A `0.2` molal aqueous solution of a weak acid `(HX)` is `20` percent ionised. The freezing point of this solution is (Given `K_(f)=1.86.^(@)CKgmol^-1` for water):
A
`-0.45^(@)C`
B
`-0.90^(@)C`
C
`-0.31^(@)C`
D
`-0.53^(@)C`
Text Solution
Verified by Experts
The correct Answer is:
A
`DeltaT_(f)=0.2xx1.2xx1.86=0.45` therefore freezing point `=-0.45^(@)C`
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