He barium nitrate is a salt composed of a barium atom (Ba) and the nitrate ion (NO 3 ). It appears as a white crystalline solid at room temperature and exists in nature as a very rare mineral known as nitrobarite. Its properties make it a toxic compound that must be handled carefully.
In fact, this compound has multiple uses in the military industry, since it can be linked to other chemical substances and added to the formulations of explosives and arsonists, among others.
Index
- 1 Formula
- 2 Chemical structure
- 3 Dissociation
- 4 Applications
- 5 Physical and chemical properties
- 6 References
Formula
Barium nitrate, also called barium dinitrate, has the chemical formula Ba (NO 3 ) 2 , and it is usually manufactured through two methods.
The first of these involves the dissolution of small pieces of barium carbonate (BaCO 3 ) in a nitric acid medium (HNO 3 , a highly corrosive mineral acid), allowing then the iron impurities to precipitate and then this mixture is filtered, evaporated and crystallized.
The second method is done through the combination of barium chloride (BaCl 2 , one of the barium salts of greater solubility in water) with a pre-heated solution of sodium nitrate. This generates a reaction that results in the separation of barium nitrate crystals from the mixture.
Chemical structure
This salt has characteristics of cubic crystalline structure or anhydrous octahedra.
Its chemical structure is as follows:
Dissociation
At elevated temperatures (592 ° C), barium nitrate decomposes to form barium oxide (BaO), nitrogen dioxide (NO) 2 ) and oxygen (O 2 ), according to the following chemical reaction:
2Ba (NO 3 ) 2 + Heat → 2BaO + 4NO 2 + O 2
In media with high concentrations of nitric oxide (NO), the decomposition of barium nitrate produces a compound called barium nitrite (Ba (NO 2 ) 2 ), according to the following equation:
Bath 3 ) 2 + 2NO → Ba (NO 2 ) 2 + 2NO 2
Reactions with soluble sulfates of metal or sulfuric acid (H 2 SW 4 ) generate barium sulfate (BaSO 4 ). The vast majority of insoluble barium salts, such as carbonate (BaCO) 3 ), oxalate (BaC 2 OR 4 ) or metal phosphate (Ba 3 (PO4) 2 ), are precipitated by similar reactions of double decomposition.
Applications
This substance in powder form is an oxidizing agent and reacts significantly with common reducing agents.
When this salt is mixed with other metals, such as aluminum or zinc in its finely divided forms, or with alloys such as aluminum-magnesium, it ignites and explodes on impact. For this reason, barium nitrate is considered an excellent component of military weapons and explosives.
Linked with trinitrotoluene (commercially known as TNT, or C) 6 H 2 (DO NOT 2 ) 3 CH 3 ) and a binder (regularly paraffin wax), this salt forms a compound called Baratol, which has explosive properties. The high density of barium nitrate makes Baratol also acquire a higher density, making it more effective in its function.
Barium nitrate also binds with aluminum powder, a formula that results in the formation of flashing gunpowder, which is used primarily in fireworks and theatrical pyrotechnics.
This flashing gunpowder has also seen uses in the production of flares (as anti-missile measures of aircraft) and stun grenades. In addition, this substance is highly explosive.
This salt is combined with the reactant mixture called termite to form a variation of this called termate, which generates short and very powerful flashes of very high temperatures in small areas for a short time.
Termate-TH3 is a termate that contains 29% by weight composition of barium nitrate, which helps to increase the thermal effect, generate flames and significantly reduce the ignition temperature of the termate.
The termates are usually used in the production of incendiary grenades and have the function of destroying tank armor and military structures.
In addition, barium nitrate was one of the most used ingredients in the production of incendiary charges used by the British in their warplanes during World War II, which armed with incendiary ammunition that served to destroy enemy aircraft.
Finally, this salt has uses in the process of manufacturing barium oxide, in the industry of thermionic valves and, as already said, in the creation of pyrotechnics, especially those of green colors.
Physical and chemical properties
The salt appears as a white solid, hygroscopic and odorless, which is poorly soluble in water and totally insoluble in alcohols.
It has a molar mass of 261.337 g / mol, a density of 3.24 g / cm 3 and a melting point of 592 ° C. When it reaches its boiling point, it decomposes, as mentioned above. At room temperature it has a solubility in water of 10.5 g / 100 ml.
It is considered stable, but it is a strong oxidizing agent and must be kept away from combustible materials to prevent fires. It has sensitivity to water and should not be mixed with acids or anhydrous.
In high concentrations (for example, containers) they must be isolated from substances that can cause them to react, as they can explode in a violent way.
Like any other soluble barium compound, it is a toxic substance for animals and humans.
It should not be inhaled or consumed, as symptoms of poisoning (especially hardening of the facial muscles), vomiting, diarrhea, abdominal pains, muscle tremors, anxiety, weakness, respiratory distress, cardiac irregularity and seizures may occur.
Death can occur as a result of a poisoning with this substance, a few hours or a few days after presentation.
The inhalation of barium nitrate generates irritation in the respiratory mucosa and, in both modes of poisoning, solutions of sulphate salts must be prepared to apply first aid to the affected person.
In case of spills, it should be isolated from combustible substances and materials and, in case of fire, it should never come in contact with dry chemicals or foams. The area should be flooded with water if the fire is larger.
References
- Wikipedia. (s.f.). Wikipedia. Retrieved from en.wikipedia.org
- Mabus. (s.f.). ScienceMadness. Retrieved from sciencemadness.org
- United States Incendiary Bomb TH3-M50A3. (s.f.). Retrieved from ammunitionpages.com
- Cameo Chemicals. (s.f.). Retrieved from cameochemicals.noaa.gov
- Chemspider (s.f.). Retrieved from chemspider.com