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Sesame Oil
Henry Su December 12, 2001

Chapter Notes Chemistry 221
Chapter 13 Dr. Rahni

Titrating Polyfunctional Acids and Bases

13A—Polyfunctional Acids

-Phosphoric Acid is a typical polyfunctional acid

H3PO4 + H2O ( H2PO4- + H3O+ Ka1 = [H3O+] [H2PO4-] = 7.11e-3 [H3PO4 ]

H2PO4- + H2O ( HPO4-2 + H3O+ Ka2 = [H3O+] [H2PO4-2] = 6.32e-8 [H2PO4- ]

HPO4-2 + H2O ( PO4-3 + H3O+ Ka3 = [H3O+] [PO4-3] = 4.5e-13 [HPO4-2]

Ka1> Ka2> Ka3

13B—Describing Polyfunctional Bases

CO3-2 + H2O ( HCO3- + OH- Kb1 = [HCO3-] [OH-] = Kw = 2.13e-4 [CO3-2] Ka2

HCO3- + H2O ( H2CO3 + OH- Kb2 = [H2CO3] [OH-] = Kw = 6.7e-4 [HCO3-] Ka2

13C—Finding the pH of Solutions of Amphiprotic Salts

-Amphiprotic salts are formed during neutralization titration of polyfunctional acids and bases -An amphiprotic salt is a species that can act as an acid and as a base when dissolved in a suitable solvent

HA- + H2O ( A-2 + H3O+ (acidic)
HA- + H2O ( H2A + OH- (basic)

[H3O+] = (( Ka1 Ka2) (approx.) (eq 13-4)

|Example: Calculate the hydronium ion concentration of a 0.100 M NaHCO3 solution. |
|We first examine the assumptions leading to Equation 13-4. The dissociation constants for H2CO3 are Ka1 = 1.5e-4 and Ka2 = |
|4.69e-11. |
|[H3O+] = ((1.5e-4 x 4.69e-11) = 8.4e-8 M |

13D—Constructing Titration Curves for Polyfunctional Acids

-Compounds with two or more acid functional groups yield multiple endpoints in a titration, provided the functional groups differ sufficiently in strengths as acids.
-Included in a titration curve for a weak
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