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(C) $1$. According to Raoult's law, adding a non-volatile solute decreases the vapour pressure of the solvent.$2$. The decrease in vapour pressure lea

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The osmotic pressure of an electrolytic solution is greater than a non-electrolytic solution of the same concentration.

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(C) $1$. According to Raoult's law, adding a non-volatile solute decreases the vapour pressure of the solvent.$2$. The decrease in vapour pressure leads to an elevation in the boiling point of the solvent.$3$. Osmotic pressure is a colligative property, which depends on the number of particles. Electrolytes dissociate into multiple ions, increasing the number of particles compared to non-electrolytes at the same concentration, thus resulting in higher osmotic pressure.$4$. Freezing point depression is a colligative property, but the freezing point itself is not.

Identify the correct statement from the following.

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The freezing point of an aqueous solution which contains $5\%$ by mass urea,$1.0\%$ by mass $KCl$,and $10\%$ by mass glucose is ........ $K$. $\left( K_f(H_2O) = 1.86 \ K \ kg \ mol^{-1} \right)$

For a $0.2 \ m$ aqueous solution of a weak acid $HX$,the degree of ionization is $0.3$. If $K_f$ for water is $1.85 \ K \ kg \ mol^{-1}$,the freezing point of the solution will be close to .......... $^oC$.

The Van't Hoff factor of the compound $K_3[Fe(CN)_6]$ is

Observe the following statements:
Statement-$I$: The boiling point of $0.1 \ M$ urea solution is less than that of $0.1 \ M$ $KCl$ solution.
Statement-$II$: Elevation of boiling point is inversely proportional to molar mass of solute.
The correct answer is:

For a $0.25 \ m$ solution of $SrCl_2$,the van't Hoff factor is found to be $2.5$. What will be the effective molality of the solution in $m$?

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