Part AAs a technician in a large pharmaceutical research firm, you need to produce 450.mL of 1.00 M a phosphate buffer solution of \rm pH = 7.16. The {\rm p}K_{\rm a} of \rm {H_2PO_4}^- is 7.21. You have 2.00 \rm L of 1.00 \rm M~KH_2PO_4 solution and 1.50 \rm L of 1.00 \rm M~K_2HPO_4 solution, as well as a carboy of pure distilled \rm H_2O. How much 1.00 \rm M~KH_2PO_4 will you need to make this solution?Express your answer numerically in milliliters to three significant figures. Volume of \rm KH_2PO_4 needed = \rm mL PART B The Henderson-Hasselbalch equation in medicineCarbon dioxide (\rm CO_2) and bicarbonate (\rm {HCO_3}^-) concentrations in the bloodstream are physiologically controlled to keep blood pH constant at a normal value of 7.4.Physicians use the following modified form of the Henderson-Hasselbalch equation to track changes in blood pH:\rm pH = p{\it K}_a + log \frac{[{HCO_3}^-]}{(0.030)({\it P}_{CO_2})}where \rm [{HCO_3}^-] is given in millimoles/liter and the arterial blood partial pressure of \rm CO_2 is given in \rm mmHg. The {\rm p}K_{\rm a} of carbonic acid is 6.1. Hyperventilation causes a physiological state in which the concentration of \rm CO_2 in the bloodstream drops. The drop in the partial pressure of \rm CO_2 constricts arteries and reduces blood flow to the brain, causing dizziness or even fainting.Part BIf the normal physiological concentration of \rm {HCO_3}^- is 24 {\rm m}M, what is the pH of blood if P_{\rm CO_2} drops to 24.0mmHg ?Express your answer numerically using one decimal place. pH =
Part AAs a technician in a large pharmaceutical research firm, you need to produce 450.mL of 1.00 M a phosphate buffer solution of \rm pH = 7.16. The {\rm p}K_{\rm a} of \rm {H_2PO_4}^- is 7.21. You have 2.00 \rm L of 1.00 \rm M~KH_2PO_4 solution and 1.50 \rm L of 1.00 \rm M~K_2HPO_4 solution, as well as a carboy of pure distilled \rm H_2O. How much 1.00 \rm M~KH_2PO_4 will you need to make this solution?Express your answer numerically in milliliters to three significant figures. Volume of \rm KH_2PO_4 needed = \rm mL PART B The Henderson-Hasselbalch equation in medicineCarbon dioxide (\rm CO_2) and bicarbonate (\rm {HCO_3}^-) concentrations in the bloodstream are physiologically controlled to keep blood pH constant at a normal value of 7.4.Physicians use the following modified form of the Henderson-Hasselbalch equation to track changes in blood pH:\rm pH = p{\it K}_a + log \frac{[{HCO_3}^-]}{(0.030)({\it P}_{CO_2})}where \rm [{HCO_3}^-] is given in millimoles/liter and the arterial blood partial pressure of \rm CO_2 is given in \rm mmHg. The {\rm p}K_{\rm a} of carbonic acid is 6.1. Hyperventilation causes a physiological state in which the concentration of \rm CO_2 in the bloodstream drops. The drop in the partial pressure of \rm CO_2 constricts arteries and reduces blood flow to the brain, causing dizziness or even fainting.Part BIf the normal physiological concentration of \rm {HCO_3}^- is 24 {\rm m}M, what is the pH of blood if P_{\rm CO_2} drops to 24.0mmHg ?Express your answer numerically using one decimal place. pH =
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