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Dichloroacetic acid has a dissociation constant of K = 3.32 x 10-2. Calculate the dogree of dissociation for a 0.0715 m solution of this acid from the Debye-Hückel Imiting law using an iteratve calculation until the answer is constant to within +2 in the second decimal place. Express your answer in percent to three significant figures.

Dichloroacetic acid has a dissociation constant of K = 3.32 x 10-2. Calculate the dogree of dissociation for a 0.0715 m solution of this acid from the Debye-Hückel Imiting law using an iteratve calculation until the answer is constant to within +2 in the second decimal place. Express your answer in percent to three significant figures.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Please answer question correctly and both a and part b

Dichloroacetic acid has a dissociation constant of K = 3.32 x 10-2. %3D Calculate the degree of dissociation for a 0.0715 m solution of this acid from the Debye-Hackol imiting law using an iterative calculation until the answer is constant to within +2 in the second decimal place. Express your answer in percent to three significant figures. Repeat the calculation assuming that the mean ionic activity coefficient is one. Express your answer in percent to three significant figures.
Transcribed Image Text:Dichloroacetic acid has a dissociation constant of K = 3.32 x 10-2. %3D Calculate the degree of dissociation for a 0.0715 m solution of this acid from the Debye-Hackol imiting law using an iterative calculation until the answer is constant to within +2 in the second decimal place. Express your answer in percent to three significant figures. Repeat the calculation assuming that the mean ionic activity coefficient is one. Express your answer in percent to three significant figures.
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