Chemistry
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Part A 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 = 7.00. The pKa of H2PO4 is 7.21. %3D 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 H2O. How much 1.00 mol L KH2PO4 will you need to make this solution? Express your answer to three significant digits with the appropriate units. > View Available Hint(s) HA ? Volume of KH2PO4 needed = Value Units Submit Previous Answers X Incorrect; Try Again; 5 attempts remaining The Henderson-Hasselbalch equation in medicine (ICOOoncentrations in the bloodstream are physiologically controlled to keep
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Transcribed Image Text:Part A 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 = 7.00. The pKa of H2PO4 is 7.21. %3D 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 H2O. How much 1.00 mol L KH2PO4 will you need to make this solution? Express your answer to three significant digits with the appropriate units. > View Available Hint(s) HA ? Volume of KH2PO4 needed = Value Units Submit Previous Answers X Incorrect; Try Again; 5 attempts remaining The Henderson-Hasselbalch equation in medicine (ICOOoncentrations in the bloodstream are physiologically controlled to keep
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: [HCO3 pH = pKa+ log 0.030)(Pco,) 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 HCO3 is 24 mmol L-, what is the pH of blood if Pco, drops to 35.0 mmHg ? Express your answer numerically using two decimal places. View Available Hint(s) Αφ ? pH =
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Transcribed Image Text: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: [HCO3 pH = pKa+ log 0.030)(Pco,) 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 HCO3 is 24 mmol L-, what is the pH of blood if Pco, drops to 35.0 mmHg ? Express your answer numerically using two decimal places. View Available Hint(s) Αφ ? pH =
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