Final answer:
If pressure greater than the osmotic pressure is applied on a solution side separated by a semipermeable membrane, reverse osmosis occurs, allowing solvent to flow from higher to lower solute concentration, commonly used in desalination.
Step-by-step explanation:
When pressure is applied to the solution side that is greater than the osmotic pressure, the natural process of osmosis is reversed. This scenario is called reverse osmosis. In osmosis, solvent typically moves from a region of lower solute concentration to a region of higher solute concentration. However, if additional pressure is applied, solvent moves from the region of higher solute concentration to the region of lower solute concentration. This is because the applied pressure exceeds the osmotic pressure that would normally draw water towards the solute.
The practical application of this principle is observed in desalination processes, where reverse osmosis is used to produce drinkable water from saltwater. When pressure greater than the osmotic pressure is applied to the seawater, the water molecules are forced to move across the semipermeable membrane, leaving the salts behind, thereby purifying the water.