Write the equilibrium constant expression for acetic acid, and calculate a K value and an apparent percent dissociation for each concentration + ICE tables for 0.10 M HC2H302 +0.010 M +0.0010 M. (ph for 0.10M is 3.3, pH for 0.010 M is 3.7, ph for0.0010 M is 4.4) HA(aq) = H+(aq) + A-(aq)

Write the equilibrium constant expression for acetic acid, and calculate a K value and an apparent percent dissociation for each concentration + ICE tables for 0.10 M HC2H302 +0.010 M +0.0010 M. (ph for 0.10M is 3.3, pH for 0.010 M is 3.7, ph for0.0010 M is 4.4) HA(aq) = H+(aq) + A-(aq)

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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Question

Write the equilibrium constant expression for acetic acid, and calculate a K value and an apparent percent dissociation for each concentration + ICE tables
for 0.10 M HC2H302 +0.010 M +0.0010 M. (ph for 0.10M is 3.3, pH for 0.010 M is 3.7, ph for0.0010 M is 4.4) HA(aq) = H+(aq) + A-(aq)

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