(C) The depression in freezing point is given by the formula: $\Delta T_f = K_f \times m$,where $m$ is the molality of the solution.Here,$\Delta T_f =

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(C) The depression in freezing point is given by the formula: $\Delta T_f = K_f \times m$,where $m$ is the molality of the solution.Here,$\Delta T_f = 0 - (-6) = 6 \ K$.$K_f = 1.86 \ K \ kg \ mol^{-1}$.Mass of solvent $(W_A)$ $= 4 \ kg$.Molar mass of solute $(M_B)$ $= 62 \ g \ mol^{-1}$.Molality $(m)$ $= \frac{W_B}{M_B \times W_A (\text{in } kg)}$.Substituting the values: $6 = 1.86 \times \frac{W_B}{62 \times 4}$.$W_B = \frac{6 \times 62 \times 4}{1.86}$.$W_B = \frac{1488}{1.86} = 800 \ g$.

Class 12 Chemistry Solutions Depression of freezing point of the solvent

Medium

Ethylene glycol is used as an antifreeze in cold climates. To prevent $4 \ kg$ of water from freezing at $-6^{\circ}C$,how many grams of ethylene glycol must be added? (Given for water: $K_f = 1.86 \ K \ kg \ mol^{-1}$,Molar mass of ethylene glycol $= 62 \ g \ mol^{-1}$)

A
$400.00$
B
$304.60$
C
$800.00$
D
$204.30$

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Depression of freezing point of the solvent

$K_{f}$ (water) $= 1.86 \ K \ kg \ mol^{-1}$. The temperature at which ice begins to separate from a mixture of $10$ mass $\%$ ethylene glycol is (in $^{\circ} C$)

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Identify the concentration of the solution from the following such that the values of $\Delta T_{f}$ and $K_{f}$ are the same.

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The molar freezing point constant for water is $1.86\,^{\circ}C\,kg\,mol^{-1}$. If $342\,g$ of cane sugar $(C_{12}H_{22}O_{11})$ are dissolved in $1000\,g$ of water,the solution will freeze at $............\,^{\circ}C$.

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Calculate the molar mass of a nonvolatile solute when $1.5 \ g$ of it is dissolved in $90 \ g$ of solvent,decreasing its freezing point by $0.25 \ K$. Given: $K_{f} = 1.2 \ K \ kg \ mol^{-1}$.

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What will be the freezing point of a $1\%$ aqueous solution of $Ca(NO_3)_2$?

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Ethylene glycol is used as an antifreeze in cold climates. To prevent $4 \ kg$ of water from freezing at $-6^{\circ}C$,how many grams of ethylene glycol must be added? (Given for water: $K_f = 1.86 \ K \ kg \ mol^{-1}$,Molar mass of ethylene glycol $= 62 \ g \ mol^{-1}$)

Similar Questions

$K_{f}$ (water) $= 1.86 \ K \ kg \ mol^{-1}$. The temperature at which ice begins to separate from a mixture of $10$ mass $\%$ ethylene glycol is (in $^{\circ} C$)

Identify the concentration of the solution from the following such that the values of $\Delta T_{f}$ and $K_{f}$ are the same.

The molar freezing point constant for water is $1.86\,^{\circ}C\,kg\,mol^{-1}$. If $342\,g$ of cane sugar $(C_{12}H_{22}O_{11})$ are dissolved in $1000\,g$ of water,the solution will freeze at $............\,^{\circ}C$.

Calculate the molar mass of a nonvolatile solute when $1.5 \ g$ of it is dissolved in $90 \ g$ of solvent,decreasing its freezing point by $0.25 \ K$. Given: $K_{f} = 1.2 \ K \ kg \ mol^{-1}$.

What will be the freezing point of a $1\%$ aqueous solution of $Ca(NO_3)_2$?

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