|May22-08, 03:07 AM||#1|
How much OH- must be added to achieve desired pH?
1. The problem statement, all variables and given/known data
Glycine which has a pKa of 9.6 can exist in protonated form (-NH3+) or as the free base (-NH2) because of the reversible equalibrium R-NH3+ <------> R-NH2 + H+.
How much 5 M KOH must be added to 1.0 L of 0.1 M glycine at pH 9 to bring the pH to exactly 10?
2. Relevant equations
3. The attempt at a solution
I have spent a couple hours trying to figure this out but don't really know where to start. A couple hints might point me in the right direction
|May22-08, 03:48 AM||#2|
When you add KOH to pH 9 glycine solution you are in fact neutralizing -NH3+.
Use Henderon-Hasselbalch equation to calculate amount of -NH3+ in solution at pH 9 and 10, then it is a simple stoichiometry.
|May22-08, 10:45 AM||#3|
Thanks Borek, very helpful :).
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