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 solute `=222*6`g
Molar mass of solute, `C_(2)H_(4)(OH)_(2)`
`=12xx2+4+2(12+1)=62g` `mol^(-1)`
`therefore"Moles of solute"=(222*6)/(62)=3*59`
Mass of solvent `=200g`
`thereforeMolality=(3*59)/(200)xx1000=17*95" mol "kg^(-1)`
Total mass of solution `=422*5g`
volume of solution `=(442*6)/(1*072)=394*21mL`.
`therefore"Molarity"=(3*59)/(394*2)xx1000=9*1" mol "L^(-1)`