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The concentration of SO2 in the troposphere over a certain region is 0.87 ppm by volume. The gas dissolves rainwater as follows: =2 SO2(g) + H2O(1) H*(aq) + HSO3¯¯(aq) Given that the equilibrium constant for the preceding reaction is 1.3 × 102, calculate the pH of the rainwater. Assume that the reaction does not affect the partial pressure of SO2. pH=5.6 X

The concentration of SO2 in the troposphere over a certain region is 0.87 ppm by volume. The gas dissolves rainwater as follows: =2 SO2(g) + H2O(1) H*(aq) + HSO3¯¯(aq) Given that the equilibrium constant for the preceding reaction is 1.3 × 102, calculate the pH of the rainwater. Assume that the reaction does not affect the partial pressure of SO2. pH=5.6 X

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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The concentration of SO2 in the troposphere over a certain region is 0.87 ppm by volume. The gas dissolves rainwater as follows: =2 SO2(g) + H2O(1) H*(aq) + HSO3¯¯(aq) Given that the equilibrium constant for the preceding reaction is 1.3 × 102, calculate the pH of the rainwater. Assume that the reaction does not affect the partial pressure of SO2. pH=5.6 X
Transcribed Image Text:The concentration of SO2 in the troposphere over a certain region is 0.87 ppm by volume. The gas dissolves rainwater as follows: =2 SO2(g) + H2O(1) H*(aq) + HSO3¯¯(aq) Given that the equilibrium constant for the preceding reaction is 1.3 × 102, calculate the pH of the rainwater. Assume that the reaction does not affect the partial pressure of SO2. pH=5.6 X
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