(B) The depression in freezing point is given by $\Delta T_f = i \times K_f \times m$. Since $K_f$ and $m$ are constant,$\Delta T_f \propto i$. Freezi

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(B) The depression in freezing point is given by $\Delta T_f = i \times K_f \times m$. Since $K_f$ and $m$ are constant,$\Delta T_f \propto i$. Freezing point $T_f = T_f^0 - \Delta T_f = 273 - (i \times K_f \times 0.1)$. For sucrose,$i=1$,$\Delta T_f = 273 - 272 = 1 \, K$. Thus,$K_f \times 0.1 = 1$. $T_f = 273 - i$. For $a. \ BaCl_2$ $(i=3)$: $T_f = 273 - 3 = 270 \, K$ $(q)$. For $b. \ NaCl$ $(i=2)$: $T_f = 273 - 2 = 271 \, K$ $(p)$. For $c. \ K_3[Fe(CN)_6]$ $(i=4)$: $T_f = 273 - 4 = 269 \, K$ $(s)$. For $d. \ Al_2(SO_4)_3$ $(i=5)$: $T_f = 273 - 5 = 268 \, K$ $(r)$. Therefore,the correct match is $a-q, b-p, c-s, d-r$.

Class 12 Chemistry Solutions Depression of freezing point of the solvent

Medium

Column-$I$ (Various solutions) Column-$II$ (Freezing point)

$a$. $0.1 \, M \ BaCl_2$ solution $p$. $271 \, K$

$b$. $0.1 \, M \ NaCl$ solution $q$. $270 \, K$

$c$. $0.1 \, M \ K_3[Fe(CN)_6]$ solution $r$. $268 \, K$

$d$. $0.1 \, M \ Al_2(SO_4)_3$ solution $s$. $269 \, K$

Given: Freezing point of $0.1 \, M$ sucrose solution $= 272 \, K$ and freezing point of water $= 273 \, K$.
Which of the following options shows the correct matches?

Column-$I$ (Various solutions)	Column-$II$ (Freezing point)
$a$. $0.1 \, M \ BaCl_2$ solution	$p$. $271 \, K$
$b$. $0.1 \, M \ NaCl$ solution	$q$. $270 \, K$
$c$. $0.1 \, M \ K_3[Fe(CN)_6]$ solution	$r$. $268 \, K$
$d$. $0.1 \, M \ Al_2(SO_4)_3$ solution	$s$. $269 \, K$

A
$a-r, b-p, c-s, d-q$
B
$a-q, b-p, c-s, d-r$
C
$a-q, b-s, c-p, d-r$
D
$a-s, b-q, c-r, d-q$

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Depression of freezing point of the solvent

What is the freezing point depression constant of a solvent,$50 \ g$ of which contains $1 \ g$ of a non-volatile solute (molar mass $256 \ g \ mol^{-1}$) and the decrease in freezing point is $0.40 \ K$?

MediumJEE MAIN 2025

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Calculate the mass of ascorbic acid $(\text{C}_6\text{H}_8\text{O}_6)$ to be dissolved in $75 \text{ g}$ of acetic acid to lower its melting point by $1.5^\circ\text{C}$. $[K_f = 3.9 \text{ K kg mol}^{-1}, \text{H} = 1, \text{C} = 12, \text{O} = 16 \text{ amu}]$ (in $\text{ g}$)

DifficultGUJCET 2026

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An aqueous solution containing $0.2 \ g$ of a non-volatile solute '$A$' in $21.5 \ g$ of water freezes at $272.814 \ K$. If the freezing point of water is $273.16 \ K$,the molar mass (in $g \ mol^{-1}$) of solute '$A$' is $[K_f(H_2O) = 1.86 \ K \ kg \ mol^{-1}]$

MediumAP EAMCET 2025

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Ethylene glycol is used as an anti-freezing agent. Calculate the amount of ethylene glycol to be added to $4 \ kg$ of water to prevent it from freezing at $-6 \ ^{\circ}C$. ($K_f$ for water $= 1.85 \ K \ kg \ mol^{-1}$) (molar mass of $(CH_2OH)_2 = 62 \ g \ mol^{-1}$) .......... $g$.

Medium

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What is observed during the depression of freezing point?

Easy

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Similar Questions

What is the freezing point depression constant of a solvent,$50 \ g$ of which contains $1 \ g$ of a non-volatile solute (molar mass $256 \ g \ mol^{-1}$) and the decrease in freezing point is $0.40 \ K$?

Calculate the mass of ascorbic acid $(\text{C}_6\text{H}_8\text{O}_6)$ to be dissolved in $75 \text{ g}$ of acetic acid to lower its melting point by $1.5^\circ\text{C}$. $[K_f = 3.9 \text{ K kg mol}^{-1}, \text{H} = 1, \text{C} = 12, \text{O} = 16 \text{ amu}]$ (in $\text{ g}$)

An aqueous solution containing $0.2 \ g$ of a non-volatile solute '$A$' in $21.5 \ g$ of water freezes at $272.814 \ K$. If the freezing point of water is $273.16 \ K$,the molar mass (in $g \ mol^{-1}$) of solute '$A$' is $[K_f(H_2O) = 1.86 \ K \ kg \ mol^{-1}]$

Ethylene glycol is used as an anti-freezing agent. Calculate the amount of ethylene glycol to be added to $4 \ kg$ of water to prevent it from freezing at $-6 \ ^{\circ}C$. ($K_f$ for water $= 1.85 \ K \ kg \ mol^{-1}$) (molar mass of $(CH_2OH)_2 = 62 \ g \ mol^{-1}$) .......... $g$.

What is observed during the depression of freezing point?

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