A 0.1 molal aqueous solution of a weak electrolyte, HX, freezes at -0.208 °C. Assuming ideal behavior, what is the van't Hoff factor (i) for HX in this solution? (K$_f$ for water = 1.86 K kg mol$^{-1}$)

${\rm{0}}{\rm{.004}}\;{\rm{M}}\;{\rm{N}}{{\rm{a}}_2}{\rm{S}}{{\rm{O}}_4}$ is isotonic with 0.01 M glucose.Degree of dissociation of ${\rm{N}}{{\rm{a}}_2}{\rm{S}}{{\rm{O}}_4}$ is

The boiling point of an aqueous solution of a non-volatile solute is $100.15^\circ C$. What is the freezing point of an aqueous solution obtained by diluting the above solution with an equal volume of water? The values of ${k_b}\;and\;{k_f}$ for water are $0.512^\circ C$ and $1.86^\circ C\;K\;{\rm{molalit}}{{\rm{y}}^{ - 1}}$

If sodium sulphate is considered to be completely dissociated into cations and anions in aqueous solution, the change in freezing point of water $\Delta {T_f}$, when 0.01 mole of sodium sulphate is dissolved in 1 kg of water, is $({k_f} = 1.86\;{\rm{K}}\;{\rm{kg mo}}{{\rm{l}}^{ - 1}})$

At temperature $327^\circ C$ and concentration C osmotic pressure of a solution is p, the same solutions at concentration C/2 and a temperature $427^\circ C$ shows osmotic pressure 2 atm, value of p will be

Vapour pressure of chloroform $\left( {{\rm{CHC}}{{\rm{l}}_3}} \right)$ and dichloromethane $\left( {{\rm{C}}{{\rm{H}}_2}{\rm{C}}{{\rm{l}}_2}} \right)\;\;at\;25^\circ C$ are 200 mm Hg and 41.5 mm Hg respectively. Vapour pressure of the solution obtained by mixing 25.5 g of $\left( {{\rm{CHC}}{{\rm{l}}_3}} \right)$ and 40 g of ${{\rm{C}}{{\rm{H}}_2}{\rm{C}}{{\rm{l}}_2}}$ at the same temperature will be :

(Molecular mass of ${\rm{CHC}}{{\rm{l}}_3} = 119.5\;\;u$ and molecular mass of ${\rm{C}}{{\rm{H}}_2}{\rm{C}}{{\rm{l}}_2} = 85\;u)$

The osmotic pressure $(At\;27^\circ C)$ of an aqueous solution (200 mL) containing 6 g of a protein is $2 imes {10^{ - 3}}\;{\rm{atm}}.$ If $R = 0.080{\rm{ }}L - atm{\rm{ }}\;mo{l^{ - 1}}{K^{ - 1}},$ the molecular weight of protein is

A 0.1 molal aqueous solution of a weak electrolyte, HX, freezes at -0.208 °C. Assuming ideal behavior, what is the van't Hoff factor (i) for HX in this solution? (K$_f$ for water = 1.86 K kg mol$^{-1}$)

Vapour pressure of chloroform $\left( {{\rm{CHC}}{{\rm{l}}_3}} \right)$ and dichloromethane $\left( {{\rm{C}}{{\rm{H}}_2}{\rm{C}}{{\rm{l}}_2}} \right)\;\;at\;25^\circ C$ are 200 mm Hg and 41.5 mm Hg respectively. Vapour pressure of the solution obtained by mixing 25.5 g of $\left( {{\rm{CHC}}{{\rm{l}}_3}} \right)$ and 40 g of ${{\rm{C}}{{\rm{H}}_2}{\rm{C}}{{\rm{l}}_2}}$ at the same temperature will be :

(Molecular mass of ${\rm{CHC}}{{\rm{l}}_3} = 119.5\;\;u$ and molecular mass of ${\rm{C}}{{\rm{H}}_2}{\rm{C}}{{\rm{l}}_2} = 85\;u)$

The freezing point (in\;^\circ C) of a solution containing $0.1\;g\;of\;{{\rm{K}}_3}\left[ {{\rm{Fe}}{{\left( {{\rm{CN}}} \right)}_6}} \right]$ (mol.wt.329) in 100 g of water is : $({K_f} = 1.86\;K\;{\rm{kg}}\;{\rm{mo}}{{\rm{l}}^{ - 1}})$

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