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 by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter13: Fundamental Equilibrium Concepts
Section: Chapter Questions
Problem 101E: A 0.010 M solution of the weak acid HA has an osmotic pressure (see chapter on solutions and...
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