How would the freezing point depression of a `0.05`m `CaCl_(2)` solution compare with that of a NaCl solution ? It would be :

Why is the freezing point depresslon of 0.1 M NaCl solution nearly twice that of 0.1 M glocose solution ?

Explain, why freezing point depression of 0.1M NaCl is nearly twice that of 0.1M glucose solution.

Elevation in boiling point of 0.1 m CaCl_(2) , solution less / more than 0.1 m NaCl solution.

Why the freezing point depression (DeltaT_(f)) of 0.4 M NaCl solution is nearly twice than that of 0.4M glucose solution ? Among equimolal aqueous solutions of MgCl_(2),NaCl,FeCl_(2) and C_(12)H_(22)O_(11) , which has high osmotic pressure ? Why ?

Why is freezing point depression of 0.01 M sodium chloride solution nearly twice that of 0.01 M glucose solution ?

Answer the following questions : Why the freezing point depression ( DeltaT_(f) ) of 0.4M NaCl solution is nearly twice than that of 0.4M glucose solution ?

The depression in freezing point expected for 0.6 m Al_2(SO_4)_3 solution will be n times compared with 0.2 m Na_2SO_4 solution. The value of n is

The molecular weight of NaCl determined by studying freezing point depression of its 0.5% aqueous solution is 30. The apparent degree of dissociation of NaCl is: