A buffer solution contains dissolved C6H5NH2 and C6H5NH3CI. The initial concentration of C6H5NH2 is 0.50 M and the pH of the buffer is 4.20. Determine the concentration of C6H5NH3* in the solution. The value of Kb for C6H5NH2 is 3.8 x 10 10.

A buffer solution contains dissolved C6H5NH2 and C6H5NH3CI. The initial concentration of C6H5NH2 is 0.50 M and the pH of the buffer is 4.20. Determine the concentration of C6H5NH3* in the solution. The value of Kb for C6H5NH2 is 3.8 x 10 10.

General, Organic, and Biological Chemistry

7th Edition

ISBN:9781285853918

Author:H. Stephen Stoker

Publisher:H. Stephen Stoker

Chapter10: Acids, Bases, And Salts

Section: Chapter Questions

Problem 10.126EP: What is the pH of a buffer that is 0.175 M in a weak acid and 0.200 M in the acids conjugate base?...

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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

A buffer solution contains dissolved C6H5NH2 and C6H5NH3CI. The initial
concentration of C6H5NH2 is 0.50 M and the pH of the buffer is 4.20. Determine
the concentration of C6H5NH3* in the solution. The value of Kb for C6H5NH2 is
3.8 x 10 10.

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