how can i calculate x? kb= 4.27x10^-10 From the equilibrium valuesKb[4.79x 10-6+ x] x [4.79 x 10-6+[0.8037-x]= 4.72 x 10-1-10On solving for x, we getx = [OH-] = 1.3735 × 10-5 moles/L.

x is the degree of dissociation

Answered: From the equilibrium values Kb [4.79x…

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

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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Question

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.

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