Find the pH for the following buffers. Give a balanced reaction equation in all cases. Use the Henderson-Hasselbalch equation to solve these 3 problems!!A buffer consisting of 0.12 M sodium carbonate and 0.82 M sodium bicarbonate (Ka= 4.7x10-11)b) What is the pH of 500 mL of solution containing 0.125 mol/L of propanoic acid(C3H6O2) and 0.375 mol/L of sodium propanoate (C3H5O2Na)? (Ka for propanoic acid is 5.52 × 10-5.)c) A frequently used buffer in biological systems, including IV fluids, is a phosphate buffered saline solution (“PBS”), which contains 8.00 g of NaCl buffered with 1.44 g of Na2HPO4.2H2O and 0.24 g of KH2PO4 and per liter of solution. What is its pH?(It is a very good idea to write out the reaction for this equilibrium first!)Ka values of the phosphates: see Appendix H for acid-ionization constants.

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Answered: Find the pH for the following buffers.…

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

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Find the pH for the following buffers. Give a balanced reaction equation in all cases. Use the Henderson-Hasselbalch equation to solve these 3 problems!!

A buffer consisting of 0.12 M sodium carbonate and 0.82 M sodium bicarbonate (Ka= 4.7x10^-11)

b) What is the pH of 500 mL of solution containing 0.125 mol/L of propanoic acid(C₃H₆O₂) and 0.375 mol/L of sodium propanoate (C₃H₅O₂Na)? (Ka for propanoic acid is 5.52 × 10^-5.)
c) A frequently used buffer in biological systems, including IV fluids, is a phosphate buffered saline solution (“PBS”), which contains 8.00 g of NaCl buffered with 1.44 g of Na₂HPO₄.2H₂O and 0.24 g of KH₂PO₄ and per liter of solution. What is its pH?