The osmatic pressure of a 5% (wt./vol) solution of cane sugar at $150^\circ C$ is

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 :

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

Equimolar solutions of two non-electrolytes in the same solvent should have :

If the various terms in the below given expressions have usual meanings, the van’t Hoff factor (i) cannot be calculated by which one of the expressions?

Which of the given solutions has highest osmotic pressure?

The statement “the relative lowering of the vapour pressure is equal to th ratio ot moles of the solute to the total number of the moles in the solution” refers to

1.0 g of a non-electrolyte solute (molar mass 250 g ${\rm{mo}}{{\rm{l}}^{ - 1}}$) was dissolved in 51.2 g of benzene. If the freezing point depression constant of benzene is 5.12 K kg ${\rm{mo}}{{\rm{l}}^{ - 1}}$, the lowering in freezing point will be :

The freezing point of equimolal aqueous solution will be highest for

What is the amount of urea dissolved per litre if its aqueous solution is isotonic with 10% cane sugar solution? (mol.wt.of urea =60)

At $25^\circ C$ , the highest osmotic pressure is exhibited by 0.1 M solution of