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<div class="moz-cite-prefix">On 10/20/2015 08:03 PM, wrote:<br>
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cite="mid:63b734372db4410b9bc2a0178968c1a7@spiderman.MercerU.local"
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<div dir="ltr">Hi Dr. Pounds,
<div> How exactly do I find the mmol of excess HCL and the mmol
of CaCO3? What values do I use?</div>
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<div>Thanks, <br clear="all">
<div><br>
</div>
-- <br>
<div class="gmail_signature">
<br>
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<br>
<font face="serif">The excess millimoles of HCl was what was
titrated with your HCl. So... <br>
<br>
<br>
(volume of base in ml) (molarity of base)<br>
<br>
The millimoles of acid neutralized by the antacid tablet is
therefore<br>
<br>
(20.0 ml)(molarity of acid) - </font><font face="serif"><font
face="serif">(volume of base in ml) (molarity of base)<br>
<br>
<br>
</font>2 moles of HCl are neutralized for each mole of CaCO3 so
take the moles of acid neutralized by the tablet and divide this
quantity by two to get the mmol of CaCO3 per tablet. Multiply
this number by the molar mass of CaCO3 to get the mg CaCO3 per
tablet.<br>
</font><br>
<br>
<pre class="moz-signature" cols="72">--
Andrew J. Pounds, Ph.D. (<a class="moz-txt-link-abbreviated" href="mailto:pounds_aj@mercer.edu">pounds_aj@mercer.edu</a>)
Professor of Chemistry and Computer Science
Mercer University, Macon, GA 31207 (478) 301-5627
<a class="moz-txt-link-freetext" href="http://faculty.mercer.edu/pounds_aj">http://faculty.mercer.edu/pounds_aj</a>
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