Blood is isotonic with

$300 \ mL$ of an aqueous solution of a protein contains $2.52 \ g$ of the protein. If the osmotic pressure of such a solution at $300 \ K$ is $5.04 \times 10^{-3} \ bar$,the molar mass of the protein in $g \ mol^{-1}$ is:

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

$A$ solution containing $10 \ g/L$ of urea is isotonic with a $5\%$ solution of a non-electrolyte solute. The molecular mass of the non-electrolyte solute is ..... $g/mol$.

$A$ solution has an osmotic pressure of $x \ kPa$ at $300 \ K$ having $1 \ mole$ of solute in $10.5 \ m^{3}$ of solution. If its osmotic pressure is reduced to $(\frac{1}{10})$th of its initial value,what is the new volume of solution (in $m^{3}$)?

At a certain temperature,the osmotic pressure of a $0.25 \, M$ solution of a non-electrolyte is $\pi \, bar$. What will be the osmotic pressure of a $0.125 \, M \, Ba(NO_3)_2$ solution at the same temperature?