Osmotic Pressure problem
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Osmotic Pressure problem

[From: ] [author: ] [Date: 13-02-26] [Hit: ]
The osmotic pressure of solution is 0.56 torr at 25 degrees Celsius. what is the molar mass of the protein.R = 62.here M = .56 / 1 x 62.......
A 7.3x10^-2 mg sample of protein is dissolved in H2O to make 0.25ml of solution. The osmotic pressure of solution is 0.56 torr at 25 degrees Celsius. what is the molar mass of the protein.

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Pi = i M R T
where

i is the dimensionless van 't Hoff factor
M is the molarity
R = 62.363 L Torr K−1 mol−1
is the gas constant
T is the thermodynamic (absolute) temperature

here M = .56 / 1 x 62.363 x (25+273) =3.013 x 10 ^-05 moles / liter

we also have 7.3x10^-5 g in .25 mL or 7.3x10^-5 x 1000 / .25 g in 1 liter = 0.292 g per liter

we in 1 liter have 0.292 g of solute = 3.013 x 10 ^-05 moles

mass of 1 mole = 0.292 g / 3.013 x 10 ^-05 mol = 9700 g / mole .. molar mass of the protein
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