IodineForLunch
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strontium perchlorate
OK, I think I've come up with a feasible way of producing strontium perchlorate. This is entirely theoretical, but all numbers and amounts are based
on math, and the following reaction:
Sr(NO3)2 + 2 KClO4 = Sr(ClO4)2 + 2KNO3
Note that the other byproduct is saltpeter; always useful. It's really not a
wasteful reaction. Here is my proposed step-by-step plan:
1. Dissolve 212 grams of strontium nitrate in 250 ml of very hot (90 degrees
celsius) water.
2. While keeping the water hot, slowly add 276 grams of potassium perchlorate,
while stirring, until all has dissolved. If the perchlorate does not dissolve,
the reaction is not working.
3. Boil the liquid down to 150 ml. At this point, take the reaction container
away from it's heat source and place it in an ice bath. Keep the ice bath fresh
by adding new ice until the liquid in the reaction container has dropped to 5
degrees celsuis.
4. Remove the beaker from the ice bath, and there should be a thick layer of
precipitate on the bottom of the beaker. This is saltpeter. Filter out the
saltpeter, dry it, and then use it for whatever you'd normally use saltpeter
for (note that it will contain a small amount of both strontium nitrate and
strontion perchlorate, and thus will impart a red color to most mixtures).
5. The remaining liquid contains strontium perchlorate in solution with about
8% saltpeter impurity. Boil away the remaining water to obtain the strontium
nitrate.
Calculated yield: 270 g Sr(ClO4)2 and 202 g KNO3
WARNING: Strontium perchlorate is a powerful oxidizer. Do not attempt the
above reaction until I risk life and limb by attempting to do so. However,
feel free to comment on the feasibility of it, and to give me tips and
suggestions for further efficiencizing the process.
David Hansen
I set acetic anhydride aflame.
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Polverone
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A reasonable first attempt...
If only all reactions were this simple! Alas, potassium perchlorate is one of the most insoluble potassium compounds in existence. You're not going to
be able to do things the way you would like to. I think you would do better starting with strontium hydroxide or carbonate and ammonium perchlorate,
as in the method I've posted for making nitrates.
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vulture
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Does anyone has any info about the solubility of strontium (per)chlorate?
One shouldn't accept or resort to the mutilation of science to appease the mentally impaired.
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Madog
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stronium carbonate or hydroxide would be best to use.
what about sodium perchlorate. im sure that is fairly soluble.
Most people outgrow their pyro tendencies, we are the ones who\'s tendencies outgrew us.
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IodineForLunch
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hmmm
So, an insoluble compound cannot react with a solution of another compound? That's what you're telling me, but I've never heard that before.
Strontium perchlorate is extremely soluble in cold water, but potassium nitrate is not, which is how they're filitered.
I see no reason why they would not react.
David Hansen
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Polverone
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Strontium perchlorate, strontium nitrate, and potassium nitrate are all considerably more soluble than potassium perchlorate. The reaction that you
have written is reversible. Not only can strontium nitrate react with potassium perchlorate to form strontium perchlorate and potassium nitrate, but
potassium nitrate and strontium perchlorate can react to form potassium perchlorate and strontium nitrate again. It's just a soup full of ions
constantly trading components. And since potassium perchlorate is by far the most insoluble member of all the compounds in solution, the equilibrium
is going to strongly favor it.
Ammonium perchlorate would work because, first of all, ammonium perchlorate is much more soluble than potassium perchlorate, and second, because by
boiling the solution (containing strontium carbonate and ammonium perchlorate, as well as ammonium carbonate and strontium perchlorate) you can
*disturb* the equilibrium by removing ammonia and carbon dioxide from the system, forcing the eventual complete formation of strontium perchlorate.
Sodium perchlorate will form a better equilibrium mixture than potassium perchlorate would, but you can't boil it to shift the equilibrium, and if you
want to use the strontium perchlorate for pyrotechnics then you definitely don't want it contaminated with sodium compounds.
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IodineForLunch
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Thanks for the help guys. Can it be done with strontium carbonate and ammonium perchlorate?
David Hansen
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IodineForLunch
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I am definitely going to try the SrCO3 and NH4ClO4 method. Now, there won't be anything left in solution after the boiling but the strontium
perchlorate, right? Or will certain ammonia and carbon compounds remain?
David Hansen
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Polverone
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The reaction will probably take some time (multiple hours) of heating to complete. I don't know how hygroscopic strontium perchlorate is; it may be
difficult to dry completely. But you won't have leftover ammonia or carbon compounds if you balance the reactants properly and heat them long enough.
A small amount of leftover ammonium perchlorate or strontium carbonate shouldn't cause problems in pyrotechnic formulas (which I assume this is for)
anyhow.
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IodineForLunch
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Strontium perchlorate is hygroscopic, unlike barium perchlorate, which is not. I am assuming the metal carbonate / ammonium perchlorate
method can be used to produce a wide range of perchlorates.
David Hansen
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PHILOU Zrealone
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Most perchlorates except KClO4 are quite hygroscopic and hard to dehydrate.They are therefore used as dehydratants in organic solvants and many
accidents have been reported...you know traces of solvant and heating of polluted perchlorate cristalls to dehydrate them --> BOOM!
The rules of precipitation apply here the less soluble of all salts will rule the equilibrium and be dropped of the system (liquid here).
So actually, you have many possibilities to make Sr(ClO4)2!
1) HClO4 + Sr (sulfide, nitrite, carbonate, oxyde, hydroxyde)...sulfide evolves H2S toxic and stinky, nitrite evolves toxic NOx; all the other are
unsmelling and non toxic!
2)NH4ClO4 + Sr crabonate/hydroxyde or oxyde will evolve NH3!
3)SrCl2 + electricity and O2 --> hypochlorites, chlorites, chlorates and finally perchlorates...this way is used to make Ca(ClO4)2!
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