budullewraagh

i dunno. youd have to be careful with how much current you add to your solution...and on second thought i dont think it would work because with organic solvents, you aren't ionizing the salt or hydroxide.

oh you just can't do that. if you really want potassium, just take a binary salt, namely the chloride, or the hydroxide, put a blowtorch to it and electrolyze it. just a few notes: do it outside; from the chloride chlorine gas is produced. also, this may cause balls of molten potassium metal to fly out of your mixture. this is where it gets dangerous. your potassium product may explode if it's hot and it comes into contact with too many oxidizing gases too quickly. plus, you wouldnt want a ball of molten potassium to hit you in the eye. as well, you have to catch the potassium and put it in motor oil or something of the like immediately...or you could do it under argon. if you decide to do this, i suggest you go through everything with us beforehand...oh, and document whatever you do with pictures/video

well, thats why you do it under argon...

i was thinking of doing that at very high temps but they would exceed the decomp temp of NH3. you could thermite potassium out with finely divided aluminum or magnesium under the right conditions. yes i know this doesnt make sense what with reduction and oxidation potentials but i've read some accounts of this sort of thing actually working

ammonia wont react with potassium nitrate. i was thinking of a really obscure method involving high temperature reduction with other metals

"NH3(aq) is a weak base in equilibrium. NH3(aq) + H2O(l) <=> NH4+ + OH-" to the former, yes. to the latter, no, not really. it's been recently found that ammonia in solution is NH3(aq), not NH4OH(aq)

can't say i have. i should look into them though

"Ammonia dissolves in water and react with water to form ammonium ions and hydroxide ions. NH3(aq)+ H2O(l)+ HCl(aq)----> H2O(l)+ NH4Cl(aq) Or NH4OH(aq)+HCl(aq)---->NH4Cl(aq)+H2O(l) Moreover, can anyone write down the ionic equation of hydrogen chloride gas dissolve in sodium hydroxide?" ammonia in water is NH3(aq) not NH4OH. hydrogen chloride gas doesn't really dissolve in sodium hydroxide. it just reacts with the sodium hydroxide, forming a soluble salt.

you could cool it quite a bit. relative to other gases, it goes to liquid at a higher temperature. still, you don't want to work with liquid ammonia. ever work with the 3% solution? yeah, it doesnt smell good. also isn't too good with the lungs and all. now, that's a 3% solution so you're only experiencing the vapor from the vapor pressure so it's a very, very small amount you're exposed to. and it smells awful. think of what the gas would be like, thick as it rises from the liquid.

calcium hydroxide will not dissolve in acidic solutions. calcium hydroxide will react with the acid and the product may be soluble in the resulting conditions.

it would be impressive and that's why i used the word "theoretically"

Ca2+ is a calcium atom and i never said it wasnt. but really, as a rule of thumb you should refer to Ca+2 as calcium cations and Ca as calcium atoms

no, the chloride and nitrate would be calcium cations. you'd be vague if you were calling them calcium atoms.

check around digital libraries

ok, what's a calcium atom then? i said calcium atom in the first place, referring to the pure element which happens to be a metal. and no, of course i dont think calcium chloride is a basic salt. who mentioned chloride anions?

a calcium atom when added to water becomes basic, as the hydroxide is formed

oh and with regard to your last post. theoretically then, you could add one calcium atom to a solution of bisulfate and it would all decompose over time, right?

"That still doesn't make sense. You're saying that if the calcium hydroxide and sulfuric acid are in equal concentrations, that it will form water and calcium sulfate. But if you have an amount of sulfuric acid that exceeds the amount of calcium hydroxide, the calcium hydroxide will no longer be a strong base and will fail to neutralize the sulfuric acid. I find that very hard to believe. Calcium hydroxide is a strong base so it has no problem neutralizing a weak acid. Saying that it can't neutralize the weak acid just doesn't make sense. That's like saying that sodium hydroxide is unable to neutralize formic acid because formic acid has a small Ka." you arent following me at all. think of it. if there is an excess of sulfuric acid, there will be some bisulfate formed. if there is a 2:1 ratio, there will be no sulfate and all bisulfate. consider: 1 mole of Ca(OH)2 1 mole of H2SO4 you get 1 mole of CaSO4 1 mole of Ca(OH)2 1.5 moles of H2SO4 according to your theory we would end up with 0.5 moles of H2SO4, unreacted, with 1 mole of CaSO4. the H2SO4 reacts with CaSO4 to form Ca(HSO4)2 do you follow?

it depends on the concentrations. sulfuric is a strong acid, but the second hydronium cation's dissociation constant is a bit high. if you had 2 parts sulfuric per calcium hydroxide, you'd get the bisulfate. if you did it 1:1 you'd get calcium sulfate, and it would probably go to completion

ok ok let me clear this up. krypton can only oxidize REASONABLY to +2, and this is with fluorine under high pressure. it forms clathrates like Kr8(H2O)46 and Kr(quinol)3 as well as [KrF]+[AsF6]- and of course the difluoride which decomposes in water. a higher fluoride has been made and apparently a salt of an oxyacid has been made. ArKr+ and KrH+ have been made and some people say they made either KrXe or KrXe+. nonetheless, just about all of these compounds/ions have been made in recent years... and really, none of these compounds are remotely stable. the difluoride is certainly reasonable to make, but still not particularly easy for people like us...well, considering you have to use elemental fluorine. anyway, the concept of a higher oxide/oxyacid or salt like KrO4 is, for all intents and purposes, impossible to make and contain for any reasonable amount of time. KrO4-2 still is a stretch. KrO3 sounds possible and KrO3-2 more probable. anyway that's just my ten cents

if you have 3 parts H2SO4 for every 1 part Ca(OH)2 then you have the bisulfate, water and an excess of sulfuric acid

it depends on what socialist principles are adopted. there are some aspects that are very effective and others that are less so

"As an example, the ammonia ion is notorious for making AZIDES, like our good old nitrogen tri-iodide, which is now known as iodine AZIDE!" azide is the N3- anion. the ammonium cation is NH4+. nitrogen triiodide is not iodine azide. theoretically iodine azide would be IN3, where the formal charge on I is +1 and the azide is, as usual, -1. that just doesn't work. "So, your ammonia gas, known to Danes as AmmoniAk (ammony-ACK!), has changed its name to the internationally-approved ... TADAAAHH!!! AZAN! (or azane)." no, because azane would involve N3-. ammonia is NH3. it's trivalent nitrogen. think of it: amine, ammonia, ammonium. they all refer to trivalent nitrogen with nitrogen.

well it's easier to do than that. add lead dust/powder to, say, hydrogen peroxide. no need to fuse potassium nitrate and do it that way.

"acetoning". you mean adding acetone to match heads? that shouldn't be problematic. btw, "caps" contain an incredibly small amount of armstrong's mixture: red phosphorus and potassium chlorate. it's incredibly sensitive. never make it, ever.