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.
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.
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter16: Reactions Between Acids And Bases
Section: Chapter Questions
Problem 16.78QE
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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?
(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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