Calculate the molar mass of a solute when $4 \ g$ of it is dissolved in $1 \ dm^3$ of solvent,having an osmotic pressure of $2 \ atm$ at $300 \ K$. $[R = 0.082 \ dm^3 \ atm \ K^{-1} \ mol^{-1}]$

If a $6.84\% \ (w/v)$ solution of sucrose (molar mass $342 \ g/mol$) is isotonic with a $1.52\% \ (w/v)$ solution of thiocarbamide,what is the molar mass of thiocarbamide?

Which one of the following pairs of solutions will be isotonic at the same temperature?

Which of the following statements associated with an isotonic solution is not correct?

$A$ solution of $12 \ g$ of non-electrolyte $(A)$ prepared by dissolving it in $1000 \ mL$ of water exerts the same osmotic pressure as that of a $0.05 \ M$ glucose solution at the same temperature. The empirical formula of $A$ is $CH_2O$. The molecular mass of $A$ is $.......... \ g \ mol^{-1}$. (Nearest integer)

In a container,$0.1 \, M \, NaCl$ and $0.05 \, M \, BaCl_2$ solutions are separated by a semi-permeable membrane. Which of the following is correct?