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?

The solubility of CO2 in water at 3.63 atm= 3.2 x 10-2x3.63=0.116 mol/l

The molar mass of MnBr2=55+80x2=215 g/mol

So 119g MnBr2=119/215=0.553 mol MnBr2

Assuming the volume of the solution is the same as the volume of water, which is 210/1000=0.21 L.

Then the molality =0.553/0.21=2.64 mol/L

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