we have below equation to be used:
Ka = Kw/Kb
Kw is dissociation constant of water whose value is 1.0*10^-14 at 25 oC
Ka = (1.0*10^-14)/Kb
Ka = (1.0*10^-14)/1.8*10^-5
Ka = 5.556*10^-10
NH4+ + H2O -----> NH3 + H+
5.3*10^-2 0 0
5.3*10^-2-x x x
Ka = [H+][NH3]/[NH4+]
Ka = x*x/(c-x)
Assuming small x approximation, that is lets assume that x can be ignored as compared to c
So, above expression becomes
Ka = x*x/(c)
so, x = sqrt (Ka*c)
x = sqrt ((5.556*10^-10)*5.3*10^-2) = 5.426*10^-6
since c is much greater than x, our assumption is correct
so, x = 5.426*10^-6 M
so,
[H+] = x = 5.426*10^-6 M
we have below equation to be used:
pH = -log [H+]
= -log (5.426*10^-6)
= 5.27
Answer: 5.27
Feel free to comment below if you have any doubts or if this answer do not work
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