Calculate the osmotic pressure of $0.03 \ mol$ of non-electrolyte solute dissolved in $0.1 \ dm^3$ of water at $300 \ K \ [R=0.0821 \ dm^3 \ atm \ mol^{-1} \ K^{-1}]$ (in $atm$)

$A$ solution containing $6.0 \ g$ of urea is isotonic with a solution containing $10 \ g$ of a non-electrolytic solute $X$. The molar mass of $X$ (in $g \ mol^{-1}$) is

Which of the following sets of solutions of urea (mol. mass $60 \ g \ mol^{-1}$) and sucrose (mol. mass $342 \ g \ mol^{-1}$) is isotonic?

At $17^\circ C$,the osmotic pressure of an aqueous solution of sucrose $(C_{12}H_{22}O_{11})$ containing $34.2 \ g/L$ is $P$. What concentration of glucose $(C_6H_{12}O_6)$ in $g/L$ would be isotonic with this solution?

Which of the following conditions is correct for reverse osmosis? [$C =$ Concentration of solution in $mol \ L^{-1}$; $T =$ Temperature in Kelvin scale; $P_{ext} =$ External pressure; $\pi = CRT =$ Osmotic pressure]

Which of the following can pass through a semi-permeable membrane?