1. Titration Curves

2. pH mL of Base added 7 O Strong acid with strong Base O Equivalence at pH 7

3. pH mL of Base added >7 l Weak acid with strong Base l Equivalence at pH >7 l When the acid is neutralized it makes a weak base 7

4. pH mL of acid added 7 l Strong base with strong acid l Equivalence at pH 7

5. pH mL of acid added <7 l Weak base with strong acid l Equivalence at pH <7 l When the base is neutralized it makes a weak acid 7

6. Strong acid with Strong Base  Change to moles  Do the stoichiometry. BRA Chart  There is no equilibrium.  They both dissociate completely.  The reaction is H + + OH -  HOH  Use [H + ] or [OH - ] to figure pH or pOH  The titration of 50.0 mL of 0.200 M HNO 3 with 0.100 M NaOH

7. Weak acid with Strong base O There is an equilibrium. O Do stoichiometry. O Use moles BRA Chart O Determine major species O Then do equilibrium. RICE Chart O Titrate 50.0 mL of 0.10 M HF (Ka = 7.2 x 10 -4 ) with 0.10 M NaOH

8. Summary O Strong acid and base just stoichiometry. O Weak acid with 0 ml of base - K a O Weak acid before equivalence point – Stoichiometry first BRA Chart – Then Henderson-Hasselbach RICE Chart O Weak acid at equivalence point- K b -Calculate concentration O Weak acid after equivalence - leftover strong base. -Calculate concentration

9. Summary O Weak base before equivalence point. – Stoichiometry first BRA Chart – Then Henderson-Hasselbach RICE Chart O Weak base at equivalence point K a. -Calculate concentration O Weak base after equivalence – left over strong acid. -Calculate concentration