The osmotic pressure of $1 \, M$ solution at $27 \, ^\circ C$ is ........... $atm$.

In case of osmosis,solvent molecules move from:

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: $(R = 0.083 \text{ L bar mol}^{-1} \text{ K}^{-1})$

At $300 \, K$,$36 \, g$ of glucose present in a litre of its solution has an osmotic pressure of $4.98 \, bar$. If the osmotic pressure of the solution is $1.52 \, bar$ at the same temperature,what would be its concentration?

$A$ $0.002 \, M$ solution of $NaCl$ having a degree of dissociation of $90 \%$ at $27 \, ^{\circ}C$ has an osmotic pressure equal to:

Which of the following colligative properties is useful to determine the molar masses of proteins, polymers, or colloids with the greatest precision?