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▼ Part A As a technician in a large pharmaceutical research firm, you need to produce 450. mL of 1.00 M potassium phosphate buffer solution of pH = 6.91. The pK, 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 MK₂HPO4 stock solution, and a carboy of pure distilled H₂O. How much 1.00 M KH₂PO4 will you need to make this solution? Express your answer to three significant digits with the appropriate units. View Available Hint(s) Volume of KH₂PO4 needed = HA Value Units ?

▼ Part A As a technician in a large pharmaceutical research firm, you need to produce 450. mL of 1.00 M potassium phosphate buffer solution of pH = 6.91. The pK, 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 MK₂HPO4 stock solution, and a carboy of pure distilled H₂O. How much 1.00 M KH₂PO4 will you need to make this solution? Express your answer to three significant digits with the appropriate units. View Available Hint(s) Volume of KH₂PO4 needed = HA Value Units ?

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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The Henderson-Hasselbalch equation relates the pH of a buffer solution to the pKa of its conjugate acid and the ratio of the concentrations of the conjugate base and acid. The equation is important in laboratory work that makes use of buffered solutions, in industrial processes where pH needs to be controlled, and in medicine, where understanding the Henderson-Hasselbalch equation is critical for the control of blood pH. Part A As a technician in a large pharmaceutical research firm, you need to produce 450. mL of 1.00 M potassium phosphate buffer solution of pH = 6.91. The pK₁ 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? Express your answer to three significant digits with the appropriate units. View Available Hint(s) 2 Volume of KH₂PO4 needed = Value Review | Constants | Periodic Table Submit μà Units ?
Transcribed Image Text:The Henderson-Hasselbalch equation relates the pH of a buffer solution to the pKa of its conjugate acid and the ratio of the concentrations of the conjugate base and acid. The equation is important in laboratory work that makes use of buffered solutions, in industrial processes where pH needs to be controlled, and in medicine, where understanding the Henderson-Hasselbalch equation is critical for the control of blood pH. Part A As a technician in a large pharmaceutical research firm, you need to produce 450. mL of 1.00 M potassium phosphate buffer solution of pH = 6.91. The pK₁ 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? Express your answer to three significant digits with the appropriate units. View Available Hint(s) 2 Volume of KH₂PO4 needed = Value Review | Constants | Periodic Table Submit μà 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: [HCO3 ] pH = pKa + log- (0.030) (Pco₂) where [HCO3] is given in millimoles/liter and the arterial blood partial pressure of CO2 is given in mmHg. The pK₂ 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 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 mM, what is the pH of blood if Pco₂ drops to 21.0 mmHg ? Express your answer numerically using two decimal places.
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) (Pco₂) where [HCO3] is given in millimoles/liter and the arterial blood partial pressure of CO2 is given in mmHg. The pK₂ 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 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 mM, what is the pH of blood if Pco₂ drops to 21.0 mmHg ? Express your answer numerically using two decimal places.
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