- #1
ReidMerrill
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Homework Statement
Phosphate, present to an extent of 0.01 M, is one of the main buffers in blood plasma, whose pH is 7.45. Would phosphate be as useful if the plasma pH were 8.5?
Homework Equations
pH = pKa+log[A/HA]
Ka1 = 7.11x10^-3 pka1= 2.148
Ka2=6.34x10^-8 pka2= 7.198
Ka3 = 4.22x10^-13 pka3=12.375
The Attempt at a Solution
Since the pH would still be between pka2 and pka3 so the phosphate would not gain or lose a hydrogen because of that change and the henderson-hasselbalch equation would still use the same pka. Does this mean it would be just as effective at pH 8.5 or am I missing something?