potassium nitrate
#1
Posted 11 April 2006 - 12:35 PM
I've seen this question at a Swedish pyro/he forum, but they don't seem to have a clue, so I thought it would be better to ask here..
is there some way to make potassium nitrate from NaNO3 and KCl?
the reaction is nice
NaNO3 + KCl = NaCl + KNO3
just that I don't know how I will make them react with each other..
don't care about the difficulties with separating them, I know it's very hard..
and don?t say that it is cheaper just to buy KNO3, because I know that to
#2
Posted 11 April 2006 - 01:07 PM
Another method could be fractional crystallisation. You will need a Potassium Nitrate crystal for this. You would get one by allowing the solution to cool, and picking out the largest Potassium Nitrate Crystal, then boiling the solution again to re dissolve the precipitate. I believe Potassium Nitrate will produce long needle crystals when precipitating out slowly, so look for the largest one of them. Then, suspend the crystal in the solution, and the Potassium Nitrate will form on the suspended crystal.
There is a bit more too it than that, but thats the general idea behind it anyway. The link below makes for an interesting read...
http://www.waynesthi...om/crystals.htm
#3
Posted 11 April 2006 - 01:54 PM
kno3 is virtually insoluble in alcohol, but the nacl, kcl, and nano3 are all partially soluble.
but if you just want it for bp, skip my step.
#4
Posted 11 April 2006 - 02:49 PM
finaly something makes sense.
so, its just mix same amount of moles of nano3 and kcl in boiling water, and let it crystallize?
1 mole of nano3 and 1 of kcl will give me 101g of kno3 and 58g nacl3. that?s pretty nice actually.
will test this later, will post the result!
now, to one other problem. (not really a problem but..)
I?ve only found a salt which is 66%kcl and 33%nacl.
is there anyway to separate those?
because that will give me 37g of extra nacl per mole of kcl..
one other thing, this fractional crystallization, will it only form kno3 crystals on a kno3 crystal? then would that be the best way to get it out.
#5
Posted 11 April 2006 - 03:07 PM
#6
Posted 11 April 2006 - 04:14 PM
now, to one other problem. (not really a problem but..)
I?ve only found a salt which is 66%kcl and 33%nacl.
is there anyway to separate those?
because that will give me 37g of extra nacl per mole of kcl..
one other thing, this fractional crystallization, will it only form kno3 crystals on a kno3 crystal? then would that be the best way to get it out.
If needed in quantity, KCl can be produced easily with K2SO4 ("Sulphate of Potash") and CaCl2 (used as a drying agent, to reduce condensation).
Dissolve K2SO4 first, boil well and leave to cool, CaSO4 precipitates out. Filter through fine cloth, then coffee filter.
If there is any doubt over the purity of the ingredients, add a slight excess of K2SO4 rather than the (hygroscopic)CaCl2.
Any K2SO4 left in the KCl will crystallise out first.
#7
Posted 11 April 2006 - 09:55 PM
thx!
1 mole of nano3 and 1 of kcl will give me 101g of kno3 and 58g nacl3. that?s pretty nice actually.
will test this later, will post the result!
now, to one other problem. (not really a problem but..)
I?ve only found a salt which is 66%kcl and 33%nacl.
is there anyway to separate those?
because that will give me 37g of extra nacl per mole of kcl..
the impurity of 33% nacl will not affect the reaction. i've used it before and had great success making kclo3.
and btw, the yeilds won't be that great, they never are.
#8
Posted 17 April 2006 - 09:14 AM
http://www.vk2zay.net/
#9
Posted 23 June 2006 - 08:23 PM
today i bought potassium nitrate from an agriculture shop.it is good for use it in pyro compositions?
Thanks
#10
Posted 23 June 2006 - 08:50 PM
hello.
today i bought potassium nitrate from an agriculture shop.it is good for use it in pyro compositions?
Thanks
Garden grade Potassium Nitrate is fine for pyrotechnics use, this has already been discussed before if you search the forum.
#11
Posted 29 July 2006 - 03:36 PM
K2CO3(aq) + Ca(NO3)2(aq) => 2 KNO3(aq) + CaCO3(s)
I've used it several times until I got my hand in 100kg pure KNO3 for a fair price (below 100?).
All the chemicals are readly aviable, but calcium nitrate have a unknown amount of crystal water, so it's difficult to find out the exact ratio between the two reacting chemicals.
#12
Posted 31 July 2006 - 10:00 PM
#13
Posted 01 August 2006 - 09:28 AM
Or just measure how much i need to get the reaction stop precipitating.
Edited by Anders Greenman, 01 August 2006 - 09:28 AM.
#14
Posted 01 August 2006 - 10:43 AM
http://www.vk2zay.net/
#15
Posted 01 August 2006 - 04:10 PM
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