Van't Hoff's Factor

Relative decrease in vapour pressure is $0.4$ for a solution containing $1\mathrm{ }\mathrm{m}\mathrm{o}\mathrm{l}\mathrm{e}\mathrm{ }\mathrm{A}\mathrm{B}$ in $3\mathrm{ }\mathrm{m}\mathrm{o}\mathrm{l}\mathrm{ }{\mathrm{H}}_2\mathrm{O}$, therefore $\mathrm{A}\mathrm{B}$ is ionised at the extent of

If the osmotic pressure of a 0.010 M aqueous solution of sucrose at ${27}^{\text{o}}\text{C}$ is 0.25 atm, then the osmotic pressure of a 0.010 M aqueous solution of NaCl at ${27}^{\text{o}}\text{C}$ is

What are the minimum values of the Van't Hoff factors in a solute undergoing dimerisation and trimerisation?

Which of the following is the correct value of degree of association $\left(\mathrm{\alpha }\right)$ in terms of van't Hoff factor ($i$) is:

Which of the following is the correct value of degree of dissociation $\left(\mathrm{\alpha }\right)$ in terms of van't Hoff factor ($i$) is:

Integral value of van't hoff factor for ${\mathrm{K}}_2{\mathrm{SO}}_4$:

Which of the following will show maximum lowering in vapour pressure:

${\mathrm{Ba}}^{2+},{\mathrm{CN}}^{-}$, And ${\mathrm{Co}}^{2+}$ form an ionic compound. If the complex is supposed to $75\%$ ionised in water with van't Hoff factor $=4$, what is the coordination number of ${\mathrm{Co}}^{2+}$ in the complex?

Four solutions of ${\mathrm{K}}_2{\mathrm{SO}}_4$ with the concentration $0.1 \mathrm{m}, 0.01 \mathrm{m}, 0.001 \mathrm{m}$ and $0.0001 \mathrm{m}$ are available. The maximum value of van't Hoff factor, $\mathrm{i}$ corresponds to:

The vapour density of undecomposed ${\mathrm{N}}_2{\mathrm{O}}_4$ is $46$. When heated, vapour density decreased to $24.5$ due to its dissociation to ${\mathrm{NO}}_2$. The percent dissociation of ${\mathrm{N}}_2{\mathrm{O}}_4$ at the final temperature is :

The Van't Hoff's factor for $0.1 \mathrm{M} \mathrm{Ba}{\left({\mathrm{NO}}_3\right)}_2$ solution is $2.74$. The degree of dissociation is:

${\mathrm{Ba}}^{2+},{\mathrm{CN}}^{-},$ and ${\mathrm{Co}}^{2+}$ form an ionic compound. If the complex is supposed to $75\%$ ionized in water with van't Hoff factor $=4,$ what is the coordination number of ${\mathrm{Co}}^{2+}$ in the complex ?

The value of Van't Hoff factor (i) for ${\mathrm{K}}_3\left[\mathrm{Fe}(\mathrm{CN}{)}_6\right]$ is $\mathrm{X}$, if it undergoes $75\%$ dissociation in aqueous medium, calculate $4\mathrm{X}$?

The degree of dissociation of an electrolyte is $\alpha$ and its van't Hoff factor is $\mathrm{i}$. The number of ions obtained by complete dissociation of $1$ molecule of the electrolyte is:

The Van't Hoff factor of solutes $\mathrm{A}, \mathrm{B}$ and $\mathrm{C}$ in aqueous solutions are $0.8, 1.6$ and $1.2$ respectively. The freezing point of equimolar solutions follow the order :

Which one of the following electrolyte has the same value of vant'Hoff factor $\left(\mathrm{i}\right)$ as that of ${\mathrm{Al}}_2 ({\mathrm{SO}}_4{)}_3$(If $60\%$ ionised) :-

The vapour density of ${\mathrm{PCl}}_5$ is $104.25$ but when heated to $230°\mathrm{C}$, its vapour density is reduced to $62$. The degree of dissociation of ${\mathrm{PCl}}_5$ at this temperature will be:-

In a $0.2$ molal aqueous solution, a weak acid $\left(\mathrm{HX}\right)$ is $20\%$ ionized. The freezing point of this solution is :-

$\left({\mathrm{K}}_{\mathrm{f}}=1.86 \mathrm{K}.{\mathrm{m}}^{-1}\right)$

The molecular weight of $\mathrm{NaCl}$,  determined by studying freezing point depression of its $0.5\%$ aqueous solution is $30$. The apparent degree of dissociation of $\mathrm{NaCl}$ is:-

The value of observed and calculated molecular weight of calcium nitrate are $65$ and $164$. The degree of dissociation of $\mathrm{Ca}{\left({\mathrm{NO}}_3\right)}_2$ will be:-