The amino acid glycine (H2N—CH2—COOH) can participate in the following equilibria in water:
H2N—CH2—COOH + H2O ⇌ H2N—CH2—COO- + H3O+ Ka = 4.3 × 10-3
H2N—CH2—COOH + H2O ⇌ H3N—CH2—COOH + OH– Kb = 6.0 × 10-5
(a) Use the values of Ka and Kb to estimate the equilibrium constant for the intramolecular proton transfer to form a zwitterion:
H2N—CH2—COOH ⇌ +H3N—CH2—COO–
(b) What is the pH of a 0.050 M aqueous solution of glycine?
(c) What would be the predominant form of glycine in a solution with pH 13? With pH 1?
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