The freezing point of a $0.0020 \ m$ aqueous solution of $[CO(NH_3)_5(NO_2)]$ is $-0.00732 \ ^oC$. The number of ions produced (van't Hoff factor,$i$) when $1 \ mol$ of this ionic compound is dissolved in water is ..... $(K_f = 1.86 \ K \ kg \ mol^{-1})$

In equimolar solutions of glucose,$NaCl$,and $BaCl_2$,the order of osmotic pressure is as follows:

Calculate the molality of an aqueous solution of an electrolyte that freezes at $-0.93 \text{ }^\circ\text{C}$. Given that $K_f$ for water is $1.86 \text{ K kg mol}^{-1}$ and the van't Hoff factor $(i)$ is $1.25$. (Freezing point of pure water $= 0 \text{ }^\circ\text{C}$) (in $\text{ m}$)

$17.4\% \ (W/V)$ solution of potassium sulphate (mol. $wt. = 174$) is isotonic with $4\% \ (W/V)$ aqueous solution of $NaOH$. If $NaOH$ is $100\%$ ionised,the degree of ionisation of potassium sulphate is $........... \ \%$.

When mercuric iodide $(HgI_2)$ is added to an aqueous solution of potassium iodide $(KI)$,the

The depression in freezing point for $0.01 \ m$ aqueous solution of $K_{x}[Fe(CN)_6]$ is $0.0744 \ K$. The molal depression constant for solvent is $1.86 \ K \ kg \ mol^{-1}$. If the solute undergoes complete dissociation,what is the correct molecular formula for the solute?