Calculate the osmotic pressure of a $20\%$ (w/v) anhydrous $CaCl_2$ solution at $0^\circ C$. Assume $100\%$ ionization. (in $\text{atm}$)

Assertion : If red blood cells were removed from the body and placed in pure water,pressure inside the cells increases.
Reason : The concentration of salt content in the cells increases.

$A$ solution contains a non-volatile solute of molecular mass $M_p$. Which of the following can be used to calculate the molecular mass of the solute in terms of osmotic pressure ($m = \text{Mass of solute}$,$V = \text{Volume of solution}$,and $\pi = \text{Osmotic pressure}$)?

$50 \ mL$ of $0.2$ molal urea solution (density $= 1.012 \ g \ mL^{-1}$ at $300 \ K$) is mixed with $250 \ mL$ of a solution containing $0.06 \ g$ of urea. Both the solutions were prepared in the same solvent. The osmotic pressure (in Torr) of the resulting solution at $300 \ K$ is . . . . . $[\Delta_{mix} V = 0]$

Under identical conditions,which solution has the highest osmotic pressure?

$A$ $5.25\%$ solution of a substance is isotonic with a $1.5\%$ solution of urea (molar mass $= 60\ g\ mol^{-1}$) in the same solvent. If the densities of both the solutions are assumed to be equal to $1.0\ g\ cm^{-3},$ the molar mass of the substance will be .............. $g\ mol^{-1}$.