02-10-2023-0716 - PBS/AZIDE Wislicenus process

https://us.vwr.com/store/product/21257220/1x-pbs-phosphate-buffered-saline-0-05-sodium-azide-teknova

https://www.frontiersin.org/articles/10.3389/fmicb.2013.00179/full

https://www.jstor.org/stable/4452774

https://journals.plos.org/plospathogens/article?id=10.1371/journal.ppat.1002417

https://elifesciences.org/articles/35449

https://en.wikipedia.org/wiki/Sodium_azide

https://www.scbt.com/p/pbs-with-azide
Preparation

The common synthesis method is the "Wislicenus process", which proceeds in two steps in liquid ammonia. In the first step, ammonia is converted to sodium amide by metallic sodium: 2 Na + 2 NH3 → 2 NaNH2 + H2

It is a redox reaction in which metallic sodium gives an electron to a proton of ammonia which is reduced in hydrogen gas. Sodium easily dissolves in liquid ammonia to produce hydrated electrons responsible of the blue color of the resulting liquid. The Na+ and NH−2 ions are produced by this reaction.

The sodium amide is subsequently combined with nitrous oxide: 2 NaNH2 + N2O → NaN3 + NaOH + NH3

These reactions are the basis of the industrial route, which produced about 250 tons per year in 2004, with production increasing due to the increased use of airbags.[5]
Laboratory methods

Curtius and Thiele developed another production process, where a nitrite ester is converted to sodium azide using hydrazine. This method is suited for laboratory preparation of sodium azide: 2 NaNO2 + 2 C2H5OH + H2SO4 → 2 C2H5ONO + Na2SO4 + 2 H2OC2H5ONO + N2H4·H2O + NaOH → NaN3 + C2H5OH + 3 H2O

Alternatively the salt can be obtained by the reaction of sodium nitrate with sodium amide.[8]
Chemical reactions

Treatment of sodium azide with strong acids gives hydrazoic acid, which is also extremely toxic: H+ + N−3 → HN3

Aqueous solutions contain minute amounts of hydrogen azide, the formation of which is described by the following equilibrium: N−3 + H2O ⇌ HN3 + OH−, K = 10−4.6

Sodium azide can be destroyed by treatment with nitrous acid solution:[9] 2 NaN3 + 2 HNO2 → 3 N2 + 2 NO + 2 NaOH
Applications
Automobile airbags and aircraft evacuation slides

Older airbag formulations contained mixtures of oxidizers and sodium azide and other agents including ignitors and accelerants. An electronic controller detonates this mixture during an automobile crash: 2 NaN3 → 2 Na + 3 N2

The same reaction occurs upon heating the salt to approximately 300 °C. The sodium that is formed is a potential hazard alone and, in automobile airbags, it is converted by reaction with other ingredients, such as potassium nitrate and silica. In the latter case, innocuous sodium silicates are generated.[10] While sodium azide is still used in evacuation slides on modern aircraft, newer-generation automotive air bags contain less sensitive explosives such as nitroguanidine or guanidine nitrate.
Organic and inorganic synthesis

Due to its explosion hazard, sodium azide is of only limited value in industrial-scale organic chemistry. In the laboratory, it is used in organic synthesis to introduce the azide functional group by displacement of halides. The azide functional group can thereafter be converted to an amine by reduction with either SnCl2 in ethanol or lithium aluminium hydride or a tertiary phosphine, such as triphenylphosphine in the Staudinger reaction, with Raney nickel or with hydrogen sulfide in pyridine.

Sodium azide is a versatile precursor to other inorganic azide compounds, e.g., lead azide and silver azide, which are used in detonators as primary explosives. These azides are significantly more sensitive to premature detonation than sodium azide and thus have limited applications. Lead and silver azide can be made via double displacement reaction with sodium azide and their respective nitrate (most commonly) or acetate salts. Sodium azide can also react with the chloride salts of certain alkaline earth metals in aqueous solution, such as barium chloride or strontium chloride to respectively produce barium azide and strontium azide, which are also relatively sensitive primarily explosive materials. These azides can be recovered from solution through careful desiccation.
Biochemistry and biomedical uses

Sodium azide is a useful probe reagent and a preservative.

In hospitals and laboratories, it is a biocide; it is especially important in bulk reagents and stock solutions which may otherwise support bacterial growth where the sodium azide acts as a bacteriostatic by inhibiting cytochrome oxidase in gram-negative bacteria; however, some gram-positive bacteria (streptococci, pneumococci, lactobacilli) are intrinsically resistant.[11]
Agricultural uses

It is used in agriculture for pest control of soil-borne pathogens such as Meloidogyne incognita or Helicotylenchus dihystera.[12]

It is also used as a mutagen for crop selection of plants such as rice,[13] barley[14] or oats.[15]
Safety considerations

Sodium azide can be fatally toxic,[16] and even minute amounts can cause symptoms. The toxicity of this compound is comparable to that of soluble alkali cyanides,[17] although no toxicity has been reported from spent airbags.[18]

It produces extrapyramidal symptoms with necrosis of the cerebral cortex, cerebellum, and basal ganglia. Toxicity may also include hypotension,[19] blindness and hepatic necrosis. Sodium azide increases cyclic GMP levels in the brain and liver by activation of guanylate cyclase.[20]

Sodium azide solutions react with metallic ions to precipitate metal azides, which can be shock sensitive and explosive. This should be considered for choosing a non-metallic transport container for sodium azide solutions in the laboratory. This can also create potentially dangerous situations if azide solutions should be directly disposed down the drain into a sanitary sewer system. Metal in the plumbing system could react, forming highly sensitive metal azide crystals which could accumulate over years. Adequate precautions are necessary for the safe and environmentally responsible disposal of azide solution residues.[21]

 
https://en.wikipedia.org/wiki/Sodium_azide