How will you show that elevation in boiling point is a colligative property?

Explanation

Boiling point of a liquid is the temperature at which its vapour pressure becomes equal to the atmospheric pressure. As the vapour pressure of a solution containing a nonvolatile solute is lower than that of the pure solvent, it boiling point will be higher than that of the pure solvent as shown in figure. The increase in boiling point is known as elevation in boiling point, `Delta T_b`.

`Delta T_b=T_b-T_b^@` (where `Delta T_b` is elevation in boiling point and is difference between boiling point of solution `T_b` and boiling point of solvent at pure state `T_b^@`).
`Delta T_b = K_b m` (where, m=molality)
`K_b` is molal elevation constant or ebullioscopic constant. Molecular mass of solute can be calculated as
`Delta T_b=(K_b.W_B xx 1000)/(M_B xx W_A)`
`M_B=K_b.(W_B)/(W_A)xx(1000)/(Delta T_b)`
where, `W_B` and `W_A` = mass of solute and solvent respectively.
`K_b` has units of `K // m` or K kg `mol^(-1)`, for water.
where `K_b = 0.52 K kg mol^(-1)`.