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From the equilibrium values Kb [4.79x 10-6+x] x [4.79 × 10-6+ X [0.8037-x] = 4.72 x 10-10 On solving for x, we get x= [OH-] = 1.3735 × 10-5 moles/L.

From the equilibrium values Kb [4.79x 10-6+x] x [4.79 × 10-6+ X [0.8037-x] = 4.72 x 10-10 On solving for x, we get x= [OH-] = 1.3735 × 10-5 moles/L.

Principles of Modern Chemistry
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
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 1P
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how can i calculate x? kb= 4.27x10^-10
From the equilibrium values Kb [4.79x 10-6+ x] x [4.79 x 10-6+ [0.8037-x] = 4.72 x 10-1 -10 On solving for x, we get x = [OH-] = 1.3735 × 10-5 moles/L.
Transcribed Image Text:From the equilibrium values Kb [4.79x 10-6+ x] x [4.79 x 10-6+ [0.8037-x] = 4.72 x 10-1 -10 On solving for x, we get x = [OH-] = 1.3735 × 10-5 moles/L.
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