The elevation in boiling point for one ...

The elevation in boiling point for one molal solution of a solute in a solvent is called

Boiling point constant

Molal elevation constant

Cryoscopic constant

Molecular elevation constant

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For [CrCl_(3).xNH_(3)] , elevation in boiling point of one molal solution is double of one molal solution of glucose , hence x is if complex is 100% ionised :

Elevation in the boiling point for 1 molal solution of glucose is 2K. The depression in the freezing point for 2 molal solution of glucose in the same solvent is 2K. The relation between K_(b) and K_(f) is

For [CrCl_(3).xNH_(3)] elevation in boiling point of one molal solution is double of one molal urea solution, hence x is (Given that the complex is 100% ionised)

If 1 g of solute (molar mass = 50 g mol^(-1) ) is dissolved in 50 g of solvent and the elevation in boiling point is 1 K. The molar boiling constant of the solvent is

For [CrCl_(3).xNH_(3)] , elevation in boiling point of the one molal solution is triple of one molal aqueous solution of urea. Assuming 100% ionisation of complex molecule, calculate the value of x.

Calculate elevation in boiling point for 2 molal aqueous solution of glucose. (Given K_b(H_(2)O) = 0.5 kg mol^(-1) )

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:

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. Elevation in b.p of an aqueous urea solution is 0.52^(@) (K_(b) = 0.52^(@) mol^(-1)kg) . Hence, mole fraction of urea in this solution is:

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