Prove that Ka x Kb = Kw for a conjugate acid/base pair.
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The equation of the dissociation of a weak acid HA in solution is:
HA + H2O <===> H3O+ + A¯
and its Ka expression is:
[H3O+] [A¯] | |
Ka = | ---------------- |
[HA] |
The equation for the ionization of a weak base A¯ in solution is:
A¯ + H2O <===> HA + OH¯
and its Kb expression is:
[HA] [OH¯] | |
Kb = | ---------------- |
[A¯] |
Rearrange the Ka expression above as follows:
[H3O+] | [HA] | |
---------- | = | --------- |
Ka | [A¯] |
and substitute the left-hand portion into the Kb expression from above to obtain:
[H3O+] [OH¯] | |
Kb = | -------------------- |
Ka |
Since the equation for the ionization of water is:
Kw = [H3O+] [OH¯]
by substitution and rearrangement, we obtain:
KaKb = Kw
Hope this helped.
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