(1)

Number of moles of acetic acid:

$\left(n_{C{H}_{3}COOH}\right)=\frac{\mathrm{Given} \mathrm{mass}}{\mathrm{Molar} \mathrm{mass}}=\frac{180g}{60gmo{l}^{-1}}=3mol$

Number of moles of benzoic acid:

$\left(n_{C_6{H}_{5}COOH}\right)=\frac{\mathrm{Given} \mathrm{mass}}{\mathrm{Molar} \mathrm{mass}}=\frac{180g}{122gmo{l}^{-1}}=1.475mol$

Number of moles of glucose:

$\left(n_{C_6{H}_{12}{O}_6}\right)=\frac{\mathrm{Given} \mathrm{mass}}{\mathrm{Molar} \mathrm{mass}}=\frac{180g}{180gmo{l}^{-1}}=1mol$

In water, carboxylic acids undergo dissociation, resulting in an increase in the number of particles, consequently contributing towards increasing the value of the colligative property.

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In benzene, carboxylic acids undergo dimerisation, resulting in a decrease in the number of particles, consequently contributing towards decreasing the value of the colligative property.

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Glucose does not dissociate or associate in water.
As the most number of particles are produced in (1), it has the highest depression in freezing point.
Assuming complete dissociation of acetic acid in water, $\mathrm{i}=2$. 
Assuming complete association of acetic acid and benzoic acid in benzene $(i=\frac{1}{2})$. 
Assuming 1 kg of solvent in each case, various $\Delta T_f$ values are as follows: