Sciencemadness Discussion Board - urea perchlorate

urea perchlorate

garage chemist - 28-1-2005 at 09:22

I'll soon get some KClO4 and distill 72% (azeotropic, nonexplosive) Perchloric acid from this.

Urea perchlorate hasn't been covered before, so let's discuss it. I never saw a procedure for it either.
It could be made by mixing dilute solution of HClO4 with conc. solution of urea and filtering (if it has low solubility) or evaporating the solution.

Will this be a primary or secondary HE?

PainKilla - 28-1-2005 at 09:29

It probably doesn't exist, on top of that it is damn near impossible to get HClO4 from KClO4. You are better off starting from NaClO4. That is the procedure used for making it usaully. Only problem is that IIRC its explosive too and not very cheap. On top of that, I don't see how urea perchlorate would even be possible. Carbamide Percholate? Unlikely. :p

chemoleo - 28-1-2005 at 09:46

Nono, urea forms nitrates too, which is fairly insoluble, so there is no reason why perchlorates couldn't form. There is however a description of guanidine perchlorate somewhere (which is better), and ethylendiamine perchlorate, even hydrazine perchlorate. The latter three have known VoDs, they are quite high.
From my experience with nitrate salts of amines, the perchlorates should be more sensitive, but very hygroscopic.

So you want to distill HClO4? make sure it is dilute.
Why wouldnt it work, Painkilla, i.e. dil H2So4 + KClO4? It would be slower than with NaClo4, granted, but should still work.

PainKilla - 28-1-2005 at 09:49

I remember trying to find a way to do it myself but coudln't find one. Ill try to pull up a few references..... It can be done but it is very difficult to actually do, especially with KClO4.

Fixed.

link

[Edited on 28-1-2005 by PainKilla]

garage chemist - 28-1-2005 at 13:05

72% Perchloric acid has a constant boiling point of 203°C at atmospheric pressure and is not classified as being explosive. It has an oily consistency and looks exactly like conc. H2SO4.
However, the anhydrous acid (which has a low viscosity) explodes on warming even before it reaches its boiling point and can also spontaneously detonate at room temp. without any obvious reason. It can only be distilled in vacuum and with extreme safety measurements.

NaClO4 seems to be very difficult to get, because most suppliers only sell NH4ClO4 and KClO4. The former could be boiled with NaOH though.
KClO4 can not be transformed into any other perchlorate salt by recristallisation, because of its very low solubility. Hence the need to make HClO4.

BromicAcid - 28-1-2005 at 13:07

Gahhh, someone fix the above links!

Distilling perchloric acid is no easy task as you've probably already read, how is he going to make sure the HClO4 is dillute Chemoleo if he's distilling, the azeotrope will come over, or do you mean to say he should make sure he dillutes it before reacting it with the urea?

As I've already posted in the perchloric acid thread I've tried this (prep of HClO4 from KClO4 with H2SO4) with limited sucess, if you want I could U2U you specifics.

Edit: My post kind of overlaps with the above, be sure to distill under reduced pressure, at atmospheric pressure up to 20% of the HClO4 can decompose and explosions have known to result, even a speck of dust can cause them.

[Edited on 1/28/2005 by BromicAcid]

chemoleo - 1-2-2005 at 17:12

Garagechemist, there is a prep on the production of HClO4 from KClO4 using H2SO4.
For details (and since you can read German), have a look at Brauer's inorganic chemistry preps, page 327 (Vol 1). You can download it from the FTP.
If someone wants more details let me know.

Quote:

It probably doesn't exist,

Be careful with such statements if there is no evidence...

S.C. Wack - 1-2-2005 at 18:38

...especially when a search of google and espacenet reveals its preparation and use in explosive compositions.

[Edited on 2-2-2005 by S.C. Wack]

Axt - 1-2-2005 at 19:20

PATR listing of Urea Perchlorate (I havn't fixed the spelling errors due to OCR):

Quote:

CH5CI.N205,; mw 160.52;
N 17.46%; OB to C02 +4.98%; v hydroscopic and unstable white crysts; mp, explds on heating without burning. V sol in w. CA Registry No [1872-07-6]. Prepn is by the interaction of equimolar amounts of urea and perchloric acid in acetic acid followed by solvent evapn. Its
impact sensy is comparable to that of TNT
(Refs 1 and 17a) The perchlorate has been incorporated into
more than several expl compns. Shiino et al claim in their patent (Ref 23) that a liq expl of high deton vel can be made by dissolving solid aromatic nitro compds into aq urea perchlorate.
Thus, PA (5) is dissolved in 85% aq urea perchlorate (95 wt p) to obtain a liq expl having a d of 1.6g/cc and a deton vel of 6520rn/sec. In the invention of Fujiwara et al (Ref 24) an expl slurry of improved stability is claimed consisting of a mixt of combustible solids in aq urea perchlorate
soln. Typically, powdered K perchlorate
(30) and powdered ferrosilicon (30) are
added to 85% aq urea perchlorate (50 wt p) to form a slurry-like expl having a d of 1.7 lg/cc and a deton vel of 3700m/see, as well as high stability. In another patent, Shiino et al (Ref 25) claim a process for the prepn of the expl
perchlorate, per se. Thus, 430g of urea are added slowly to 1000gof715Z0 aq perchloric acid at <20° to give the 1:1 urea perchlorate salt crysts. The patent shown in Ref 26 suggests the use of the perchlorate in an underwater blasting slurry when incorporated with materials
such as PA. The claimed impact sensy is > 60cm (5-kg wt from 60cm resulting in 0/6 trials).
Fujiwara et al, as a result of their work, (Refs 29& 30) with aq urea perchlorate solns mixed with various organic substances, report that with detonatable materials such as PA, the solns
formed are impact insensitive but powerful
expls exhibiting two distinct deton modes: low vel deton (LVD) (’u 1900rn/see) and high vel deton p 6000m/see). Mixts with nondetonatable
substances as ~trobenzene or dimethylformamide show only LVD, requiring an extremely high critical initiation pressure of approx 40kbar.

AndersHoveland - 29-6-2011 at 13:46

There is a big russian explosives site that claims that when urea perchlorate is ground in a mortar and pestle there are little popping sounds, presumably as the little granules detonate, so it is probably advisable to be fairly careful when handling energetic perchlorate salts. Here is a link to the site, but be WARNED, despite the site having a huge library of information and decent content, it is also, for some reason, smeared in pornographic video pictures, not to mention that the entire site is in russian.
http://www.pirotek.info/Vv2/oktonitrocuban.htm

[Edited on 29-6-2011 by AndersHoveland]

Amazing what floats to the surface here...!

The WiZard is In - 29-6-2011 at 16:52

You can read H H Willard original preparation of perchloric
acid 1912 from ammonium perchlorate in the J. Amer. Chem. Soc.,
34, 1480 @ Google.com/books.

http://tinyurl.com/5vxo2v4

woelen - 29-6-2011 at 22:58

I cannot read that link, apparently it only is accessible if you're from the US. Is it possible to extract a PDF and post that? I have quite some ammonium perchlorate (we can buy that over here without too much hassle, as long as it is in the form of somewhat bigger crystals) and if HClO4 can be made from that in a safe way then I would like to know of that.

Rosco Bodine - 30-6-2011 at 01:04

The preparation of perchloric acid Willard JACS 34, 1480, 1912

Attachment: The preparation of Perchloric acid.pdf (431kB)
This file has been downloaded 1183 times

The WiZard is In - 30-6-2011 at 09:27

Quote: Originally posted by The WiZard is In

You can read H H Willard original preparation of perchloric
acid 1912 from ammonium perchlorate in the J. Amer. Chem. Soc.,
34, 1480 @ Google.com/books.

http://tinyurl.com/5vxo2v4

This me thinks dobe a easier synthesis. Brauer is in la Science Most Mad's library.

The Merck Index

Monograph Number: 0007153
Title: Perchloric Acid
CAS Registry Number: 7601-90-3
Molecular Formula: ClHO4
Molecular Weight: 100.46
Percent Composition: Cl 35.29%, H 1.00%, O 63.70%
Line Formula: HClO4
Literature References: Prepd from potassium perchlorate and
sulfuric acid: Schmeisser in Handbook of Preparative Inorganic
Chemistry vol. 1, G. Brauer, Ed. (Academic Press, New York, 2nd
ed., 1963) pp 318-320. Comprehensive monograph: J. C.
Schumacher, Perchlorates (Reinhold, New York, 1960).

Properties: The anhydr acid is a colorless, volatile, very
hygroscopic liquid. d22 1.768; bp11 19°. Dec when distilled at
atmospheric pressure, sometimes with explosive violence. mp -
112°. Combines vigorously with water with evolution of heat.
Undergoes spontaneous and explosive decompn, hence it is
marketed only in mixture with water contg 60-70% HClO4, density
1.5 and 1.6, respectively. The aq acid is very caustic and may
deflagrate in contact with oxidizable substances. Density of aq
solns at 15°: 1% = 1.0050; 10% = 1.0597; 20% = 1.1279; 30%
= 1.2067; 40% = 1.2991; 50% = 1.4103; 60% = 1.5389; 70% =
1.6736. Density of aq solns at 25°: 65.0% = 1.597; 70.0% =
1.664; 75.0% = 1.731.
Melting point: mp -112°
Boiling point: bp11 19°
Density: d22 1.768; Density of aq solns at 15°: 1% = 1.0050;
10% = 1.0597; 20% = 1.1279; 30% = 1.2067; 40% = 1.2991;
50% = 1.4103; 60% = 1.5389; 70% = 1.6736.

CAUTION: Corrosive to skin, mucous membranes.

Use: The acid in analytical chemistry as an oxidizer and for
separation of potassium from sodium. Its salts for explosives and
for plating of metals.

---
Add a little excitement to your chemistry with anhydrous perchloric
acid.

If you have, dobe knowing someone who has? Yes. An academic
affiliation you maybe able to get a free copy of these from
GF Smith Chemical Company.

If'n you do — perhaps you can obtain a second copy (it is a newer version of my copy) of —
Perchloric Acid and Perchlorates, for me.

Thanks.

quicksilver - 30-6-2011 at 11:48

RE: the pamphlet, how old was it & was it a 4 page academic hand-out? I still have a few friends who are teaching.

I never bothered with it personally. A plating company in town had a great deal of it (60-70% acid) & it was very inexpensive.

The WiZard is In - 30-6-2011 at 13:53

Quote: Originally posted by quicksilver

RE: the pamphlet, how old was it & was it a 4 page academic hand-out? I still have a few friends who are teaching.

I never bothered with it personally. A plating company in town had a great deal of it (60-70% acid) & it was very inexpensive.

Perchloric Acid and Perchlorates 1979, I believe they have a newer
edition is 189 pages.

The Wet Chemical Oxidation... 1965, 105 pages.

V/ v/ difficult to find outside a library though it has been
reprinted by UMI Books on Demand (of which my copy is.), but still v/ v/ useful —

J Schumacer Ed.
Perchlorates: Their Properties, Manufacture and Uses
Reinhold Publishing
1960

---
Maybe of use —

Accession Number : AD0242192
Title : CHLORATES AND PERCHLORATES THEIR MANUFACTURE,
PROPERTIES AND USES
Corporate Author : SOUTHWEST RESEARCH INST SAN ANTONIO TX
Personal Author(s) : WARREN, FRANCIS A. ; MILLAR, JOHN D.
Handle / proxy Url : http://handle.dtic.mil/100.2/AD242192
Report Date : 15 MAY 1960
Pagination or Media Count : 754
Descriptors : *CHLORATES, *PERCHLORATES, PRODUCTION,
CHEMICAL PROPERTIES, SYNTHESIS(CHEMISTRY), EXPLOSIVES,
CHEMICAL REACTIONS, PYROTECHNICS.

Subject Categories : INORGANIC CHEMISTRY
INDUSTRIAL CHEMISTRY AND CHEMICAL PROCESSING

I bought a 35mm microfilm copy (the only version available)
from the NTIS years ago (US #4.00). I never found the need to
spend US $300 or so for a blow back. I could have run it through
my Nikon Coolscan 5000 (Don't buy one!).... lets see 754 pages
times 133 meg. per page equals .... X-bytes... lots of bytes.

If'n you search la DTIC you will find a pub on the production
of perchlorates by chemical means, I have found it interesting,
if not useful.

I just shit-canned my blow back from microfiche (at the time
MF's were only US $4.00 from the NTIS compared to YAHOO $$ for
a print version) on that old time slimy/heavy paper of ....

Accession Number : AD0900260
Title : Engineering Design Handbook. Principles of Explosive Behavior
Descriptive Note : Pamphlet
Corporate Author : ARMY MATERIEL COMMAND ALEXANDRIA VA

Handle / proxy Url : http://handle.dtic.mil/100.2/AD900260

Report Date : 10 APR 1972

Pagination or Media Count : 381

Abstract : This document contains reports on: (1) Energy of
explosives, (2) Thermal decomposition of explosives, (3)
Measurement of detonation properties, (4) Elementary theory of
the plane detonation wave, (5) Application of theory to condensed
explosives, (6) Structure of the plane detonation wave: finite
reaction zone, (7) Detonation waves of cylindrical and spherical
symmetry, (8) Thermal explosion, (9) Initiation of detonation by
shock waves, (10) Initiation and growth of detonation from impact,
friction, and thermal sources, (11) Shock waves from explosive
charges, and (12) Computer programs for explosive calculations.

Descriptors : *EXPLOSIVES, X RAY PHOTOGRAPHY,
FRAGMENTATION, LIQUIDS, THERMODYNAMICS, SHOCK WAVES,
EXPLOSIVE CHARGES, GASES, THERMOCHEMISTRY, HANDBOOKS,
FRICTION, DECOMPOSITION, HYDRODYNAMICS, PYROLYSIS,
DETONATIONS, EQUATIONS OF STATE, UNDERWATER, RADIATION
EFFECTS, COMPUTER PROGRAMS, REACTION KINETICS

Subject Categories : AMMUNITION AND EXPLOSIVES

NB — This is not a how-to book, it is? Yes! Tres technical.

dann2 - 30-6-2011 at 15:01

'The Perchlorates' is available here:

http://www.archive.org/details/pwechloratesthei001740mbp

Thanks for 'The Chlorates and Perchlorates' Mr. Wizard.
Seen a ref. to it years ago but was always unable to find it.

Perchloric acid (book) is available for viewing here:
http://babel.hathitrust.org/cgi/pt?id=uc1.l0064462088

Anyone know how to download the thing.

Perchloric acid and Perchlorates can be had from Amazong for 27.50 Dollars.

I enclose 'Perchloric acid' from Russian Journal for your enjoyment.

Dann2

[Edited on 30-6-2011 by dann2]

Attachment: perkacid.pdf (1.9MB)
This file has been downloaded 1070 times

[Edited on 30-6-2011 by dann2]

AndersHoveland - 30-6-2011 at 15:34

I had always suspected that anhydrous aluminum perchlorate might be explosive, but despite devoting several paragraphs to this compound, they do not mention anything about it being explosive.

section containing some information about perchloric acid here:
https://sites.google.com/site/energeticscribble/perchloric-a...
it is not intended to be comprehensive or completely reliable, but perhaps one of you will find something interesting

franklyn - 1-7-2011 at 00:50

4 parts (H2N)2CO • HClO4 to one part CH3NO2 by weight is oxygen balanced
and Velocity of detonation is ~ 6500 m/s

3 (H2N)2CO • HClO4 + 2 CH3NO2 => 5 CO2 + 9 H2O + 3 HCl + 4 N2

Attachment: Urea Perchlorate Nitromethane US4047987.pdf (951kB)
This file has been downloaded 980 times
Attachment: Urea Perchlorate Nitromethane GB2080280.pdf (443kB)
This file has been downloaded 957 times

Commercially NH4ClO4 is made by dissolving NH4Cl with NaClO4 in water.
The less soluble NH4ClO4 precipitates and is filtered off, leaving NaCl in solution.
See => PATR 2700, P 146
Crystallization of Ammonium-Perchlorate from Solution of
Electrolytically Produced Sodium-Perchlorate in a Pilot Scale Plant
www.nt.ntnu.no/users/skoge/prost/proceedings/ecce6_sep07/upl...
www.soapgoods.com/Ammonium-Chloride-p-773.html
http://smokechemicals.com/shop/index.php?main_page=product_i...

NH4ClO4 can be also made by dissolving (NH4)2SO4 with KClO4 in water,.
(NH4)2SO4 + 2 KClO4 => K2SO4 + 2 NH4ClO4
See => Attachment: Solubilities of alkali metal perchlorates at 25 C & NH4ClO4 Prep.rtf (10kB)
This file has been downloaded 922 times
www.soapgoods.com/Ammonium-Sulfate-p-714.html
http://smokechemicals.com/shop/index.php?main_page=product_i...

In the same way to make (H2N)2CO • HClO4 , neutralize muriatic acid (36 % HCl solution )
with Urea, then mix in the stoichiometric amount of NaClO4.
(NH2)2CO • HCl + NaClO4 => NaCl + (NH2)2CO • HClO4
See the patent US4047987above
Activity Coefficients of Hydrochloric Acid in Hydrgen Chloride Metal Perchlorate Water Systems
http://pdf.lookchem.com/pdf/22/73c04100-f498-4ab9-a4ee-44af8...

NH4ClO4 can be used instead
(NH2)2CO • HCl + NH4ClO4 => NH4Cl + (NH2)2CO • HClO4
www.soapgoods.com/Urea-Prilled-Commercial-p-751.html
www.hobbychemicalsupply.com/servlet/the-123/Ammonium-Perchlo...

In Methanol or Acetone the opposite occurs , NaCl is practically insoluble in those
solvents but (H2N)2CO • HClO4 is solvated. It is possible to use KClO4 instead
in this way (NH2)2CO • HCl + KClO4 => KCl + (NH2)2CO • HClO4
www.soapgoods.com/Urea-Prilled-Commercial-p-751.html
http://smokechemicals.com/shop/index.php?main_page=product_i...

Perchloric acd from NH4ClO4 oxidation
http://thesis.library.caltech.edu/4743
http://thesis.library.caltech.edu/4743/1/Adams_hc_1925.pdf

_______________________________________________________

@ AndersHoveland

Al(ClO4)3 • 6 N2H4

Attachment: Al & Mg Perchlorate Hydrazine cmplexes US4053567.pdf (316kB)
This file has been downloaded 948 times

.

Rosco Bodine - 1-7-2011 at 06:53

It would probably be interesting to see if double decomposition occurs upon mixing urea nitrate and ammonium perchlorate, perhaps slurrying with minimal water or maybe a little 91% isopropanol and warming.

Ammonium perchlorate added to a melt of ammonium nitrate and urea as a slurry with urea nitrate might also undergo a double decomposition where the urea perchlorate forms in situ in considerable amount and the resulting reaction mixture may be a useful explosive.

[Edited on 1-7-2011 by Rosco Bodine]

Urea Perchlorate directly from sodium perchlorate

AndersHoveland - 23-1-2012 at 13:52

606g of urea were added to 1040g of 35% hydrochloric acid and dissolved with stirring. Next, 1405 g of sodium perchlorate was added and the mixture stirred vigorously for ten minutes at 40degC. The mixture was then colled to 20degC. The sodium chlorides which precipitated was separated by filtration and discarded. The filtrate now contained about 65% urea perchlorate, still contaminated with remaining sodium chloride. Under reduced pressure (and keeping the temperature below 80degC) some of the water was boiled out to concentrate the solution. While still hot, the solution was filtered to remove the remaining sodium chloride, the crystals of which collected in the filter were again discarded. This last procedure was repeated again, the solution passing through the filter containing urea perchlorate, with almost all of the sodium chloride removed.

A mix of urea perchlorate (70%) and nitromethane (30%) has a detonation velocity of about 7070 m/sec, and a drop height sensitivity of 60cm

[Edited on 23-1-2012 by AndersHoveland]

AirCowPeaCock - 23-1-2012 at 15:04

Forgive me if I'm being stupid. But wouldn't "drop height sensitivity" vary with mass?

watson.fawkes - 23-1-2012 at 16:34

Quote: Originally posted by AirCowPeaCock

Forgive me if I'm being stupid. But wouldn't "drop height sensitivity" vary with mass?

Remember Galileo and that leaning tower?

AndersHoveland - 23-1-2012 at 21:26

"Drop height" sensitivity actually refers to a heavy metal "hammer" (5kg weight t.ex.) being dropped on the substance, where statistically there is a 50 percent chance of detonation. It does not refer to dropping the substance itself!

AirCowPeaCock - 24-1-2012 at 07:36

Oh, that makes sense! I feel stupid now!

Its like an LD50, but with blowing oneself to bits, not dieing of toxicity.

Although wouldn't the KE over surface area still effect the value?
or would we be looking at speed instead of force?

[Edited on 1-24-2012 by AirCowPeaCock]

Adas - 24-1-2012 at 11:11

Have you thought about Biuret perchlorate? Biuret can be easily made by heating urea, so why not to try it?

Adas - 27-1-2012 at 13:55

Here is a paper describing biuret perchlorate detection.
Biuret Perchlorate

It is pretty strange that oxygen is protonated instead of NH2 group.

AndersHoveland - 27-1-2012 at 14:45

Quote: Originally posted by Adas

It is pretty strange that oxygen is protonated instead of NH2 group.

The oxygen would be protonated rather than an amine group because the amine group is electron donating to the oxygen.

This is the reason why amides groups are so much less reactive than ketones, aldehydes, or amines.

[Edited on 27-1-2012 by AndersHoveland]

ecos - 27-9-2015 at 14:09

Urea Perchlorate seems interesting material. it has much Nitrogen. I made a search for it but couldnt find much info rather than :

any more info about its properties ?

deltaH - 30-9-2015 at 07:56

Urea perchlorate (and also urea nitrate) are very impractical energetic materials because of their high acidity and simultaneous hygroscopicity... a really bad combo. Urea is a very weak base with a pKb(BH+)=0.18 (wikipedia), so it only forms salts with strong acids and those salts are themselves very acidic indeed.

In some respect, urea perchlorate can be viewed as a source of anhydrous perchloric acid, i.e. because of the ease with which it can be deprotonated. Since perchloric acid forms dangerous and sensitive explosives with a wide range of materials, this is a further reason that this perchlorate hasn't made it into mainstream use.

Indeed as has been stated earlier on in this thread, the related guanidinium perchlorate, being the salt of a strong base and acid, is a MUCH better way to go.

specialactivitieSK - 1-10-2015 at 00:40

Better is Guanidine Perchlorate formed by reacting Sodium Perchlorate with Guanidine Hydrochloride.

Non-hygroscopic, moderately sensitive to impact and has considerable power.

1,15 g/ccm = 6000 m/s
400 cm3

It's Explosive appropriate force tetryl.

[Edited on 1-10-2015 by specialactivitieSK]

PHILOU Zrealone - 15-10-2015 at 09:53

Even better would be:

-Biguanidine diperchlorate
H2N-C(=NH)-NH-C(=NH)-NH2 . 2 HClO4

-Pentaerythritamine tetrapechlorate
C(-CH2-NH2)4. 4 HClO4

ecos - 15-10-2015 at 12:48

Quote: Originally posted by PHILOU Zrealone

Even better would be:

-Biguanidine diperchlorate
H2N-C(=NH)-NH-C(=NH)-NH2 . 2 HClO4

-Pentaerythritamine tetrapechlorate
C(-CH2-NH2)4. 4 HClO4

unfortunately, I didnt find any info about both materials on google.

specialactivitieSK - 16-10-2015 at 05:25

Biguanide diperchlorate and process for preparation thereof
US 4340755 A :

http://www.google.com/patents/US4340755

Would it be possible, by reaction Biguanide hydrochloride with sodium perchlorate ?

[Edited on 16-10-2015 by specialactivitieSK]

[Edited on 16-10-2015 by specialactivitieSK]

PHILOU Zrealone - 16-10-2015 at 10:26

Quote: Originally posted by specialactivitieSK

Yes possible.

Also another interesting possibility:
H2N-C(=NH)-C(=NH)-NH2 . 2 HClO4
the diperchlorate of the diimino derivative of oxalamide

[Edited on 16-10-2015 by PHILOU Zrealone]

ecos - 17-11-2015 at 05:08

Quote: Originally posted by specialactivitieSK

Biguanide diperchlorate and process for preparation thereof
US 4340755 A :

http://www.google.com/patents/US4340755

Would it be possible, by reaction Biguanide hydrochloride with sodium perchlorate ?

[Edited on 16-10-2015 by specialactivitieSK]

[Edited on 16-10-2015 by specialactivitieSK]

I could synthesis now perchlorate and I would like to go further and make Biguanide diperchlorate !
sorry if my question looks very basic but i found very hard ways to synthesis Biguanide
isn't there some practical steps to be synthesis Biguanide at home in my small lab?