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Old Apr 9th 2017, 09:15 AM   #1
jimenezs
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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
3ml= 4.82
1/2 Veq1 = 5.19
at Veq1
3 mL past Veq1
at 1/2 way between Veq1 and Veq2
at 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 10:18 AM. Reason: Forgot molarity
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general chemistry, titration, weak acid



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