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<div class="moz-cite-prefix">On 07/22/2015 08:57 PM, wrote:<br>
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<p>Hi Dr. Pounds,</p>
<p><br>
</p>
<p>I just had a question about one of the example problems on
the powerpoint for chapter 17. On slide 12, 100 mL of 1.00M of
HCL was added to the solution made in the previous slide. It
says that the H+ will combine with the acetate ion and form
acetic acid. Does this mean that it is a reverse reaction? If
so, why does the ICE table signify that it is a forward
reaction (since it is positive on the products side)? </p>
<p><br>
</p>
<p>Thank you,</p>
<p><br>
</p>
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<br>
There are two separate things happening here. <br>
<br>
First, when you add the strong acid it immediately dissociates and,
if there is conjugate base available, forms the weak acid. This
has nothing to do with the ICE table. <br>
<br>
The second thing that happens is that the system then establishes
equilibrium based on these new initial concentrations. The <img
style="vertical-align: middle"
src="cid:part1.01050809.06010500@mercer.edu" alt="$K_a$"> value is
a dissociation constant, and as such we write ICE table for the
dissociation of the weak acid to form the hydronium ion and the
conjugate base of the weak acid.<br>
<br>
HA + H<img style="vertical-align: middle"
src="cid:part2.00080601.07000506@mercer.edu" alt="$_2$">O -> H<img
style="vertical-align: middle"
src="cid:part3.01070807.07020909@mercer.edu" alt="$_3$">O<img
style="vertical-align: middle"
src="cid:part4.04030904.07010602@mercer.edu" alt="$^+$"> + A<img
style="vertical-align: middle"
src="cid:part5.02040100.00070805@mercer.edu" alt="$^-$"><br>
<br>
<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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