| Pages:
1
..
21
22
23 |
dettoo456
Hazard to Others
Posts: 291
Registered: 12-9-2021
Member Is Offline
|
|
High modulus, pyrolized polyacrylonitrile (carbon fiber) can be used to drastically enhance CMDB (and likely other types of) propellant burning rates.
And carbon black is slightly energetic on its own - coal fires. Other than that, metal fuels are the closest thing to an elemental EM you’ll find.
Carbon fiber propellant catalyst pdf:
https://patentimages.storage.googleapis.com/4b/c9/f1/f77511a...
|
|
|
Nemo_Tenetur
Hazard to Self
Posts: 72
Registered: 13-12-2023
Location: Germany
Member Is Offline
|
|
Ag2BTA
Anyone here with information about the disilver salt of bistetrazolylamine? I found this substance mentioned in "laser ignition of energetic
materials" by S Rafi Ahmad and Michael Cartwright 10 years ago:
The copper and silver salt of bis tetrazolyl amine CuBTA (46) and Ag2BTA (47) have been trialled as primary explosives (...) the performance of
these materials is a little unpredictable, and they should be treated with extreme care - particulary the silver bistetrazolamine. There is
insufficient data in the literature to fully characterize their properties as primer compositions."
[Edited on 11-2-2024 by Nemo_Tenetur]
|
|
|
dettoo456
Hazard to Others
Posts: 291
Registered: 12-9-2021
Member Is Offline
|
|
I couldn’t find any info on the silver salt, but the 5,5’-bis(tetrazolyl)amine is light sensitive on its own (much less energetic as compared to a
detonation).
https://doi.org/10.1016/j.chemosphere.2019.125008
Laser sensitive EMs are pretty common though, laser initiation systems far less so.
|
|
|
Nemo_Tenetur
Hazard to Self
Posts: 72
Registered: 13-12-2023
Location: Germany
Member Is Offline
|
|
EP 2 679 567 A2
There is an european patent filed in 2012, but the information is pretty sparse.
Impact sensitivity greater than one Joule, friction sensitivity greater than 20 Newton, decomposition temperature 360 degree centigrade (sic!)
Detonation was observed with 200 mW @ 532 nm wavelenght.
The chromium (III) salt is even more thermally stable, but deflagrates only.
The synthesis is also described and easy, so I´ll give it a try next time.
Attachment: EP2679567A2 BTA.pdf (141kB)
This file has been downloaded 475 times
|
|
|
Mush
National Hazard
Posts: 641
Registered: 27-12-2008
Member Is Offline
Mood: No Mood
|
|
Recent Progress on Synthesis, Characterization, and Performance of Energetic Cocrystals: A Review
Molecules 2022, 27(15), 4775; https://doi.org/10.3390/molecules27154775
Abstract
In the niche area of energetic materials, a balance between energy and safety is extremely important. To address this “energy–safety
contradiction”, energetic cocrystals have been introduced. The investigation of the synthesis methods, characteristics, and efficacy of energetic
cocrystals is of the utmost importance for optimizing their design and development. This review covers (i) various synthesis methods for energetic
cocrystals; (ii) discusses their characteristics such as structural properties, detonation performance, sensitivity analysis, thermal properties, and
morphology mapping, along with other properties such as oxygen balance, solubility, and fluorescence; and (iii) performance with respect to energy
contents (detonation velocity and pressure) and sensitivity. This is followed by concluding remarks together with future perspectives.
Keywords:
energetic materials; cocrystallization; detonation performance; characterizations of ECCs
The Study of Co-Crystallization of Trinitrophenol (TNP) and Ammonium Nitrate (AN) As a Potential Method for Enhanced Stability
DOI: https://doi.org/10.51584/IJRIAS.2025.100500035
Received: 16 April 2025; Accepted: 28 April 2025; Published: 05 June 2025
ABSTRACT
This study explores the co-crystallization of trinitrophenol (TNP) and ammonium nitrate (AN) using a slow solvent evaporation method at a 1:1 molar
ratio. The co-crystal formation and its potential for improved explosive stability were investigated. Characterization techniques including
Fourier-Transform Infrared Spectroscopy (FTIR), X-ray Diffraction (XRD), and Differential Scanning Calorimetry (DSC) were employed. FTIR analysis
revealed new peaks corresponding to functional group interactions between TNP and AN, indicating co-crystal formation. XRD confirmed the presence of
new diffraction peaks not observed in the individual components, further supporting co-crystallization. DSC analysis demonstrated a significant shift
in thermal behaviour compared to TNP and AN. The co-crystal exhibited a glass transition, melting point, and decomposition temperature distinct from
the single components. These observations suggest interactions between TNP’s -OH groups and Ammonium NH4+ ions, leading to the formation of a more
stable ammonium picrate co-crystal. The altered thermal profile indicates a potential improvement in the co-crystal’s stability compared to the
individual explosives.
Synthesis of environmentally friendly energetic cocrystal derived from commodity
10.1039/d4cc04037f
Abstract
Ammonium nitrate (AN) is a green oxidizer in the field of energetic materials. However, hygroscopicity and phase transitions have prevented AN from
being put into practical use. To address these two drawbacks, a cocrystallization technique was applied to AN in this study. An AN/glycine (Gly)
cocrystal was newly prepared and characterized; both AN/Gly and AN/sarcosine exhibited decreased hygroscopicity and did not exhibit a phase
transition.
chemicals
Enhancement of the burning performance of ammonium nitrate via cocrystallization
Abstract
Ammonium nitrate (AN) is a low-cost oxidizer with a low environmental impact; however, its low burning rate limits its application. In this study, a
cocrystallization technique was used to enhance the burning performance of AN. An AN/4- amino-1,2,4-triazole (4ATA) cocrystal (molar ratio = 1:1) was
prepared, and its crystal structure was investigated using single-crystal X-ray diffraction. The friction sensitivity test proved to be sufficiently
safe for the treatment of the cocrystal. 5-Amino-1H-tetrazole/strontium nitrate was blended with the AN/4ATA cocrystal or with a simple mixture of AN
and 4ATA to evaluate the burning behavior using the deflagration test. The test results showed enhanced burning performance for the composition
containing the AN/4ATA cocrystal compared to that containing the mixture of AN and 4ATA. The hygroscopicity test revealed that cocrystallization
suppressed the hygroscopicity and also resulted in the phase stabilization of AN, as confirmed from sealed cell-differential scanning calorimetry
analysis.
"In our previous
studies, we prepared novel cocrystals of 1Htetrazole/
sodium perchlorate (SP), 1,2,4triazole/SP, 3amino1,2,4
triazole/SP, and 4amino1,2,4triazole (4ATA)/SP. All four
cocrystals showed higher burning performances than the
corresponding mixtures of parent materials 13)15). To the
best of our knowledge, the series of studies undertaken by
our research group are the only ones that focus on the effect
of cocrystallization on the burning performance of a
mixture of fuel and oxidizer."
Three Insensitive Energetic Co-crystalsof 1-Nitronaphthalene, with 2,4,6-Trinitrotoluene (TNT),2,4,6-Trinitrophenol (Picric Acid) and
D-MannitolHexanitrate (MHN)
Central European Journal of Energetic Materials, 2015, 12(1), 47-62
Abstract: Co-crystallization is proposed as an effective method to alter the physicochemical
properties of energetic materials, e.g. density, sensitivity and solubility.
As reported in this paper, it was found that 1-nitronaphthalene could form cocrystals
with TNT, picric acid and MHN in a 1:1 molecular ratio. The sensitivity
and thermal stability of the 1-nitronaphthalene co-crystals was greatly improved
compared with that of pure TNT, picric acid and MHN. In addition, the melting
points of TNT, picric acid and MHN were lowered through co-crystallization with
1-nitronaphthalene. The electrostatic potential surface of 1-nitronaphthalene,
calculated by the DFT method, showed that the electron-rich 1-nitronaphthalene
has a tendency to be a proton donor and to co-crystallize with other energetic
materials. The structures of the co-crystals of 1-nitronaphthalene with TNT and
picric acid were characterized by single crystal X-ray diffraction (SXRD). The
1-nitronaphthalene/MHN co-crystal was studied by powder X-ray diffraction
(PXRD), differential scanning calorimetry (DSC) and FTIR.
[Edited on 16-10-2025 by Mush]
|
|
|
Microtek
National Hazard
Posts: 979
Registered: 23-9-2002
Member Is Offline
Mood: No Mood
|
|
Recently I have been looking at furazan derivatives again. There are a number of procedures for diaminofurazan (DAF) from hydroxylamine hydrochloride
and glyoxal which does not require a pressure reactor. The dehydration/cyclization step is done either in a high boiling polar solvent such as
ethylene glycol, or in concentrated aqueous urea solution with reflux for 12 hours. I have not had much success with the EG processes, but I suspect
there is some additive in my EG that is the culprit. The H2O/urea system works fine but I have noticed a fairly large amount of white crystalline
sublimate that collects in the condenser.
This compound puzzles me. It is non-flammable, water soluble and does not melt on application of heat from either above or below but rather
sublimates. When heated from below on a piece of Al foil this creates a sort of Liedenfrost effect that makes it skate around on the foil without
melting.
I initially thought it might be hydroxylamine freebase, maybe as an adduct with water, but that doesn't track with the non-flammability.
Does anyone have an idea as to what it might be?
|
|
|
Axt
National Hazard
Posts: 966
Registered: 28-1-2003
Member Is Offline
Mood: No Mood
|
|
No idea, but you could check its pH in water, then see if it reduced AgNO3 solution. Or just throw it in a nitration bath and see what happens 
Is this regarding the dinitramino analogue of DNAF?
|
|
|
Axt
National Hazard
Posts: 966
Registered: 28-1-2003
Member Is Offline
Mood: No Mood
|
|
Just a thought, probably thinking too exotic. Ammonium carbonate would likely act like that.
|
|
|
Microtek
National Hazard
Posts: 979
Registered: 23-9-2002
Member Is Offline
Mood: No Mood
|
|
Ammonium carbonate is probably the most likely. It is a very substantial amount and may provide insight into why the yield is not so good for these
preparations (especially if calculated from hydroxylamine basis).
And, yes, I am considering nitrogen rich salts of furazan derivatives such as dinitraminofurazan or dinitraminoazoxyfurazan. I found a reference to
the coupling of DAF to DAAF using just Oxone rather than H2O2/H2SO4 that worked quite well, and since it should be fairly straight forward to nitrate
DAAF, it seemed natural to invetigate the salts.
|
|
|
Axt
National Hazard
Posts: 966
Registered: 28-1-2003
Member Is Offline
Mood: No Mood
|
|
TODO is another possibility. 4H-[1,2,3]triazolo[4,5-c][1,2,5]oxadiazole 5-oxide. d. 1.934 g/cm3, VOD 9250 m/s, DP 43.1 GPa free acid decomposes at 89C
though.
Supposedly DAF can be nitrated simply in 70% HNO3, involves a gay solvent extraction, but that's just with ethyl acetate.
From supporting info of ACS Appl. Energy Mater. 2020, 3, 9401−9407.
3,4-Dinitraminofurazan (6)
3,4-Diaminofurazan 5 (1 g, 10 mmol) was added in portions to a vigorously stirred 70% HNO3 (8 g, 5.6 mL, d = 1.42 g cm−3) at 25 °C. After that, the
reaction mixture was stirred at ambient temperature for 2 h (as the reaction progressed, 3,4-diaminofurazan was completely dissolved). The solution
was poured out into ice water (60 mL) and extracted with ethyl acetate (2 × 60 mL). The combined organic phases were washed with water (2 × 60 mL),
dried over magnesium sulfate and concentrated under reduced pressure without heating. The obtained product (1.4 g, 76%) was identical to the
3,4-dinitraminofurazan synthesized by Tang et al.17 and was used without further purification.
Potassium 5-oxido-[1,2,3]triazolo[4,5-c][1,2,5]oxadiazol-4-ide (2a)
3,4-Dinitraminofurazan 6 (1.9 g, 10 mmol) was added in portions to a vigorously stirred and cooled (15 °C) solution of 93% H2SO4 (1050 mg, 10 mmol, d
= 1.83 g·cm–3) in Ac2O (20 mL). After that, the reaction mixture was stirred for 30 min at ambient temperature. The solution was poured into
ice water (200 mL) and stirred for 30 min until Ac2O was completely hydrolyzed. Then AcOK (3 g, 30 mmol) was added in portions while stirring. The
solution was extracted with ethyl acetate (2 × 200 mL), and the combined organic extracts were washed with H2O (100 mL). Water fractions
S4 were combined, and water was evaporated in vacuo. Acetonitrile (100 ml) was added to the brown residue and the suspension was vigorously stirred
for 5 min. Then the precipitate (mainly inorganic salts) was filtered off. The solvent was evaporated in vacuo and the residue was recrystallized from
MeOH to give K salt 2a (1.05 g) identical to that described previously.1 The mother liquor was concentrated under reduced pressure and the crude
product was purified by flash chromatography (ethyl acetate/methanol, 5:1) to give an additional amount of the K salt as light yellow solid (200 mg).
Overall yield: 1.25 g (74%); 13C NMR (125.8 MHz, d6-DMSO): δ = 160.9 (С-3a, C-6a) ppm; 14N NMR (36.1 MHz, d6-DMSO): δ = –3 (N-5, ∆ν1/2 = 15
Hz), –20 (2N, N-1, N-3, ∆ν1/2 = 540 Hz), –129 (2N, N-4, N-6, ∆ν1/2 = 600 Hz) ppm; elemental analysis calcd (%) for C2KN5O2: C 14.55, H 0.00,
N 42.41; found C 14.83, H 0.00, N 42.15.
4H-[1,2,3]triazolo[4,5-c][1,2,5]oxadiazole 5-oxide (1)
To a suspension of K salt 2a (0.5 g, 3 mmol) in MeOH (10 mL) ion-exchange resin (Amberlite IR 120, H-form, 1.4 g) was added and the mixture was
vigorously stirred for 2 h at room temperature. The ion-exchange resin was filtered off and the solvent was evaporated in vacuo. Diethyl ether (20
mL) was added to the residue. The white solid that formed was filtered off and washed with diethyl ether (5 mL). The filtrate was concentrated under
reduced pressure to give pale beige viscous oil that crystallized in a few hours. Yield: 362 mg (95%); light beige solid; m.p. 89 °C (decomp.); 13C
NMR (150.9 MHz, d6-DMSO): δ 160.9 (С-3a, C-6a) ppm; 14N NMR (43.4 MHz, d6-DMSO): δ = –5 (N-5, ∆ν1/2 = 13 Hz), –20 (2N, N-1, N-3, ∆ν1/2 =
275 Hz), –121 (2N, N-4, N-6, ∆ν1/2 = 300 Hz) ppm; 13C NMR (125.8 MHz, d6-acetone): δ = 155.2 (С-3a, C-6a) ppm; 14N NMR (36.1 MHz, d6
acetone): δ = –5 (2N, N-1, N-3, ∆ν1/2 = 615 Hz), –38 (N-5, ∆ν1/2 = 50 Hz), –150 (2N, N-4, N-6, ∆ν1/2 = 600 Hz) ppm; IR (KBr): ν˜
1092, 1337, 1466, 1500, 3057 cm-1; MS (EI, 70 eV) m/z : 97 [M-NO]+, 83 [M-N2O]+; HRMS (ESI) m/z [M-H]– calcd for C2HN5O2: 126.0047, found: 126.0050;
elemental analysis calcd (%) for C2HN5O2: C 18.91, H 0.79, N 55.12; found C 19.17, H 0.73, N 53.41.
|
|
|
Microtek
National Hazard
Posts: 979
Registered: 23-9-2002
Member Is Offline
Mood: No Mood
|
|
I found a chinese (!) paper about new methods of preparing DAF (https://www.energetic-materials.org.cn/hnclen/article/abstra...). The full-text is publicly available, but in chinese. Here is an AI-translated
excerpt. Beware of potential translation errors:
"2.2.1 Preparation of Supported Solid Base Catalyst
The activated carbon support was boiled in 30% nitric acid at 90 °C for 4 hours, washed with water until neutral, and dried. Then, 100 g of activated
carbon was immersed in a potassium hydroxide solution overnight. The moisture was evaporated to dryness using a rotary evaporator. Under nitrogen
protection, the sample was dried at 130 °C for 2 hours, then calcined by raising the temperature to 500 °C and holding for 4 hours to obtain the
supported solid base catalyst. The KOH loading was 5% (mass fraction).
2.2.2 Synthesis of 3,4-Diaminofurazan Under Supported Solid Base Catalysis
15 g of 3,4-diaminoethanedioxime was dissolved in 187.5 g of distilled water and transferred into an autoclave. Then, 52.5 g of the supported solid
base catalyst was added. After purging the air in the system with nitrogen, the autoclave was sealed and heated to 150 °C for 4 hours. The pressure
change inside the autoclave was recorded.
After completion of the reaction, the mother liquor was allowed to cool naturally to room temperature, where a white solid precipitated. The solid was
filtered and washed with water to obtain the product, with a yield of 91.2%.
m.p.: 179–180 °C.
IR (KBr, cm⁻¹): 3435, 3322 (—NH₂), 1646, 1589 (C—NH—O).
¹H NMR (DMSO): δ 5.8 (4H, NH₂)."
If true, this would be a sufficiently high yield that DAF-based materials could become interesting from more than an academic perspective.
[Edited on 2-12-2025 by Microtek]
|
|
|
Axt
National Hazard
Posts: 966
Registered: 28-1-2003
Member Is Offline
Mood: No Mood
|
|
I had some DAF from ages ago, so I treated 1 gram with TCCA in acetonitrile (1:2 molar eq. in 50 mL solutions). This is the literature route to the
bicyclic "difurazanotetrazocine", so 2 furazan rings joined through two azo bridges. I mistakenly added the TCCA slowly to the DAF whereas as
published it should be done the other way around, this may be important.
The lit runs a 2hr soxhlet extraction with hexane, this sounds like a pain in the arse so I just evaporated the acetonitrile and digested the remains
with NaOH/water and filtered the orange suspension. It seems to have worked.
You have to be careful with this stuff, it flashes violently on ignition, a fair comparison on the vehemicity scale would liken it to NHN or
dinitrobenzenediazonium perchlorate. It detonates easily and strongly under the hammer and when briskly rubbed with the hammer on rusty steel. I
wouldn't be surprised if C4N8O2 has initiating properties.
Testing the mp it was way off, lit gives 54C mine kind of beads up a bit at 100C then more major melting at over 200C. This may be the result of
adding the TCCA to DAF instead of DAF to TCCA. May also be because I didn't extract it with hexane. I checked the lit for higher oligomers and found
the props for the tetramer and its mp was 212C.
Both the dimer and tetramer have similar densities and heats of formation thus would be expected to have similar detonation properties. The tetramer
has published values of 8550m/s and 31.9GPa. No sensitivity data for the tetramer but the dimer is 4 cm with 2.5 kg weight where HMX was 25 cm.
[Edited on 10-12-2025 by Axt]
|
|
|
Microtek
National Hazard
Posts: 979
Registered: 23-9-2002
Member Is Offline
Mood: No Mood
|
|
It might also form polymers and I wouldn't be surprised if the higher homologues were favoured when an excess of DAF was present. Regardless, the
potential for a metal free primary is interesting. I might have to look into that. At the moment I'm building a proper pressure reactor to see if I
can make the above referenced procedure work. While the reported yields are not that much higher ( ca. 50% vs ca. 70 % total from glyoxal), the major
expense is the hydroxylamine which is usually used in large excess such as 10 equivalents when doing the one-pot synthesis.
Another possibility is to perform the dehydration of DAG without solvent (https://revues.imist.ma/index.php/morjchem/article/view/7392). This gives a melt that solidifies on cooling and must then be worked up to remove
impurities. Reported yields are around 70 %. I tried it one a 1 gram scale and got around 50%, though I didn't use nearly as much ethyl acetate as the
authors. I suppose Soxhlet extraction would be a viable way to conserve solvent.
|
|
|
Axt
National Hazard
Posts: 966
Registered: 28-1-2003
Member Is Offline
Mood: No Mood
|
|
Have you entertained the thought of the microwave preparation:
One pot synthesis of DAF from glyoxime: An aqueous solution
of sodium hydroxide (100 ml 7.5 M) was added to glyoxime
(17.6 g, 0.2 mol) and mixture was kept under stirring. Subsequently,
hydroxylamine hydrochloride (27.8 g, 0.4 mol) was added, and
the contents were irradiated in the microwave oven at the power of
300 W for 2–3 min. During this period, a break of 30 s was given
when the reaction mixture started boiling. The flask was taken out of
the microwave oven after 3 min when the vigorous reaction started.
The reaction was allowed to subside at room temperature.
The reaction mixture was further irradiated in microwave oven for
30 min with a break of 30 s, whenever required (see above), using a
power of 800 W and was cooled to get a solid product. After washing
with water, DAF (14g, 70 %) was isolated.
It's out of India and half the stuff out of India is retarded but it looks plausible, its written descriptively not vaguely. It's from the paper
"Microwave mediated fast synthesis of diaminoglyoxime and 3,4-diaminofurazan: key synthons for the synthesis of high energy density materials". 2005.
I've never tried it. The only "microwave mediated" prep I've tried was sulphanilic acid via microwaving aniline and sulphuric acid which went
surprisingly well. I've also tried microwaving ethylene glycol with urea for ethyleneurea but this was a total failure.
|
|
|
Axt
National Hazard
Posts: 966
Registered: 28-1-2003
Member Is Offline
Mood: No Mood
|
|
Difurazanotetrazocine (DFT), 40 mg in a single layer of foil was negative to DDT, just flashed with a pop.
100 mg of DFT lightly pressed over 600 mg hand pressed PETN was positive with full detonation. Below compares the DFT initiated charge with a
commercial #8. The #8 should be around 800 mg PETN with ASA primary and reinforcing cap.
|
|
|
Microtek
National Hazard
Posts: 979
Registered: 23-9-2002
Member Is Offline
Mood: No Mood
|
|
I tried that exact preparation many years ago but found that once the mixture started boiling, cooling for 30 s at room temp removed so little heat
from the mix that it started boiling again in a matter of seconds when replaced in the oven. That means you will have to babysit the reaction for
maybe 4-6 hours. Perhaps if more heat can be removed during the cooling intervals such as with a water bath, it might be workable.
DFT seems very interesting, I think I have to experiment with it myself.
|
|
|
Axt
National Hazard
Posts: 966
Registered: 28-1-2003
Member Is Offline
Mood: No Mood
|
|
Yeh I got to reading the old furazan pre-pub thread https://www.sciencemadness.org/talk/viewthread.php?tid=5813 I don't remember doing any of it, being 18 years old, but I mention the same result of
the microwave prep as you. It just boils the instant power is reapplied. I guess you could run it slowly on defrost mode (so auto intermittent mode)
and run it to dry and extract the result. I even seem to have had some obsession with DFT back then (I have a fetish for small symmetric molecules,
they are pretty) but it was never tried. There was no mention of it being an actual primary explosive.
I think it would be worth trying adding DAF to sodium dichloroisocyanurate in water instead of TCCA in acetonitrile similar to the azotriazole
reaction on route to BLG-1. The TCCA reaction is very easy but avoiding the need for acetonitrile would be great.
|
|
|
Microtek
National Hazard
Posts: 979
Registered: 23-9-2002
Member Is Offline
Mood: No Mood
|
|
Another possibility might be using Oxone for the oxidative coupling, though it might give DAAF instead. I don't know if the azoxy version of DFT would
be stable enough to exist, but this might also be a possibility.
|
|
|
Axt
National Hazard
Posts: 966
Registered: 28-1-2003
Member Is Offline
Mood: No Mood
|
|
Yeh I did stir some DAF in oxone and received a high yield of DAAF, it will respond with a weak snap to a very strong hammer blow. The reduced azo
(non-oxy) bridged compound is meant to be just as insensitive. I've been trying to find reference to the sensitivity of the larger azofurazan
macrocycles but have not found anything. I'll attach the article on DFT that mentions its sensitivity. I referred to this back in the 19yo thread but
mentioned it's too old to be available online, its online now.
"DFT is a dangerous primary explosive with a drop height of approximately 4 cm (2.5 kg. Type 12, HMX=25 cm). We believe the sensitivity is due to the
boat configuration as the azo-group's n-electrons are orthogonal to the x-electrons in the furazan rings, and thus no stabilization through
delocalization can occur."
They do refer to an attempt at oxidising the DFT to azoxy but received only a low yield of monoazoxy compound and gave up. I have seen reference to
oxidation of the tetramer to tetraazoxy yes very dense very powerful but it required oleum/persulphate ie. super Caro's acid.
I tried sodium dichlorisocyanurate (1.2 g DAF, 10.2 g SDCIC, 10. g 90% acetic acid / molar ratio 1:4:16) It turns orange instantly but left stirred
for an hour then digested with 12 g NaOH whereby the solution turned dark brown. Filtering this leaves the same orange highly sensitive DFT. Its
annoyingly fine and difficult to filter, I digested my filter paper with NaOH in the process.
[Edited on 13-12-2025 by Axt]
Attachment: azo, azoxyfurazans and difurazanotetrazocine (TCCA oxidation).pdf (648kB)
This file has been downloaded 15 times
|
|
|
| Pages:
1
..
21
22
23 |
|
![[*]](images/xpblue/default_icon.gif){kind=icon}
