Perhaps the easier question is this:
If i have an excess of [OH-] ions in a solution, and use a weak acid to neutralize it, will the weak acid eventually completely dissociate?
My logic is the following:
At first, the weak acid would only partially dissociate, but all of the dissociated H+ ions would get totally consumed by neutralizing OH- ions. So to maintain equilibrium, the weak acid would partially dissociate again, and again all of the dissociated H+ ions would get totally consumed, and this cycle would continue until the weak acid is totally dissociated.