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Chemistry

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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!

  • Chemistry -

    The ICE chart is not applicable in this case (actually you MAY use it but it's simpler to go another way). Use the Henderson-Hasselbalch 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%.

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