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 °C. Find the molal depression constant of the solvent.

• 0.01

• 0.001

• 0.0001

• 0.1

Which of the following dissolves in ionic solvents?

• C₆H₆

• CH₃OH

• CCl₄

• C₅H₁₂

If M, W and V represent molar mass of solute, then mass of solute and volume of solution in litres respectively, which among following equations is true?

• $\mathrm{\pi } = \frac{\mathrm{MWR}}{\mathrm{TV}}$

• $\mathrm{\pi } = \frac{\mathrm{TMR}}{\mathrm{WV}}$

• $\mathrm{\pi } = \frac{\mathrm{TWR}}{\mathrm{VM}}$

• $\mathrm{\pi } = \frac{\mathrm{TRV}}{\mathrm{WM}}$

Which of the following compounds has highest boiling point?

• Propan-1-ol

• n-butane

• Chloroethane

• Propanal

van't Hoff factor of centimolal solution of K₃[Fe(CN)₆] is 3.333. Calculate the per cent dissociation of K₃[Fe(CN)₆].

• 33.33

• 0.78

• 78

• 23.33

The osmotic pressure of solution containing 34.2 g of cane sugar (molar mass = 342 g mol^-1) in 1 L of solution at 20°C is (Given R = 0.082 L atm K^-1 mol^-1)

• 2.40 atm

• 3.6 atm

• 24 atm

• 0.0024 atm

Solubility product (K_sp) of saturated PbCl₂ in water is 1.8 × 10^-4 mol³ dm^-9. What is the concentration of Pb²⁺ in the solution?

• (0.45 × 10^-4)^1/3 mol dm^-3

• (1.8 × 10^-4)^1/3 mol dm^-3

• (0.9 × 10^-4)^1/3 mol dm^-3

• (2.0 × 10^-4)^1/3 mol dm^-3

348.

The freezing point of equimolal solution will be highest for

• C₆H₅NH₃Cl

• D- fructose

• AgNO₃

• Ca(NO₃)₂

One mole of an unknown compound was treated with excess water and resulted in the evolution of two moles of a readily combustible gas. The resulting solution was treated with CO₂ and resulted in the formation of white turbidity. The unknown compound is

• Ca

• CaH₂

• Ca(OH)₂

• Ca(NO₃)₂

If the boiling point difference between that two liquids is not much, the ............ method is used to separate them

• Simple distillation

• Distillation under reduced pressure

• Steam distillation

• Differential extraction