The elevation in boiling point of a solution of a solution dTb is related with molality of solution (m) by the relation dTb=[(R Tb2/Δ Îv a p)][(M1/1 + m M1)], where M1 is molar mass of solvent and Δ Hv a p is heat of vaporization of solvent. For a dilute solution, the relation (( partial Tb/ partial m))m arrow 0 gives:

Question

The elevation in boiling point of a solution of a solution dTb is related with molality of solution (m) by the relation dTb=[(R Tb2/Δ Îv a p)][(M1/1 + m M1)], where M1 is molar mass of solvent and Δ Hv a p is heat of vaporization of solvent. For a dilute solution, the relation (( partial Tb/ partial m))m arrow 0 gives: (A) Molal ebullioscopic constant (B) Elevation in boiling point (C) Boiling point of solvent (D) Elevation in boiling point ( text(ΔT) textb text) becomes more predominant

Tardigrade Admin · Accepted Answer

(( partial Tb/ partial m))m arrow 0=(R Tb2 M1/Δ Îv a p)=Kb .

Molal ebullioscopic constant

Elevation in boiling point

Boiling point of solvent

Elevation in boiling point $((ΔT)_{b})$ becomes more predominant

$(\frac{\partial T _{b}}{\partial m})_{m \to 0} = \frac{R T _{b}^{2} M _{1}}{Δ H _{v a p}} = K_{b}$ .

Molal ebullioscopic constant

Elevation in boiling point

Boiling point of solvent

Elevation in boiling point ((ΔT)b​) becomes more predominant

(∂m∂Tb​​)m→0​=ΔHvap​RTb2​M1​​=Kb​ .

Elevation in boiling point $((ΔT)_{b})$ becomes more predominant

$(\frac{\partial T _{b}}{\partial m})_{m \to 0} = \frac{R T _{b}^{2} M _{1}}{Δ H _{v a p}} = K_{b}$ .