In determining the pH of 0.010 M solution of weak acid, HCNO, which equations are relevant in the systematic treatment ofequilibrium. (K, = 3.47 x 10-4)%3Da) [H3O*][OH-] = 1.00 × 10-14b) 3.47 x 10-4 = [H*][CNO¯]/[HCNO]c) 2.88 x-11 = [HCNO][OH ]/[CNO¯]d) [H3O*] = [OH-] + [CNO"]e) [OH]+ [CNO¯] = 2[H3O*]%Df) 0.010 = [HCNO] + [CNO¯]g) [CNO] + [OH]) = [HCNO]abCef

In determining the pH of 0.010M solution of weak acid, HCNO, which equations are relevant in the systematic treatment of equilibrium. (Ka = 3.47 x 10-4) %3D a) [H3O*][OH-] = 1.00 × 10-14 b) 3.47 x 10-4 = [H*][CNO¯]/[HCNO] c) 2.88 x 10-11 = [HCNO][OH¯]/[CNO¯] d) [H3O*] = [OH-] + [CNO"] e) [OH] + [CNO ) = 2[H3O*] f) 0.010 = [HCNO] + [CNO] g) [CNO-] + [OH¯] = [HCNO] a O e O f

In determining the pH of 0.010M solution of weak acid, HCNO, which equations are relevant in the systematic treatment of equilibrium. (Ka = 3.47 x 10-4) %3D a) [H3O][OH-] = 1.00 × 10-14 b) 3.47 x 10-4 = [H][CNO¯]/[HCNO] c) 2.88 x 10-11 = [HCNO][OH¯]/[CNO¯] d) [H3O] = [OH-] + [CNO"] e) [OH] + [CNO ) = 2[H3O] f) 0.010 = [HCNO] + [CNO] g) [CNO-] + [OH¯] = [HCNO] a O e O f

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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