EquationProblems1

Thanks OldChemE. Appreciated. I heated to about 65 Celsius for 75 minutes to reduce the solution by about 50%, then cooled to 2 Celcius overnight and filtered in the morning. A large amount of crystals had precipitated which I tested for nitrates and found none/very little to be present. So I'll warm the filtrate today to evaporate off all the water and see whether it yields the ammonium nitrate I'm hoping for. Will revert in a day or so. If it does, I'll guess I'll need an assay for NH4NO3 - as you say, there are all sorts of ions floating about so it'll be interesting to see what has combined.

Jeez, I thought I was posting on a forum where people had at least a rudimentary knowledge of chemistry! I didn't think I'd need to point out that solubility varies with temperature, given that this is after all the whole basis of recrystallization. Think it might be you reaching for that textbook ...

Studiot, may I ask you not to post againn as you're not a chemist, nor a physicist if you're unaware that enthalpy drives the direction of a reaction.

On the contrary, it does mean it will because a reaction will occur based on the laws of empalthy. Please ensure contributions show actual knowledge of the subject matter. Studio - I've done so, and KNO3 dissolves just fine. Much better 8n warm water though. But what''s your point?

I was needing a little help balancing an equation: I'm exploring various ways of making NH4NO3. (And if your contribution is to tell me I'll end up on some watch list for even mentioning the compound, please keep your ridiculous ill-informed paranoia to yourself - if I was a terrorist, I'd be buying NH4NO3 fertiliser, not making a few grams!). Having successfully mixed NaHSO4 with NaNO3 and neutralised with NH3, I balanced to give Na2SO4 + NH4NO3. So I replaced the nitrate salt with KNO3, and expected an eqimolar precipitate of Na2SO4 and K2SO4 (and of course the NH4NO3 in solution). However, I've tried a few equation balancers online, and they tell me it's an "impossible reaction". Am I wrong, or are they? (My reasoning is that the NO3 and the NH3 combine, mopping up the extra H's liberated by the highly acidic NaHSO4/KNO3 mixture. This leaves K and 2Na and SO4 floating around combining with one another) S'Ok - think I've done it: 2 NaHSO4 + 2 KNO3 + 2 NH3 = K2SO4 + Na2SO4 + 2 NH4NO3