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]

Which of the following solutions has the highest concentration of H+ ions?

A. pH 2

B. pH 5

C. pH 7

D. pH 9

Which of the following is a common application of a weak acid?

A. Battery acid

B. Digestion in the stomach

C. Preservative in food

D. Cleaning rust from metals

If the concentration of H+ ions in a solution is 1 x 10^-4 M, what is the pH of the solution?

A. 4

B. 6

C. 7

D. 10

Which of the following best describes the relationship between pH and [H+]?

A. Directly proportional

B. Inversely proportional

C. No relationship

D. Exponential relationship

A solution with a pH of 11 is:

A. Strongly acidic

B. Weakly acidic

C. Weakly basic

D. Strongly basic

a) Define a "conjugate base" and provide an example. [2]

b) If H2SO4 donates a proton, identify its conjugate base. [2]

c) Explain the relationship between an acid and its conjugate base in terms of proton transfer. [3]

a) What is the significance of pH in everyday life? Provide two examples. [3]

b) Explain how the pH of the soil can affect plant growth. [3]

c) Describe a method to adjust the pH of the soil to make it more suitable for plant growth. [2]

a) Define pH and explain its scale. [2]

b) A certain solution has a [H+] concentration of 1 x 10^-9 mol/L. Calculate its pH. [2]

c) If the pH of a solution decreases from 7 to 5, by what factor has the [H+] concentration changed? [3]

d) Identify a common substance with a pH close to the calculated value in part b. [2]

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

b) Given that hydrochloric acid (HCl) is a strong acid, predict its behaviour when dissolved in water. [2]

c) Define a conjugate acid-base pair and provide an example using water and the hydroxide ion. [3]

d) If a solution has a pH of 4, what would be its pOH? [2]

a) Describe the applications of pH in the agricultural industry. [3]

b) Explain how the pH of rainwater can be affected by industrial emissions. [3]

c) If a farmer wanted to neutralise an acidic soil with a pH of 5, what substance could they add, and why? [3]

d) How does the degree of ionisation relate to the strength of an acid or base? [2]