Question 1

Which of the following correctly represents the dissociation equation for beryllium chloride ($\mathrm{BeCl_2}$) in water?

Accepted Answer

$\mathrm{BeCl_2 (s) \rightarrow Be^{2+} (aq) + 2Cl^- (aq)}$

Question 2

What does molarity ($M$) describe in a chemical solution?

Accepted Answer

The number of moles of solute per liter of solution

Question 3

Which of the following best defines an acid according to the Brønsted-Lowry theory?

Accepted Answer

A substance that donates a proton ($\mathrm{H^+}$) to another substance

Question 4

When an acid is added to water, what happens to the $[\mathrm{H^+}]$, $[\mathrm{OH^-}]$, and pH of the solution?

Accepted Answer

$[\mathrm{H^+}]$ increases, $[\mathrm{OH^-}]$ decreases, pH decreases

Question 5

Which of the following best defines a base according to the Arrhenius definition?

Accepted Answer

A substance that increases the concentration of $\mathrm{OH^-}$ ions in water

Question 6

If a base is added to a solution, what happens to the $[\mathrm{H^+}]$, $[\mathrm{OH^-}]$, and pH?

Accepted Answer

$[\mathrm{H^+}]$ decreases, $[\mathrm{OH^-}]$ increases, pH increases

Question 7

What is the minimum and maximum value of the pH scale in aqueous solutions at 25°C?

Accepted Answer

Minimum: 0, Maximum: 14

Question 8

A solution has $[\mathrm{H^+}] = 1 	imes 10^{-2}\ \mathrm{M}$. What is the pH of the solution, and is it acidic or basic?

Accepted Answer

pH = 2, acidic

Question 9

A solution has $[\mathrm{OH^-}] = 1 	imes 10^{-3}\ \mathrm{M}$. What is the pOH and pH of the solution? Is it acidic or basic?

Accepted Answer

pOH = 3, pH = 11, basic

Question 10

Which solution is more acidic: one with a pH of 8 or one with a pH of 5?

Accepted Answer

The solution with a pH of 5

Question 11

A solution with a pH of 10 is how many times more basic than a solution with a pH of 8?

Accepted Answer

100 times

Question 12

A solution with a pH of 2 is how many times more acidic than a solution with a pH of 6?

Accepted Answer

10,000 times

Question 13

What is the main difference between a strong acid and a weak acid?

Accepted Answer

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

Question 14

What happens when an acid is combined with a base in an aqueous solution?

Accepted Answer

They undergo a neutralization reaction to form water and a salt

Question 15

Which of the following best describes a buffer solution?

Accepted Answer

A solution that resists changes in pH when small amounts of acid or base are added

Question 16

Which of the following is a real-life example of a buffer system in the human body?

Accepted Answer

The bicarbonate ($\mathrm{HCO_3^-}$) and carbonic acid ($\mathrm{H_2CO_3}$) system in blood

Question 17

Which of the following equations correctly relates pH and $[\mathrm{H^+}]$?

Accepted Answer

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

Question 18

A student adds 0.1 mol of hydrochloric acid ($\mathrm{HCl}$) to 1 L of pure water. What is the resulting pH, assuming complete dissociation?

Accepted Answer

pH = 1

Question 19

Which of the following best explains why strong acids conduct electricity better than weak acids at the same concentration?

Accepted Answer

Strong acids completely ionize, producing more ions to carry charge

Acids, Bases, and Solutions: Key Concepts and Applications

Study Guide - Practice Questions