The osmotic pressure of equimolar solutions of $BaCl_2$,$NaCl$,and glucose follows the order:

$A$ $5.25\%$ 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 .............. $g\ mol^{-1}$.

$A$ solution containing $8.6 \ g$ of urea per liter is isotonic with a $0.5\% \ (w/v)$ solution of a non-volatile organic solute. What is the molar mass of the organic solute?

When $10 \ g$ of glucose $(P_1)$,$10 \ g$ of urea $(P_2)$,and $10 \ g$ of sucrose $(P_3)$ are dissolved in $250 \ mL$ of water,what is the relationship between their osmotic pressures at $273 \ K$?

Which of the following solutions does not flow in either direction when separated by a semipermeable membrane? (Molar mass: glucose $= 180 \ g \ mol^{-1}$,urea $= 60 \ g \ mol^{-1}$)

Which among the following colligative properties is useful to determine molar masses of very expensive solutes?