More simply put, what is the difference between freezing and precipitation when considering a mixture?

Take two scenarios:

First a mineral in water. If the temperature of this solution is lowered, the solubility of the mineral will decrease and eventually precipitate out of solution. This could be done in a cascade type setup so that each time, the solution is cooled further and the liquid phase becomes more and more concentrated in water.

Second, consider a mixture of ethanol and water. Here too, I could lower the temperature until crystals first form. They would be almost pure water, leaving behind a solution higher in concentration in alcohol. I could repeat this procedure until I reach the eutectic mixture.

In both cases, a drop in temperature is allowing a solid phase to form out of an aqueous solution, yet one is referred to as partial crystallization and the other is referred to as partial freezing. I am not sure I see the difference.

  • $\begingroup$ @Jan not correct. Many salts are more soluble at higher temperature. A solution just barely saturated at 90 °C will crystallise abundant solids when cooled down to 0 °C. Calcium chloride is one such salt. $\endgroup$
    – Gimelist
    Sep 20 '16 at 9:34
  • $\begingroup$ @Michael Oh, I see my error. I overlooked the in between mineral and water and thought the question were about mineral water. In mineral water, of course, the concentration of ions is much too low. But for a mineral dissolved in water that’s different. $\endgroup$
    – Jan
    Sep 20 '16 at 9:49
  • $\begingroup$ Surely the key difference is whether you are making crystals of the solvent or the thing dissolved in the solvent. Crystallisation relies on solutes having lower solubility at lower temperature (usually) and this work to purify the dissolved compound. If you want to purify the solvent (or concentrate the remaining components) you partially freeze it removing the purer crystals of solvent. $\endgroup$
    – matt_black
    Nov 19 '16 at 13:31

There is no difference. Strictly speaking, "freezing" does not necessarily include crystalline solids, and may include amorphous materials that precipitate out of solution. But, this does not really matter in the context of these eutectic (or similar) systems.

I suspect the latter is referred to as "partial freezing" because the solid is water, whereas it is more general in the former. We rarely speak of water crystallising to ice, but rather water freezing to ice. This is more of a linguistic issue than scientific.


Your Answer

By clicking “Post Your Answer”, you agree to our terms of service, privacy policy and cookie policy

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