Given a diprotic acid, H2A, with two ionization constants of Ka1 = 4.89× 10–4 an

Question

Given a diprotic acid, H2A, with two ionization constants of Ka1 = 4.89× 10–4 and Ka2 = 5.68× 10–11, calculate the pH and molar concentrations of H2A, HA–, and A2– for each of the solutions below.

x10- Map Given a diprotic acid, H2A, with two ionization constants of Ka4.89x 10-4 and Ka2 5.68x 10-1 calculate the pH and molar concentrations of H2A, HA-, and A for each of the solutions below (a) a 0.165 M solution of H2A [H,A] PH HA Number Number Number (b) a 0.165 M solution of NaHA [H,A] HA Number Number Number (c) a 0.165 M solution of Na2 [HA] (HA- pH Number Number Number

Explanation / Answer

a) 0.165 M

4.89 x 10-4 = (x2) / 0.165

x = 0.8982 x  10-4

PH =-log [H+]

    = - log [0.8982 x 10-4]

= 3.95

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