How is the molecular mass of a solute related to the depression in freezing point of the solution?

Define the terms: Depression in freezing point.

The depression in freezing point is directly proportional to

0.01 M solution each of ura, common salt and sodium sulphate are taken, the ratio of depression in freezing point of thes solutions is

In comparison to a 0.01 M solution of glucose, the depression in freezing point of a 0.01M MgCl_2 solution is :

How will you calculate the molecular mass of a solute with the help of relative lowering in vapour pressure of a solution of a non volatile solute?

How will you show that depression in freezing point is a colligative property?

MX_2 dissociates into M^(2+) and X^- ions in an aqueous soluton, with a degree of dissciation of 0.5. The ratio of the observed depressio of freezing point of the aqueous solution to the value of the depression of freezing point in the absence of ionic dissociation is