Water is in equilibrium with the atmosphere at pH of 6.5. If the partial pressure of carbon dioxide in the atmosphere is 10-3.5 atm. What would be the water alkalinity? (Henry's Constant for CO2 in Water = 101.5 mole/L atm, use K1 = 10-6.3 K2 = 10-10.3). The carbonate equilibrium is defined by the following equations: CO2(aq) +H2O S H¿CO3 H2CO3 5 H* + HCO; HCO; 5 H + CO; Keg = 3.50 X 10² K = 4.20 X 10-7 K2 = 4.69 X 10*"

Water is in equilibrium with the atmosphere at pH of 6.5. If the partial pressure of carbon dioxide in the atmosphere is 10-3.5 atm. What would be the water alkalinity? (Henry's Constant for CO2 in Water = 101.5 mole/L atm, use K1 = 10-6.3 K2 = 10-10.3). The carbonate equilibrium is defined by the following equations: CO2(aq) +H2O S H¿CO3 H2CO3 5 H* + HCO; HCO; 5 H + CO; Keg = 3.50 X 10² K = 4.20 X 10-7 K2 = 4.69 X 10*"

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter13: Acids And Bases

Section: Chapter Questions

Problem 188IP: Isocyanic acid (HNCO) can be prepared by heating sodium cyanate in the presence of solid oxalic acid...

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