When a substance is distributed between two immiscible solvents and remains in the same state in the solvent I, while, dissociates in the solvent II. If the concentration of solute are ${c_{\rm{I}}}\;{\rm{and}}\;{c_{{\rm{II}}}}$ in phase I and II respectively then :

Aqueous solution of $0.004\;M\;{\rm{N}}{{\rm{a}}_2}{\rm{S}}{{\rm{O}}_4}$ and $0.01\;M$ glucose are isotonic. The degree of dissociation of ${\rm{N}}{{\rm{a}}_2}{\rm{S}}{{\rm{O}}_4}$ is :

The relative lowering of vapour pressure of an aqueous solution containing non-volatile solute is 0.0125. The molality of the solution is

In two solutions having different osmotic pressure, the solution of higher osmotic pressure is called :

Consider the following aqueous solutions and assume 100% ionisation in electrolytes

I. 0.1 m urea

II. 0.04 m ${\rm{A}}{{\rm{l}}_2}{\left( {{\rm{S}}{{\rm{O}}_4}} \right)_3}$

III. 0.05 m ${\rm{CaC}}{{\rm{l}}_2}$

IV. 0.005 m NaCl

The correct statement regarding the above solution is

If $0.1\;M$ solutions of each electrolyte are taken and if all electrolytes are completely dissociated, then whose boiling point will be highest ?

A 0.001 molal solution of $\left[ {{\rm{Pt}}{{\left( {{\rm{N}}{{\rm{H}}_3}} \right)}_4}{\rm{C}}{{\rm{l}}_4}} \right]$ in water has a freezing point depression of $0.0054^\circ C$. If ${k_f}$ for water is 1.80, the correct formulation of the above molecule is :

Which of the given solutions has highest osmotic pressure?

A solution's osmotic pressure ($\Pi$) is plotted against its concentration in $\mathrm{mol\ L^{-1}}$. The resulting straight line has a slope of $20.58 \mathrm{L\ bar\ mol^{-1}}$. If the ideal gas constant R is $0.083 \mathrm{L\ bar\ mol^{-1}\ K^{-1}}$, at what temperature was the osmotic pressure measured?

Mole fraction of solute in an aqueous solution which boils at 100.104. ${K_b}\;for\;{{\rm{H}}_2}{\rm{O}} = 0.52\;K\;{\rm{molalit}}{{\rm{y}}^{ - 1}}$:

If a $5.25\% {\rm{ }}\;\left( {wt./vol.} \right)$ solution of a non-electrolyte is isotonic with $1.50\% {\rm{ }}\;\left( {wt./vol.} \right)$ solution of urea, $\left( {mol - wt{\rm{ }} = 60} \right)$ is the same solvent then the molecular weight of non-electrolyte is :