Depression in Freezing Point of the Solvent

The freezing point of equimolal aqueous solutions will be highest for

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

Reason :Sodium chloride depresses the freezing point of water.

Calculate the molal depression constant of a solution, which freezes at $15°\mathrm{C}$. The latent heat of fusion is $180.7{\mathrm{Jg}}^{-1}$

$2 \mathrm{g}$ of a non-electrolyte solute (molar mass is $500 \mathrm{g}{ \mathrm{mol}}^{-1}$ ) was dissolved in$57.3 \mathrm{g}$ of xylene. If the freezing point depression constant ${\mathrm{K}}_{\mathrm{f}}$ of Xylene is $4.3 \mathrm{K} \mathrm{kg}{ \mathrm{mol}}^{-1}$. Then the depression in freezing point of Xylene is

Which of the following statements is false?

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?

It is seen that sprinkling of salt helps in clearing the snow covered roads in hills. What is the phenomenon involved in the process?

Same amount of the following complexes $\mathrm{I},\mathrm{ }\mathrm{II},\mathrm{ }\mathrm{III}$ is used to prepare three different solutions by dissolving in water. The correct order of freezing points will be :

$\mathrm{I}.\mathrm{ }\left[\mathrm{Co}{\left({\mathrm{NH}}_3\right)}_3{\left({\mathrm{NO}}_2\right)}_3\right]$

$\mathrm{II}.\left[\mathrm{Co}{\left({\mathrm{NH}}_3\right)}_5\left({\mathrm{NO}}_2\right)\right]{\left[\mathrm{Co}{\left({\mathrm{NH}}_3\right)}_2{\left({\mathrm{NO}}_2\right)}_4\right]}_2$

$\mathrm{III}.\mathrm{ }\left[\mathrm{Co}{\left({\mathrm{NH}}_3\right)}_4{\left({\mathrm{NO}}_2\right)}_2\right]\left[\mathrm{Co}{\left({\mathrm{NH}}_3\right)}_2{\left({\mathrm{NO}}_2\right)}_4\right]$

[Given: ${\mathrm{K}}_{\mathrm{f}}\left({\mathrm{H}}_2\mathrm{O}\right)=1{.86}^{\mathrm{o}}\mathrm{C}/\mathrm{m}$ ]

Find out the amount of water (in g) separated as ice, if a solution containing $62 \mathrm{g}$ ethylene glycol in $250 \mathrm{g}$ water is cooled to $-{10}^{° }\mathrm{C}$ . ${\mathrm{K}}_{\mathrm{f}}$ for water is $1.86 \mathrm{K}\mathrm{ }\mathrm{kg}\mathrm{ }{\mathrm{mol}}^{-1}$ .

Among the following, which solution has lowest freezing point?

Which solvent results in maximum depression in freezing point of the solution?

What is the freezing point of aqueous solution containing 20% w/w urea and 20% w/w NaOH?
Given:- ${\mathrm{K}}_{\mathrm{f}}$ of ${\mathrm{H}}_2\mathrm{O}\mathrm{ }$is $1.8 \mathrm{K}\mathrm{ }\mathrm{k}\mathrm{g}\mathrm{ }\mathrm{m}\mathrm{o}{\mathrm{l}}^{-1}$

What is the weight of glucose, if glucose is added to 1 litre water to such an extent that $\frac{\mathrm{\Delta }{\mathrm{T}}_{\mathrm{f}}}{{\mathrm{K}}_{\mathrm{f}}}$ becomes equal to 1/1000?