Question 1

Which of the following best describes the process of water ionization?

Accepted Answer

Water molecules dissociate into $H^+$ and $OH^-$ ions, and this process is reversible.

Question 2

A solution has a $[H^+]$ concentration of $1 	imes 10^{-7}$ M. What is the pH of the solution?

Accepted Answer

$7$

Question 3

Which of the following equations correctly represents the relationship between pH and $[H^+]$?

Accepted Answer

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

Question 4

If the $[H^+]$ concentration of a solution increases, what happens to the $[OH^-]$ concentration?

Accepted Answer

It decreases.

Question 5

Which of the following statements about strong acids is correct?

Accepted Answer

Strong acids ionize completely in water, releasing all possible $H^+$ ions.

Question 6

A weak base such as ammonia ($NH_3$) reacts with $H^+$ ions in water to form which product?

Accepted Answer

$NH_4^+$

Question 7

If a solution has a pH of 4, what is the $[H^+]$ concentration in molarity?

Accepted Answer

$1 	imes 10^{-4}$ M

Question 8

Which of the following best explains why strong bases like $NaOH$ increase the $OH^-$ concentration in water?

Accepted Answer

They dissociate completely, releasing $OH^-$ ions into solution.

Question 9

A solution with a pH of 3 has how many times higher $[H^+]$ concentration than a solution with pH 7?

Accepted Answer

$10,000$ times higher

Question 10

Which of the following is a correct statement about weak acids?

Accepted Answer

Weak acids ionize incompletely or reversibly in water.

Question 11

If the $[H^+]$ concentration of a solution is $0.01$ M, what is the pH?

Accepted Answer

$2$

Question 12

Which of the following is true about the relationship between acids and bases?

Accepted Answer

Acids increase $H^+$ concentration, while bases decrease $H^+$ concentration.

Question 13

A buffer solution is important in biological systems because it:

Accepted Answer

Resists changes in pH when small amounts of acid or base are added.

Question 14

If the $[H^+]$ concentration of a solution is $1 	imes 10^{-8}$ M, what is the pH?

Accepted Answer

$8$

Question 15

Which of the following is a real-world example of a strong acid?

Accepted Answer

Hydrochloric acid ($HCl$)

Question 16

A solution has a $[H^+]$ concentration of $100$ mM. What is the pH?

Accepted Answer

$1$

Question 17

Which of the following best describes the effect of adding a strong base to pure water?

Accepted Answer

The $OH^-$ concentration increases and the $H^+$ concentration decreases.

Question 18

Which of the following is true about the pH scale?

Accepted Answer

Each step on the pH scale represents a tenfold difference in $[H^+]$ concentration.

Question 19

If 1 mole of $HCl$ (hydrochloric acid, a strong acid) is dissolved in 100 L of water, what will be the $[H^+]$ concentration?

Accepted Answer

$0.01$ M

Question 20

If 1 mole of $CH_3COOH$ (acetic acid, a weak acid) is dissolved in 100 L of water, what will be the $[H^+]$ concentration?

Accepted Answer

Less than $0.01$ M

Acids, Bases, and the pH Scale Lab 2 Part 1 of 3

Study Guide - Practice Questions