If the concentration of CO, in the atmosphere were to reach 600 ppm what would be the concentration of COz in water at 25°C that is in equilibrium with that air. Put your answer in mg/L. The Henry's Law Constant for CO, is 3.38 x 102 mol/L-atm and the partial pressure of water at 25°C is 0.0313 atm. If the equilibrium concentration of CO. in water was to reach 0.89 mg/L, what would the resulting pH be? The equilibrium constant (K1) for the reaction of CO2 in water is 4.45 x 107.

If the concentration of CO, in the atmosphere were to reach 600 ppm what would be the concentration of COz in water at 25°C that is in equilibrium with that air. Put your answer in mg/L. The Henry's Law Constant for CO, is 3.38 x 102 mol/L-atm and the partial pressure of water at 25°C is 0.0313 atm. If the equilibrium concentration of CO. in water was to reach 0.89 mg/L, what would the resulting pH be? The equilibrium constant (K1) for the reaction of CO2 in water is 4.45 x 107.

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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