(a) Let a be the dissociation of the weak acid
HA <---> H + + A-
initial conc. c 0 0
change -ca +ca +ca
Equb. conc. c(1-a) ca ca
Dissociation constant , Ka = ca x ca / ( c(1-a)
= c a2 / (1-a)
In the case of weak acids a is very small so 1-a is taken as 1
So Ka = ca2
==> a = √ ( Ka / c )
Given Ka = 1.8x10-4
c = concentration = 0.036 M
Plug the values we get a = 0.0707
∴ % dissociation = 0.0707 x 100 = 7.07%
(b) when c = 3.7x10-4M
Then a = 0.697
∴ % dissociation = 0.697 x 100 = 69.7%
(c) when c = 1.25 M
Then a = 0.012
∴ % dissociation = 0.012 x 100 = 1.2%
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