# Does freezing a solution with water always cause the water to separate and form the ice lattice?

I'm curious, I was trying to look into the affect of freezing a solution with water even when the solution is completely miscible. I came across something that detailed this regarding salt water and basically said when it gets low enough to freeze, the water forms it's tell-tale lattice basically pushing the salts out so the ice itself is pure water and less dense (considerably less dense because the salt solution allowed the density to increase all the way to the lowered freezing point).

I am curious, is this a general fact of the behaviour of any solution with water regardless of miscibility? Are there water solutions which break up the lattice while still allowing freezing, or does the affect of blocking the formation of that lattice completely block the solution from freezing altogether no matter what? Are there water solutions which will freeze solid even with the lattice without just separating the non-water compounds?

Note: I recognize amorphous ice can be created with wizardry, but my question is more in regards to the typical behaviour on earth.

• related: "impurities in ice" – Dale Aug 20 '13 at 22:34
• It's worth noting that from a non-chemical perspective, if you freeze the water fast enough (with, e.g. liquid nitrogen), the impurities just get included in the glassy amorphous ice no matter what they are. – Aesin Aug 21 '13 at 23:51
• @Aesin right, I've heard if water is frozen quickly enough it can freeze before the hydrogen bonds can form so the lattice isn't created – Jimmy Hoffa Aug 22 '13 at 1:25
• @JimmyHoffa that is what the amorphous ice is, according to the wikipedia article :-) Also interestingly, although most ice on earth is in the lattice form, apparently in space most of it is amorphous. So likely the most common form of solid H2O is actually not the one we have in abundance – Brian Aug 22 '13 at 10:22

The purification that occurs when an aqueous solution freezes is called Fractional Freezing and is based on the idea that impurities of a solvent (and this can be any solvent, not just water) have a much lower solubility in the solid phase of the solvent relative to the liquid phase. Several techniques for performing fractional freezing for purification purposes can be found here. As the solid is formed, the impurities are expelled into the liquid that hasn't yet solidified. The purified crystals can then be removed by physical methods (e.g. filtration). In the case of water, where ice is less dense than the liquid phase, the purified crystals float to the top of the impurity-laden liquid. This is probably the reason why some people have observed a layer of impurities deep within a block of ice. As mentioned above, the process is not limited to just water, and freeze crystallization is use to eliminate the purities of silicon wafers and has been known for many years as a way to make hard liquor. This latter use of fractional freezing is close to the OPs question, which inquires about miscible substances (in this case, ethanol and water). Despite their miscibility, ethanol and water can be separated by fractional freezing, just like they can be separated by fractional distillation. Certain substances cannot be separated completely using distillation, and these substances are called azeotropes. Water and ethanol make an azeotropic mixture that is approximately 95% water. (So the moonshine you were thinking of making using the reference above will be limited to 190 proof.) What I find interesting is the following figure,

which shows the freezing point of water/ethanol mixtures as a function of ethanol content. At a point around 95% there is a significant dip in the freezing point. At this point, called the eutectic point, the solution behaves as if it is a single component (much like an azeotrope) and will not likely be separable through 'simple' fractional freezing means. Note I use the term simple because azeotropes can be separated using special distillation techniques.

So in summary: fractional freezing will work with any aqueous solution, regardless of the miscibility of the components, unless the component ratio is close the eutectic point. We don't need to limit ourselves to aqueous solutions, as many species can be purified in this manner. The purification mechanism is not so much a factor of the crystal lattice, but the relative solute solubilities in the solid and liquid phases of the solvent. Finally, many water solutions will freeze solid even with impurities. This and other types of separations work on equilibrium processes, and multiple iterations are necessary to "completely" remove impurities. (or more correct, remove the impurities to a level that is acceptable for your application.)

• Thanks for the information, though perhaps it wasn't clear in my question, I wasn't curious about purification, my curiosity was entirely regarding freezing water without causing the lattice which I understand (maybe inaccurately?) to be the reason it becomes less dense when frozen; that is I am curious if you can freeze water in such a way as to not cause it to become less dense by way of a solution as opposed to by way of rapid-freezing. – Jimmy Hoffa Aug 27 '13 at 14:55
• @JimmyHoffa If that is the case, then we need to watch the terminology used. When you use solution in your title and miscible in your question, that suggests water with multiple components. In my answer, I'm calling all solutes "impurities" that get removed upon freezing due to the process described. One does not need to invoke the lattice of solid water to explain this phenomenon. – bobthechemist Aug 28 '13 at 0:20
• @JimmyHoffa As for freezing water in such a way to make it less dense, this can't be done without additional pressure. See the links in this reference, one of which has some useful figures. – bobthechemist Aug 28 '13 at 0:23
• Thanks! That's exactly what I had figured and just wanted verification! I am way out of my depth on this topic as a whole, so my apologies for the confusion. My chemistry knowledge starts and ends with the the fact that there is a periodic table heh. Didn't know I was asking about a eutectic system, but sounds like even with a eutectic system the solid is analogous to the solid forms of the system's members alone. – Jimmy Hoffa Aug 28 '13 at 0:55

The situation you are describing is known as a eutectic system. Whether a system is at the eutectic point depends upon both the materials composing the solution as well as the relative amounts of each. A solution of A and B that are not at eutectic compositions will freeze out one component until a eutectic composition is achieved. While a eutectic system will simultaneously solidify both components, many systems will freeze solid A and solid B (the two being interdeispersed) and not solid AB, though some systems do solidify as mixed (metal alloys, for example).

Water and sodium chloride form a eutectic at about 23% NaCl by weight. You can see a phse diagram for water and NaCl at this University of Calgary page. Note than a eutectic can consist of more than two components, as mentioned by the University of Calgary page.

• If you have a eutectic system and you freeze it, does it become consistently dispered solid A and solid B as opposed to arbitrarily dispersed; and the lattice with water will still be formed? My curiosity is regarding the lattice specifically and the ability to freeze a solution with water that freezes consistently and without the lattice. Does a eutectic freeze solid AB with an altogether different solid form than the typical solid form than the independent components? – Jimmy Hoffa Aug 26 '13 at 18:57
• Ah that link appears to explain it with the phase diagram, sufficient amount of NaCl and when frozen its no longer frozen H2O, but frozen 2H2O + NaCl which may logically have a different solid form than frozen H2O. Is this a correct understanding? – Jimmy Hoffa Aug 26 '13 at 19:07
• @JimmyHoffa Some eutectic systems freeze as solid solutions, though I'm not aware of any off the top of my head that involve water. If I come across any, I'll be sure to post it and let you know. The dot formula of NaCl and water refers the the hydrate. Read more about it here: en.wikipedia.org/wiki/Hydrate – buckminst Aug 30 '13 at 3:59
• So the dot formula of NaCl and water are a 'hydrate' which may have a different solid structure than the solid of water, correct? Or is it only refered to as a 'hydrate' terminologically, though the actual thing being referred to is still water structurally? – Jimmy Hoffa Aug 30 '13 at 17:48