The observed freezing point depression of a 0.01 m aqueous solution of a weak acid HA is 0.0205 °C. If the $K_f$ of water is 1.86 K kg/mol, which expression correctly calculates the percent ionization of the weak acid?

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

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

The order of osmotic pressure of isomolar solution of $BaC{l_2},NaCl\;and\;sucrose$ is

5% (wt./vol.) aqueous NaCl solution and 5% (wt./vol.) aqueous KCl solution are :

Solutions A, B, C and D are respectively 0.1 M glucose, $0.05\;M{\rm{ }}NaCl,$ $0.05\;M\;{\rm{BaC}}{{\rm{l}}_2}$ and $0.1\;M\;\;{\rm{AlC}}{{\rm{l}}_3}{\rm{.}}$ Which one of the following pairs is isotonic?

If the elevation in boiling point of a solution of 10 g of solute (mol. wt. = 100 g of water is $\Delta {T_b}$, the ebullioscopic constant of water is

If for a sucrose solution elevation in boiling point is $0.1^\circ C$ then what will be boiling point of${\rm{NaCl}}$ solution for the same molal concentration?

Two solutions of ${\rm{KN}}{{\rm{O}}_3}$ and ${\rm{C}}{{\rm{H}}_3}{\rm{COOH}}$ are prepared separately. Molarity of both is $0.1\;M$ and osmatic pressures are ${p_1}\;and\;{p_2}$ respectively. The correct relationship between the osmatic pressures is

A $0.002\;m$ aqueous solution of an ionic compound ${\rm{Co}}{\left( {{\rm{N}}{{\rm{H}}_3}} \right)_5}\left( {{\rm{N}}{{\rm{O}}_2}} \right){\rm{Cl}}$ freezes at $- 0.00732^\circ {\rm{C}}$. Number of moles of ions which 1 mol of ionic compound produces on being dissolved in water will be :$\left( {{K_f} = + 1.86^\circ {\rm{C}}/{\rm{m}}} \right)$

Which of the following solutions will have highest boiling point