What is the solubility of CO2� in water at a pressure of 3.63 atm?� The Henry's Law constant for CO2 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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