500 g of water containing 27 g of a non-volatile solute will boil at 100.156°C .Calculate the molar mass of the solute. Given boiling point of water = 100°C, Kb = 0.52 K kg mol 1.
Answers
Answered by
1
Answer:
Elevation of Boiling-point describes that the boiling point of a liquid (a solvent) will be higher when another compound is added, meaning that a solution has a higher boiling point than a pure solvent. This happens whenever a non-volatile solute, such as a salt, is added to a pure solvent, such as water.
Elevation of boiling point ( ΔTb ) is the difference between the boiling points of the solution and the pure solvent:
ΔTb=Tb−Tb0
Elevation of boiling point can be calculated as ΔTb=m.Kb
where m is the concentration of the solute expressed in molality and Kb is the molal boiling point elevation constant of the solvent.
m=m1M2m2
m2= mass of solute
m1= mass of solvent
M2= molecular wt. of solute.
From ΔTb=m.Kb
We get,
M2=ΔTbKb.m1m2
Similar questions