Van't Hoff's Factor

What is degree of association ?

A quantity of $1.04 \mathrm{g}$ of ${\mathrm{CoCl}}_3.6{\mathrm{NH}}_3\left(\mathrm{Molecular} \mathrm{weight}=267\right)$ was dissolved in $100 \mathrm{g} \mathrm{of} {\mathrm{H}}_2\mathrm{O}$. The freezing point of the solution was $-0.{29}^{\circ }\mathrm{C}$. How many moles of solute particle exist in the solution for each mole of solute introduced? ${\mathrm{K}}_{\mathrm{f}}$ for water $=1.{86}^{\circ }\mathrm{C} {\mathrm{m}}^{-1}$

In terms of osmotic pressure $\left(\mathrm{\pi }\right)$, volume of the solution$\left(\mathrm{V}\right)$ containing $\mathrm{n}$ moles of the solute, and van't Hoff factor $\mathrm{i}$ at a temperature $\mathrm{T}$, osmotic pressure $\mathrm{\pi }=\frac{\mathrm{n}}{\mathrm{V}}\times$_____.

If Van't Hoff factor is less than unity, this shows that solute undergoes _____ in the solution.

What is Van't Hoff factor for a compound which undergoes tetramerisation in an organic solvent?

When is the value of Van't Hoff factor more than one?

Give an example of a compound in which hydrogen bonding results in the formation of a dimer.

Arrange the following solutions in increasing order of their Van't Hoff factor:

$0.1 \mathrm{M} {\mathrm{CaCl}}_2, 0.1 \mathrm{M} \mathrm{KCl}, 0.1 \mathrm{M} {\mathrm{Al}}_2{\left({\mathrm{SO}}_4\right)}_3, 0.1 \mathrm{M} {\mathrm{C}}_{12}{\mathrm{H}}_{22}{\mathrm{O}}_{11}$

What would be the value of Van't Hoff factor for a dilute aqueous solution of ${\mathrm{K}}_2{\mathrm{SO}}_4$?

How is the colligative property of solution changed when a solute in a solution undergoes dissociation.

How is the colligative property of solution changed when a solute in a solution undergoes association.

How much molecular mass of $\mathrm{NaCl}$ is obtained experimentally using colligative properties?

A certain mass of a substance when dissolved in $100 \mathrm{g} {\mathrm{C}}_6{\mathrm{H}}_6$ lowers the freezing point by $1.28° \mathrm{C}$. The same mass of the solute dissolved in $100 \mathrm{g}$ water lowers its freezing point by $1.40° \mathrm{C}$. If the substance has normal molecular mass in benzene and is completely dissociated in water, how many ions does it dissociate in water? ${\mathrm{K}}_{\mathrm{f}}$ for water $1.86$ and ${\mathrm{K}}_{\mathrm{f}}$ for benzene is  $5.12 \mathrm{K} \mathrm{Kg} {\mathrm{mol}}^{-1}$.

A solution of a monobasic acid with molarity $3\times {10}^{-2} \mathrm{M}$ has a freezing point depression of $0.6° \mathrm{C}$. Calculate ${\mathrm{pK}}_{\mathrm{a}}$ of the acid. (Molal depression constant of water is $1.86°\mathrm{C}/\mathrm{m}$.

The Van't Hoff factor for a compound which undergo dissociation in one solvent and association in other solvents is respectively

The depression in the freezing point for $1 \mathrm{M}$ urea, $1 \mathrm{M}$ glucose, and $1 \mathrm{M}$ sodium chloride in the ratio

Van't Hoff factor for $0.1 \mathrm{M}$ ideal solution is

Four solutions of ${\mathrm{K}}_2{\mathrm{SO}}_4$ with the concentrations $0.1 \mathrm{m}, 0.01\mathrm{m}, 0.001 \mathrm{m}$ and $0.0001 \mathrm{m}$ are available. The maximum value of Van't Hoff factors, correspond to 

Calculate the osmotic pressure of a $0.1 \mathrm{M}$ monobasic acid if its $\mathrm{pH}$ is $2.0$ at ${25}^{\mathrm{o}}\mathrm{C}$.

Equimolal solutions of $\mathrm{NaCl}$ and ${\mathrm{BaCl}}_2$ are prepared in water. Freezing point of $\mathrm{NaCl}$ is found to be $-2^{\mathrm{o}}\mathrm{C}$. What freezing point do you expect for ${\mathrm{BaCl}}_2$ solution ?