The pH of the river adjacent to the site is governed by the carbonic acid/bicarbonate buffer system as well as dissolved ions from the surrounding environment. Carbon dioxide from the atmosphere dissolves in river water to form carbonic acid by the following equilibrium: CO2{ag) + H2O = H2CO3(ag) pKa1 = 2.77 Carbonic acid dissociates in water to form the bicarbonate and carbonate ions by the following equilibrium reactions. H2CO3(ag) + H20 H30 + (ag) + HCO3 - (ag)_ pKa2 = 3.70 HCO3 - (ag) + H20 H30 + (ag) + CO3 2- (ag) pKa3 = 10.33 (a) The following equilibrium accounts for the fact that carbon dioxide is in equilibrium in carbonic acid when dissolved in water. CO2(ag) + 2H20 S H30 + (ag) + HCO3 - (ag) K= ? Calculate the value of the equilibrium constant, K for this reaction. Show all working

The pH of the river adjacent to the site is governed by the carbonic acid/bicarbonate buffer system as well as dissolved ions from the surrounding environment. Carbon dioxide from the atmosphere dissolves in river water to form carbonic acid by the following equilibrium: CO2{ag) + H2O = H2CO3(ag) pKa1 = 2.77 Carbonic acid dissociates in water to form the bicarbonate and carbonate ions by the following equilibrium reactions. H2CO3(ag) + H20 H30 + (ag) + HCO3 - (ag)_ pKa2 = 3.70 HCO3 - (ag) + H20 H30 + (ag) + CO3 2- (ag) pKa3 = 10.33 (a) The following equilibrium accounts for the fact that carbon dioxide is in equilibrium in carbonic acid when dissolved in water. CO2(ag) + 2H20 S H30 + (ag) + HCO3 - (ag) K= ? Calculate the value of the equilibrium constant, K for this reaction. Show all working

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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