<p>Will you have to know how to find the exact pH of the titration of a weak acid/conjugate base through calculations? (Not just eyeballing the graph and finding the middle of the steepest point)</p>
<p>You mean use the Henderson-Hasselbalch equation? You need to be able to use that.</p>
<p>There is a little bit of confusion in the original question. There is never a "weak acid/conjugate base" titration. When a weak acid is titrated with a strong base, there are four distinct reagions in the curve, each with its own method of finding pH. (1) The initial point is a solution with only a weak acid. As with any solution containing only weak acid, do a Ka icebox. (2) During the titration (before the endpoint) the base has neutralized some of the acid, converting it to conjugate base, so the resultant solution is a mixture of weak acid/conjugate base. As with any weak acid/conj base mixture, do the Henderson-Hasselbalch calculation. (3) At the endpoint, all the weak acid has been neutralized - the only significant species present is the conjugate base. As with any solution containing only a weak base, do a weak base icebox using Kb= Kw/Ka. (4) After the endpoint, the solution contains a mixture of weak base and strong base (from the excess base that was added.) As with any mixture of strong base/weak base ignore the weak base and do pH = 14-log [OH-].
Yes, you need to know how to do all four of these calculations.</p>
<p>^^ ty.........</p>