Chemistry problem, calculate percent ionization

[afcwestwarrior]

acetic acid is a weak acid that ionizes in solution as follows
CH3COOH--->CH3COO- + H+

if the freezing point of a .106 m CH3COOH solution is -.203 celsius, calculate the percent of the acid that has undergone ionization.

here's what i did, i took .203 celsius=i)1.86 celsius/m (.106m)

then i put .203/1.86(.106)=.103 which is i
then i took .103/2*100=5.15%
2 is the actual number formula units dissolved in the solution,

so did i do it right, it's a weak acid right, but I'm not sure if the percent is right

 

[afcwestwarrior]

so anyone know how to figure this out