At $27\,^oC$,the osmotic pressure of a solution containing $36\,g$ of glucose per liter is $4.92\,atm$. If the osmotic pressure of the solution is adjusted to $1.5\,atm$ at the same temperature,what will be its concentration?

What is the effect of external pressure on the osmotic pressure $(OP)$ of a solution?

Which of the following $0.1 \ M$ solutions has the maximum osmotic pressure at $25^o \ C$?

Which of the following conditions is correct for reverse osmosis? [$C =$ Concentration of solution in $mol \ L^{-1}$; $T =$ Temperature in Kelvin scale; $P_{ext} =$ External pressure; $\pi = CRT =$ Osmotic pressure]

The process in which solvent molecules pass through a semipermeable membrane is called:

Solution $A$ is prepared by dissolving $1 \text{ g}$ of a protein (molar mass = $50000 \text{ g mol}^{-1}$) in $0.5 \text{ L}$ of water at $300 \text{ K}$. Its osmotic pressure is $x \text{ bar}$. Solution $B$ is made by dissolving $2 \text{ g}$ of the same protein in $1 \text{ L}$ of water at $300 \text{ K}$. The osmotic pressure of solution $B$ is $y \text{ bar}$. The entire solution of $A$ is mixed with the entire solution of $B$ at the same temperature. The osmotic pressure of the resultant solution is $z \text{ bar}$. $x, y$ and $z$ respectively are: $(R = 0.083 \text{ L bar mol}^{-1} \text{ K}^{-1})$