1. Ionic Equilibria (I) Acids and bases

2. Ionic Equilibria (I) 1. How do we identify acids and bases?

4. Ionic Equilibria (I) 2. How do we identify conjugate acids and bases?

6. Ionic Equilibria (I) 3. How do we know whether an acid/ base is strong or weak?

8. Ionic Equilibria (I) 4. How do we calculate pH of an acid/ base?

10. Ionic Equilibria (I) 4. How do we calculate pH of an acid/ base? (II) Determine strong or weak Strong acids ionise completely in aqueous solution. [H 3 O + ] = [HA]  pH = - log [HA] Strong bases ionise completely in aqueous solution. [OH - ] = [B]  pOH = - log [B] Strong Acid Strong Base

11. Ionic Equilibria (I) 4. How do we calculate pH of an acid/ base? (II) Determine strong or weak Weak bases ionise partially in aqueous solution. [OH - ] < [B]  pOH = - log [OH – ] Weak Acid Weak Base Weak acids ionise partially in aqueous solution. [H 3 O + ] < [HA]  pH = - log [H 3 O + ] [H 3 O + ] = K a × [HA] [OH – ] = K b × [B]

12. Ionic Equilibria (II) Salts

13. Ionic Equilibria (II) 5. How do we know if a salt is neutral, acidic or basic?

17. Ionic Equilibria (II) 6. How do we calculate the pH of a salt solution?

20. Ionic Equilibria (III) Solubility Equilibria - sparingly soluble salts

21. Ionic Equilibria (III) 7. How do know if a salt is sparingly soluble?

24. Ionic Equilibria (III) Type 1 Questions K sp solubility conc. of ions Given the value of one of the above (e.g. K sp ), find the other 2 values (solubility and conc. of ions)

28. Ionic Equilibria (I) Tutorial Q1cii) A weak acid dissociates partially producing less moles of H + ions than moles of acid. e.g. 10 moles of a weak acid HA may produce only 0.1 mole of H + But when a weak acid reacts with another reagent (e.g. metal or alkali), the weak acid will react completely. e.g. All 10 moles of HA will be reacted when added to excess NaOH