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Ethylene glycol (molar mass = 62 g mol ^...

Ethylene glycol (molar mass = 62 `g mol ^(-1))` is a common automobile antifreeze. Calculate the freezing point of a solution containing `12.4` of this substance in 100 g of water. Would it be advisable to keep this substance in the car radiator during summer? (`K_(f)` for water= `1.86 k kg//mol) (K_(b)` for water `= 0.512 K kg//mol.)`

Text Solution

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`Delta T_(b) = K _(b) xx (W_(B))/(M _(B)) xx ( 1000 )/( W _(A)) = 0.512 xx (12.4)/(62) xx (100)/(100) = 1. 024 K`
Since water boils at `100^(@)C,` so a solution containing ethylene glycol will boil at `101.024 ^(@)C,` so it is advisable to keep this substance in car radiator during summer.
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