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

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