Van't Hoff's Factor

Select the correct statements:

The freezing point depression of $0.1$ molal solution of benzoic acid in benzene is $0.256 \mathrm{K}$. ${\mathrm{K}}_{\mathrm{f}}$ for benzene is $5.12 \mathrm{K} \mathrm{kg} {\mathrm{mol}}^{-1}$. What conclusion can you draw about the molecular state of benzoic acid in benzene?

When $0.3\mathrm{g}$ of acetic acid is dissolved in $30 \mathrm{g}$ of benzene the freezing point is lowered by $0.45℃$. Deduce the value of van't Hoff factor. It is given that ${\mathrm{K}}_{\mathrm{f}}$(benzene)=$5.12 \mathrm{K} \mathrm{kg} {\mathrm{mol}}^{-1}$.

Consider $0.1 \mathrm{M}$ solutions of two solutes $\mathrm{X}$ and $\mathrm{Y}$. The solute $\mathrm{X}$behaves univalent strong electrolyte while the solute $\mathrm{Y}$dimerises completely in solution. Which of the following statements are correct regarding these solutions?

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:

Van't Hoff factor is the ratio of abnormal molar mass to the normal molar mass.

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

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:-

Colligative properties are directly proportional to the molar mass of the solute.

The partial dissociation appears to be a major factor in determining the properties of weak electrolytes and the degree of dissociation for weak electrolyte at dilution v is given by $\text{α}=\frac{{\text{Λ}}_{\text{v}}}{{\text{Λ}}_{\infty }}$. The strong electrolytes on the other hand do not obey this relation and the variation of molar conductivity for strong electrolytes is given by ${\text{Λ}}_{\text{v}}={\text{Λ}}_{\infty }-{\text{bc}}^{1/2}$.

The graph plotted for log ($\text{i-1}$)vs. log ${\text{Λ}}_{\text{v}}$, where i is van't Hoff factor for uni-univalent electrolyte and ${\text{Λ}}_{\text{v}}$, is its molar conductivity at concentration c does not show the following characteristics:

The van’t Hoff factor $\mathrm{i}$ for a compound which undergoes dissociation in one solvent and association in another solvent is respectively

Van’t Hoff factor $\mathrm{i}$ is given by the expression _____.

Which of the following $0.1 \mathrm{M}$ aqueous solutions will exert highest osmotic pressure?

Derive the equation:

$\mathrm{\alpha }=\frac{\mathrm{M} \left(\mathrm{theoretical}\right)-\mathrm{M} \left(\mathrm{observed}\right)}{\mathrm{M} \left(\mathrm{observed}\right) \left(\mathrm{n}\text{'}-1\right)}$

Derive the equation:

$\mathrm{\alpha }=\frac{\mathrm{i}-1}{\mathrm{n}\text{'}-1}$

Explain: Van't Hoff factor

Explain abnormal osmotic pressure.

Which of the following solutions will exhibit highest osmotic pressure?

Consider the separate solution of $0.500 M C_2{H}_{5}OH (aq.),0.100 M M{g}_3{\left(P{O}_4\right)}_2(aq.),0.250 M KBr\left(aq\right)$ and $0.125 M N{a}_{3}P{O}_4(aq.),$ at ${25}^{o}C.$  Which statement is true about these solutions, assuming all salts to be strong electrolytes?