Osmotic pressure is the pressure that must be applied to prevent the movement of water through a semipermeable membrane. It is directly proportional to the concentration of solute in the solution. The higher the concentration of solute, the higher the osmotic pressure.


In this case, we have three solutions - 2M NaCl, 1M glucose, and 2M urea. To determine which solution has the minimum osmotic pressure, we need to calculate the osmotic pressure of each solution and compare them.


The formula for calculating osmotic pressure is:

Osmotic pressure = Molarity x Gas constant x Temperature

Where,
Molarity - concentration of solute in moles per liter
Gas constant - 0.0821 L atm/mol K
Temperature - temperature in Kelvin


For 2M NaCl solution,
Molarity = 2 mol/L
Temperature = 298 K
Osmotic pressure = 2 x 0.0821 x 298 = 48.8 atm


For 1M glucose solution,
Molarity = 1 mol/L
Temperature = 298 K
Osmotic pressure = 1 x 0.0821 x 298 = 24.4 atm


For 2M urea solution,
Molarity = 2 mol/L
Temperature = 298 K
Osmotic pressure = 2 x 0.0821 x 298 = 48.8 atm


From the above calculations, we can see that both NaCl and urea solutions have the same osmotic pressure of 48.8 atm, while the glucose solution has a lower osmotic pressure of 24.4 atm. Therefore, the answer is option (b) - 200 ml of 1M glucose solution will have the minimum osmotic pressure.

B 1 m glucose.... i for glucose =1 therefore π= 1*1RT ...i for nacl 2therefore π=2 *2RT ...i for urea 1 therefore π=1*2 RT