Find the percent ionization of a 0.200 M HC2H3O2 solution at 25 C [Ka(HC2H3O2)=1.8x10^-5]
Lets write the dissociation equation of HC2H3O2
HC2H3O2 -----> H+ + C2H3O2-
0.2 0 0
0.2-x x x
Ka = [H+][C2H3O2-]/[HC2H3O2]
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 ((1.8*10^-5)*0.2) = 1.897*10^-3
since c is much greater than x, our assumption is correct
so, x = 1.897*10^-3 M
% dissociation = (x*100)/c
= 1.897*10^-3*100/0.200
= 0.9487 %
Answer: = 0.949 %
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