Given a diprotic acid, H2A, with two ionization constants of Ka1 = 3.9× 10–2 and Ka2 = 5.9× 10–8.
Calculate the pH and molar concentrations of each protonated form for a:
(a)0.135 M solution of H2A
pH=
[H2A]=
[HA]=
[A2-]=
(b)0.135 M solution of NaHA
pH=
[H2A]=
[HA]=
[A2-]=
(c)0.135 M solution of Na2A
pH=
[H2A]=
[HA]=
[A2-]=
1 answer
I showed you how to get started at your earlier post. I should point out, too, that [A^2-] is not a protonated form for H2A.
1 answer