Osmotic Pressure

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Osmotic pressure (π) of a dilute solution relates to concentration via:

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1. **van't Hoff Equation**: Analogous to the ideal gas law ($PV = nRT$), dilute solutions follow $\pi V = nRT$.
2. **Concentration ($c$)**: Since $n/V$ is the Molar concentration ($c$ or $M$),
3. **Equation**: **$\pi = cRT$**.
   - $\pi$: Osmotic pressure (measured in $atm$ or $bar$).
   - $c$: Molarity ($mol/L$).
   - $R$: Gas constant ($0.0821 L \cdot atm / K \cdot mol$).
   - $T$: Absolute temperature ($Kelvin$).
4. **Application**: This is the most suitable colligative property for determining the molar masses of large biomolecules (like proteins) due to measurable pressures even at low concentrations.

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