An aqueous solution 1L salt solution contains 100g of NaCI. Calcaulte the melting point and boiling point of the solution at 1 atm
No. of moles = Nacl
n= 100g / 58.44g/mol = 1.71116 moles
volume of solution = 1L
Molality of solution = n/volume = 1.71116 /1 = 1.71116m
(A) At pressure 1 atm the value of Kb (elevation constant) for water = 0.51o C/m
therefore elevation in boiling point ΔTb = m x kb
ΔTb = 1.71116 m x 0.51oC/m = 0.8726 oC
Boiling point of water = 100oC = T
final Boiling point = T + ΔTb = 100 + 0.8726 = 100.8726oC
(B) now at 1 atm pressure the freezing point depression constant Kf = 1.86oC/m
ΔTf = m x kf
ΔTf = 1.71116 m x 1.86oC/m = 3.18276oC
Freezing point of water = 0oC = Tf
Final freezing point of solution = Tf - ΔTf = 0- 3.18276oC = -3.18276oC
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