Abnormal Molar Mass

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:

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

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:

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 molecular masses

Explain abnormal osmotic pressure.

Which of the following solutions will exhibit highest osmotic pressure?

If the freezing point of a $0.01$ molal aqueous solution of a cobalt $\left(\mathrm{III}\right)$ bromide-ammonia complex (which behaves as a strong electrolyte) is  $-0.0557°\mathrm{C}$ , the number of bromide(s) in the coordination sphere of the complex is [ ${\mathrm{K}}_{\mathrm{f}}$ for water $=1.86 \mathrm{K}$  $\mathrm{kg} \mathrm{m}\mathrm{o}{\mathrm{l}}^{-1}$ ]

van't Hoff factor, when benzoic acid is dissolved in benzene, will be

${\mathrm{K}}_2{\mathrm{HgI}}_4$ is 40% ionised in aqueous solution. The value of its van't Hoff factor $\left(\mathrm{i}\right)$ is:

A complex K₂[HgI₄] has α = 40%. What will be it's Van't hoff factor?

When an electrolyte is dissociated in solution, the van't Hoff factor $\left(\mathrm{i}\right)$ is

Which has the highest boiling point?

Statement - 1: The vapour pressure of $0.1 \mathrm{M}$ sugar solution is more than solution $0.1 \mathrm{M} \mathrm{KCl}$. Because

Statement - 2: Lowering of vapour pressure is directly proportional to the number of particles present in the solution.