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The freezing point of solution containin...

The freezing point of solution containing `0.2 g` of acetic acid in `20.0 g` of benzene is lowered by `0.45^(@)C`. Calculate the degree of association of acetic acid in benzene.
`(K_(f)=5.12 K^(@) mol^(-1) kg^(-1))`

Text Solution

Verified by Experts

Given, `w=0.2 g, W= 20 g, DeltaT=45^(@)C`
`because DeltaT=(1000xxk'_(f)xxw)/(mxxW)`
or `0.45=(1000xx5.12xx0.2)/(20xxm)`
`:. M ("observed")=113.78`
Now for `{:(,2CH_(3)hArr,(CH_(3)COOH)_(2),,),("Before association",1,0,,),("After association",1-alpha,a//2,,):}`
where `alpha` is degree of association.
`:. (m_("Normal"))/(m_("overserved"))=1-alpha+(alpha)/(2)`
or `(60)/(11.78)=1-alpha+(alpha)/(2)`
or `alpha= 0.945 or 94.5%`
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