An analytical chemist is titrating 130.3 mL of a 0.6200M solution of methylamine (CH3NH₂) with a 0.3500M solution of HIO3. The pK₂ of methylamine is 3.36. Calculate the pH of the base solution after the chemist has added 260.8 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. -0 pH = X

An analytical chemist is titrating 130.3 mL of a 0.6200M solution of methylamine (CH3NH₂) with a 0.3500M solution of HIO3. The pK₂ of methylamine is 3.36. Calculate the pH of the base solution after the chemist has added 260.8 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. -0 pH = X

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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