Adilute aqueous solution of an organic compound soluble in water is formed by dissolving 2.35 g of the compound in water to form 0.250 l of solution. the resulting solution has an osmotic pressure of 0.605 atm at25∘cassuming that the organic compound is a nonelectrolyte, what is its molar mass?

Explanation:

1) Osmotic pressure is a colligative property, which means that it depends on the number of particles of solute present in the solvent.

2) The mathematical expression that relates osmotic pressure with the concentration of solute is:

Where:

3) Here:

4) Calculate M

             = 0.605 atm / (1 × 0.08206 L atm mol⁻¹ K⁻¹ × 298.15 K) =

             = 0.0247 atm (three significant figures)

5) Calculate number of moles, from molarity definition:

            ⇒ n = M × V (in liters) = 0.0247 M × 0.250 liter =

                    = 0.00618 moles

6) Calculate molar mass:

                             = 2.35 g / 0.00618 moles

                             = 380 g/mol ← answer

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explanation:

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