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As a technician in a large pharmaceutical research firm, you need to produce 450. mL of a potassium dihydrogen phosphate buffer solution of pH = 6.86. 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 M K₂HPO4 stock solution, and a carboy of pure distilled H₂O. How much 1.00 M KH₂PO4 will you need to make this solution? (Assume additive volumes.) Express your answer to three significant digits with the appropriate units.

As a technician in a large pharmaceutical research firm, you need to produce 450. mL of a potassium dihydrogen phosphate buffer solution of pH = 6.86. 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 M K₂HPO4 stock solution, and a carboy of pure distilled H₂O. How much 1.00 M KH₂PO4 will you need to make this solution? (Assume additive volumes.) Express your answer to three significant digits with the appropriate 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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Part A As a technician in a large pharmaceutical research firm, you need to produce 450. mL of a potassium dihydrogen phosphate buffer solution of pH = 6.86. The pK of H,PO is 7.21. You have the following supplies: 2.00 L of 1.00 M KH,PO stock solution, 1.50 L of 1.00 M K, HPO stock solution, and a carboy of pure distilled H2O. How much 1.00 M KH,PO will you need to make this solution? (Assume additive volumes.) Express your answer to three significant digits with the appropriate units. Part b
The Henderson-Hasselbalch equation relates the pH of a buffer solution to the pK₂ 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 a potassium dihydrogen phosphate buffer solution of pH = 6.86. The pK₂ 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? (Assume additive volumes.) Express your answer to three significant digits with the appropriate units. ▾ View Available Hint(s) ▶ Hint 1. How to approach the problem Hint 2. Find the ratio of conjugate base to conjugate acid Hint 3. How to find the volume of acid needed Roorcon
Transcribed Image Text:The Henderson-Hasselbalch equation relates the pH of a buffer solution to the pK₂ 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 a potassium dihydrogen phosphate buffer solution of pH = 6.86. The pK₂ 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? (Assume additive volumes.) Express your answer to three significant digits with the appropriate units. ▾ View Available Hint(s) ▶ Hint 1. How to approach the problem Hint 2. Find the ratio of conjugate base to conjugate acid Hint 3. How to find the volume of acid needed Roorcon
The Henderson-Hasselbalch equation relates the pH of a buffer solution to the pKa of its conjugate acid and the ratio of the concentrations f 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 critical for the control of blood pH. Part B If the normal physiological concentration of HCO3 is 24 mM, what is the pH of blood if Pco₂ drops to 34.0 mmHg ? Express your answer numerically using two decimal places. ▾ View Available Hint(s) Hint 1. How to approach the problem To solve this problem, substitute the known quantities for pKa of carbonic acid, the concentration of HCO3, and the partial pressure of CO₂ into the modified Henderson- Hasselbalch equation and solve for the pH value. ΠΫΠΙ ΑΣΦ 4 [HCO3] pH = pK₂ + log (0.030) (Pco₂) ?
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 f 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 critical for the control of blood pH. Part B If the normal physiological concentration of HCO3 is 24 mM, what is the pH of blood if Pco₂ drops to 34.0 mmHg ? Express your answer numerically using two decimal places. ▾ View Available Hint(s) Hint 1. How to approach the problem To solve this problem, substitute the known quantities for pKa of carbonic acid, the concentration of HCO3, and the partial pressure of CO₂ into the modified Henderson- Hasselbalch equation and solve for the pH value. ΠΫΠΙ ΑΣΦ 4 [HCO3] pH = pK₂ + log (0.030) (Pco₂) ?
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