Q: If the $$pOH of a $$solution is $$4.0$$, what is the $$[OH^-]$$ concentration?

$$1.0 \times 10$$^{-4}$$\ \mathrm{M}$$

Q: A solution at $$25^\circC $$has $$[H_3O^+] = 2.0 \times 10$$^{-8}$$\ \mathrm{M}. $$What is the $$[OH^-] in $$this solution?

$$5.0 \times 10$$^{-7}$$\ \mathrm{M}$$

Q: A patient with GERD is monitored using a pH sensor in the esophagus. If the sensor records a pH of $$2.0$$, what is the $$[H_3O^+] in $$the esophagus?

$$1.0 \times 10$$^{-2}$$\ \mathrm{M}$$

Question 1

Which of the following statements best explains why hydrochloric acid ($$\mathrm{HCl}) is $$classified as a strong acid?

Accepted Answer

It completely ionizes in aqueous solution, donating all of its $$\mathrm{H^+}$$ ions.

Question 2

A solution has a hydronium ion concentration of $$1.0 	imes 10$$^{-5}$$\ \mathrm{M}. $$What is the pH of this solution?

Accepted Answer

$$5.0$$

Question 3

Which of the following best describes the difference between the Arrhenius and Brønsted-Lowry definitions of acids and bases?

Accepted Answer

Arrhenius acids produce $$\mathrm{H^+} in $$solution, while Brønsted-Lowry acids donate $$\mathrm{H^+} to $$another species.

Question 4

A student adds sodium acetate ($$\mathrm{NaCH_3COO}$$), a salt of a weak acid, to water. What will happen to the pH of the solution?

Accepted Answer

The pH will increase because the acetate ion acts as a weak base.

Question 5

Which of the following equations correctly represents the autoionization of water?

Accepted Answer

$$\mathrm{2H_2O (l) \rightarrow H_3O^+ (aq) + OH^- (aq)}$$

Question 6

If the $$pOH of a $$solution is $$4.0$$, what is the $$[OH^-]$$ concentration?

Accepted Answer

$$1.0 	imes 10$$^{-4}$$\ \mathrm{M}$$

Question 7

Which of the following is NOT a property of bases?

Accepted Answer

They change blue litmus paper to red.

Question 8

A solution at $$25^\circC $$has $$[H_3O^+] = 2.0 	imes 10$$^{-8}$$\ \mathrm{M}. $$What is the $$[OH^-] in $$this solution?

Accepted Answer

$$5.0 	imes 10$$^{-7}$$\ \mathrm{M}$$

Question 9

Which of the following statements about the conjugate base of a strong acid is correct?

Accepted Answer

It is pH neutral and does not react with water.

Question 10

A patient with GERD is monitored using a pH sensor in the esophagus. If the sensor records a pH of $$2.0$$, what is the $$[H_3O^+] in $$the esophagus?

Accepted Answer

$$1.0 	imes 10$$^{-2}$$\ \mathrm{M}$$

Question 11

Which of the following acids is diprotic and classified as a strong acid?

Accepted Answer

Sulfuric acid ($$\mathrm{H_2SO_4})$$

Question 12

Which of the following best describes why water is considered amphoteric?

Accepted Answer

It can act as both an acid and a base depending on the reaction.

Question 13

A solution has a $$pH of$$ $$11.0. $$What is its $$pOH$$?

Accepted Answer

$$3.0$$

Question 14

Which of the following statements about the relationship between $$K_a$$, $$K_b$$, and $$K_w is $$correct?

Accepted Answer

$$K_a 	imes K_b = K_w$$

Question 15

Which of the following is a property of carboxylic acids?

Accepted Answer

They contain a $$-\mathrm{COOH}$$ group.

Question 16

Which of the following best explains why the $$[H_3O^+]$$ from water is negligible in a strong acid solution?

Accepted Answer

The strong acid completely ionizes, producing much more $$[H_3O^+]$$ than water's autoionization.

Question 17

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

Accepted Answer

Sodium chloride ($$\mathrm{NaCl})$$

Question 18

A weak acid has a $$K_a$$ value of $$1.0 	imes 10$$^{-5}$$. Which statement is true?

Accepted Answer

Only a small fraction of the acid molecules ionize in water.

Question 19

Which of the following best describes the effect of a cation from a weak base on the pH of a solution?

Accepted Answer

It will hydrolyze water and make the solution acidic.

Question 20

Which of the following is the correct formula for calculating the $$pH of a $$solution given $$[H_3O^+]$$?

Accepted Answer

$$pH = -\log [H_3O^+]$$

Acids, Bases, and Aqueous Equilibria: Study Notes

Study Guide - Practice Questions

Study Guide - Flashcards