Question

What is the boiling point elevation?

Answer 1

Hint: The elevation in boiling point is a colligative property, which implies that it is dependent on the presence of broken down particles and their number, yet not their identity. It is an impact of the dilution of the dissolvable within the sight of a solute. We have to know that boiling points of solutions are more than that of pure solvent.

Complete step by step answer:
We can say that Boiling point elevation is a colligative property of matter, for example it is reliant upon the solute-to-solvent proportion yet not on the solute's identity. We can infer that the rise in the edge of boiling over of a solution relies upon the measure of solute added to it. When the concentration of solute in solution is greater, the boiling point elevation is greater.
We could say that boiling point elevation describes the expansion in the increase of boiling over of a dissolvable upon the expansion of a solute. We could say at the point when a non-volatile solute is added to a dissolvable, the solution contains a higher limit than that of the pure dissolvable. For example, the edge of boiling point of a solution of sodium chloride (salt) and water is more prominent than that of pure water.
We could write the equation of elevation in boiling point as,
$\Delta {T_b} = i \times {K_b} \times m$
Here, the Van’t Hoff factor is expressed as i.
Ebullioscopic constant is expressed as ${K_b}$.
Molality of the solute is expressed as m.
We can determine the boiling point of solution using the boiling point of pure solvent and elevation in boiling point. The sum of the boiling point of pure solvent and elevation in boiling point gives the boiling point of solution.

Note: The colligative properties of a solution rely upon the relative numbers of solute and solvent particles; they don't rely upon the nature of the particles. Colligative properties change with respect to the concentration of particles of solute. We have to know that other colligative properties lowering in vapor pressure, depression in freezing point and osmotic pressure.