The osmotic pressure of a sugar solution at $300 \ K$ is $2.46 \ atm$. What is the concentration of the solution (in $M$)?

At a constant temperature,the osmotic pressures of a $1.5 \ M \ NH_4NO_3$ aqueous solution and an $x \ M \ Al_2(SO_4)_3$ aqueous solution are approximately equal. Find the value of $x$. (Assume $100 \%$ dissociation of the solute in the solution.)

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 $g$)

$A$ solution of sucrose (molar mass $= 342 \ g \ mol^{-1}$) is prepared by dissolving $68.4 \ g$ of it per litre of the solution. What is its osmotic pressure in $atm$ at $273 \ K$? (Given: $R = 0.082 \ L \ atm \ K^{-1} \ mol^{-1}$)

$A$ solution of a substance containing $1.05 \ g$ per $100 \ mL$ was found to be isotonic with $3 \% (w/v)$ glucose solution. The molecular mass of the substance is :

Find out the osmotic pressure of a $0.2 \, M$ solution of glucose at $300 \, K$. (in $, \text{atm}$)