An antifreeze solution is prepared from `222.6 g` of ethylene glycol `[C_(2)H_(4)(OH)_(2)]` and `200 g` of water. Calculate the molality of the solution. If the density of the solution is `1.072g mL^(-1)` then what shall be the molarity of the solution?

Explanation

`"Mass of the solute, "C_(2)H_(4)(OH)_(4)="22.6 g, Molar mass of "C_(2)H_(4)(OH)_(2)="62 g mol"^(-1)`
`therefore" Moles of the solute"=("222.6 g")/("62 g mol"^(-1))="3.59 , Mass of the solvent = 200 g = 0.200 kg"`
`"Molality "=("3.59 moles")/("0.200 kg")="17.95 mol kg"^(-1)`
`"Total mass of the solution = 422.6 g"`
`"Volume of the soltuion "=("422.6 g")/("1.072 g ml"^(-1))="394.2 ml = 0.3942 L , Molarity "=("3.59 moles")/("0.3942 L")="9.11 mol L"^(-1)`.