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As a technician in a large pharmaceutical research firm, you need to produce 150.mL of a 1.00 M phosphate buffer solution of pH = 7.10. The pKa of H2PO4- is 7.21. You have 2.00 L of 1.00 M KH2PO4 solution and 1.50 L of 1.00 M K2HPO4 solution, as well as a carboy of pure distilled H2O. How much 1.00 M KH2PO4 will you need to make this solution? I got the Henderson Hasselbalch ration (.776) but don't know where to go from there

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