Answer:
1) The value of the
is 0.07742°C/m.
2) 0.261°C is the freezing-point depression of a solution.
Explanation:
1) 


where,
=Elevation in boiling point
= boiling point constant of solvent= 3.63 °C/m
1 - van't Hoff factor (non-electrolyte solute)
m = molality
We have : 
m = 3.1 m




The value of the
is 0.07742°C/m.
2) 


where,
=depression in freezing point
= freezing point constant of solvent= 1.86°C/m
1 - van't Hoff factor (non-electrolyte solute)
m = molality
We have , Moles of solute = 0.705 mol
Mass of solvent = 5.02 kg

m = 



0.261°C is the freezing-point depression of a solution.