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<div class="moz-cite-prefix">On 04/14/2013 05:31 PM, wrote:<br>
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<div style="direction: ltr;font-family: Tahoma;color:
#000000;font-size: 10pt;">I'm confused on how to find the pKa of
the unknown in the lab. My only idea would to be to find the
[H+] and do an icebox. Is that right?</div>
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In part II number 3, when you recombine the neutralized half of
the weak acid with the half that you kept separate you have made a
"buffer". You combined solution contains a weak acid that is
titrated halfway to its endpoint. By definition, the pH of this
solution is equal to the pKa of the weak acid.<br>
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<pre class="moz-signature" cols="72">--
Andrew J. Pounds, Ph.D. (<a class="moz-txt-link-abbreviated" href="mailto:pounds@theochem.mercer.edu">pounds@theochem.mercer.edu</a>)
Associate Professor of Chemistry and Computer Science
Mercer University, Macon, GA 31207 (478) 301-5627
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