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

If $3 \ g$ of glucose (molar mass $= 180 \ g \ mol^{-1}$) is dissolved in $60 \ g$ of water at $15^{\circ} C$,the osmotic pressure of the solution will be (in $atm$)

Solutions $A, B, C$ and $D$ are respectively $0.2 \ M$ urea,$0.10 \ M$ $NaCl$,$0.05 \ M$ $BaCl_{2}$ and $0.05 \ M$ $AlCl_{3}$. All solutions are isotonic with each other except:

At $27\,^oC$,the osmotic pressure of a solution containing $36\,g$ of glucose per liter is $4.92\,atm$. If the osmotic pressure of the solution is adjusted to $1.5\,atm$ at the same temperature,what will be its concentration?

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

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 $g$)