An analytical chemist is titrating 85.2 mL of a 0.3900 M solution of aniline (C6H5NH2) with a 0.3200M solution of HNO3. The pKÅ of aniline is 9.37. Calculate the pH of the base solution after the chemist has added 118.9 mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places. pH =
An analytical chemist is titrating 85.2 mL of a 0.3900 M solution of aniline (C6H5NH2) with a 0.3200M solution of HNO3. The pKÅ of aniline is 9.37. Calculate the pH of the base solution after the chemist has added 118.9 mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places. pH =
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter15: Acid–base Equilibria
Section: Chapter Questions
Problem 55P
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