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How many moles of H2PO4 and HPO4 would be needed to prepare 1.0 L of a 0.01M phosphate buffer with a pH of 6.82?

Use the Henderson-Hasselbalch equation.
pH = pKa + log (base)/(acid).

Thank you, but I guess what my question should have been is what is the acid in this question and what is the base. I would assume that both H2PO4 and HPO4 are acids and phosphate is the base but Im not sure.

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