In an aqueous solution of a certain acid with pKa = 7.33 the pH is 4.59. Calculate the percent of the acid that is dissociated in this solution. Round your answer to 2 significant digits.
pKa = -log Ka
7.33 = -log Ka
Ka = 4.677*10^-8
Let the concentration of HA be c
use:
pH = -log [H+]
4.59 = -log [H+]
[H+] = 2.57*10^-5 M
HA dissociates as:
HA -----> H+ + A-
c 0 0
c-x x x
x = [H+] = 2.57*10^-5 M
Ka = [H+][A-]/[HA]
Ka = x*x/(c-x)
4.677*10^-8 = 2.57*10^-5*2.57*10^-5/(c-2.57*10^-5)
c-2.57*10^-5 = 1.413*10^-2
c=1.415*10^-2 M
% dissociation = x*100/c
= (2.57*10^-5)*100 / (1.415*10^-2)
= 0.182 %
Answer: 0.18 %
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