Chemistry
posted by howie on .
Calculate the percent ionization of cyanic acid, Ka=2.0x10^4, in a buffer soln that is .50M HCNO and .10M NaCNO.
Answer is .20%.
So,I know that NaCNO>Na+ + CNO
so [CNO]=.10M from ICF chart.
and then HCNO <=>H+ + CNO
where: [HCNO]= .5
and [CNO]=.1
With an ice table , i keep on getting x=.001 which means the percent ionization would be 1% instead of .2%
Help!

The ICE chart is not applicable in this case (actually you MAY use it but it's simpler to go another way). Use the HendersonHasselbalch equation, since this is a buffered solution, to solve for pH of the solution and convert that to H^+, then solve the percent ionization. I worked the problem and I did obtain 0.2%.