[shoofy2]

Once again, my chemistry texts failed to provide a satisfactory answer to my dilemma:

When titrating a weak acid with a strong base, I know that the pH at the equivalence point will be higher than pH 7, since the strong base releases all its OH- ions while the weak acid only disassociates partially. But here is my problem: wouldn't the OH- and H+ form water, and thus, by Le Chatelier's Principle, cause the weak acid to push out even more H+ ions? Eventually, the OH- would "draw out" all the H+ from the weak acid, thus giving a neutral equivalence point.

What's wrong here?

Thanks for your time.
 

[Borek]

At the equivalence point you have a solution of salt of a weak acid. Anion is a conjugate base and will react with water.