Determining [H30+] in a 1.4x10^-2 solution of CH3COOH

Determining [H30+] in a solution of CH3COOH?

Where Ka = 1.7X10^-5

formula simplified pH=(pKa-logc)/2

Ka=1.75*10^-5 pKa= log (1/Ka) =log ( 1/1.7*10^-5)=4.77

pH= (4.77-log (0.014))/2=(4.77-(-1.854))/2=3.312

[H3O]+ =10^-3.312=4.876*10^-4 mole/L of ions [H3O+]