SAM4CH
Hazard to Others
Posts: 162
Registered: 16-7-2004
Location: TA
Member Is Offline
Mood: PERFECT
|
|
Lead Perchlorate
Did any one try to make Lead Perchlorate?
What about its VOD and its sensitivity?
Sam
|
|
|
unionised
International Hazard
Posts: 5105
Registered: 1-11-2003
Location: UK
Member Is Offline
Mood: No Mood
|
|
It's oviously going to be an oxidiser, but is it esplosive on its own?
|
|
|
BromicAcid
International Hazard
Posts: 3227
Registered: 13-7-2003
Location: Wisconsin
Member Is Offline
Mood: Rock n' Roll
|
|
Yeah, it's explosive on its own, to what degree I do not know. There are plenty of compounds that have no oxidizing properties that are explosive,
like lead thiocyanate or the acetylides, so is it a stretch for lead perchlorate to be explosive? Afterall perchloric acid is usually used with
caution in the undergraduate labratory due to the danger it has with forming perchlorates in fume hood exhausts which can cause explosions on their
removal. Lead perchlorate is commerically avalible as the hydrate and in solutions of up to 50%, the hydrate gives the warning that it should not be
allowed to react under conditions where it could be further dehydrated.
|
|
|
SAM4CH
Hazard to Others
Posts: 162
Registered: 16-7-2004
Location: TA
Member Is Offline
Mood: PERFECT
|
|
I made few grams of it (molten lead acetate+molten sodium perchlorate) and stirred for 10-15 minutes, then I remmember something around it and walk
few step, then I found me on the floor!! it was a very very powerful explosion!!??
The amount I used = 20-25 grams
Please I need more about its properties!!
[Edited on 11-12-2005 by SAM4CH]
Sam
|
|
|
Axt
National Hazard
Posts: 778
Registered: 28-1-2003
Member Is Offline
Mood: No Mood
|
|
| Quote: | Originally posted by SAM4CH
The amount I used = 20-25 grams
Please I need more about its properties!!
|
Properties of what? You didnt make lead perchlorate. You mixed an oxidiser with a fuel, tried to melt it, now wonder why it exploded!
NaClO4 + Pb(C2H3O2)2 Forms an explosive double salt Pb(C2H3O2)(ClO4), but I believe its too soluble to precipitate from the sodium salts.
http://www.sciencemadness.org/talk/viewthread.php?tid=2953#p...
Substituting NaClO4 for NaBrO3 <i>"the explosion of 50mg (caused by shock or heat) is so powerful that a thick-walled container would
shatter!"</i>. Your lucky to get away with this one, considering you stood there stirring 400-500x more.
[Edited on 12-12-2005 by Axt]
|
|
|
Rosco Bodine
Banned
Posts: 6370
Registered: 29-9-2004
Member Is Offline
Mood: analytical
|
|
Lead Perchlorate is a candidate also as a component
of a possible double salt with Basic Lead Picrate ,
and possible higher complexes with Basic Lead Picrate .
It would be interesting to form the possible clathrate :
Basic Lead Picrate / Lead Acetate / Lead Perchlorate
The aminoacetate or formate substituted for the acetate may be interesting also . Any of these may also form
quadruple salt complexes with Lead Azide and should be capable of further adsorption of large amounts of Lead Azide . Lead Nitrate may or may not
need to be an included
part of such complexes . If so , then even a five member complex is a possibility .
Another good possibility for a triple salt is Basic Lead Picrate / Lead Nitrate / Lead Perchlorate having similar potential for complexes with Lead
Azide .
Basic Lead Picrate / Lead Nitrate / Lead Chlorate is already known as a triple salt clathrate . It appears to adsorb more lead azide than will the
simpler Basic Lead Picrate / Lead Nitrate double salt , and forms a more powerful
" azo-clathrate " . A single experiment indicated the
probability of an azo-clathrate having 5 Lead Azides adsorbed for each unit of the triple salt , compared to
4 Lead Azides for the double salt .
The intimate contact of Lead Perchlorate with any other
lead salts which would be provided by the energetic matrix
of a basic lead picrate clathrate , would very likely enhance
whatever energetic properties such salts would have in
other more simple combinations . So if you are going to
experiment with Lead Perchlorate , you should definitely
experiment with some of these sorts of complexes .
For many of these complexes you won't need perchloric acid or lead perchlorate as a precursor , but simply a source of
perchlorate ion provided by a soluble perchlorate salt to
react in situ with some other lead salt like lead nitrate . If
the solubility of the desired perchlorate containing complex is favorably low compared with the solubility of the salt providing the perchlorate ion ,
the reaction will proceed as
a double decomposition source for lead perchlorate being bound to the low solubility complex , even if under simpler conditions the same double
decomposition would not occur .
[Edited on 14-12-2005 by Rosco Bodine]
|
|
|
![[*]](images/xpblue/default_icon.gif){kind=icon}
