📚 Part 1: Definitions and Concepts

1. According to the Brønsted-Lowry theory, an acid is a substance that:

Accepts protons (H⁺ ions)

Donates protons (H⁺ ions)

Produces OH⁻ ions in solution

Has a pH greater than 7

2. Which of the following best describes a strong acid?

Partially ionises in aqueous solution

Completely ionises in aqueous solution

Has a very high concentration

Cannot be neutralised by bases

3. An amphiprotic substance can:

Only donate protons

Only accept protons

Both donate and accept protons

Neither donate nor accept protons

4. Which of the following are examples of polyprotic acids? (Select all that apply)

HCl

H₂SO₄

H₃PO₄

CH₃COOH

✏️ Part 2: Chemical Equations and Reactions

5. Write the equation for hydrochloric acid (HCl) dissolving in water. Include the conjugate acid-base pairs.

6. Write the equation showing ammonia (NH₃) acting as a base in water.

7. Sodium acetate (CH₃COONa) forms a basic solution when dissolved in water. Write the equation for this reaction and explain why the solution is basic.

8. Water (H₂O) is amphiprotic. Write two equations showing water acting as both an acid and a base.

🧪 Part 3: Analysis and Application

9. For the acid-base reaction: HF + H₂O ⇌ H₃O⁺ + F⁻

a) Identify the conjugate acid-base pairs: _______________ and _______________

b) If HF is a weak acid, what can you conclude about the strength of F⁻ as a base?

10. Explain the difference between a monoprotic and polyprotic acid, giving one example of each with their ionisation equations.

11. Ammonium chloride (NH₄Cl) forms an acidic solution when dissolved in water. Write the equation for this reaction and explain why the solution becomes acidic.