What is the solubility of CO_{2}� in water at a pressure of 3.63 atm?� The Henry's Law constant for CO_{2} in water is 3.2 x 10^{-2}�mol/(L atm).

A mass of 119 g of manganese dibromide is dissolved in 210 g of water. What is the molality of the solution?

Gas Solubility = K x Gas Pressure.

It’s been given to you that this k = 3.2 x 10 ^{2} mol/L atm. And P is 3.63 atm.

Thus, by plugging in numbers into this formula : Gas Solubility (C gas) = 3.2 x 10 ^{2} mol/L atm X 3.63 atm = 11.62 mol/L (since atm units are cancelled out).

Good Luck!

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