The Ka of a monoprotic weak acid is 2.45*10^-3. What is the percent ionization of a 0.137 M solution of this acid?

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accessdenied · Answer

So, we know the concentration of the weak acid initially and the Ka is a ratio of products to reactant.
   HA  <-->  H+  +   A-.
The percent ionization would be the concentration of H+  coming out in equilibrium per molar HA we had started with.  So we must first find the concentration of H+ at equilibrium (ICE chart) and then take the ratio of [H+] created over the initial [HA] started with.  Does that sound good?