CBSE
Multiple Choice QuestionsThe freezing point depression of 0.001 m Kx[Fe(CN)6] is 7.1x 10-3 K. The value of x will be [Given, Kf = 1.86 KKg mol-1 for water].
2
4
3
1
The average molar heat capacity at constant volume of gaseous mixture contained 2 moles of each of two ideal gases X (CV , m = R) and Y (CV , m = R)
2R
3R
4R
8R
The Ka of an acid is 3.2 x 10-5. The degree of dissociation of the acid at concentration of 0.2 M is
6.0 x 10-2
1.26 x 10-2
4.0 x 10-2
0.04 x 10-3
What would be the freezing point of aqueous solution containing 17g of C2H5OH in 1000 g of water?
0.34°C
0.0°C
-0.34°C
-0.69°C
The pH of a solution is 5.0. If H+ ion concentration is decreased 100 times. Then the solution will be :
neutral
more acidic
basic
of the same acidity
At a temperature, vapour pressure of pure benzene is 640 mm Hg. On dissolving 2.175 g of a non-volatile solid solute in 39.0 g benzene, vapour pressure of the solution if found to be 600 mm Hg. The molecular mass of solute is:
65.25
54.94
63.55
87.62
If the solubility of an aqueous solution of Mg(OH)2 , be X mole litre then ksp of Mg(OH)2 is:
4X3
108X5
27X4
9X
Addition of a non-volatile solute causes lowering in vapour pressure of a solvent from 0.8 atm to 0.2 atm. What is the
mole fraction of solvent?
0.25
0.75
0.50
Cannot be predicted
A storage battery contains a solution of H2SO4 38% by weight. At this concentration, the van't Hoff factor is 2.50. At what temperature will the battery contents freeze? (Kf =1.80 mol' kg)
243.92 K
298 K
240.92 K
273 K
50 cm3 ethylene glycol is dissolved in 50 g water. Freezing point of solution is -34°C. Assuming ideal behaviour than density of ethylene glycol is (for water , Kf =1.86 K kg mol-1)
1.273 g/cm3
2.173 g/cm3
1.133 g /cm3
2.612 g/cm3
