At a temperature of $27\,^oC$,$0.6\,g$ of a solute is dissolved in $0.1\,L$ of solvent,resulting in an osmotic pressure of $1.23\,atm$. The molar mass of the solute is .......... $g\,mol^{-1}$.

At a certain temperature,a $1.6 \%$ solution of an unknown substance is isotonic with a $2.4 \%$ solution of Urea. If both solutions have the same solvent and the same density of $1 \ g/cm^3$,what is the molecular mass of the unknown substance in $g/mol$? [Molecular mass of urea $= 60 \ g/mol$]

Assertion : If red blood cells were removed from the body and placed in pure water,pressure inside the cells increases.
Reason : The concentration of salt content in the cells increases.

If $A$ contains $2\% \ NaCl$ and it is separated by a semipermeable membrane from $B$ which contains $10\% \ NaCl$,which event will occur?

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

$A$ solution is prepared by dissolving $0.6 \ g$ of urea (molar mass $= 60 \ g \ mol^{-1}$) and $1.8 \ g$ of glucose (molar mass $= 180 \ g \ mol^{-1}$) in $100 \ mL$ of water at $27 \ ^oC$. The osmotic pressure of the solution is : ............. $atm$ $(R = 0.08206 \ L \ atm \ K^{-1} \ mol^{-1})$