Osmosis is the movement of solvent molecules through a semipermeable membrane from a region of lower solute concentration to a region of higher solute concentration. It aims to equalize the concentrations on both sides of the membrane.
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Osmosis occurs because of the difference in chemical potential between solutions on either side of a semipermeable membrane.
It is a vital process in biological systems, influencing cell turgor and nutrient uptake.
In osmosis, water is typically the solvent that moves across the membrane.
Osmotic pressure can be calculated using the formula $\Pi = iMRT$, where $\Pi$ represents osmotic pressure, $i$ is the van 't Hoff factor, $M$ is molarity, $R$ is the gas constant, and $T$ is temperature in Kelvin.
Reverse osmosis, used for water purification, involves applying pressure to overcome natural osmotic pressure and force water through a membrane against its concentration gradient.
Review Questions
What drives the movement of solvent molecules during osmosis?
How does osmosis affect cells placed in hypotonic and hypertonic solutions?
What equation can be used to calculate osmotic pressure?
Properties that depend on the number of solute particles but not their identity; includes boiling point elevation, freezing point depression, vapor pressure lowering, and osmotic pressure.