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Nitric acidEdit

Formula: HNO3Edit

Description: Nitric acid is not used in pyrotechnic compositions but it can be used to prepare a variety of usefull nitrates from carbonates, hydroxides, oxides or free elements. It is used in the explosives industry in the preparation of a lot of commonly used explosives (eg TNT, RDX, PETN, nitrocellulose ). Most high explosives have no use in fireworks, though nitrocellulose is used in some fireworks compositions as an acetone  soluble binder.

Hazards: Nitric acid is corrosive. The fumes are dangerous to the lungs, eyes and skin. Skin will be stained yellow upon contact. Avoid all contact with both liquid and fumes. Wear eye and skin protection (lab apron, gloves, safety glasses, etc). In some reactions (especially those with metals) a brown gas will develop: nitrogen dioxide . It is very toxic, corrosive and will attack your lungs badly. Only work with nitric acid with adequate ventilation and proper protective clothing. Don't use any solutions more concentrated than 60%. Don't try to prepare high explosives at home and don't allow any organic material to contact nitric acid accidentially because that may result in the formation of dangerously explosive and/or sensitive materials.

Sources: It is possible to prepare nitric acid in several ways. It can also be bought at some drug stores. It is sold at professional gardening suppliers and at welding shops (it is used to passivate stainless steel after welding). One way to prepare it is by distilling a mixture of sulfuric acid  and sodium nitrate . This process is dangerous and requires some equipment. This method is probably too dangerous for the average amateur pyro. Another possible method is by precipitating barium sulfate  from a barium nitrate  solution by adding sulfuric acid . What remains is a nitric acid solution. It should be possible to prepare quite concentrated solutions by using concentrated sulfuric acid and a saturated (not hot!) barium nitrate solution. It is important that the sulfuric acid is added to the barium nitrate solution and not the other way around. The mixing of the liquids will produce heat and if the barium nitrate solution is added to the sulfuric acid it could cause sudden boiling and splatting. Therefore, add the sulfuric acid slowly to the barium nitrate while constantly stirring. Allow the mixture to cool from time to time if it gets too hot. A white precipitate of barium sulfate  should form. The mixture is then filtered through a sintered glass filter to obtain clear solution of nitric acid. Another method would consist of equal ammounts of sulfuric acid and potassium nitrate  heated a retort. The retort is heated until the solution starts bubbling, and the nitric acid evaporates. The acid then condenses in the neck of the retort, and drips out the end into a seperate flask that is submurged in chilled water. After the reaction is complete, the resulting nitric acid is around 80-95% pure. This process yields red fuming nitric acid, which you'll see fumes coming out of the flask when the lid is removed. A byproduct of this reaction is potassium hydrogen sulfate  (KHSO4), which appears as a white crystaline mass at the bottom of the retort.

ReferencesEdit

http://www.wfvisser.dds.nl/EN/cheminfo_EN.html Wikipedia: Nitric Acid - Laboratory Synthesis



NOTE: I have found several facts above that are completely incorrect.

Nitric acid formed by normal STP distillation/retort condensation is NOT 100% HNO3. It is the most concentrated that can be achieved without vacuum distillation, because Nitric acid forms an azeotrope with water at 67-68%. one cannot go any higher without a vacuum distillation setup.

- You're wrong. If you use the Potassium nitrate and concentrated sulfuric acid method, you get concentrated fuming nitric acid.

Distillation at home can be done with a setup involving a sealed bucket, a Teflon or strong plastic pipe, ice, and a collecting jug. One can use KNO3 and H2SO4

This equation will give you the ratio:

KNO3 + H2SO4 --> KHSO4 + HNO3. Try adding excess KNO3 and less H2SO4.

I am not wrong. Please search up fuming nitric acid. Fuming nitric acid is defined as nitric acid at a concentration above 68%, which is the azeotrope with water. Fuming nitric acid is expensive and reactive. Fuming nitric acid also contains an excess of the NO2 + species of ion which allows very nice nitrations (no H2SO4 required for many reactions). The equation you have is correct, but the medium is water. Pure HNO3 is produced as a vapor, and must be dissolved in water to become liquid nitric acid.

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