Depression in Freezing Point of the Solvent

The freezing point depression constant $\left({\mathrm{K}}_{\mathrm{f}}\right)$ of benzene is $5.12\mathrm{Kkg}{ \mathrm{mol}}^{-1}$. Assuming $100\%$ dimerization of acetic acid in benzene, the freezing point depression of $0.2\mathrm{m}$ solution of acetic acid is

If sodium sulphate is considered to be completely dissociated into cations and anions in an aqueous solution, the change in the freezing point of water, when $0.01 \mathrm{mol}$ of sodium sulphate is dissolved in $1 \mathrm{Kg}$ of water, is $\left({\mathrm{K}}_{\mathrm{f}}=1.86 \mathrm{K} \mathrm{Kg} {\mathrm{mol}}^{-1}\right)$

Ethylene glycol is used as an antifreeze in cold climates. Mass of ethylene glycol which should be added to $4 \mathrm{Kg}$ of water to prevent it from freezing at $-6° \mathrm{C}$ will be: [${\mathrm{K}}_{\mathrm{f}}$ for water $=1.86 \mathrm{K} \mathrm{Kg} {\mathrm{mol}}^{-1}$, and molar mass of ethylene glycol $=62 \mathrm{g} {\mathrm{mol}}^{-1}$]

Camphor is often used in molecular mass determination because 

The molal freezing constant of water is $1.86° \mathrm{C}/\mathrm{M}$. Therefore, the freezing point of $0.1 \mathrm{m}$$\mathrm{NaCl}$ solution in water expected to be

Calculate the amount of ice separated out from this solution if the solution of $18 \mathrm{g}$ of glucose in $1000 \mathrm{g}$ of water is cooled to $-0.2°\mathrm{C}$.

The freezing point of equimolal aqueous solutions will be highest for

Assertion: Camphor is usually used in molecular mass determination.

Reason: Camphor has low cryoscopic constant and therefore, causes greater depression in freezing point.

Assertion: Sodium chloride is used to clear snow on the roads.

Reason :Sodium chloride depresses the freezing point of water.

${\mathrm{PtCl}}_4\mathbf{·}6{\mathrm{H}}_2\mathrm{O}$ can exist as a hydrated complex. $1 \mathrm{molal}$ aqueous solution has a depression in freezing point of $3.72°\mathrm{C}$. Assume, $100\%$ ionization and ${\mathrm{K}}_{\mathrm{f}} \left({\mathrm{H}}_2\mathrm{O}\right)=1.86 \mathrm{K} {\mathrm{mol}}^{-1} \mathrm{kg}$. Then the complex is

Which of the following statements is false?

The freezing point of an equimolal aqueous solution will be the highest for

The depression in freezing point of $0.01 \mathrm{m}$ aqueous solution of urea, sodium chloride and sodium sulphate is in the ratio :

Which is the correct relationship between molal depression constant and enthalpy of fusion ?

$1.00 \mathrm{g}$ of a non-electrolyte solute dissolved in $50 \mathrm{g}$ of benzene lowered the freezing point of benzene by $0.40 \mathrm{K}$. The freezing point depression constant of benzene is $5.12 \mathrm{K}$ $\mathrm{kg} {\mathrm{mol}}^{-1}$. Find the molar mass of the solute.

Which of the following will have maximum depression in freezing point?