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13 Dec 2019

The solubility of CO2 in water at 25 °C and PCO2 = 1 atm is 0.034 mol/L. What is its water solubility under normal atmospheric conditions (in air, carbon dioxide is about 380 ppmv) assuming that CO2 obeys Henry’s law? Please write each equations????

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Casey Durgan
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17 Dec 2019

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Related questions

Given that the solubility of O2 in water at 25oC is 8.70 ppm, calculate (a) the concentration of dissolved O2 in mol L-1 and (b) the value of the Henry’s law constant, in mol L-1 kPa-1, for O2 at this temperature? The atmospheric pressure is 1.00 atm. (Hint: the mole fraction of oxygen in air is 0.210).

The Henry’s law constant for CO2 in water at 25 °C is 3.1 × 10-2 M atm-1. (a) What is the solubility of CO2 in water at this temperature if the solution is in contact with air at normal atmospheric pressure? (b) Assume that all of this CO2 is in the form of H2CO3 produced by the reaction between CO2 and H2O:

CO2(aq) + H2O(l) H2CO3(aq)

What is the pH of this solution?

Henry's law constant for CO2 in the water at 25°C is 3.1 * 10^-2 M atm^-1.

a. What is the solubility of CO2 in the water at this temperature if the solution is in contact with air at normal atmospheric pressure? The mole fraction of CO2 in the air is 0.000375. Express your answer using two significant figures.

b. Assume that all of this CO2 is in the form of H2CO3 produced by the reaction between CO2 and H2O:

CO2 (aq) + H2O (l) => H2CO3 (aq).

What is the pH of this solution? Express your answer using two decimal places.

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