A solution is prepared by dissolving 1.8 g of a non-volatile solute in 90 g of water. The vapor pressure of the solution is found to be 23.375 mm Hg at 25°C. If the vapor pressure of pure water at 25°C is 23.76 mm Hg, what is the molar mass of the solute? (Molar mass of water = 18 g/mol)

The elevation in boiling point for one molal solution of a solute in a solvent is called :

A solution is prepared by dissolving 1.8 g of a non-volatile solute in 90 g of water. The vapor pressure of the solution is found to be 23.375 mm Hg at 25°C. If the vapor pressure of pure water at 25°C is 23.76 mm Hg, what is the molar mass of the solute? (Molar mass of water = 18 g/mol)

Molal elevation constant of a liquid is :

What is the freezing point of a solution containing 8.1 g HBr in 100 g water assuming the acid to be 90% ionised? $({k_f}\;{\rm{for}}\;{\rm{ wt}}{\rm{.}} = 1.86\;{\rm{K }}\;{\rm{mo}}{{\rm{l}}^{ - 1}})$

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 :

A 5.25% solution of a substance is isotonic with a 1.5% solution of urea (molar mass $= 60\;g\;{\rm{mo}}{{\rm{l}}^{ - 1}}$) in the same solvent. If the densities of both the solutions are assumed to be equal to ${\rm{1}}{\rm{.0}}\;{\rm{g}}\;{\rm{c}}{{\rm{m}}^{ - 3}},$ molarmass of the substance will be

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 :

A solution of sucrose (Molar mass = 342 g/mol) is prepared by dissolving 68.4 g of it per litre of solution, what is its osmotic pressure $(R = 0.082\;{\rm{ }}L{\rm{ }}atm\;{{\rm{K}}^{ - 1}}\;{\rm{mo}}{{\rm{l}}^{ - 1}})$ at 273 K?

Which method cannot be used to find out the molecular weight of non-volatile solute?

Insulin ${\left( {{{\rm{C}}_2}{{\rm{H}}_{10}}{{\rm{O}}_5}} \right)_n}$ is dissolved in a suitable solvent and the osmotic pressure $\left( {\rm{\pi }} \right)$ of solutions of various concentrations $C\left( {{\rm{g}}/{\rm{c}}{{\rm{m}}^3}} \right)$ is measured at $20^\circ C$. the slope of a plot of ${\rm{\pi }}$ against $C$ is formed to be $4.65 imes {10^{ - 3}}$. The molecular weight of the insulin is :