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As a technician in a large pharmaceutical research firm, you need to produce 150. mL of 1.00 mol L potassium phosphate buffer solution of pH = 7.09. The pKa of H2PO4 is 7.21. You have the following supplies: 2.00 L of 1.00 mol L KH2PO4 stock solution, 1.50 L of 1.00 mol L K2HPO4 stock solution, and a carboy of pure distilled H20. How much 1.00 mol L KH3PO4 will you need to make this solution? Express your answer to three significant digits with the appropriate units. The Henderson-Hasselbalch equation in medicine Carbon dioxide (CO2) and bicarbonate (HCO3) concentrations in the bloodstream are physiologically controlled to keep blood pH constant at a normal value of 7.40. Physicians use the following modified form of the Henderson-Hasselbalch equation to track changes in blood pH: pH = pKa + log- [HCO3 ] (0.030)(Pco2 where [HCO3] is given in millimoles/litre and the arterial blood partial pressure of CO2 is given in mmHg. The pKa of carbonic acid is 6.1. Hyperventilation causes a physiological state in which the concentration of CO2 in the bloodstream drops. The drop in the partial pressure of CO2 constricts arteries and reduces blood flow to the brain, causing dizziness or even fainting. Part B If the normal physiological concentration of HC03 is 24 mmol L-1, what is the pH of blood if PCo, drops to 23.0 mmHg ? Express your answer numerically using two decimal places. • View Available Hint(s) ΑΣΦ ? pH = Submit As a technician in a large pharmaceutical research firm, you need to produce 150. mL of 1.00 mol L potassium phosphate buffer solution of pH = 7.09. The pKa of H2PO4 is 7.21. You have the following supplies: 2.00 L of 1.00 mol L KH2PO4 stock solution, 1.50 L of 1.00 mol L K2HPO4 stock solution, and a carboy of pure distilled H20. How much 1.00 mol L KH3PO4 will you need to make this solution? Express your answer to three significant digits with the appropriate units. The Henderson-Hasselbalch equation in medicine Carbon dioxide (CO2) and bicarbonate (HCO3) concentrations in the bloodstream are physiologically controlled to keep blood pH constant at a normal value of 7.40. Physicians use the following modified form of the Henderson-Hasselbalch equation to track changes in blood pH: pH = pKa + log- [HCO3 ] (0.030)(Pco2 where [HCO3] is given in millimoles/litre and the arterial blood partial pressure of CO2 is given in mmHg. The pKa of carbonic acid is 6.1. Hyperventilation causes a physiological state in which the concentration of CO2 in the bloodstream drops. The drop in the partial pressure of CO2 constricts arteries and reduces blood flow to the brain, causing dizziness or even fainting. Part B If the normal physiological concentration of HC03 is 24 mmol L-1, what is the pH of blood if PCo, drops to 23.0 mmHg ? Express your answer numerically using two decimal places. • View Available Hint(s) ΑΣΦ ? pH = Submit
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part A The pH of a buffer can be calculated using the Henderson equation which is given below pH ... View the full answer
Related Book For
Fundamentals of biochemistry Life at the Molecular Level
ISBN: 978-0470547847
4th edition
Authors: Donald Voet, Judith G. Voet, Charlotte W. Pratt
Posted Date:
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