Which substance can be recovered easily from its solution by crystallisation?
413983
Copper sulphate as I recall.
849149
Sure.  Any element can be purified.\n\nNitrogen is fairly easy.  All you have to do is liquify air and let the oxygen and other gases boil off at higher temperatures.  Just reduce the liquid down to around 75 degrees Kelvin.  Water vapor, CO2, and Nitrogen oxides will form solids, which you can decant the liquid from.  Then raise the temperature to about 78 degrees and the nitrogen will boil off (at 77.K, -196C), leaving oxygen which boils at 13 degrees higher.  Collect the gas, nitrogen, that boils off.  If you need to make it even purer, repeat the separation process with the "pure" nitrogen.
654238
A solution cannot have a structure unless it is frozen solid. Starch will be present in the hemiacetal form in it.
32450
Yes.  You can form a supersaturated solution with salt and boiling hot water in a glass jar.  Tie a pencil to one end of a string and a paperclip to the other.  Allow the pencil to rest on the top of the jar so the paperclip can hang in the solution, almost touching the bottom of the jar.  Allow the jar to sit undisturbed and you'll see crystals forming within 24 hours.
592262
sodium chloride definately or cesium fluoride (not sure)-evaporation of water solution\n\npresume you mean cubic close packing
479476
You need to know concentrations to determine the amount of substance that precipitates out by using solubility products. In this case the precipitate will be CaSO4, so the solubility product will be given by:\n\nk=[Ca(+2)]*[SO4(-2)]\n\nWhere k is the equilibrium constant (probably a given), and [Ca(+2)] & [SO4(-2)] are the concentrations of Ca(+2) and SO4(-2) in the solution. Any amounts greater than the equilbrium concentration will precipitate out as a solid.
977174
Removal and recovery of magnesium, strontium and barium \n\nMagnesium is removed from brine by contacting the brine with calcium hydroxide at temperatures above about 80.degree. C. but below the boiling point of the brine. The contacting results in the formation of magnesium hydroxide precipitate which is substantially insoluble in the mother liquor at those temperatures and strontium hydroxide which is dissolved in the mother liquor. When the contacting is carried out at a temperature above about 90.degree. C., magnesium hydroxide precipitate is fast settling and filterable; accordingly, it is removed from the mother liquor by a conventional process, such as filtering. The mother liquor is then cooled to cause the precipitation of at least a substantial part of strontium hydroxide present in the mother liquor. The precipitate of strontium hydroxide is recovered by a conventional process such as filtering. If precipitation upon cooling is insufficient, carbon dioxide gas is introduced into the mother liquor to effect the precipitation of strontium hydroxide. Barium can be removed and recovered in the form of barium sulfate by reacting the remaining mother liquor with sodium sulfate. In order to produce a faster-settling precipitate of magnesium hydroxide, the brine is contacted with a sufficient amount of a solution or slurry of calcium hydroxide in water to bring the concentration of magnesium in the resulting liquid to the range from about 0.023 mols of magnesium per liter to about 0.04 mols of magnesium per liter.
1157628
It depends on the activation energy and the relative energy states of the products.\n\nIn the gas phase, the sodium chloride and water formed are at such  a more stable configuration (as evidenced by the fact that this reaction is highly exothermic), that it is effectively irreversible.\n\nIn solution, however, you will find sodium ions, chloride ions, and -- due to the natural behavior of water -- a small amount of hydronium ions and hydroxide ions.\n\nSo, in solution, the reaction becomes a tiny bit more reversible, but not nearly enough to regenerate significant amounts of your starting products.  The equilibrium is heavily weighted towards the products (sodium ions, chloride ions, and water) because of the energetics of the reaction.
260628
Recystalize in methanol or water. Check the Merck index for a recrystallization solvent.
395302
mixture is combining substances, solution is dissolving a substance in another
761616
One that will ideally:\n1) dissolve the component that you wish to collect but not the others. Then you can do a filtration, collect the filtrate and evaporate off the solvent to get back the component that you want.\nOR\n2) dissolve all those that you don't wish to collect but not the component that you want. Then you can do a filtration and collect the component that you want as the residue.\n\nHope this helps :)
320284
It is not possible.  Observe the chemical equation:\nAg2SO4(s) + AgNO3(s) --> Ag2SO4(s) + AgNO3(s)\n\nIn order for a substance to dissolve, it must be in an aqueous solution.
29066
The answer should be Hydrolysis.
969567
You can evaporate, or distill off the water.  Then you'll get the CuSO4, along with any non-volatile impurities that may be present.  Or you can do a recrystalization.  You boil the solution until the CuSO4 just starts to crystalize out.  Then you let the solution cool.  As it cools, the solubility of the salt decreases, and more & more of it crystalizes.  When cooling, you may end up with a super-saturated solution, instead of crystals being formed.  In that case, scratching the inside of the beaker with a glass rod will initiate the crystalization process.  With recrystalization, the product is also purified.
829885
By converting it into a acid forms and than to recrystallize( or to convert into a  water soluble forms) it again.Reconstitution is just a form of making more refined.
1107804
if i recall correctly you are mixing two (or more) substances together, generally liquid, and solids form and precipitate out of solution.  (basically some solid chunks form from the mixture of the liquid)
304001
I suggest that you create a supersaturated solution first. Reason being that the more highly saturated the solution, the better the formation of the crystal and the larger the end product. This can easily be done by heating your solvent to a very high temperature and stiring in copious amounts of whatever is going to make up your crystal. Lower the heat as it goes and you should idealy end up with a very viscous solution, not so much of a liquid but more to the kind of stuff you get when you mix a bit of cornstarch with water. Thereafter dump everything in a beaker or bowl and suspend a thin wax thread in the solution itself. Cover up the bowl and leave to set for a few days. If you have done it correctly you should see a very nice, large crystal forming. Just a note though, don't let the thread touch the bottom of the bowl or even any thing other than the solution, or your crystal will be lopsided