Van't Hoff's Factor

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:

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?

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.

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?

$0.01 \mathrm{M}$ solution of glucose is isotonic with a $0.004 \mathrm{M}$solution of sodium sulphate at the same temperature. The apparent percentage dissociation of ${\mathrm{Na}}_2{\mathrm{SO}}_4$ is 

A salt ${\mathrm{MX}}_2$ has van't Hoff factor equal to $2$, then what will be its degree of dissociation in water?

The freezing point of water of a $0.01 \mathrm{molal} \mathrm{NaCl}$ solution is depressed by $0.37\mathrm{℃}$. The freezing point of $0.02 \mathrm{molal}$ solution of urea is depressed by:

Which of the following species cannot have a Van't Hoff factor greater than $1?$

Which of the following cannot have Van't Hoff factor i > 1?

The electrolyte solution show abnormal colligative properties. To account for this effect we define a quantity called the Van't Hoff factor given by

$i=\frac{Actualnumberofparticlesinsolutionafterdissociation}{Numberofformulaunitsinitiallydissolvedinsolution}$

$i=1$ (for non-electrolytes)

$i>1$ (for electrolytes, undergoing dissociation)

$i<1$ (for solutes, undergoing association)

Answer the following questions:

If ${\mathrm{pK}}_{\mathrm{a}}=4$ and ${\text{K}}_{\text{a}}={\text{Cα}}^{\text{2}}$, then find van't Hoff factor for a weak HA type acid, when $\mathrm{C}=0.01 \mathrm{M}$.

If a 0.004 M solution of $\mathrm{N}{\mathrm{a}}_2\mathrm{S}{\mathrm{O}}_4$ is isotonic with a 0.010 M solution of glucose at same temperature. Then what is the apparent degree of dissociation of $\mathrm{N}{\mathrm{a}}_2\mathrm{S}{\mathrm{O}}_4$ is

In a galvanic cell, after running the cell for sometime, the concentration of the electrolyte is automatically raised to 3 m HCl. Molar conductivity of the 3 m HCl is about 240 S $\mathrm{c}{\mathrm{m}}^2\mathrm{m}\mathrm{o}{\mathrm{l}}^{-1}$ and limiting molar conductivity of $\mathrm{HCl}$ is about 420 S $\mathrm{c}{\mathrm{m}}^2\mathrm{m}\mathrm{o}{\mathrm{l}}^{-1}$ . If ${\mathrm{K}}_{\mathrm{b}}$ of water is 0.52 K kg $\mathrm{m}\mathrm{o}{\mathrm{l}}^{-1}$ , calculate the boiling point of the electrolyte at the end of the experiment.

${\mathrm{K}}_2\left[\mathrm{H}\mathrm{g}{\mathrm{I}}_4\right]$ is $55\%$ ionised in aqueous solution. The value of Van't Hoff factor is