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Osmosis is the movement of solvent molecules (usually water) across a semipermeable membrane from an area of lower solute concentration to an area of higher solute concentration. This movement occurs in an attempt to equalize the concentration of solute on both sides of the membrane, resulting in the diffusion of solvent molecules across the membrane.
Osmotic pressure is the pressure that must be applied to a solution to prevent the inward flow of water across a semipermeable membrane due to osmosis. It's a colligative property, meaning it depends only on the number of solute particles present in the solution, not on their identity. Osmotic pressure is directly proportional to the concentration of solute particles in the solution.
The advantage of using osmotic pressure over other colligative properties (such as freezing point depression or boiling point elevation) for the determination of molar masses of solutes in solutions lies in its sensitivity. Osmotic pressure measurements can be highly accurate and precise, particularly for dilute solutions where other colligative properties may be difficult to measure accurately. Additionally, osmotic pressure measurements can be made over a wide range of concentrations, making it applicable to a variety of solute concentrations. This versatility makes osmotic pressure a valuable tool in determining the molar masses of solutes in solutions.
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