I'm struggling with an weak acid / strong base titration of a diprotic acid.. question
How would you get the pH of the solution after the 2nd equivalence point has been reached?
titrating 100 mL of 1.0 M oxalic acid with 1.0 M NaOH
Acid dissociation constants of oxalic acid are Ka1= 5.36X10^-2 and Ka2= 5.3X10^-5
-It would take a total of 200 mL of NaOh to reach the equivalence point
What is the pH after 50 mL of NaOH has been added after the 2nd equivalence point has been reached?
Is the only thing I have to consider the excess diluted NaOH?
- 0.05 L X 1.0 M = 0.05 moles base
- 0.05 / 0.250 L = 0.2 M base
pOH = -log (0.2) = 0.699
pH = 14 - 0.699 = 13.30
Is this correct?
Thanks in advance!