Concentration of H3O+ = 0.13 M
concentration of OH- = 7.7 x 10^-14 M
concentration of HSeO4- = 0.11 M
concentration of SeO4^2- = 0.010 M
First dissociation
H2SeO4 (aq) + H2O (l)
HSeO4- (aq) + H3O+ (aq)
Since Ka1 is very large, all H2SeO4 dissociates to HSeO4- and H3O+
now concentration of HSeO4- = initial concentration of H2SeO4 = 0.12 M
concentration of H3O+ = initial concentration of H2SeO4 = 0.12 M
Second dissociation
ICE table | HSeO4- (aq) | H2O (l) | ![]() |
SeO4^2- (aq) | H3O+ (aq) |
Initial conc. | 0.12 M | - | 0 | 0.12 M | |
Change | -x | - | +x | +x | |
Equilibrium conc. | 0.12 M - x | - | +x | 0.12 M + x |
Ka2 = [SeO4^2-]eq[H3O+]eq / [HSeO4-]eq
1.2 x 10^-2 = [(x) * (0.12 M + x)] / (0.12 M - x)
Solving for x, x = 0.010 M
[H3O+] = 0.12 M + x
[H3O+] = 0.12 M + 0.010 M
[H3O+] = 0.13 M
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