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A dilute aqueous solution of an organic compound soluble in water is formed by dissolving 2.53...

A dilute aqueous solution of an organic compound soluble in water is formed by dissolving 2.53 g of the compound in water to form 0.250 L of solution. The resulting solution has an osmotic pressure of 0.673 atm at 25°C. Assuming that the organic compound is a nonelectrolyte, what is its molar mass?

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Answer #1

The osmotic pressure P = CRT ====1)

C = molar concentration R = gas constant = 0.0821Latm/molK T = temperature in K = 273 + 25 = 298K

C = No. of moles / Volume of solution in liters

No. of moles = Mass in grams / Molecular mass

C = mass in grams / (Molecular mass X volume in liters)

0.673 = C X 0.082 X 298

C = 0.673 / 0.082 X 298 = 0.027M

C = Mass in grams / Molecular mass X volume in liters

Molecular mass = mass in grams / C X volume in liters

Molecular mass = 2.53 / 0.25 X 0.027 = 374.81

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