The greater the percent ionization the larger will be the equilibrium constant.
Consider the HCN which is 0.007% ionization. For a 0.10 M solution, 0.00007(.10) will give the [H+] = 7 x 10^-6
K = [H+][CN-]/[HCN]
K = 7 x 10^-6*(7 x 10^-6)/0.1
K = 4.9 x 10^-10
Consider the HClO2 which is 28.2%. [H+] = 0.28(0.10) = 0.028. Substituting in the K expression
0.028(0.028)/0.10 - 0.028 which will give a larger equilibrium constant.
