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Titration curve | Topic profile

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Latest threads on titration curve:

Undergraduate General Chemistry Forum
Started 2 weeks, 3 days ago (2009-12-09 12:52:00)  by bioguy2
okay so i am having trouble trying to figure out how to do a titration curve for this particular problem.  if 30.00 mL of .2000 M NaOH and 30.00 mL of .300 M NH3 is titrated with .400 M HCl, sketch the curve while showing work for each point on the curve.  So i understand how to do this problem if it was a diprotic acid, but i am not sure how to start this problem with both .300 NH3 and .2000 M ...
Undergraduate General Chemistry Forum
Started 1 week, 4 days ago (2009-12-15 12:44:00)  by Borek
There will be one, continuous titration curve. Its calculation can be a little bit tricky at the end of NaOH neutralization - when 99.9% of NaOH is neutralized you may expect pH to go fast down (inflection point) - but it can't, as curve must be continuous. Here ammonia starts to play important role, even if NaOH is not yet 100% neutralized.
High School Chemistry Forum
Started 1 month ago (2009-11-26 06:54:00)  by hanagasumi
Hi everyone:   I got this lab for the titration curve, and the lab is trying to find the neutralization equation for acetic acid and NaOH. then we are asked to calculate the Ka for the dissociation of the acetic acid, and the pH will be determined by doing the lab, how should I calculate the Ka?  And I'm really confused what this lab is doing, please *delete me*!
High School Chemistry Forum
Started 1 month ago (2009-11-26 11:16:00)  by renge ishyo
You can get the pKa directly from your graph. First find the volume of the endpoint (the point where the slope of your graph changes most abruptly from low PH to high pH). Next, divide the endpoint volume by 2 to get the volume added halfway to the endpoint. The pH at the volume halfway to the endpoint is equal to the pKa. You can find the Ka from pKa = -log[Ka] or solving for Ka: 10 -pKa = Ka.
 

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