For a diprotic acid, why does the autoionization of water have a greater impact on the pH at the second equivalence point?
for example H2A is diprotic acid
H2A + H2O -----------> HA- + H3O+
now for second dissociation.
HA- + H2O -------> A-2 + H3O+
Ka of HA- is lower compared to HA
so second dissociation is slower compared to first.
and already solution contaion H3O+ ions from first dissociation so second dissociation becomes much weaker due to common ion effect.
so H3O+ from second dissociation is very less.
so autoionization of H2O has greater impact.
while in first dissociation more H3O+ comes from H2A
so autoionization do nothave much impact.
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