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May 23, 2010. 11:56 PMPeter.Steele
says:
You gotta be kidding me.
If I've got Ammonium Nitrate, I've got MUCH better things to do with it than expend it making a less entertaining substance.
If I've got Ammonium Nitrate, I've got MUCH better things to do with it than expend it making a less entertaining substance.
Aug 10, 2010. 7:54 PMcorey11
says:
What's more entertaing than makin black powder with this and blowing something up? Nothing so go get a life.
I don't give a flying f=ck what you think is better or entertaining, i'm trying to show chemistry. So shove it.
Jul 1, 2010. 2:18 PMiloveairsoftstuff
says:
lol. halarious. that is really funny. nice ible and cool chemistry, but it does seem like kind of a waste of NH4NO3.
Feb 3, 2010. 12:46 AMxxaaron1015Xx
says:
i dont get it, do u have to evaporate the water, but if u do you have two different chemicals, fussed into one crystal, or do crystal for when u freeze it?
Apr 29, 2010. 9:13 PMtreznick
says:
Since the solution is concentrated with ionic species, it will not freeze at 0 Celsius. When the Ammonium Nitrate and Potassium Chloride are mixed in aqueous solution, all four ionic species (NH4+, NO3-, K+, Cl-) are present in solution. Of all of the possible ionic compounds that can be formed by these different species, KNO3 (potassium nitrate) has the lowest solubility, that is to say, that when you decrease the temperature of the solution, KNO3 will fall out of solution the fastest. Since precipitating KNO3 pulls K+ and NO3- ions out of solution, the equilibrium between the species is unbalanced, and more ammonium nitrate and potassium chloride dissociate, forming more KNO3. Of course, the solubility difference is not substantial enough to yield a completely pure product; NH4Cl, NH4NO3, and KCl will be present in small amounts in the final product. This is why using KOH, as opposed to KCl, is favored. The dissociated OH- anions will deprotonate the ammonioum cation, forming water and ammonia gas. If done under gentle heating, the solubility of the subsequent gaseous product is so low that it will effervesce from solution, pulling the equilibrium equation towards the production of more KNO3. In either process, crystals are filtered out to remove excess solute and impurities. Recrystalization could be employed to purify the products, but it would be much easier to just purchase KNO3 than go through all the trouble.
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