|Feb4-06, 03:29 PM||#1|
Acid Base Titration: Finding pH
I am having trouble with acid-base titration excercises. 0.02 L butanoic acid @ 0.1 M is titrated with 0.01 L NaOH solution @ 0.1 M. The Ka of butanoic acid is 1.54X10^-5. Find the pH. The answer is 4.81. I know how to find the pH when no NaOH is added, but I really dont see how the Ka fits in when adding a base. An explanation would really be appreciated. Thanks.
|Feb4-06, 06:16 PM||#2|
First you have a weak acid solution, then it is a buffer so you should use Henderson-Hasselbalch equation and finally you have conjugate base solution with pH defined by hydrolyzis.
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