how are percent ionization values similar to equilibrium constant values? explain your reasoning and identify which weak acid would have the smallest equilibrium constant.

weak acid

percent ionization

hno2

6.2%

hclo2

28.2%

hcn

0.007%

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.

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