What is the solubility of CO2(g) in water at 20 0C if the partial pressure in the air is 0.00031 atm? Note that at 1.00 atm the solubility of CO2(g) is 0.034 M in water.
To find the solubility of CO2(g) in water at 20 °C, you can use Henry's law, which states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid.
According to the information given, at 1.00 atm the solubility of CO2(g) is 0.034 M in water. Therefore, the constant of proportionality (Henry's law constant) can be calculated as follows:
Henry's law constant (k) = solubility/partial pressure
k = 0.034 M / 1.00 atm
Now, you can use this constant to find the solubility of CO2(g) at a partial pressure of 0.00031 atm:
Solubility = k * partial pressure
Solubility = (0.034 M / 1.00 atm) * 0.00031 atm
Simplifying the expression gives:
Solubility = 0.000001054 M
Therefore, the solubility of CO2(g) in water at 20 °C when the partial pressure is 0.00031 atm is approximately 0.000001054 M.