Given that `DeltaT_(f)` is the depression in freezing point of the solvent in a solution of a non-volatile solute of molarity `m`,the quantity `underset(m rarr0)(Lt) (DeltaT_(f)//m)` is equal to ……………. .

Freezing point of a solvent containing a non volatile solute

Consider following figure and answer the questions at the end of it. Figure explains elevation in boiling point when a non-volatile solute is added to a solvent. Variation of vapour pressure with temperature and showing elevation in boiling point. Given that DeltaT_(b) is the elevation in boiling point of the solvent in a solution of molality m then underset(mto0)(Lt)((DeltaT_(b))/(m)) is equal to

Figure explains elevation in boiling point when a non-volatile solute is added to a solvent. Variation of vapour pressure with temperaure and elevation in boiling point is marked. Given that DeltaT_(b) is the elevation in boiling point of the solvent in a solution of molarity m then lim_(m rarr 0) ((Delta T_(b))/(m)) is equal to:

If all symbols have their usual meaning, then for a non-volatile non-electrolyte solute Lt_(m rarr 0) ((DeltaT_(f))/(m)) is equal to

Why is freezing point depressed when a non-volatile solute is added to a solvent ?

Explain depression in freezing point. How depression in freezing point can be used to find molar mass of a non-volatile solute

If DeltaT_(f) is the depression in freezing point for the electrolyte and DeltaT_(f)^(@) for the non-electrolyte of the same concentration, then Van't Hoff factor (i) is