<p>For the SAT II chem, will there be a question asking to calculate a titration? I've never been taught titrations and I find it hard to do one without a calculator. A quick look through the prac tests in Barrons looks like there aren't that many calculations, but I would liked some opinions :)</p>
<p>Uhh from what I remember of the test there was maybe one out of one hundred and fifteen questions on titrations. And the numbers were easy, like the powers cancelled and it was totally doable without a calculator!</p>
<p>Thanks! Here’s a question from Sparknotes. It’s not that hard until the end. How would I know what the log of 0.11 is? Will a question like this show up?</p>
<p>What is the pH of a solution of 0.36 M HCl, 0.62 M NaOH, and 0.15 M HNO3?</p>
<p>Solution for Problem 1:
Hydrochloric acid and nitric acid are strong acids, and sodium hydroxide is a strong base; these all dissociate completely. The total [H+] from the two acids is 0.51 M and [OH-] from NaOH is 0.62 M. Therefore, 0.51 moles per liter of H+ will react with 0.51 moles per liter of OH- to form water. That leaves a 0.11 M NaOH solution. The pOH of a 0.11 M NaOH solution is 0.96 pOH units, and the pH is 13.04 pH units.</p>
<p>Edit: <a href=“http://www.sparknotes.com/chemistry/acidsbases/phcalc/problems.html[/url]”>http://www.sparknotes.com/chemistry/acidsbases/phcalc/problems.html</a> actually Ill just post the link</p>
<p>You won’t be expected to calculate log(0.11) exactly, but you can estimate. log(0.11) is about log(0.10) which is -1. Therefore the pH would be 14-1 = 13. The answer choices you have will all be sufficiently different to allow you to estimate like this, for example you might be asked to pick from</p>
<p>10
11
12
13
14</p>
<p>And 13 is clearly closest.</p>
<p>For Titrations use the formula MaVa=MbVb </p>
<p>Ma=Molarity of Acid, Mb= Molarity of Base, Va= Volume of acid, Vb= Volume of base</p>