Ka of a monoprotic weak acid = 6.55 × 10^-3
concentration of acid = 0.176 M
HA ------------------> H+ + A-
0.176Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â
0Â Â Â Â Â Â Â Â 0
0.176 -
x                  Â
x         x
Ka = x^2 / 0.176 - x
6.55 × 10^-3 = x^2 / 0.176 - x
x = 0.0308
[H+] = 0.0308 M
percent ionization % = ([H+] / initial concentration ) x 100
                               Â
= (0.0308 / 0.176) x 100
                               Â
= 17.5%
percent ionization % = 17.5%
