1. What is the difference between a strong acid and a weak acid? In your answer identify one example (name and chemical formula) of a strong acid and one example of a weak acid. Also include balanced chemical equations to show the ionisation of each of these two acids in water.?
2. What is pH? Write the equation used to calculate pH. ?
3. What is meant by the equivalence point of a titration? (b) What is meant by the endpoint of a titration?
4. What is the function of the indicator in titration?
5. Write a balanced equation for the reaction between aqueous hydrochloric acid (HCl) and aqueous sodium hydroxide (NaOH)?
6. Write a balanced equation for the reaction between aqueous acetic acid (CH₃COOH) and aqueous sodium hydroxide (NaOH)?
7. Write down the equation for the chemical reaction for the following buffer system

8. (H₂CO₃/HCO₃^-) when (i) a small amount of acid (H₃O⁺) is added and (ii) a small amount of base (OH^-) is added.

   A small amount of acid is added:

   A small amount of base is added:

9. The pH of a buffer can be calculated using the Henderson-Hasselbalch equation. = + [ ] / [ ] . Calculate the pH of a buffer solution containing 0.750 mol L^-1 lactic acid (HC₃H₅O₃) and 0.250 mol L^-1 sodium lactate (which contains the lactate ion C₃H₅O₃^-, the conjugate base of lactic acid), given that the pK_a of lactic acid is 3.85.

10. . Explain how you could increase the capacity of the buffer solution in Question 10.

    In your answer identify the specific concentrations (in mol L^-1) of the lactic acid (weak acid) and lactate ion (conjugate base) that could be used to prepare a buffer solution with a higher capacity than that in Question 10