I do not understand why for mixtures freezing point is lower than melting point. Are not the two representing the same equilibrium between solid and liquid which we are approaching from two different sides, so why should the temperature at which this happens be different for the two cases?

  • 1
    $\begingroup$ related chemistry.stackexchange.com/questions/42300/… $\endgroup$
    – Mithoron
    Jun 7, 2016 at 19:53
  • 2
    $\begingroup$ No, they are not. They represent two different situations with different compositions of solid and liquid phases (this could be understood in two ways, and both are correct: the composition is different between solid and liquid, and also different between situations). So no, it is not the same equilibrium. $\endgroup$ Jun 7, 2016 at 20:02
  • $\begingroup$ @Ivan Neretin will you please explain in detail why these do not represent the same equilibrium.Thanks in advance. $\endgroup$
    – user30853
    Jun 8, 2016 at 19:05

1 Answer 1


The Bodner research group at Purdue University has posted this excellent description of the difference between melting point and freezing point:

Pure, crystalline solids have a characteristic melting point, the temperature at which the solid melts to become a liquid. The transition between the solid and the liquid is so sharp for small samples of a pure substance that melting points can be measured to $\pu{0.1^\circ C}$. The melting point of solid oxygen, for example, is $\pu{-218.4^\circ C}$.

Liquids have a characteristic temperature at which they turn into solids, known as their freezing point. In theory, the melting point of a solid should be the same as the freezing point of the liquid. In practice, small differences between these quantities can be observed.

It is difficult, if not impossible, to heat a solid above its melting point because the heat that enters the solid at its melting point is used to convert the solid into a liquid. It is possible, however, to cool some liquids to temperatures below their freezing points without forming a solid. When this is done, the liquid is said to be supercooled.

An example of a supercooled liquid can be made by heating solid sodium acetate trihydrate ($\ce{NaCH3CO2 . 3H2O}$). When this solid melts, the sodium acetate dissolves in the water that was trapped in the crystal to form a solution. When the solution cools to room temperature, it should solidify. But it often doesn't. If a small crystal of sodium acetate trihydrate is added to the liquid, however, the contents of the flask solidify within seconds.

A liquid can become supercooled because the particles in a solid are packed in a regular structure that is characteristic of that particular substance. Some of these solids form very easily; others do not. Some need a particle of dust, or a seed crystal, to act as a site on which the crystal can grow. In order to form crystals of sodium acetate trihydrate, $\ce{Na+}$ ions, $\ce{CH3CO2-}$ ions, and water molecules must come together in the proper orientation. It is difficult for these particles to organize themselves, but a seed crystal can provide the framework on which the proper arrangement of ions and water molecules can grow.

Because it is difficult to heat solids to temperatures above their melting points, and because pure solids tend to melt over a very small temperature range, melting points are often used to help identify compounds. We can distinguish between the three sugars known as glucose ($\vartheta_\mathrm m = \pu{150^\circ C}$), fructose ($\vartheta_\mathrm m = 103{-}\pu{105^\circ C}$), and sucrose ($\vartheta_\mathrm m = 185{-}\pu{186^\circ C}$), for example, by determining the melting point of a small sample.

Measurements of the melting point of a solid can also provide information about the purity of the substance. Pure, crystalline solids melt over a very narrow range of temperatures, whereas mixtures melt over a broad temperature range. Mixtures also tend to melt at temperatures below the melting points of the pure solids.

  • 1
    $\begingroup$ In my opinion (but not in Martin’s, for example) this is a plagiarising answer because all it does is copy from a source and state that source. $\endgroup$
    – Jan
    Nov 4, 2017 at 12:07
  • $\begingroup$ plagiarism is passing someone else's work off as your own. if you cite the source, it's not plagiarism $\endgroup$
    – pentane
    Jan 28, 2018 at 0:13

Your Answer

By clicking “Post Your Answer”, you agree to our terms of service and acknowledge you have read our privacy policy.

Not the answer you're looking for? Browse other questions tagged or ask your own question.