<p>When you're titrating a weak acid with a strong base, what exactly is neutralized? Is it just the part of the acid that is dissociated (the H+ ions already in solution), or does all of the acid present get neutralized, because as the reaction takes place, more of the acid dissociates to reestablish equilibrium?</p>
<p>the pH will be < 7.</p>
<p>Runner - the second part of what you said is correct. You can think of the strong base as "pulling" all of the H's off the weak acid.</p>
<p>Ex: 50mL of 0.1M acetic acid will be neutralized when .005 moles of NaOH is added to it.</p>
<p>Actually, the pH will be greater than 7. All the hydroxides will neutralize the H's, both the ones dissociated and the ones that are not. It's then the conjugate base of the weak acid that undergoes hydrolysis, relasing separate OH's that make the solution basic.</p>
<p>I thought the pH is >7 since some of the conjugate base will take up some H+ to from the weak acid.</p>
<p>yes, but they get those H+'s from water, leaving OH- behind.</p>
<p>Ex (C2H3O2)- + H2O --> HC2H3O2 + OH-</p>
<p>I think both explanations are good actually, but the best wold be:</p>
<p>"Conjugate base removes H+ from solution and leaves behind OH- in order to reform its weak acid."</p>
<p>Yes, my bad. I read strong acid + weak base. pH > 7 for strong base + weak acid, pH < 7 for strong acid + weak base.</p>