If the $O.P.$ (Osmotic Pressure) of $1 \ M$ solutions of the following compounds in water can be measured,which one will show the maximum $O.P.$?

Calculate the approximate $\Delta T_b$ (in $K$) for $0.001 \ m$ $KCl$ solution, if its van't-Hoff factor is $1.98$ [$K_b$ of water is $0.52 \ K \ kg \ mol^{-1}$].

The measured osmotic pressure of a solution prepared by dissolving $17.4 \ mg$ of $K_2SO_4$ in $2 \ L$ of water at $27^{\circ} C$ is $3.735 \times 10^{-3} \ bar$. The van't Hoff factor is $(R = 0.083 \ L \ bar \ K^{-1} \ mol^{-1}$; atomic weights $K = 39, S = 32, O = 16)$.

$MX_{2}$ dissociates into $M^{2+}$ and $X^{-}$ ions in an aqueous solution,with a degree of dissociation $(\alpha)$ of $0.5$. The ratio of the observed depression of freezing point of the aqueous solution to the value of the depression of freezing point in the absence of ionic dissociation is

The relationship between the van’t Hoff factor $(i)$ and the degree of dissociation $(\alpha)$ is:

If the freezing point of a $0.01 \ m$ aqueous solution of a cobalt $(III)$ chloride-ammonia complex (which behaves as a strong electrolyte) is $-0.0558^{\circ} C$,the number of chloride $(Cl^-)$ ions in the coordination sphere of the complex is.
$\left[ K_{f} \text{ of water } = 1.86 \ K \ kg \ mol^{-1} \right]$