<p>i have a couple questions that im confused on for my AP Chem class--</p>
<p>first, when a weak base is titrated with a strong acid, what is the pH at equivalence point??</p>
<p>( i know that for weak acid/strong bases the pH is less than 1... at least im fairly certain)</p>
<p>and when weak bases are titrated with weak acids, whats the pH at equivalence point? </p>
<p>Thanks!</p>
<p>Depends on the pH of the weak acid/base-I had a titration that was at pH 6.1.</p>
<p>well, I think when a weak base is titrated w/ a vert strong acid, then the pH is very small <the solution="" is="" acidic="">
when a weak base is titrated to a weak acid, the pH is about 7 <approximately neutral=""></approximately></the></p>
<p>okay, weak base + strong acid</p>
<p>lets use NH3 + HCl, weak base and strong acid</p>
<p>NH3 + HCl --> NH4+ + Cl-, then equilibrium the NH4+
NH4+ <--> NH3 + H+</p>
<p>the presence of the H+ after, drops the pH to less than 7 (can't give accurate values without real chemicals)</p>
<p>weak acid + strong base would be the exact opposite, pH would be over 7 at the equivalence point</p>
<p>HC2H3O2 (acetic acid) + NaOH --> H2O + Na+ + C2H3O2-
C2H3O2- + H2O <--> HC2H3O2 + OH-</p>
<p>the extra OH- makes equivalence point greater than 7</p>
<p>i dont think we covered weak bases w/ weak acids
but it depends on how weak the bases and acids are (whether its like HC2H3O2 or like HPO4- or somethin)
in general however, it will be around 7.</p>