Foundation Level (Fail → Pass)

Basic prompts to build essential understanding.

1. Define pH.

2. What is an acid? What is a base?

3. Write the formula for calculating pH from [H⁺].

4. Define a strong acid and give one example.

5. Define a weak acid and give one example.

6. What is Kw?

7. State the pH of a neutral solution at 25°C.

8. What is meant by the term “buffer solution”?

9. Give one example of a natural buffer in the human body.

10. Define solubility in simple terms.

 Intermediate Level (Pass → Credit)

Prompts requiring explanation, calculations, and conceptual reasoning.

1. Explain why strong acids fully dissociate in water.

2. Calculate the pH of a 1 × 10⁻³ mol dm⁻³ HCl solution.

3. Explain how weak acids partially dissociate.

4. Write the Ka expression for a weak acid HA.

5. Explain how a buffer resists changes in pH.

6. Describe how to prepare an acidic buffer.

7. Use the Henderson–Hasselbalch equation to calculate pH.

8. Explain the common ion effect.

9. Define Ksp and explain its significance.

10. Predict whether a precipitate will form using ionic product vs Ksp.

Advanced Level (Credit → Distinction)

Higher-order analysis, calculations, and multi-step reasoning.

1. Analyse how temperature affects Kw and pH neutrality.

2. Derive the Henderson–Hasselbalch equation.

3. Predict pH changes when small amounts of strong acid are added to a buffer.

4. Explain how polyprotic acids dissociate stepwise.

5. Evaluate how pH affects solubility of ionic salts.

6. Calculate the pH of a mixture containing both weak acid and salt.

7. Analyse how pH influences the equilibrium of amphiprotic species.

8. Solve multi-step buffer problems involving dilution.

9. Compare and contrast strong and weak base equilibria.

10. Use Ksp to calculate molar solubility in complex ionic systems.