Calculate the pH that results when 2.35 mL of a 0.0125 M aqueous solution of KOH is added to 23.50 mL of an 0.0132 M aqueous solution of methylamine (CH3NH2, Kb = 4.2 x 10–4). Show your work and justify any approximations made.

Calculate the pH that results when 2.35 mL of a 0.0125 M aqueous solution of KOH is added to 23.50 mL of an 0.0132 M aqueous solution of methylamine (CH3NH2, Kb = 4.2 x 10–4). Show your work and justify any approximations made.

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 16.27QE

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Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

Calculate the pH that results when 2.35 mL of a 0.0125 M aqueous solution of KOH is added to 23.50 mL of an 0.0132 M aqueous solution of methylamine (CH₃NH₂, K_b = 4.2 x 10^–4). Show your work and justify any approximations made.

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