Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: mpire344 on September 03, 2009, 09:49:08 PM
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I need to determine the volumes of 0.10 M NaH2PO4 and 0.10 M Na2HPO4 that need to be mixed
together to produce 100 mL of a buffer at pH 7.0. The second pKa of H3PO4 is 7.2.
The problem I seem to run into is that the molarities of the two components are too weak to create that buffer in a combined total 100 mL of each of the compounds.
Any help would be appreciated.
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Show your calculations, no problems with getting correct pH with these solutions.
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7= 7.2 + log A/HA
A/HA= 0.630
A= 0.630HA
Let X = amount of H2PO4 used (mL)
0.630X + X = 100 Ml (volume of buffer needed for problem)
x= 61.31 mL H2PO4
100ml-61.31= 38.69 mL HPO4
Is this method methodologically sound? When I calculate moles of each using this method and insert the corresponding answers into the Henderson-Hasselbach equation, I get a ph thats greater than 7.
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Looks perfect to me.
Perhaps you do something wrong when you are trying to calculate pH afterwards.
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Borek, I realize what I was doing wrong.
When I was calculating base/acid ratio for Henderson-Hasselbach, I was subtracting A- moles from HA moles because I thought one neutralized the other.
Anyways thanks for your help.
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Snacks for all. Huzzah!