(D) The formula for freezing point depression is $\Delta T_f = K_f \times m$,where $m$ is the molality of the solution.Molality $m = \frac{\text{moles

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(D) The formula for freezing point depression is $\Delta T_f = K_f \times m$,where $m$ is the molality of the solution.Molality $m = \frac{\text{moles of solute}}{\text{mass of solvent in kg}} = \frac{0.8 \ g / 64 \ g \ mol^{-1}}{43 \ g / 1000} = \frac{0.0125 \ mol}{0.043 \ kg} \approx 0.2907 \ mol \ kg^{-1}$.Given $\Delta T_f = 0.34 \ K$,we have $0.34 = K_f \times 0.2907$.$K_f = \frac{0.34}{0.2907} \approx 1.169 \ K \ kg \ mol^{-1}$.Rounding to two decimal places,$K_f \approx 1.17 \ K \ kg \ mol^{-1}$.

Class 12 Chemistry Solutions Depression of freezing point of the solvent

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Calculate the cryoscopic constant $(K_f)$ when $0.8 \ g$ of a non-volatile solute with a molar mass of $64 \ g \ mol^{-1}$ is dissolved in $43 \ g$ of a solvent,lowering the freezing point by $0.34 \ K$.

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A
$2.5 \ K \ kg \ mol^{-1}$
B
$2.0 \ K \ kg \ mol^{-1}$
C
$0.85 \ K \ kg \ mol^{-1}$
D
$1.17 \ K \ kg \ mol^{-1}$

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Depression of freezing point of the solvent

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If a $0.4 \text{ molal}$ solution of a nonvolatile solute in an organic solvent decreases its freezing point by $2.4 \text{ K}$, then the molal depression constant $(K_f)$ of the solvent will be:

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Calculate the cryoscopic constant $(K_f)$ of a solvent if the depression in freezing point of a $0.3 \text{ m}$ solution of a nonelectrolyte is $0.48 \text{ K}$.

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The freezing point of $1 \%$ solution of lead nitrate in water will be

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When $36 \ g$ of a non-volatile,non-electrolytic solute having the empirical formula $CH_2O$ is dissolved in $1.2 \ kg$ of water,the solution freezes at $-0.93 \ ^\circ C$. The molecular formula of the solute is ($K_f$ of water $= 1.86 \ K \ kg \ mol^{-1}$)

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What is the molar mass of a solute when $5 \ g$ of solute dissolved in $70 \ g$ of solvent lowers its freezing point by $2.5 \ K$? Given $K_f = 3.5 \ K \ kg \ mol^{-1}$.

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Calculate the cryoscopic constant $(K_f)$ when $0.8 \ g$ of a non-volatile solute with a molar mass of $64 \ g \ mol^{-1}$ is dissolved in $43 \ g$ of a solvent,lowering the freezing point by $0.34 \ K$.

Similar Questions

If a $0.4 \text{ molal}$ solution of a nonvolatile solute in an organic solvent decreases its freezing point by $2.4 \text{ K}$, then the molal depression constant $(K_f)$ of the solvent will be:

Calculate the cryoscopic constant $(K_f)$ of a solvent if the depression in freezing point of a $0.3 \text{ m}$ solution of a nonelectrolyte is $0.48 \text{ K}$.

The freezing point of $1 \%$ solution of lead nitrate in water will be

When $36 \ g$ of a non-volatile,non-electrolytic solute having the empirical formula $CH_2O$ is dissolved in $1.2 \ kg$ of water,the solution freezes at $-0.93 \ ^\circ C$. The molecular formula of the solute is ($K_f$ of water $= 1.86 \ K \ kg \ mol^{-1}$)

What is the molar mass of a solute when $5 \ g$ of solute dissolved in $70 \ g$ of solvent lowers its freezing point by $2.5 \ K$? Given $K_f = 3.5 \ K \ kg \ mol^{-1}$.

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