Topic 14 - How far? Reversible reactions

Chemical Equilibria

1. Explain in terms of rates of the forward and reverse reactions, what is meant by a reversible reaction and dynamic equilibrium.
2. Deduce expressions for the equilibrium constant term of concentrations, K_c.
3. Deduce expressions for the equilibrium constant term of partial pressures, K_p.
4. Calculate the quantities present at equilibrium from given data.
5. State Le Chatelier’s principle and apply it to deduce qualitatively the effects of changes in temperature, concentration and pressure on a system at equilibrium.
6. Deduce whether changes in concentration, pressure or temperature or the presence of a catalyst affects the value of the equilibrium constant for a reaction.
7. Predict whether a system is capable of spontaneous change, using S and K_c as indicators of thermodynamic feasibility and the position of equilibrium (qualitative discussion only).
8. Discuss and interpret the relative effect of change in temperature and pressure on a system at equilibrium in terms of its entropy change.

Acid-Base Equilibria

1. Recall and use the Brønsted-Lowry theory of acids and bases.
2. Explain qualitatively the difference in behaviour between strong and weak acids.
3. Explain the term pH and use it to calculate its value.
4. Explain the term K_w.
5. Explain the terms K_a, and pK_a.
6. Calculate [H⁺_(aq)] and pH values for strong and weak acids and bases.
7. Describe the changes in pH during acid-base titrations and explain these changes in terms of the strength of acids and bases.
8. Explain how acid-base indicators work.
9. List what makes an effective indicator.
10. Explain how to chose an indicator for a titration.
11. Explain how buffer solutions control pH.
12. Discuss the application of buffers.
13. Calculate the pH of a buffer solution.

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