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$^{-1}$)

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?

The slope of a graph plotting osmotic pressure ($\Pi$) against concentration ($\mathrm{mol\ L^{-1}}$) is found to be $41.46 \mathrm{L\ bar\ mol^{-1}}$. Using the ideal gas constant $\mathrm{R}=0.083 \mathrm{L\ bar\ mol^{-1} K^{-1}}$, determine the temperature at which the osmotic pressure measurements were conducted.

The relationship between the values of osmotic pressure of $0.1\;M$ solution of $KN{O_3}\left( {{p_1}} \right)$ and $C{H_3}COOH\left( {{p_2}} \right)$ is

The boiling point of ${{\rm{C}}_6}{{\rm{H}}_6},{\rm{C}}{{\rm{H}}_3}{\rm{OH}},{{\rm{C}}_6}{{\rm{H}}_5}{\rm{N}}{{\rm{H}}_2}\;{\rm{and}}\;{{\rm{C}}_6}{{\rm{H}}_5}{\rm{N}}{{\rm{O}}_2}$ are $80^\circ C,65^\circ C,184^\circ C\;{\rm{ and}}\;212^\circ C$ respectively. Which will show highest vapour pressure at room temperature?

What happens when an egg is kept in saturated solution of NaCl after removing its hard shell in dilHCl?

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

Depression in freezing point is 6 K for NaCl solution if ${k_f}$ for water is 1.86 K/kg mol, amount of NaCl dissolved in 1 kg water is

When mercuric iodide is added to the aqueous solution of potassium iodide, the

The freezing point depression constant $K_f$ of cyclohexane is $20.0 \, K \, kg \, mol^{-1}$. A solution of a non-electrolyte solute in cyclohexane has a molarity of $0.050 \, m$. What is the freezing point depression for this solution (rounded off to two decimal places)?

The freezing point depression constant ${\rm{(}}{{\rm{K}}_{\rm{f}}}{\rm{)}}$ of benzene is ${\rm{5}}{\rm{.12}}\,{\rm{K}}\,\,{\rm{kg }}\,{\rm{mo}}{{\rm{l}}^{ - 1}}$. The freezing point depression for the solution of molarity ${\rm{0}}{\rm{.078}}\,{\rm{m}}$ containing a non-electrolyte solute in benzene is (rounded off upto two decimal places):