A chemist added 0.15 mol of NaOH to a 1.00 L buffer that contained 0.50 M propanoic acid HC3H5O2) and 0.80 M sodium propanoate (NaC3HsO2). Ka = 1.3 x 105 . Complete an ICE box using the information provided. . Determine the pH of buffer using the ICE box information. .If 1.5 moles of NaOH was added to 1.00 L of this buffer it was found that the buffer no longer existed. Explain why this occurred.
A chemist added 0.15 mol of NaOH to a 1.00 L buffer that contained 0.50 M propanoic acid HC3H5O2) and 0.80 M sodium propanoate (NaC3HsO2). Ka = 1.3 x 105 . Complete an ICE box using the information provided. . Determine the pH of buffer using the ICE box information. .If 1.5 moles of NaOH was added to 1.00 L of this buffer it was found that the buffer no longer existed. Explain why this occurred.
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter14: Equilibria In Acid-base Solutions
Section: Chapter Questions
Problem 29QAP: A buffer is made up of 0.300 L each of 0.500 M KH2PO4 and 0.317 M K2HPO4. Assuming that volumes are...
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