1. Titrating Polyfunctional Acids and Bases

2. 1. Treating Complex Acid-Base Systems
Complex systems are defined as solutions made up of:
(1) An acid or base that has two or more acidic protons or basic functional groups
H3PO4
Ca(OH)2
(2) Two acids or bases of different strengths
HCl + CH3COOH
NaOH + CH3COO-

3. HCO3- + H2O <=> CO32- + H3O+ HCO3- + H2O <=> H2CO3 + OH-
3) An amphiprotic substance that is capable of acting as both acid and base
HCO3- + H2O <=> CO32- + H3O+
HCO3- + H2O <=> H2CO3 + OH-
NH3+CH2COO- + H2O <=> NH2CH2COO- + H3O+
NH3+CH2COO- + H2O <=> NH3+CH2COOH + OH-

6. Problems Understanding Ka1>Ka2>Ka3…
The relationship between Ka and Kb of its conjugate base.

12. Example 13-1, 2, 3
Calculate the hydronium ion concentration of 0.100M NaHCO3 solution.
Calculate the hydronium ion concentration of 1.00×10-3M Na2HPO4 solution.
Find the hydronium ion concentration of M NaH2PO4 solution.

24. Mixtures of Strong and Weak Acids
Mixtures of Strong and Weak bases?

29. Problem(P325, 13-25): Identify by letter the curve you would expect in the titration of a solution containing (a) disodium maleate, Na2M, with standard acid (1.3x10-2, 5.9x10-7) (b) pyruvic acid, HP, with standard base (3.2x10-3) (c) sodium carbonate, Na2CO3, with standard acid (1.5x10-4, 4.69x10-11)