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 ${\mathrm{K}}_2{\mathrm{SO}}_4$:

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:-

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

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 molecular masses

Explain abnormal osmotic pressure.

Which of the following solutions will exhibit highest osmotic pressure?

Arrange the following in increasing order of their boiling point. 

$0.05\mathrm{ }\mathrm{m}\mathrm{ }\mathrm{La}{\left({\mathrm{NO}}_3\right)}_3, 0.05\mathrm{ }\mathrm{m}\mathrm{ }{\mathrm{MgBr}}_2, 0.05\mathrm{ }\mathrm{m}\mathrm{ }{\mathrm{NaNO}}_3$

What will be the boiling point of the final solution if one litre solution of 1 molar $\mathrm{N}\mathrm{a}\mathrm{C}\mathrm{l}$ is mixed with 1 litre solution of 1 molar $\mathrm{C}\mathrm{a}\mathrm{C}{\mathrm{l}}_2$?

Assume 100% ionisation of $\mathrm{N}\mathrm{a}\mathrm{C}\mathrm{l}$ and $\mathrm{C}\mathrm{a}\mathrm{C}{\mathrm{l}}_2$ in the solvent and molality = molarity

Given: ${\mathrm{K}}_{\mathrm{b}}$ of the solvent is $0.50\mathrm{K}/\mathrm{m}\mathrm{o}\mathrm{l}\mathrm{a}\mathrm{l}$, boiling point of the pure solvent is 400 K.

If a solute undergoes trimerization in solution, the minimum value of the Van't Hoff factor is $\mathrm{\beta }$. What is the value of $100\times \mathrm{\beta }$ after rounding off to the nearest integer.

A complex containing ${\mathrm{K}}^{+}$, $\mathrm{Pt}\left(\mathrm{IV}\right)$ and ${\mathrm{Cl}}^{-}$ is $100\%$ ionised. Giving $\mathrm{i}=3$.

Thus, what is the following complex?