Why is the pressure applied on the surface of the solution in osmosis?

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Osmotic pressure is defined as the minimum pressure required to stop osmosis when a pure solvent and a solution are separated by a semipermeable membrane. This pressure is applied to the surface of the solution to counteract the natural movement of solvent molecules into the solution. The surface acts as a boundary between the solvent and the solution, influencing the osmotic process. Understanding this concept is crucial for grasping the dynamics of osmosis in various biological and chemical systems. The discussion highlights the importance of osmotic pressure in controlling solvent movement across membranes.
Sanjukta Ghosh
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Homework Statement


Why is the pressure applied on the surface of the solution?

Homework Equations


Definition: If a pure solvent and a solution is separated by a semipermeable membrane the minimum pressure applied on the surface of the solution to stop osmosis is called osmotic pressure.

The Attempt at a Solution

 
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Is that a homework question (as stated), or is it a more general question?
 
I think it's more a general question.

Cause the surface is a boundary between two different substances.
 
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