An analytical chemist is titrating 190.6 mL of a 0.3000M solution of methylamine (CH3NH₂) with a 0.8400M solution of HIO3. The pK, of methylamine is 3.36. Calculate the pH of the base solution after the chemist has added 80.2 mL of the HIO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HIO3 solution added. Round your answer to 2 decimal places.

An analytical chemist is titrating 190.6 mL of a 0.3000M solution of methylamine (CH3NH₂) with a 0.8400M solution of HIO3. The pK, of methylamine is 3.36. Calculate the pH of the base solution after the chemist has added 80.2 mL of the HIO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HIO3 solution added. Round your answer to 2 decimal places.

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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