A certain weak acid, HA, has a Ka value of 9.1×10−7.
Part A
Calculate the percent dissociation of HA in a 0.10 M solution.
Part B
Calculate the percent dissociation of HA in a 0.010 M solution.
Part A :
Let a be the dissociation of the weak acid,HA
HA <---> H + + A-
initial conc. c 0 0
Equb. conc. c(1-a) ca ca
Dissociation constant , Ka = ca x ca / ( c(1-a)
= c a2 / (1-α)
In the case of weak acids α is very small so 1-a is taken as 1
So Ka = ca2
==> a = √ ( Ka / c )
Given Ka = 9.1x10-7
c = concentration = 0.10 M
Plug the values we get a = 3.02 x10-3
∴ % dissociation = 3.02x10-3 x 100 = 0.3 %
Part B :
a = √ ( Ka / c )
Given Ka = 9.1x10-7
c = concentration = 0.010 M
Plug the values we get a = 9.54 x10-3
∴ % dissociation = 9.54 x10-3 x 100 = 0.95 %
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