Posted by Kelly on Tuesday, November 9, 2010 at 10:34am.
Use the Henderson-Hasselbalch equation.
5.10 = 4.74 + log(base/acid)
Calculate ratio base/acid. You know you have added 2 mmoles NaOH which will allow you to calculate acid at the pH = 5.10 point. Determine the amount mL required to neutralize that many mmoles acid, add to the 20 mL already used, then
mL x M = mL x M to arrive at the original M acid. Post your work if you get stuck. I get something like 0.072 but that is jut a quickie calculation. You need to be more precise than that. .
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