(C) The formula for depression in freezing point is $\Delta T_f = K_f \times m$. Here,$\Delta T_f = 0.2 \ K$,$K_f = 1.71 \ K \ kg \ mol^{-1}$,$M_B = 6

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(C) The formula for depression in freezing point is $\Delta T_f = K_f \times m$. Here,$\Delta T_f = 0.2 \ K$,$K_f = 1.71 \ K \ kg \ mol^{-1}$,$M_B = 60 \ g \ mol^{-1}$,and $W_A = 98 \ g$. The molality $m$ is given by $\frac{W_B \times 1000}{M_B \times W_A}$. Substituting the values: $0.2 = 1.71 \times \frac{W_B \times 1000}{60 \times 98}$. Solving for $W_B$: $W_B = \frac{0.2 \times 60 \times 98}{1.71 \times 1000} = \frac{1176}{1710} \approx 0.687 \ g$.

Class 12 Chemistry Solutions Depression of freezing point of the solvent

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What is the mass of solute having molar mass $60 \ g \ mol^{-1}$ when dissolved in $98 \ g$ of solvent decreases its freezing point by $0.2 \ K$ (in $g$)? (The numerical value of cryoscopic constant of solvent is $1.71 \ K \ kg \ mol^{-1}$)

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A
$0.5$
B
$1.5$
C
$0.687$
D
$2.0$

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Depression of freezing point of the solvent

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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.

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At the freezing point of a solution containing a nonvolatile solute,which of the following are in equilibrium?

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The molal depression constant for water is $1.86\,^{\circ}C/m$. If $342\,g$ of sugar $(C_{12}H_{22}O_{11})$ is dissolved in $1000\,g$ of water,the freezing point of the solution will be ............. $^{\circ}C$.

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What is the mass of solute having molar mass $60 \ g \ mol^{-1}$ when dissolved in $98 \ g$ of solvent decreases its freezing point by $0.2 \ K$ (in $g$)? (The numerical value of cryoscopic constant of solvent is $1.71 \ K \ kg \ mol^{-1}$)

Similar Questions

The mass of urea required to be dissolved in $500 \ mL$ of water to produce a depression in freezing point of $0.186 \ ^oC$ is ........ $g$. $(K_f = 1.86 \ ^oC/m)$

$0.05 \ mol$ of a non-volatile solute is dissolved in $500 \ g$ of water. What is the depression in freezing point of the resultant solution (in $K$)? $(K_f(H_2O) = 1.86 \ K \ kg \ mol^{-1})$

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.

At the freezing point of a solution containing a nonvolatile solute,which of the following are in equilibrium?

The molal depression constant for water is $1.86\,^{\circ}C/m$. If $342\,g$ of sugar $(C_{12}H_{22}O_{11})$ is dissolved in $1000\,g$ of water,the freezing point of the solution will be ............. $^{\circ}C$.

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