Mole fraction of a non-electrolyte in aqueous solution is `0.07`. If `K_(f)` is `1.86^(@) "mol"^(-1)kg`, depression if `f.p.,DeltaT_(f),` is:

Mole fraction of a non-electrolyte in aqueous solution is 0.07 . If K_(f)(H_(2)O) is 1.86^(@) mol^(-1) kg , depression in f.p ., DeltaT_(f) is :

Density of 1M solution of a non-electrolyte C_(6)H_(12)O_(6) is 1.18 g/mL . If K_(f) (H_(2)O) is 1.86^(@) mol^(-1) kg , solution freezes at :

Density of 1M solution of a non-electrolyte C_(6)H_(12)O_(6) is 1.18 g/mL . If K_(f) (H_(2)O) is 1.86^(@) mol^(-1) kg , solution freezes at :

The freezing point of a 0.05 molal solution of a non-electrolyte in water is: ( K_(f) = 1.86 "molality"^(-1) )

The freezing point of a 0.05 molal solution of a non-electrolyte in water is: ( K_(f) = 1.86 "molality"^(-1) )

The freezing point of 0.05 molal solution of non- electrolyte in water is _____. (K_(f) = 1.86 ^(@)Ckg mol ^(-1))

Elevation in b.p. of an aqueous urea solution is 0.52^(@), (K_(b)=0.622^(@) "mol"^(-1)kg) Hence, mole-fraction of urea in this solution is :

The freezing point of a 0.05 molal solution of a non-electrolyte in water is [K_(f)=1.86K//m]