PH of a solution whose OH ion concentration is 0.010 m/lO 10-1210-3O 12 When the following reactions come to equilibrium, does the equilibrium mixturecontain2HBR(g) H2(g) + Br2(g) Kc = 5.8 x 10-18 Reactantsmore productsO cannot determinemore reactantsOequal amounts of reactants and products

pH of the solution = 12 Answer is 'more reactants'Question 1. [OH-] = 0.010 m/L means 0.010 moles of OH- is present per litre of the solution. Therefore, [OH-] = 0.010 M pOH = -log[OH-] = -log 0.010 = 2 We know, pH + pOH = 14 Therefore, pH = 14 - pOH = 14 - 2 = 12 Therefore, pH of the solution = 12 Question 2. Equilibrium constant Kc = [H2] [Br2] / [HBr]2 Here the given Kc < 1 Hence, this indicates that in this case the equilibrium mixture contains more reactants than products. Therefore, answer is 'more reactants'

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Chemistry

PH of a solution whose OH ion concentration is 0.010 m/l 10-12 O 10-3 O 12

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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