How to find pH of a diprotic acid titrated by a strong base
Given 20.0 mL 0.25 M of H2CO3 (Ka1=6.4x10^-6 and Ka2= 6.9x10^-10) titrated by a 0.50 M solution of NaOH, Identify the following:
a) Veq1 and Veq2 = 10 mL and 20 mL respectively
b)The pH at the following points:
0ml of added titrant = 2.90
1/2 Veq1 = 5.19
3 mL past Veq1
at 1/2 way between Veq1 and Veq2
5ml past veq2.
I pretty much have up to the pH of Veq1. I don't know how to get that. I also tried doing the ones after that but i don't get the right answers at all. Any help pointed towards the right direction would be so helpful!
Last edited by jimenezs; Apr 9th 2017 at 09:18 AM.
Reason: Forgot molarity