Question

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?

Answer 1

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?