Calculate the molar mass of a solute at $300 \ K$ if $400 \ mg$ of it is dissolved in $300 \ mL$ of water to exert an osmotic pressure of $0.2 \ atm$. $(R = 0.0821 \ L \ atm \ K^{-1} \ mol^{-1})$

At $27^{\circ}C$,$0.1 \ M$,$1 \ L$ $K_4[Fe(CN)_6]$ aqueous solution and $0.1 \ M$,$1 \ L$ $FeCl_3$ aqueous solution are placed in a container separated by a semi-permeable membrane $AB$. Assume complete dissociation of both the solutes. Which of the following statements is correct?

The osmotic pressure of a sugar solution at $24^{\circ}C$ is $2.5 \ atm$. What is the concentration of the solution in moles per litre?

Equal masses of glucose,sucrose,and urea are dissolved in $V \ L$ of water to prepare separate solutions. The order of osmotic pressures $\pi_1, \pi_2$,and $\pi_3$ for glucose,sucrose,and urea respectively will be...........

$0.06 \% (w/v)$ aqueous solution of urea is isotonic with:

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