Properties such as boiling point, freezing point and vapour pressure of a pure solvent change when solute molecules are added to get homogeneous solution. These are called colligative properties. Applications of colligative properties are very useful in day-today life. One of its examples is the use of ethylene glycol and water mixture as anti-freezing liquid in the radiator of automobiles. A solution M is prepared by mixing ethanol and water. The mole fraction of ethanol in the mixture is 0.1.
Boiling point elevation constant of water =0.52 K kg/mol Boiling point elevation constant of ethanol = 1.2 k kg/mol
Boiling point of water =373 K Boiling point of ethanol =351.5 K
The boiling point of this solution is?
Now, I am aware that for a solution of a non-volatile solute in a solvent The elevation in boiling point is given as
In this case,which is the solute and which the solvent?
The material that I am studying from considers ethanol to be the solute and water,the solvent.And thus,calculates the elevation in boiling point of water. Therefore,the new boiling point is higher than that of pure water
My problem with this is,since the boiling point of a mixture of ethanol and water,for all compositions,lies between that of water(maximum) and ethanol(minimum), how can a mixture of water and ethanol of 0.1 molarity (by ethanol) have a higher boiling point than that of water?