If the osmotic pressure of a solution at $300 \ K$ is $0.0821 \ atm$,what will be the concentration of the solution in $mol/L$?

Find the amount of solute in a solution obtained by dissolving it in $2.5 \ dm^3$ of water that generates an osmotic pressure of $0.245 \ atm$ at $300 \ K$. (Molar mass of solute $= 58 \ g \ mol^{-1}$,$R = 0.0821 \ dm^3 \ atm \ K^{-1} \ mol^{-1}$) (in $g$)

Calculate the osmotic pressure of $0.5 \ M$ aqueous solution of a non-volatile solute at $300 \ K$ $\left[R = 0.0821 \ atm \ dm^3 \ K^{-1} \ mol^{-1}\right]$. (in $atm$)

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?

Which of the following pairs of solutions is expected to be isotonic at the same temperature?

If the osmotic pressure of cane sugar solution is $2.46 \ atm$ at $27^{\circ} C$,then what is the concentration (in $mol \ L^{-1}$) of the solution $(R=0.0821 \ L \ atm \ mol^{-1} \ K^{-1})$?