Sodium Azide

Why bother

If you can get to a junkyard then you don't have to bother making NaN3. Airbags have upto 100g of NaN3 in tablet form with added Fe2O3 and SiO2. These can be removed right before use by filteration. Actually some airbags did come out with RDX/AN mix, but I think it was discontinued due to the hygroscopic nature of AN. The NaN3 is encased in an Al case with gas vents to inflate the airbag. I don't think the Al case can be unscrewed easily ..... it can also be sawed but it has to be kept cool by some sort of a solvent.
Happy Aziding.

I know about the NTO topic on the E&W, I started it
It did sound like he got a good yield, although urea*HCl would also ppte if unreacted urea was present, so determining the purity of the product may be difficult.
I found a lot of methods for making semicarbazide*HCl, some of which I found patents for and posted them in "Links and Literature" on the E&W, and the one with urea is definitely the nicest. Actually, I suppose that method is even nicer if you have something like .880 ammonia solution and a pressure vessel, but since I don't have either I'd have to bubble through a massive excess of ammonia gas, either directly into the solution or into water to make an ammonia solution that could be added, and I hate working with lots of ammonia gas!
If using hydrazine, it can be stored as the sulphate or hydrochloride, and made into a solution of precisely known concentration by adding aq. NaOH. Sulphate and chloride ions might be a problem in some reactions (such as making silver or lead azides), in which case the nitrate is prepared from the sulphate using Ca(NO3)2.
I don't have any specifics for making azides from semicarbazide, I think I heard that it was possible on the Org Syn website, but they gave no details. I'm not sure if it needs a nitrite ester or not... if it could be done with NaNO2 in neutral/basic solution then it would be very good...

I haven't tried this but.....

here it is anyway.
Manganese Heptoxide
Author: Exxperts
Materials: potassium permanganate (KMnO4), sulfuric acid 92-96%
Procedure: Place 5g powdered potassium permanganate in a small beaker. To this add 5ml concentrated sulfuric acid. Gently swirl the mixture to blend the components. If unreacted permanganate remains in the bottom, add more H2SO4. Do not filter! A dark green oily liquid will have formed. This is manganese(VII) heptoxide (Mn2O7), a powerful oxidizer. It ignites almost every organic compound. Alternatively, the process can be reversed: Mix KMnO4 with an organic compound and add a few drops of conc. sulfuric acid to ignite. Some experiments to do with it: Wear a face shield and leather gloves. Twist a wad of cotton around a wooden splint, immerse this in the liquid and take it out immediately. The cotton will start burning in 1-5 seconds. Place any organic compound (sugar, flour, starch, pieces of wood, hay, paper, styrofoam...) on a fireproof surface, by addition of a few drops of Mn2O7 these will catch on fire. Flammable liquids (ethanol, gas, acetone, toluene, paint thinner...) can be lit in a similar fashion.
WARNING: Pour the flammables out in a thin layer in an open area! Never mix Mn2O7 with a liquid like acetone in a test tube or similar vessel. The mixture may be ejected violently or even explode! Never mix Mn2O7 with powdered metals, the mix will explode and unreacted Mn2O7 along with excess acid will spray in all directions!

Properties: Dark green to greenish black oily liquid. Soluble in water and sulfuric acid. Decomposes at 55°C, may explode at a slightly higher temperature, or on prolonged storage.

Barium Peroxide

Preparation: Prepare a solution of 47g of barium chloride dihydrate in 250ml water. To this solution add 250ml 30% H2O2. Add 200ml 24% aqueous ammonia solution with stirring. Let the mixture stand until no more precipitate forms. Decant the clear portion, and replace the liquid with fresh water. Repeat the decanting 2-3 times. Filter on a Buchner funnel and wash with water. Dry in a porcelain cup at 50-70°C, occasionally spreading the powder with a spatula. After the product turns into a crumbly mass, increase the temperature to 75-80°C. Store the completely dried product in a tightly sealed bottle. Yield: 55-60g of the octahydrate. The product can be further dried to the hemihydrate at 130°C. The completely anhydrous peroxide can be obtained above 200°C, but a partial loss of oxygen will occur.
Carbamide Peroxide
Author: Lagen
Using a mortar and pestle, crush 20g urea into a powder. Place this in a shallow pyrex dish and add, with stirring, 35ml of a 30% hydrogen peroxide solution. The resulting mixture should have a dough consistency. Stir in 1.5g of powdered gelatine. Let the mixture stand for 5 hours, it will solidify, forming the carbamide peroxide. Uses: In smoke compositions. Mixtures with sodium dithionite are impact sensitive.
Magnetite

Preparation: Dissolve 25 g of iron(II) sulfate heptahydrate (green vitriol) and 25 g of iron(III) (ferric) sulfate nonahydrate in 500 ml water. Add this solution to 1 liter of boiling 5% KOH solution. Filter out the precipitate, wash with hot water and remove excess moisture on a Buchner funnel. Dry in a hydrogen atmosphere over CaCl2 or conc. H2SO4. This way the dihydrate is obtained. Calcine at 300-400°C in a nitrogen atmosphere to obtain the anhydrous product.
Properties: Fe3O4, magnetite can be used instead of iron(III) oxide in thermite mixtures, to get a higher temperature. An alternative process exists, starting by precipitating Fe(OH)2 from a soluble Fe(II) salt and calcining this at 800°C, but I don't have the details.

Pyrophoric Iron
Author: Maty
Materials: oxalic acid dihydrate 20g, iron sulfate heptahydrate 44g, distilled water
Equipment: a larger heat resistant test tube, 250ml and 500ml beaker, glass rod, heat source
Procedure: Place 20g of oxalic acid and 200ml distilled water into the 500ml beaker. Distilled water is necessary, tapwater contains cations that combine with the oxalic acid to form unsoluble precipitates. Boil the solution with stirring until the oxalic acid dissolves. In another 250ml beaker dissolve 44g of iron sulfate in 200ml boiling water. Pour the iron sulfate solution into the oxalic acid solution, with stirring. A fine yellow precipitate of iron oxalate should form. Filter out the precipitate and thoroughly wash with water on the filter (sulfuric acid will have formed in the precipitate and needs to be removed). Dry the powder in a warm place, avoid too much heat. Crush the dried powder to flour consistency. Place the powder in the heat resistant tube and gently heat the tube, continue the heating until all the powder turns black. If necessary, carefully stir the powder. Warning: The black powder that has formed is pyrophoric, which means it will spontaneously ignite in air, if hot. It gives off nice yellow sparks.
Properties: You can use this powder in pyrotechny to create yellow sparks, in self-igniting mixes as well as in the production of iron sulfide. A similar procedure can be used to produce powdered copper (colours flame green).

Pyrophoric Lead
Author: Oktogen
Prepare a solution of 2g lead acetate in water and acidify it with a few drops of acetic acid. To this solution add a stoichiometric amount of tartaric acid or primary potassium tartrate (in the form of a 5% solution) in several portions, with stirring. Filter the white precipitate at reduced pressure and wash on the filter with water. Dry at 110°C. Spread out the dry material in the lower section of a specially modified test tube.
(Hold an ordinary test tube with a metal clamp and heat in a burner flame about 3cm below its mouth. Keep rotating the tube along its axis. After the glass had softened, stretch out the tube so that the neck shrinks to about 3mm diameter. After cooling make a dent in the narrow section with a file and break it apart.)

Fix the tube in a stand in a tilted position. Heat the tube evenly. After the decomposition of the lead tartrate had ceased and all the water vapour and other decomposition products had escaped, take away the tube and pour out the pyrophoric lead onto a fireproof surface. Alternatively, you could carefully fuse the tapered neck of the tube to preserve the material for later use.

Sulfur

Preparation: Dissolve 25 g of sodium thiosulfate (photographic hypo) in 83 ml of 25% acetic acid. Heat the mixture gently until the evolution of gas stops. Let the mixture stand for a day. Carefully decant the liquid portion, wash the precipitate with water to a neutral reaction. Filter on a Buchner funnel, moisten the product with acetone and dry at room temperature. Yield: 3 g of colloidal sulfur.
Potassium Nitrosocarbaminate
Author: Lagen
Procedure: Place 38 ml of methanol in a 100 ml beaker. Add 10 g of dry potassium hydroxide, in several small portions and with stirring. Wait for each portion to dissolve, then let the solution cool down. Pour off some of the resulting solution in another container, keep approx. 30 ml of solution in the beaker. Place the beaker in a salted ice bath. In another container liquefy 1g of nitrosourethane with a few drops of methanol and add 4 ml distilled water. Add the solution in one portion into the potassium hydroxide solution and let it react for 10 minutes. If nothing precipitates, add 5 ml of the spare potassium hydroxide solution and wait for another 10 minutes, then add the remainder of the KOH solution. Let the mixture stand for one hour, keep replacing the ice bath if it melts. Quickly vacuum filter the precipitate, wash several times with absolute alcohol and place immediately in a desiccator. Try to avoid unnecessary contact of the product with moist air. Yield: approx. 1 g of a pale yellow powder.
Properties: Potassium nitrosocarbaminate - NONKCOOK. Very sensitive. Detonates violently, even in small amounts, on contact with water or sulfuric acid. May detonate at slightly elevated temperatures (below 100°C). Decomposes in the presence of moisture. It can be temporarily rendered nonexplosive by the addition of ether followed by addition of alcohol. When treated in this way it can be decomposed safely by water or H2SO4.

Triaminotrinitrobenzene (TATB)
Author: Exxperts
Precursors: The 1,3,5-trichloro-benzene necessary for this synthesis may be prepared by direct chlorination of benzene using iron filings as catalyst, or more conveniently, by halogenation of aniline, removing the amino group by diazotization and boiling in ethanol.
Nitration: Into a suitable flask immersed in an oil bath place 220ml conc. H2SO4 and add 51g NaNO3. Heat the mixture to 100°C with constant stirring and hold the temperature for 20 mins. This will cause the decomposition of the nitrate by H2SO4 to form free and almost anhydrous HNO3. The H2SO4/HNO3 nitrating mix also helps to greatly reduce the destructive oxidation processes occuring in the aromatic ring during high temperature nitration.

Following that add 20g of 1,3,5-trichloro-benzene into the nitrating mix and increase the temperature to 145-155°C. A high temperature is necessary in order to completely nitrate the TCB. The temp. must be maintained close to 150°C for 4 hours, after that the mixture is allowed to cool to room temperature and then poured into a container with 800g of crushed ice. TCTNB will fall out in the form of heavy yellow crystals. The crystals are filtered out and washed with water to a pH of 6-7. Dry thoroughly at 40-60°C.

Amination: 20g of the dry TCTNB is dissolved in 150ml toluene at 90°C. Gaseous ammonia is bubbled through the solution over a period of 2 hours (the temperature is maintained at 90°C). The amount of ammonia used should be 150% of the theoretical. After the amination is completed, the redundant toluene is distilled off (either on its own or with the addition of a small amount of water to form an azeotrope). The resulting TATB (beautiful yellow crystals) is washed with 60°C water several times and dried. Yield: 13.5g TATB (95% theory).

Ethyl Nitrate without distillation
Author: Fly
Procedure: Prepare a nitrating mix using 260 ml 65% HNO3 and 300 ml 96% H2SO4. Slowly add the H2SO4 to the HNO3 with cooling and constant stirring. Let the nitrating mix cool down to 0°C in a refrigerator. In another container place 160 ml of pure ethyl alcohol and slowly add 16 ml 96% H2SO4 with cooling and stirring. Let this mix cool down to 0°C as well. Prepare a salted ice bath and place a 1L or larger beaker in it. Pour the cold nitrating mix into the beaker, place a thermometer in it and begin the addition of the cold ethanol mix. Keep stirring the mixture, adjust the rate of addition so that the temperature stays around 5°C, do not allow the temperature to rise above 10°C. When the addition is complete, continue stirring the mixture for another 5 mins. Transfer the mixture into a separatory funnel and let it stand for 15 mins. The crude ethyl nitrate should separate out, drain the acid portion. The separation should not be carried out for more than 15 mins., after that the product might start oxidizing. The crude ethyl nitrate is washed by 300 ml of cold water (shake the mixture thoroughly in a plastic bottle). Repeat the separation and wash the product again with 300 ml water, then add a small amount of NH3 solution to the mixture and shake it again. Repeat the NH3 addition until the solution is pH neutral. Repeat the separation and washing steps, check that the product is clear and colorless. Now the product can be finally separated, dried over CaCl2 and filtered. The product obtained in this way should not be stored.
Ethylenediamine dinitrate (EDDN)
Author: Locker
Procedure: Into a 750 ml beaker immersed in a salted ice bath (ice+NaCl or ice+NH4NO3) place 40 ml distilled water and slowly add 100 ml ethylenediamine. As the ethylenediamine used here is a strong base, this addition will produce a lot of heat, and the temperature may rise to approx. 70°C. Add a little water to the ice bath and let the solution cool down below 0°C. In the meantime, into another 500 ml beaker immersed in water and cracked ice place 200 ml of 65% HNO3 and allow it to cool.
When the ethylenediamine solution has cooled down, begin the slow addition of the nitric acid, with continuous stirring. Do not allow the temperature to rise above 25°C. Although an explosion is not likely, when large amounts of the two solutions come into contact, the reaction mixture could start boiling and possibly be ejected from the container.

At first the reaction will be rather violent with each small addition, but will calm down later. As soon as there are no obvious symptoms of a reaction with the addition of acid, start monitoring the pH of the mixture. Stop the additions when the pH is in the range of 5-5.5. If the pH is higher, the product will have a tendency to decompose, if it is too low, the product will be difficult to dry and may decompose as well. Stir the mixture for a few minutes. If any product crystallizes change the ice bath for a heated water bath and wait for the product to redissolve.

Pour the contents of the beaker into a shallow aluminum or enameled tray and place it in an oven, maintain the temperature at 60-70°C. The evaporation should take 6-7 hours. The product will resemble ammonium nitrate crystals in appearance. To speed up the evaporation, stir the solution ocassionally. Collect the dried product and store it in an airtight bottle (f.ex. a soda PET bottle), it is hygroscopic. Yield: 260-270g

Acetone Semicarbazone
Author: Lagen
Precursors: Zinc can be crushed to a powder at a temperature above 210°C. Battery cathodes, cleaned from MnO2, are a good improvised source. Synthesis of nitrourea is well known and can be found at many other web sites.
Place 455 ml of 31% hydrochloric acid in a suitable container and let it cool down to below 0°C in a refrigerator. Stir in 45 g of powdered nitrourea and return the solution to the refrigerator. Place 150g of zinc powder in a 800 ml beaker and add 80ml water. Place the beaker in a salted ice bath and cool the mixture to 0°C. Insert a magnetic or mechanical stirrer and start stirring the mixture. Begin the addition of the nitrourea solution; keep the additions small, especially at the beginning. The temperature should be kept below 0°C; replace the ice bath if necessary. Turn off the stirrer, let the mixture sediment and decant the liquid portion through a filter. Add 40g anhydrous sodium acetate to the filtrate and let it dissolve. Saturate the solution with sodium chloride (approx. 140g), then add 26 ml acetone. Allow the mixture to react in an ice bath for several hours. A precipitate of acetone semicarbazone addition compound with zinc chloride will form. Filter out the precipitate and wash with cold saturated sodium chloride solution, then with ice cold water. Dry the powder in an oven; the temperature should not exceed 100°C.

Place 30 g of the dried powder in a 250 ml beaker and add 70 ml of a 24% ammonia solution. Allow to react for 30 minutes, then filter out the product. Wash with a small amount of ice cold water and dry in an oven at a low temperature. Yield: 20-27g, using all of the addition product from the first stage.

Notes and Discussion: Acetone semicarbazone may be converted to semicarbazide nitrate or sulfate (see on this page) with the concentrated acids. These salts can be used for preparation of triazolone, a precursor to nitrotriazolone (NTO). Compared to the conventional synthesis using semicarbazide hydrochloride, this offers the advantage of low chloride content in the triazolone, which is beneficial for nitrotriazolone synthesis. Even more conveniently, the acetone semicarbazone can be used directly in the preparation of triazolone. See US patents # 4,927,940 and 4,999,434 for more info.

Zinc can be recycled from the waste filtrate produced in the second step. Other ways of preparing semicarbazide or its precursors exist (f.ex. reduction of nitrourea with molecular hydrogen at superatmospheric pressures in the presence of a rhodium catalyst), but this one is the most convenient for the home chemist. It does not use the toxic and carcinogenic hydrazine nor compounds thereof, and requires only very simple equipment.

Semicarbazide Sulfate
Author: Lagen
Preparation: Add 10 g acetone semicarbazone in 10 ml of 96% sulfuric acid, heat the solution gently until the powder dissolves. Allow the solution to cool and pour into 100 ml of absolute ethanol. Filter out the precipitate and crystallize from warm water.
Properties: Semicarbazide sulfate - NH2CONHNH2.H2SO4, very soluble in water, insoluble in ethanol. Large prisms, m.p. 144°C. Decomposes above 120°C, yielding mostly hydrazodicarbonamide and hydrazine sulfate. Useful for preparing triazolone, see also acetone semicarbazone.
Hope this helps

Damn ......

substitution

Ahhhhhhhh

to produce sodium azide, firstly created a mixture of NaOH and pure ammonia solution. Nextly, bubble through this N2O (gas from the whip cream container)
NH3 + N2O --> HN3 + H2O
HN3 + NaOH --> NaN3 + H2O
Indeed...
Finaly, crystalize the deadly and volatile NaN3.

Azines

In post #9 here:
http://64.233.179.104/search?q=cache:_LsyWqTz_-0J:www.roguesci.org/theforum/showthread.php%3Fthreadid%3D948+%22sodium+azide+synthesis%22&hl=en
(I have to use the Google cache as I'm not a member of the site and it asks me to login when trying to access the page)
Microtek mentions some chem.pdf file containing hydrazine and sodium azide synthesis (the post that starts with "Yes it is nitrIte, and note that if you are going to use the hydrazine to make azide, you don't need to distill.".

Would someone that has access to this pdf kindly post the file, or at least quote the procedure here? Thank you in advance.

[Edited on 19-4-2005 by Quince]

I know this is not OT in that it's not chemistry per se' but it won't last forever as a method of collecting chems. People talk about this but never give details; so I thought I would add this last bit to this thread.
As a total aside the simple method of gathering azide from an automobile is to access most any American made car from 1993-2000. They appear to have the largest amount of azide pellets in the air-bag gas generator. The gas generator is installed as a unit in most that I have seen so if you pull one you get the whole thing, the bag, the gas generator, everything. At a junk yard they will charge you about $5-30 depending upon the model due to the difficulty in pulling them. There are junk yards that pull them all the time due to an interesting fact. Side-mounted air bags blow when poolry trained locksmiths try to gain access to the car. You just can't go poking around in the door anymore to try to open the car; you'll pop the air bag.
So anyway, you can find the units for a low overall cost and some of them have a "screen" -like affair where the pellets are; you simply cut into the screen and retrieve the pellets. Others have a sheet-metal grill with is tougher. You need tin-snips of a quality made for heavy sheet metal work and it's fast going. - With no exageration you should be able to get a 500 gram bottle filled with not too much work.
I recrystalized the pellets using hot distilled water and the product I ended with was just fine, clean and white. - the largest single unit was from a dressed up "Eddy Bower" Ford Bronco with about 250 gr. in each. If you want to U2U me about details on this issue feel free; I'm done collecting and frankly there is SO much out there I can't see this creating a run on the junk yards

Quote: Originally posted by zha ke xue

First,I want to say ,although we are from PRC ,but we are not commie . Then, Hua Xue DIY and zha ke xue is not one .We are against to the govement of PRC.

Quote: Originally posted by quicksilver

Quote: Originally posted by zha ke xue   First,I want to say ,although we are from PRC ,but we are not commie . Then, Hua Xue DIY and zha ke xue is not one .We are against to the govement of PRC. You are most welcome just as any other contributor here. I am sure that the Moderators feel that as do the overwhelming majority of principled individuals here. ______________________________________ The price of chemicals in the PRC and MANY places unfortunately reflects cost savings at the expense of the citizen's land & environment. But generally many companies in the EU and USA inflate prices beyond all reason - simply greed.

^Bravery?! It is China not North Korea!

[Edited on 19-12-2009 by sonogashira]

China,the humanitarian state!?

Ah yes,my mistake! China is the very humanitarian state that censors all aspects of life and responsible for tienamen Square ANd roving execution vans that harvests innmates organs upon execution according to need for foriegn transplants.Yes that paragon of human rights state known as China ,Those brave souls. Unles your a resident of NK I would cease and desist Sonongashira.. Hmm sonagashira,sounds japanese, the superior race of the asian east if not the world.I wondered where the superior attitude came from.



[Edited on 16-1-2010 by grndpndr]

Sir, I can only assume that you are drunk judging by this and the very rude U2U you sent me.

I'm sure it is accepted where you live to hold such narrow-minded opinions, but fortunately the rest of the world is not so impoverished in their outlook. It is up to you if you are willing to believe such bullshit propaganda, but please do not state it as fact. The thousands of Chinese students in your country demonstrates the stupidity of your claims.

You are wrong in your assumptions - but I need not wonder where your superior (and ignorant) attitude comes from! God bless you, God Bless America, God Bless the War on Terror

I sincerely hope that you are met with greater success in your future quest for knowledge.

Quote: Originally posted by grndpndr

Ah yes,my mistake! China is the very humanitarian state that censors all aspects of life and responsible for tienamen Square ANd roving execution vans that harvests innmates organs upon execution according to need for foriegn transplants.Yes that paragon of human rights state known as China ,Those brave souls. Unles your a resident of NK I would cease and desist Sonongashira.. Hmm sonagashira,sounds japanese, the superior race of the asian east if not the world.I wondered where the superior attitude came from. [Edited on 16-1-2010 by grndpndr]

Chemistry is regardless of national boundaries。I hope that we will not mind if we are Chinese。As we all love chemistry。

Added:We are here to learn


[Edited on 23-2-2010 by hua xue DIY]

Quote: Originally posted by roXefeller

Sodium azide is extremely toxic. Providing an exact preparation, as asked, when you could find it yourself, is pretty reckless. I get a little spasm in the posterior just thinking of opening a bottle of sodium azide. [...]rquote]Yes, sodium azide is quite toxic, but if you fear opening a bottle of it, then I think it is a good moment to reconsider having chemistry as a hobby. Chemicals need to be treated with respect, but fear is a very bad guide. Sodium azide actually is quite easy on storage. It is not strongly hygroscopic and it does not give off vapors of HN3 when kept dry. I have a sample, which (I discovered later) was kept in a badly sealed bottle, but even after a few years of storage, the NaN3 still is perfectly fine. Many other chemicals would have been totally spoilt after even just a few months of storage in that same badly sealed bottle.

Thanks for tangenting my original warning of sodium azide toxicity into the mockery of a (overly) cautious man. Hopefully you won't downplay the warning into nothing more than voices in my head.

Quote: Originally posted by Polverone

Quote: Obviously the ammonium chloride is going to react with sodium hypochlorite to liberate chlorine gas. In that case, I'd be a bit wary; ammonium salts plus Cl2 will produce nitrogen trichloride. I've experienced a hideous scent and some violent popping before when mixing ammonium salts and calcium hypochlorite.

Quote: Originally posted by Tetra

Quote: Originally posted by Polverone   Quote: Obviously the ammonium chloride is going to react with sodium hypochlorite to liberate chlorine gas. In that case, I'd be a bit wary; ammonium salts plus Cl2 will produce nitrogen trichloride. I've experienced a hideous scent and some violent popping before when mixing ammonium salts and calcium hypochlorite. Sounds like fun.

I concur. A wonderful way to pass a late summer afternoon. Be sure to do micro amounts and stay upwind!

Quote: Originally posted by uchiacon

Hey guys, I was just thinking about whether or not I should make the hydrazine hydrate or purchase it, which is an option to me. For 250g of hydrazine hydrate, it'd be $50 or about $40USD. I don't have copper/silver/teflon coated labware, and I know the HS and NaOH reaction will eat away at glass due to the amount of hydrazine hydrate formed. Presuming that this hydrazine hydrate is of a relatively high concentration, do you think that it's just better for me to purchase the material?

Quote: Originally posted by grndpndr

Ah yes,my mistake! China is the very humanitarian state that censors all aspects of life and responsible for tienamen Square ANd roving execution vans that harvests innmates organs upon execution according to need for foriegn transplants.Yes that paragon of human rights state known as China ,Those brave souls. Unles your a resident of NK I would cease and desist Sonongashira.. Hmm sonagashira,sounds japanese, the superior race of the asian east if not the world.I wondered where the superior attitude came from. [Edited on 16-1-2010 by grndpndr]

From Sodium Azide to Chinese internet censorship.
Only on ScienceMadness.

Quote: Originally posted by Cheddite Cheese

Huh? I thought that sodium amide was reacted with nitrous oxide, not hydrazine.

Quote: Originally posted by Thraxx

In the year 2004 there was in an discussion told ,that the sodium azide could be manufactured through easy reaction between Hydrazin sulfate,Sodium nitrite and Barium hydroxid. Reaction: N2H6SO4(aq) + NaNO2(aq) + BaO2H2(s) -----> NaN3(aq) + BaSO4(s) + 4H2O(l) 130(2,86/100/OC) + 69(71,4/100/0C)+171,34(1,67/100ml/0C)------5gNaN3 …..etc. 10gHS in 400ml watter+ 5,3g NaNO2 in 10mlwatter + 13,2g Ba(OH)2 Making Barium hydroxide: Ba(OH)2: 30 g of Ba(NO3)2 with solubility 10,5/100/25C or 34/100/100C + 9g of NaOH in 150ml watter boiled and after cooled to 0C and filtrate it.The Ba (OH)2 is watter solubile 1,67g/100ml/0C. Making the reaction Filtrate with Ba(OH)2 add to 10 g of HydrazineSulfate in 400ml watter and add there 5,5g-7g NaNO2 in10ml watter.Because is not known under such condition should this reaction go,I put it 12 h in freezer and after I boiled it for to evaporace its volume on to 100 ml .After was this volume reached,I cooled it and filtered.Liquid was there 50 ml .I precipitate it with ethanol and filtered. There was 3 g of white something and reaction with AgNO3 gave something black. -------------------------------------------------------------------------------- About used chemicals : Ba(OH)2 :: mol=171,34anh. Or 315,46 octahydrate Solubility watter -1,67g/100ml/0C 3,89g/100ml/20C 20,94g/100ml/60C 101,4g/100ml/100C Other solvents low -------------------------------------------------------------------------------- NaNO2:: mol=68,995,m.p.271C Solubility watter-71,4g/100ml/0C 84,8g/100ml/25C 160g/100ml/100C Methanol-4,4g/100ml,ethanol=solubile,ether=0,3g/100ml -------------------------------------------------------------------------------- NaOH :: mol= 39,99 m.p. =318 C,density=2,13g/cm3 solubility – watter 485,7g/100ml/0C -glycerol ?, -alcohol: Ethanol= 13,9g/100ml/0C,methanol= 23,8g/100ml/0C -------------------------------------------------------------------------------- BaSO4:: mol=233,38 -solubility in watter =insolubile,in alkohol= insolubile ------------------------------------------------------------------------------- Hydrazine sulphate:: solid,mol= 130,13, m.p. 254 C solubility in watter at 20 C =30g/l or 2,86 /100 ml, at 80 C= 14,39g/100ml Insoluble in alkohol Ethanol = 0,04g/l00ml/28C H2N-NH3xHSO4 [Edited on 15-10-2016 by Thraxx] [Edited on 15-10-2016 by Thraxx]

May I ask what is your age and education level in chemistry?

You provide really a lot of informations into this post, but most of the information is not so important for the purpose of the making of NaN3...so you end up by leading us onto side ways instead of keeping us on track (Thraxx ).

If I read your procedure, I may conclude that mixing NaNO2 with N2H5OH will result into the making of NaN3...

This is something possible because I have experienced that mixing N2H5OH with phenol-phtalein (PP) makes a fushia solution...when PP is put into NaNO2 solution nothing happens (what is normal because NaNO2 is nor basic nor acidic so solution remains neutral).

When mixing fushia N2H5OH/PP solution with NaNO2 solution...discoloration occurs...not a single bubble of N2
This proves something happens to the basic stuff into the solution and that is hydrazine; the only possibility is via formation of NaN3 (via hydrazine nitrite? and immediate recombination into hydrazoic acid + water....?)
H2N-NH2 + H2O <-aq-> H2N-NH3(+) + OH(-)
NaNO2 -aq-> Na(+) + NO2(-)
H2N-NH3(+) + NO2(-) --?--> H2N-NH-N=O + H2O
H2N-NH-N=O <--> H2N-N=N-OH --> HN3 + H2O
HN3 <-aq-> H(+) + N3(-)
OH(-) + H(+) --> H2O
After simplification
H2N-NH2 + H2O + NaNO2--> NaN3 + H2O

Sadly at that time I didn't test for azide precipitation.

Into your procedure the Ba(OH)2 is only present because soluble base and source of Ba(2+) as precipitant for the SO4(2-) by forming white unsoluble BaSO4(s) (the s means solid into the aqueous phase; thus a precipitate).
I write this because you seems surprised that there is a white precipitate.

Your all procedure don't need the first step of filtration to isolate Ba(OH)2 and separate it from NaNO3, since
Ba(NO3)2(aq) + 2 NaOH(aq) <--> Ba(OH)2(aq) + 2 NaNO3(aq)
Nothing to filtrate, no unsoluble.
Thus Ba(NO3)2 and NaOH can immediatelly be reacted with N2H4.H2SO4 and the resulting BaSO4 filtrated.
Ba(NO3)2 + 2 NaOH + N2H4.H2SO4 ---> BaSO4(s) + 2 NaNO3(aq) + N2H4(aq) + 2 H2O
After filtration you are left with N2H4(aq) and NaNO3(aq).
Those can be reacted with NaNO2 because Na(+) and NO3(-) are spectator (=not entering the equation) ions.
So you come to a simple addition of N2H4(aq) to NaNO2(aq)...exactly what I simply did.

Final remark, you do a lot of experiments but you never write the final testing of your azide...the only proof azide is present, is precipitation of unsoluble azide (heavy metal), filtration recollection, drying and submitting to fire --> BOOM.
This last step is important, because many things may form a precipitate into your complex reaction scheme (too much reactants)...remember KISS KISS KISS (not only your wife or girlfriend --> Keep It Short & Simple.

Quote: Originally posted by PHILOU Zrealone

The purity is not important if you play it safe about cations and anions to take care that all ions except the azide won't make a precipitate. --> Only N3(-) and Ag(+) will precipitate, nothing else --> purity is no concern because 100%.

Quote: Originally posted by PHILOU Zrealone

Exactly what I wrote...you need more chemical basic knowledge. It is sad that you waste so much valuable reactants into much experiments without succes because of this. I hope you work on recovery too.