$?

Accepted Answer

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

Question 16

Which of the following best describes a Lewis base?

Accepted Answer

An electron pair donor

Question 17

Which of the following solutions is neutral at 25$$^\circC$$?

Accepted Answer

$$[H^+] = [OH^-] = 1.0 	imes 10$$^{-7}$$\ \mathrm{M}$$

Question 18

Which of the following is the correct formula for calculating percent ionization of a weak acid?

Accepted Answer

$$\mathrm{Percent\ ionization} = \frac{[H_3O^+]_{eq}}{[HA]_{initial}} 	imes 100$$

Question 19

Which of the following best explains why $$\mathrm{H_2O}$$ can act as both an acid and a base?

Accepted Answer

It can donate or accept a proton depending on the reaction partner.

Acid-Base Equilibria: Concepts, Calculations, and Applications

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