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 = $$14.00 - 2.70 = 11.30$$

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

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

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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