Consider equimolal aqueous solutions of `NaHSO_(4)` and NaCl with `DeltaT_(b)` and `DeltaT'_(b)` as their respective boiling point elevation . The value of `underset(m to1)("lim") (DeltaT_(b))/(DeltaT'_(b))` will be :

Consider equimolal aqueous solutions of NaHSO_(4) and Nacl with Delta T_(b) and DeltaT_(b)^(1) as their respective boiling point elevations. The value of underset (xrarrinfty)(Lt) (DeltaT_(b))/(DeltaT_(b)) will be

Consider equimolal aqueous solutions of NaHSO_4 and NaCl with triangleT_b and triangle'T_b , as their respective boiling point elevations. The value of Lim_(mrarr0) (triangleT_b)/(triangle 'T_b) will be

How are DeltaT_(b) and DeltaT_(f) related to the molar mass of the solute?

How are DeltaT_(b) and DelatT_(f) related to the molar mass of the solute ?

Consider following figure and answer the questions at the end of it. Figure explains elevation in boiling point when a non-volatile solute is added to a solvent. Variation of vapour pressure with temperature and showing elevation in boiling point. Given that DeltaT_(b) is the elevation in boiling point of the solvent in a solution of molality m then underset(mto0)(Lt)((DeltaT_(b))/(m)) is equal to

Which will have largest DeltaT_(b) ?

How is DeltaT_f and DeltaT_b related to molecular mass of a solute?

Aluminium phosphate is 100\% ionised in 0.01 molal aqueous solution . Hence , DeltaT_(b) // K_(b) is :