Using the table of the weak base below, you have chosen Ethylamine as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.52 M in this salt. The desired pH of the buffer should be equal to 10.1. Values of K, for Some Common Weak Bases Conjugate Acid Name Formula Kb NH4+ 1.8 x 10-5 Ammonia Methylamine NH3 CH3NH2 CH3NH3+ 4.38 x 10-4 C₂H5NH₂ C₂H5NH3+ 5.6 x 10-4 Ethylamine Aniline CH;NH, C6H5NH3+ Pyridine 3.8 x 10-10 1.7 x 10-⁹ C,H,N CH;NH* 1. Compute the poH of the buffer solution.

Using the table of the weak base below, you have chosen Ethylamine as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.52 M in this salt. The desired pH of the buffer should be equal to 10.1. Values of K, for Some Common Weak Bases Conjugate Acid Name Formula Kb NH4+ 1.8 x 10-5 Ammonia Methylamine NH3 CH3NH2 CH3NH3+ 4.38 x 10-4 C₂H5NH₂ C₂H5NH3+ 5.6 x 10-4 Ethylamine Aniline CH;NH, C6H5NH3+ Pyridine 3.8 x 10-10 1.7 x 10-⁹ C,H,N CH;NH* 1. Compute the poH of the buffer solution.

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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