8.2 Properties of Acids and Bases

Which of the following best describes the pH of a solution?

A. The concentration of hydroxide ions in the solution.

B. The negative logarithm of the concentration of hydrogen ions.

C. The positive logarithm of the concentration of hydroxide ions.

D. The concentration of hydrogen ions in the solution.

A solution has a pH of 3. How would you classify this solution?

A. Strongly acidic

B. Weakly acidic

C. Neutral

D. Basic

Which of the following is a characteristic of a strong acid?

A. Partial ionisation in water

B. Complete ionisation in water

C. High pH value

D. Low concentration of H+ ions

Which of the following is NOT true about weak bases?

A. They partially ionise in water.

B. They have a high pH value.

C. They release a high concentration of OH- ions.

D. They do not completely dissociate in water.

What is the pH of a neutral solution at 25°C?

A. 0

B. 5

C. 7

D. 14

a) Define pH and explain its significance in determining the acidic or basic nature of a solution. [3]

b) If a solution has a pH of 4, how would its [H+] concentration compare to a solution with a pH of 7? [2]

a) Differentiate between strong and weak acids in terms of their degree of ionisation. [3]

b) Provide an example of a strong acid and a weak acid. [2]

a) Describe the concept of "conjugate acid-base pairs" and explain how they are formed. [3]

b) If NH3 acts as a base, identify its conjugate acid. [2]

a) Describe the relationship between pH and the concentration of hydrogen ions [H+] in a solution. [2]

b) A solution has a [H+] concentration of 1 x 10^-5 mol/L. Calculate its pH. [2]

c) Based on the calculated pH, classify the solution as acidic, basic, or neutral. [2]

a) What is meant by the term "degree of ionisation" in the context of acids and bases? [3]

b) Explain why strong acids have a higher degree of ionisation compared to weak acids. [2]

c) Given that acetic acid (CH3COOH) is a weak acid, predict its degree of ionisation in water. [2]