(D) The depression in freezing point is given by $\Delta T_f = T_f^\circ - T_f = 5.5 ^\circ C - 4.48 ^\circ C = 1.02 ^\circ C$ (or $1.02 \ K$).Using t

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(D) The depression in freezing point is given by $\Delta T_f = T_f^\circ - T_f = 5.5 ^\circ C - 4.48 ^\circ C = 1.02 ^\circ C$ (or $1.02 \ K$).Using the formula for molar mass $M = \frac{K_f \times w \times 1000}{W \times \Delta T_f}$,where $w = 4.8 \ g$,$W = 60 \ g$,$K_f = 5.1 \ K \ kg \ mol^{-1}$,and $\Delta T_f = 1.02 \ K$.$M = \frac{5.1 \times 4.8 \times 1000}{60 \times 1.02} = \frac{24480}{61.2} = 400 \ g \ mol^{-1}$.

Class 12 Chemistry Solutions Depression of freezing point of the solvent

Medium

The freezing point of a solution containing $4.8 \ g$ of a compound in $60 \ g$ of benzene is $4.48 ^\circ C$. What is the molar mass of the compound $(K_f = 5.1 \ K \ kg \ mol^{-1})$,(freezing point of benzene $= 5.5 ^\circ C$)?

A
$100$
B
$200$
C
$300$
D
$400$

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Depression of freezing point of the solvent

The aqueous solution of urea has a freezing point of $-0.6\,^\circ C$. To prepare such a solution,how many grams of urea are needed to dissolve in $3\,kg$ of water? $(M = 60\,g\,mol^{-1}, K_{f} = 1.5\,^\circ C\,kg\,mol^{-1})$

Medium

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Dissolution of $1.5 \ g$ of a non-volatile solute (mol. wt. $= 60$) in $250 \ g$ of a solvent reduces its freezing point by $0.01 \ ^{\circ}C$. Find the molal depression constant of the solvent.

MediumMHT CET 2010

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Which of the following will show maximum depression in freezing point when the concentration is $0.1 \ M$?

MediumIIT 1989

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The maximum freezing point depression constant $(K_f)$ is observed for which of the following solvents?

Easy

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The freezing point of a solution prepared from $1.25 \ g$ of a non-electrolyte and $20 \ g$ of water is $271.9 \ K$. If the molar depression constant is $1.86 \ K \ kg \ mol^{-1}$,then the molar mass of the solute will be:

Medium

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The freezing point of a solution containing $4.8 \ g$ of a compound in $60 \ g$ of benzene is $4.48 ^\circ C$. What is the molar mass of the compound $(K_f = 5.1 \ K \ kg \ mol^{-1})$,(freezing point of benzene $= 5.5 ^\circ C$)?

Similar Questions

The aqueous solution of urea has a freezing point of $-0.6\,^\circ C$. To prepare such a solution,how many grams of urea are needed to dissolve in $3\,kg$ of water? $(M = 60\,g\,mol^{-1}, K_{f} = 1.5\,^\circ C\,kg\,mol^{-1})$

Dissolution of $1.5 \ g$ of a non-volatile solute (mol. wt. $= 60$) in $250 \ g$ of a solvent reduces its freezing point by $0.01 \ ^{\circ}C$. Find the molal depression constant of the solvent.

Which of the following will show maximum depression in freezing point when the concentration is $0.1 \ M$?

The maximum freezing point depression constant $(K_f)$ is observed for which of the following solvents?

The freezing point of a solution prepared from $1.25 \ g$ of a non-electrolyte and $20 \ g$ of water is $271.9 \ K$. If the molar depression constant is $1.86 \ K \ kg \ mol^{-1}$,then the molar mass of the solute will be:

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