For an aqueous solution, freezing point is -0.186^oC. Elevation of the boiling point of the same solution is:
(Given: K_f =1.86 K kg mol^-1  and K_b = 0.512 K kg mol^-1) 

1. 0.186

2. 0.0512

3. 1.86

4. 5.12

The depression in freezing point of 0.01 M aqueous solutions of urea, sodium chloride and sodium sulphate is in the ratio of:

1. 1 : 1 : 1

2. 1 : 2 : 3

3. 1 : 2 : 4

4. 2 : 2 : 3

What is the molality of the solution of a certain solute in a solvent if there is a freezing point depression of 0.184° and if the freezing point constant is 18.4 K kg mol⁻¹

1. 0.01

2. 1.00

3. 0.001

4. 100

1.00 g of a non-electrolyte solute (molar mass 250g mol) was dissolved in 51.2 g of benzene. If the freezing point depression constant, K_f of benzene is 5.12 K kg mol^-1, the freezing point of benzene will be lowered by:

If the molality of the dilute solution is doubled, then the value of a molal depression constant (K_f) will be:

1. Halved

2. Tripled

3. Unchanged

4. Doubled

A solution of sucrose (molar mass = 342 g mol^–1) has been prepared by dissolving 68.5 g of sucrose in 1000 g of water. The freezing point of the solution obtained will be: 
(k_f for water = 1.86 K kg mol^–1)
1. –0.372 ^oC
2. –0.520 ^oC
3. +0.372 ^oC
4. –0.570 ^oC

The molar freezing point constant for water is 1.86°C/mole. If 342 g of cane sugar $\left({\mathrm{C}}_{12}{\mathrm{H}}_{22}{\mathrm{O}}_{11}\right)$ is dissolved in 1000 g of water, the solution will freeze at 

1. –1.86°C

2. 1.86°C

3. –3.92°C

4. 2.42°C