Question

derive the relation between the elevation in the boiling point and the concentration of a solution​

Answer 1

Answer:

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Explanation:

The result is that in dilute ideal solutions, the extent of boiling-point elevation is directly proportional to the molal concentration (amount of substance per mass) of the solution according to the equation: ΔTb = Kb · b. where the boiling point elevation, is defined as Tb (solution) - Tb (pure solvent).

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Answer 2

ANSWER:

Elevation of Boiling Point: Elevation of boiling point on adding one mole solute to 1000 g solvent is called molal boiling point elevation constant. It is denoted by K

b

. Its unit is K kg mol

−1

, e.g. for water K

b

=0.52 K kg mol

−1

.

Derivation of relation: Increase in boiling point of the solvent, on adding non-volatile solute to the solvent is called elevation of boiling point.

ΔTb=T3−T2

where T2 = boiling point of solvent, and T3 = boiling point of solution.

Experimentally, it is observed that elevation in boiling point is directly proportional to molal concentration of solute dissolved in definite amount of the solvent.

ΔT b∝m

ΔT b=Kb×m .....(1)

Kb is proportionality constant called molal boiling point elevation constant. We know that molality of a solution is number of moles of solute in 1000g solvent. It is denoted by m.

Determination of Molecular mass of a non-volatile solute:

Say molecular mass of the solute is MM. W1g solute is present in W2 g solvent. Molality of solution is m=M1 W1× W2*1000 .........(2)

On putting value of m from equation (2) to (1),

ΔTb=M 1 ×W2

Kb ×W 1×1000

M 1= ΔT b ×W 2

K b ×W 1×1000

Molecular mass of the solute may be determined by this formula.

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