At $310 \ K$,the osmotic pressure of blood is $7.65 \ atm$. An aqueous solution of glucose will be isotonic with blood at a concentration of ........ $\%$ (weight/volume).

Arrange the following solutions according to decreasing order of osmotic pressure under similar conditions of temperature,assuming complete dissociation:
$A. 0.2 \ m \ KCl$
$B. 0.3 \ m \ MgSO_4$
$C. 0.1 \ m \ BaCl_2$
$D. 0.5 \ m \ Al_2(SO_4)_3$

$x \% (w/v)$ solution of urea is isotonic with $4 \% (w/v)$ solution of a non-volatile solute of molar mass $120 \ g \ mol^{-1}$. The value of $x$ is

$A$ solution of polystyrene in benzene contains $10 \, g/L$. The equilibrium height of the column of solution having density $0.9 \, g/mL$ in the osmometer is $11 \, cm$ at $27 \, ^\circ C$. What is the average molar mass of polystyrene? (Assume the solution is ideal)

To have an osmotic pressure equal to a solution containing $9.2 \ g$ of glucose per liter,how many grams of glucose must be dissolved in $0.5 \ L$ of solution?

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 $0.2 \ atm$. $(R = 0.0821 \ L \ atm \ K^{-1} \ mol^{-1})$