Correct Answer - Option 3 : Number of solute molecules is increased
Concept:
Osmosis:
- The phenomenon in which the flow of solvent through a semi-permeable membrane from the pure solvent to the solution takes place is osmosis.
- It involves the movement of solvent molecules only.
- Osmosis is limited to solutions only.
- Osmosis takes place through a semi-permeable membrane.
- The solvent molecules move from the solution of low solute concentration to higher solute concentration.
Osmotic pressure:
- The osmotic pressure of a solution is called the excess pressure need to be applied to a solution to prevent osmosis. i.e., to stop the passage of solvent molecules through a semi-permeable membrane into the solution.
- It is denoted by π.
- Osmotic pressure is one of the colligative properties as it depends on the number of solute molecules and not on their identity.
-
According to Van't Hoff, For a dilute solution, Osmotic pressure is given by:
\({\mathbf{\pi }}{\text{ }} = \;c{\mathbf{RT}}\;\)
\({\mathbf{\pi }}{\text{ }} = \;\frac{{{{\text{n}}_2}}}{{\text{V}}}{\mathbf{RT}}\;\) (\(\because c{\text{ = }}\frac{{{{\text{n}}_{\text{2}}}}}{{\text{V}}}\))
\({\mathbf{\pi }}{\text{V = }}\frac{{{{\text{w}}_{\text{2}}}{\text{RT}}}}{{{{\text{M}}_{\text{2}}}}}\;\) (\(\because {n_2}{\text{ = }}\frac{{{w_2}}}{{{M_2}}}\))
Where c = molar concentration/ molarity of the solution; T = Temperature; w2 = mass of solute; M2 = molecular weight of solute present in solution, R = gas constant; V = volume of solution in litres; n2 = no. of moles of solute
For a solution, at a given temperature, R and T are constant, then Osmotic pressure is:
\(\pi \propto c\)
Explanation:
Factors affecting Osmotic pressure is given below:
Factors |
proportionality |
Osmotic pressure trend |
Temperature |
\(\pi \propto T\)
|
As temperature increases, osmotic pressure increases |
Gas constant |
\(\pi \propto R\) |
R is a constant value for all solution |
No: of moles of solute |
\(\pi \propto {n_2}\) |
As no. of moles of solute increases, O.P increases |
Volume of solution |
\(\pi \propto \frac{1}{V}\) |
As volume is increased, O.P gets decreased |
The molecular mass of solute |
\(\pi \propto \frac{1}{{{{\text{M}}_{\text{2}}}}}\) |
As molar mass increase, O.P decreases |
Molarity of solution |
\(\pi \propto c\) |
As the molarity of solution increase, O.P also increase |
Hence, The Osmotic pressure of the solution increases, if the number of solute molecules is increased.