In: Chemistry
Determine the percent ionization of a 0.014 M solution of hypochlorous acid, HClO. The Ka for the acid is 3.5x10^–8.
A) 3.5x10 ^–6 %
B) 4.9x10^–9 %
C) 7.0 x 10^–3 %
D) 5.0 x10^–2 %
E) 1.58x 10^–1 %
HClO----> H+ +ClO-
Initial HClO 0.014 H+ 0 ClO- 0
let x= drop in concentration of HClO due to equilibrium
Equilibrium HClO 0.014-x H+ x ClO- x
Ka= [H+] [ClO-]/ [HClO] =3.5*10-8
x2/(0.014-x)= 3.5*10-8,
Looking at the magnitude to K, it is reasonable to approximate 0.014-x as 0.014
x2/0.014= 3.5*10-8
x2= 3.5*0.014*10-8
x =0.000021
percent ionization=100*0.000021/0.014=0.15% ( E is the closest answer)