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Part A As a technician in a large pharmaceutical research firm, you need to produce 350....

Part A As a technician in a large pharmaceutical research firm, you need to produce 350. mL of a potassium dihydrogen phosphaPart B If the normal physiological concentration of HCO3 is 24 mM, what is the pH of blood if Pco, drops to 31.0 mmHg ? Expre

Part A As a technician in a large pharmaceutical research firm, you need to produce 350. mL of a potassium dihydrogen phosphate buffer solution of pH = 6.92. The pKa of H2PO4 is 7.21. You have the following supplies: 2.00 L of 1.00 M KH2PO4 stock solution, 1.50 L of 1.00 M K2HPO4 stock solution, and a carboy of pure distilled H2O. How much 1.00 M KH2PO4 will you need to make this solution? (Assume additive volumes.) Express your answer to three significant digits with the appropriate units. ► View Available Hint(s) .: HÅR O 2 ? Volume of KH2PO4 needed = Value Units Submit
Part B If the normal physiological concentration of HCO3 is 24 mM, what is the pH of blood if Pco, drops to 31.0 mmHg ? Express your answer numerically using two decimal places. View Available Hint(s) TO ADD A O O ? pH = Submit
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Answer #1

The Ka values for the phosphoric acid are The phosphoric acid has the following ionizations H3PO4 = H2PO4 + H+ H2PO4 = HPO4-2

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The bicarbonate buffer system is CO,+H,02H,CO, 2HCO +H* pH of the buffer is determined by the Henderson equation, CO, +H20 FH

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