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?

Options

A. `9.10,17.95`
B. `10.90,16.6`
C. `12.04,17.95`
D. `18.2,16.97`

Answer

A

Explanation

`"Molality"=("moles of solute (glycol)")/("kg of solvent")=(222.6)/(62)/0.200`
`=17.95" mol "kg^(-1)`
`"Total mass of solution"=222.6+200=422.6g`
`"Volume of solution"=("mass")/("density")=(422.6)/(1.072)mL=(0.4226)/(1.072)L`
`:."Molarity"=("moles of solute")/("litre")=(22.6//62)/(0.4226//11.072)=9.10M`