What is the molar mass of a non-ionizing, non-volatile solid that when 12.9 g is dissolved in water to make 100mL of solution creates a solution with an osmotic pressure of 5.68atm at 25 degrees celsius.

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Nestor RutherfordLv2

31 Dec 2019

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An 18.6 mg sample of a protein was dissolved in water to produce 5.00mL of solution at 25 degrees celsius. The osmotic pressure of this solution was measured and found to be 2.42 x10^-3atm. What is the molar mass of this protein?

Vapour Pressure of Solutions of Non-Volatile or Volatile Solutes

31.686 g of a non-volatile solute is dissolved in 460.0 g of water.
The solute does not react with water nor dissociate in solution.
Assume that the resulting solution displays ideal Raoult's law behaviour.
At 10Â°C the vapour pressure of the solution is 9.055 torr.
The vapour pressure of pure water at 10Â°C is 9.209 torr.
Calculate the molar mass of the solute (g/mol).

See example 17.1 on pp865-6 of Zumdahl ''Chemical Principles'' 7th ed.

Now suppose, instead, that 31.686 g of a volatile solute is dissolved in 460.0 g of water.

This solute also does not react with water nor dissociate in solution.
The pure solute displays, at 10Â°C, a vapour pressure of 0.921 torr.
Again, assume an ideal solution.
If, at 10Â°C the vapour pressure of this solution is also 9.055 torr.
Calculate the molar mass of this volatile solute.

30.0 g of glucose (C₆H₁₂O₆, molar mass = 180.16 g/mol) is dissolved in 100 grams of water (molar mass 18.02). What is the mole fraction of water in solution? Note: glucose is a non-volatile solute.