Q: Calculate the pH of a solution with $[H^+] = 4.7 \times 10^{-4}$ M.

pH = $-\log(4.7 \times 10^{-4}) = 3.33$

Q: A solution of Ba(OH)$_2$ has a concentration of $1.5 \times 10^{-2}$ M. What is the pOH of the solution?

pOH = $-\log(3.0 \times 10^{-2}) = 1.52$

Q: For a monoprotic weak acid HA, the percentage of ionization is defined as:

$\dfrac{[H^+]}{[HA]_{initial}} \times 100\%$

Q: A solution of $0.060$ M monoprotic acid has a pH of $3.44$. What is the value of $K_a$ for this acid?

$K_a = \dfrac{(3.63 \times 10^{-4})^2}{0.060}$

Q: What is the pH of a solution with $[OH^-] = 2.0 \times 10^{-3}$ M?

pOH = $-\log(2.0 \times 10^{-3}) = 2.70$, pH = $14.00 - 2.70 = 11.30$

Question 1

Which of the following statements correctly describes a conjugate acid-base pair according to the Brønsted-Lowry definition?

Accepted Answer

A conjugate acid-base pair consists of two species that differ by a proton (H\^+).

Question 2

Given the reaction $\mathrm{CH_3COOH(aq) + H_2O(l) \rightarrow CH_3COO^-(aq) + H_3O^+(aq)}$, which of the following is the conjugate base of acetic acid?

Accepted Answer

$\mathrm{CH_3COO^-}$

Question 3

What is the value of $K_w$ (the ionic product of water) at 25°C?

Accepted Answer

$1.0 	imes 10^{-14}$

Question 4

Calculate the pH of a solution with $[H^+] = 4.7 	imes 10^{-4}$ M.

Accepted Answer

pH = $-\log(4.7 	imes 10^{-4}) = 3.33$

Question 5

Which of the following is a strong acid?

Accepted Answer

$\mathrm{HNO_3}$

Question 6

A solution of Ba(OH)$_2$ has a concentration of $1.5 	imes 10^{-2}$ M. What is the pOH of the solution?

Accepted Answer

pOH = $-\log(3.0 	imes 10^{-2}) = 1.52$

Question 7

Which of the following statements about weak acids is correct?

Accepted Answer

Weak acids have a small ionization constant $K_a$.

Question 8

For a monoprotic weak acid HA, the percentage of ionization is defined as:

Accepted Answer

$\dfrac{[H^+]}{[HA]_{initial}} 	imes 100\%$

Question 9

Which of the following salts will produce a basic solution when dissolved in water?

Accepted Answer

$\mathrm{CH_3COONa}$

Question 10

A solution of $0.060$ M monoprotic acid has a pH of $3.44$. What is the value of $K_a$ for this acid?

Accepted Answer

$K_a = \dfrac{(3.63 	imes 10^{-4})^2}{0.060}$

Question 11

Which of the following is true for the relationship between $K_a$ and $K_b$ for a conjugate acid-base pair?

Accepted Answer

$K_a 	imes K_b = K_w$

Question 12

Which oxide reacts with water to produce a basic solution?

Accepted Answer

$\mathrm{Na_2O}$

Question 13

What is the pH of a solution with $[OH^-] = 2.0 	imes 10^{-3}$ M?

Accepted Answer

pOH = $-\log(2.0 	imes 10^{-3}) = 2.70$, pH = $14.00 - 2.70 = 11.30$

Question 14

Which of the following is a polyprotic acid?

Accepted Answer

$\mathrm{H_2CO_3}$

Question 15

A solution contains $0.20$ M $H_2CO_3$. If $K_{a1} = 6.5 	imes 10^{-4}$, what is the concentration of $[HCO_3^-]$ after the first ionization step?

Accepted Answer

$0.14$ M

Question 16

Which of the following is the correct expression for the ionization constant of a weak base, such as ammonia?

Accepted Answer

$K_b = \dfrac{[NH_4^+][OH^-]}{[NH_3]}$

Question 17

Which of the following will produce an acidic solution when dissolved in water?

Accepted Answer

$\mathrm{NH_4Cl}$

Question 18

If the pH of a solution is 2.00, what is the concentration of $[H^+]$?

Accepted Answer

$[H^+] = 1.0 	imes 10^{-2}$ M

Acids and Bases: Properties, Equilibria, and Applications

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