After adding a solute freezing point of solution decreases to `-0.186 ^@C `. Calculate `DeltaT_b ` if `K_f = 1.86 ^@C`/ molal and `K_b = 0.52^@C`/ molal.

After adding non-volatile solute, freezing point of water decreases to -0.186^(@)C . Calculate Delta T_(b) if : K_(f) = 1.86 "K kg mol"^(-1) and K_(b) = 0.521 "K kg mol"^(-1)

For an aqueous solution freezing point is -0.186^(@)C . The boiling point of the same solution is (K_(f) = 1.86^(@)mol^(-1)kg) and (K_(b) = 0.512 mol^(-1) kg)

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)=1.86K//m]

0.15 molal solution of NaCI has freezing point -0.52 ^(@)C Calculate van't Hoff factor . (K_(f) = 1.86 K kg mol^(-1) )

An aqueous solution boils at 101^(@)C . What is the freezing point of the same solution? (Gives : K_(f) = 1.86^(@)C// m "and" K_(b) = 0.51^(@)C//m )