ANS:D - none of these

1. Volume: The osmotic pressure of a solution is not directly affected by changes in volume alone. Osmotic pressure depends on the concentration of solute particles in the solution, not the total volume of the solution. Even if the volume of the solution changes, as long as the concentration of solute particles remains constant, the osmotic pressure will not be affected.
2. Solute Concentration: Osmotic pressure is directly proportional to the concentration of solute particles in the solution. As the concentration of solute particles increases, the osmotic pressure also increases. This relationship is described by the equation: Π=𝑖𝑀𝑅𝑇Π=iMRT where:
   • ΠΠ is the osmotic pressure,
   • 𝑖i is the van't Hoff factor (the number of particles into which a solute dissociates in solution),
   • 𝑀M is the molarity of the solution (concentration of solute particles),
   • 𝑅R is the ideal gas constant,
   • 𝑇T is the temperature in Kelvin.
   This equation shows that osmotic pressure increases with an increase in solute concentration.
3. Temperature: According to the van't Hoff equation (Π=𝑖𝑀𝑅𝑇Π=iMRT), the osmotic pressure is directly proportional to temperature. Therefore, an increase in temperature would lead to an increase in osmotic pressure, and a decrease in temperature would lead to a decrease in osmotic pressure. This relationship is similar to that of other gas laws, where increasing temperature increases the pressure exerted by gas molecules.