G A student enters the lab and determines the freezing point of pure liquid to be 47.2 ºC. A nonelectrolyte unknown substance is added to the liquid, and the freezing point of the solution is determined to be 45.8 ºC. If the freezing point depression constant for the solvent is 4.60 ºC/molal, what is the molality of the solution?

Answer : The molality of the solution is, 0.304 mol/kg

Explanation :  Given,

Molal-freezing-point-depression constant for solvent =

Freezing point of pure liquid =

Freezing point of solution =

Formula used :  

where,

= change in freezing point

= freezing point of solution =

= freezing point of pure liquid =

i = Van't Hoff factor = 1 (for non-electrolyte)

= freezing point constant for solvent =

m = molality

Now put all the given values in this formula, we get

Therefore, the molality of the solution is, 0.304 mol/kg

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