Part A As a technician in a large pharmaceutical research firm, you need to prod

Question

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

Explanation / Answer

you have to solve 2 equations..because you have 2 unknowns. (volume of base)/(volume of acid) = 0.741 and (volume of base) + (volume of acid) =.45L so solve for one variable in terms of the other and substitute and you can find the answer easily...Hopefully this helps.

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