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- Homework Statement
- You are given two buffers [a) 0.1 M phosphate buffer of pH 7.7 and (b) 0.1 M phosphatebuffer at pH 6.71 . If acid is to be added to the buffers, which of them, do you think, will resist the pH changes better

- Relevant Equations
- Henderson Hesselbach Equation

pH = pKa + log([ conjugate base] /[ acid])

Here I used Henderson Hesselbach equation in both the cases , I.e

pH= pKa + log( [(PO4)3-]/ [H3PO4]) here pKa of phosphoric acid is 2.16 but the problem Is in both the cases the log part is same and Pka is also same so both will cancel out, and how can we solve? It is confusing.

pH= pKa + log( [(PO4)3-]/ [H3PO4]) here pKa of phosphoric acid is 2.16 but the problem Is in both the cases the log part is same and Pka is also same so both will cancel out, and how can we solve? It is confusing.