`K_b` and `K_f` for water are respectively 0.52 and 1.80 kg `"mol"^(-1)` respectively. For an aqueous glycolic solution freezing point is `3.72^@ C`. What is the boiling point of the solution ?

Explanation

Depression of freezing point =`Delta t_f =3.72^@C`
`DeltaT_f = K_f xx m` ,
molality `m=DeltaT_f //K_f` =3.72/1.86 =2 mol `kg^(-1)`
Elevation of boiling point =`DeltaT_b=K_b xx m`
`=0.52xx2=1.04^@C`
Boiling point of the solution =100+1.04 =`101.04^@C`