Q: If orange juice has a pH of $4.50$, what is the hydrogen ion concentration $[\mathrm{H^+}]$?

$3.16 \times 10^{-5}\ \mathrm{mol\ L^{-1}}$

Question 1

According to the Arrhenius model, which of the following best describes an acid in aqueous solution?

Accepted Answer

A substance that ionizes in solution to produce hydrogen ions $\mathrm{H^+}$.

Question 2

Which equation correctly represents the ionization of hydrochloric acid in water, including the formation of hydronium?

Accepted Answer

$\mathrm{HCl(g) + H_2O(l) \rightarrow H_3O^+(aq) + Cl^-(aq)}$

Question 3

Which of the following is a limitation of the Arrhenius model of acids and bases?

Accepted Answer

It is restricted to acids and bases that dissolve in water.

Question 4

A student dissolves sodium hydroxide ($\mathrm{NaOH}$) in water. According to the Arrhenius model, what is the primary species responsible for the basicity of the solution?

Accepted Answer

$\mathrm{OH^-}$ ions

Question 5

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

Accepted Answer

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

Question 6

Which statement best distinguishes a strong acid from a weak acid?

Accepted Answer

A strong acid ionizes completely in solution, while a weak acid ionizes only partially.

Question 7

Given the following acids: hydrochloric acid ($\mathrm{HCl}$) and ethanoic acid ($\mathrm{CH_3COOH}$), which statement is correct regarding their ionization in water?

Accepted Answer

$\mathrm{HCl}$ ionizes completely, while $\mathrm{CH_3COOH}$ ionizes partially.

Question 8

A solution has a hydrogen ion concentration of $[\mathrm{H^+}] = 1.0 	imes 10^{-4}\ \mathrm{mol\ L^{-1}}$. What is the pH of the solution?

Accepted Answer

$4.0$

Question 9

If orange juice has a pH of $4.50$, what is the hydrogen ion concentration $[\mathrm{H^+}]$?

Accepted Answer

$3.16 	imes 10^{-5}\ \mathrm{mol\ L^{-1}}$

Question 10

Which of the following best explains why non-metal oxides such as $\mathrm{CO_2}$ form acidic solutions when dissolved in water?

Accepted Answer

They react with water to form acids that ionize to produce hydrogen ions.

Question 11

Which of the following is a weak base according to the study materials?

Accepted Answer

Ammonia ($\mathrm{NH_3}$)

Question 12

A solution is defined as neutral when:

Accepted Answer

The concentrations of $\mathrm{H^+}$ and $\mathrm{OH^-}$ ions are equal.

Question 13

Which of the following equations uses a double arrow to indicate partial ionization of a weak acid?

Accepted Answer

$\mathrm{CH_3COOH(aq) \rightleftharpoons H^+(aq) + CH_3COO^-(aq)}$

Question 14

Which of the following best describes the relationship between acid strength and reaction vigor with metals?

Accepted Answer

Strong acids react more vigorously with metals than weak acids.

Question 15

Which of the following is the correct formula for calculating pH?

Accepted Answer

$\mathrm{pH = -log_{10}[H^+]}$

Question 16

A solution has a pH of $8.00$. What is the $[\mathrm{H^+}]$ concentration?

Accepted Answer

$1.0 	imes 10^{-8}\ \mathrm{mol\ L^{-1}}$

Question 17

Which of the following is true about strong bases?

Accepted Answer

They completely dissociate in water to release $\mathrm{OH^-}$ ions.

Question 18

Which of the following is a strong electrolyte?

Accepted Answer

Hydrochloric acid ($\mathrm{HCl}$)

Question 19

Which of the following best explains why the Arrhenius model cannot account for the basicity of ammonia ($\mathrm{NH_3}$) in water?

Accepted Answer

Ammonia does not contain hydroxide ions but can still increase $\mathrm{OH^-}$ concentration by reacting with water.

Acids and Bases: The Arrhenius Model, Ionization, and Strength

Study Guide - Practice Questions

Study Guide - Flashcards