Titrating Polyfunctional Acids and Bases

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Presentation transcript:

Titrating Polyfunctional Acids and Bases

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-

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-

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

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 0.0100M NaH2PO4 solution.

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

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)