6484-52-2

Usage

Uses

Used in Agricultural Industry:
Ammonium nitrate is used as a nitrogenous fertilizer for providing a source of nitrogen to plants, which increases growth and crop yields. It is popular for pasture and hay fertilization due to its lower susceptibility to volatilization or air losses when left on the soil. It is also valued by vegetable growers for its ability to provide an immediately available nitrate source of plant food.
Used in Explosives Industry:
Ammonium nitrate is used as a major component in the production of safety explosives, such as in mining and construction. When mixed with fuel oil, it creates a deflagrating explosive material. It has been used in terrorist attacks, such as the Oklahoma City bombing and the first attack on the World Trade Center in New York City.
Used in Pyrotechnics Industry:
Ammonium nitrate is used in the production of pyrotechnics, such as fireworks, due to its explosive properties.
Used in Chemical Industry:
Ammonium nitrate is used as a raw material in the production of nitrous oxide (laughing gas) and as a component in freezing mixtures.
Used in Pharmaceutical Industry:
Ammonium nitrate serves as a nutrient in the production of antibiotics and yeast, which are essential for various medical and pharmaceutical applications.
Used in Manufacturing Industry:
Ammonium nitrate is used in the production of various compounds, such as calcium ammonium nitrate and ammonium sulfate nitrate, which are used as fertilizers.
Used in Environmental Management:
Ammonium nitrate can leave behind an acid residue in the soil, which may require neutralization with lime to maintain soil health. It is also prone to leaching, which can lead to environmental concerns if not managed properly.

Brief Introduction

Ammonium nitrate, is a colorless rhombic or monoclinic crystal at room temperature. It can be decomposed into water and nitrous oxide at 210 ° C. Upon severe heating at 300 ℃ above, it is subject to decomposition into nitrogen, oxygen and water. It is soluble in water, methanol and ethanol. It dissolution in water can absorb a lot of heat and reduce the temperature. It is one of the major nitrogen fertilizer varieties in the world today, accounting for about 3.5% of the total amount of nitrogen fertilizer in our country. The nitrogen form is nitrate, which belongs to the nitrate nitrogen fertilizer. In fact, ammonium nitrate both nitrate and ammonium nitrogen, but its nature is more similar to the nitrate nitrogen fertilizer. Ammonium nitrate has no residue in the soil; and can be all absorbed by crops; being a physiological neutral fertilizer. Ammonium nitrate is suitable for a wide range of soils and crops but is most suitable for dry and dry crops especially suitable for cash crops such as tobacco, cotton and vegetables. Ammonium nitrate should not be used as a basal fertilizer, because ammonium nitrate, after being applied to the soil, has its dissociated nitrate ions be easily leached into the soil. At the same time, ammonium nitrate should not be used seed manure because of its higher nutrient content, high hygroscopicity, which will affect the germination upon contact with seeds. Ammonium nitrate, when applied in paddy field, can have its nitrogen content easily leached. Therefore, its efficiency is not comparable to other nitrogenous fertilizers of equal nitrogen content, being only equivalent to 50% -70% of that of ammonium sulfate with equal nitrogen content. The most ideal application is for topdressing, and is most suitable for top-dressing in dry land. The usage amount can be determined according to soil fertility and yield indicators. Should pay attention to the following points: Do not mix with acid fertilizers (such as superphosphate) and alkaline fertilizers (such as ash, etc.) to prevent the reduction of fertilizer efficiency. In the event of caking, gently crush it with sticks; avoid fiercely crushing it to prevent explosion. Apply sealed packaging, pay attention to moisture, heat; store way from combustibles and oxidants.

Agricultural Use

Since plant roots do not directly absorb the urea form of N to a large extent, ammonium nitrate is an efficient and immediate source of plant nutrition. It provides half of the N in the nitrate form and half in the ammonium form. The nitrate form is mobile in the soil water and immediately available for plant uptake. The ammonium fraction is taken up if roots grow nearby or after it is converted to nitrate by soil microorganisms during nitrification. Many farmers prefer an immediately available nitrate source for plant nutrition and choose ammonium nitrate as their N fertilizer. It is popular for pasture and broad acre crops since almost no ammonia volatilization losses occur, compared to urea-based fertilizers. Some 37 million metric tons (MMt) of fertilizer grade ammonium nitrate are consumed worldwide annually in agriculture, of which about 14 MMt are used as CAN. Because of its high crop recovery, its ease of use, and its suitability for in-season top dressing, ammonium nitrate is widely used, especially in many European countries.

Production

The manufacture of ammonium nitrate involves several major unit operations including solution formation and concentration; solids formation, finishing, screening, and coating; and product bagging and/or bulk shipping. In some cases, solutions may be blended for marketing as liquid fertilizers. The number of operating steps employed depends on the end product desired. For example, plants producing ammonium nitrate solutions alone use only the solution formation, solution blending, and bulk shipping operations. Plants producing a solid ammonium nitrate product may employ all of the operations. All ammonium nitrate plants produce an aqueous ammonium nitrate solution through the reaction of ammonia and nitric acid in a neutralizer as follows: NH3+HNO3 → NH4NO3 Approximately 60 percent of the ammonium nitrate produced in the U. S. is sold as a solid product. To produce a solid product, the ammonium nitrate solution is concentrated in an evaporator or concentrator. The resulting "melt" contains about 95 to 99.8 percent ammonium nitrate at approximately 149°C (300°F). This melt is then used to make solid ammonium nitrate products.

Extremely Insensitive Explosives

Ammonium nitrate is an extremely insensitive explosive that is more detrimental than the safe explosives c4. An industrial 8 # detonator (detonated c4 just 6 # on it) are not enough to detonate a mixture of sensitizer ammonium nitrate. Ammonium nitrate is the most detonating nitric acid explosives with impact sensitivity being: 50kg hammer with 50cm drop height will not cause explosion. The impact sensitivity of the famous explosive nitroglycerin: 200 g hammer at 20cm high drop height will lead to 100% explosion. And once the ammonium nitrate is dissolved in water, the detonation sensitivity is greatly reduced, for which it is impossible to detonate the ammonium nitrate with human power.

potential hazards

Ammonium nitrate readily attracts moisture from the air, and for this reason, is often stored in air-conditioned warehouses or in sealed bags. Ammonium nitrate is considered non-flammable; a fire from ammonium nitrate is very unlikely. However, it is a strong oxidizing agent that can cause combustible materials (such as wood, paper and oil) to ignite. Only under extreme conditions of heat and pressure in a confined space will ammonium nitrate explode.

Air & Water Reactions

Water soluble. Hot aqueous solutions of the nitrate above 50% conc., under confinement may decompose explosively. This process is aided catalytically with such substances as nitric acid and chloride ion, [Chem. Abs., 1982, 97, 78074].

Reactivity Profile

The hazards of AMMONIUM NITRATE have been well studied because of several extremely severe explosions [Chem. Eng., 1962, 70, 91; Bretherick, 5th Ed., 1995]. Mixtures with alkyl esters may explode, owing to the formation of alkyl nitrates. Mixtures with phosphorus, tin(II) chloride or other reducing agents may react explosively [Bretherick 1979 p. 108-109]. A mixture with aluminum powder (also zinc, cadmium, copper, magnesium, lead, cobalt, nickel, bismuth, chromium, and antimony) can be used as an explosive. A number of explosions in which ammonium nitrate and aluminum were mixed with carbon or hydrocarbons, with or without oxidizing agents have occurred [Mellor 5:219 1946-47]. A mixture with acetic acid ignites when warmed, especially if concentrated [Von Schwartz p. 322 1918]. Causes the decomposition of sodium hypochlorite within a few seconds [Mellor 2 Supp. 1:550 1956].

Hazard

May explode under confinement and high temperatures, but not readily detonated. Ventilate well. To fight fire, use large amounts of water. The material must be kept as cool as possible and removed from confinement and flooded with water in event of fire.

Health Hazard

Inhalation, ingestion or contact (skin, eyes) with vapors or substance may cause severe injury, burns or death. Fire may produce irritating, corrosive and/or toxic gases. Runoff from fire control or dilution water may cause pollution.

Fire Hazard

These substances will accelerate burning when involved in a fire. Some may decompose explosively when heated or involved in a fire. May explode from heat or contamination. Some will react explosively with hydrocarbons (fuels). May ignite combustibles (wood, paper, oil, clothing, etc.). Containers may explode when heated. Runoff may create fire or explosion hazard.

Flammability and Explosibility

Nonflammable

Safety Profile

A powerful oxidizer and an allergen. See also NITRATES. A relatively stable explosive that has, however, caused many industrial explosions. Violent or explosive spontaneous reactions with acetic anhydride + nitric acid, ammonium sulfate + potassium, copper iron(Ⅱ) sulfide, sawdust, urea, barium nitrate, hot water, and ammonium chloride + water + zinc. Forms heator shock-sensitive explosive mixtures with acetic acid, aluminum + calcium nitrate + formamide (a blasting explosive), ammonia, charcoal + metal oxides (e.g., rust, copper oxide, zinc oxide above 80℃), chloride salts (e.g., ammonium chloride, calcium chloride, iron(ⅡI) chloride, and aluminum chloride), cyanoguanidine, feruH2ers (e.g., super phosphate + organic materials above 90℃), hydrocarbon oils, powdered metals (e.g., aluminum, antimony, bismuth, cadmium, chromium, cobalt, copper, iron, lead, magnesium, manganese, nickel, tin, zinc, brass, stainless steel, titanium, and potassium), nonmetals (e.g., charcoal, and phosphorus), organic fuels (e.g., wax, oils, and stearates), potassium permanganate, sugar, sulfur, and trinitroanisole. Reaction with alkali metals (e.g., sodium) forms an explosive product. Ignites on contact with ammonium dichromate, potassium dichromate, potassium chromate, barium chloride, sodium chloride, potassium nitrate, and chromium(V1) salts. Can ignite when mixed with acetic acid. Use water in large amounts to fight fire. It is important that the mass of materials be kept cool and that burning be extinguished promptly. Ventilate well. May explode under confinement and high temperatures. When heated to decomposition it emits highly toxic fumes of NOx. Can react vigorously with reducing materials. Incompatible with, (NH4Cl + heat), (C + heat), organic matter, P, NaOCl, NaClO4. Occasional explosions in presence of oil, (NH4)2S04 with K or Na.

Potential Exposure

Used in the manufacture of liquid and solid fertilizer compositions, industrial explosives and blasting agents from ammonium nitrate, matches; antibiotics; in the production of nitrous oxide.

Metabolism

Ammonium Nitrate. Ammonium nitrate is one of the two leading nitrogen fertilizer materials on a world basis: 10% in 1997. The high N content is advantageous for the reduction of freight and application costs per unit weight of nitrogen. The presence of 50% of the nitrogen in the highly available nitrate form makes it suitable for use in regions growing crops with a short vegetation period but has the disadvantage that, because the NO3 ? ion is not adsorbed by soil, it may contribute to relatively large nitrogen losses by the leaching of increased soil nitrate into streams and groundwater. Although the application of any nitrogenous fertilizer results in some degree of soil acidification, the nitrate form is notably less acidifying than ammonium sulfate and has a lower tendency for the loss of nitrogen to the atmosphere as gaseous ammonia. The hygroscopic character of the crystalline material, coupled with its explosive nature, contributes to difficult storage and handling properties and the need for the production of purified and stabilized forms.

Shipping

Ammonium nitrate with organic coating: UN0222 Ammonium nitrate, with . 0.2% combustible substances, including any organic substance calculated as carbon, to the exclusion of any other added substance, Hazard Class: 1D; Labels:1D-Explosive (with a mass explosion hazard); D-Substances or articles which may mass detonate (with blast and/or fragment hazard) when exposed to fire. Ammonium nitrate with NO organic coating: UN1942 Ammonium nitrate, with NOT . 0.2% of combustible substances, including any organic substance calculated as carbon, to the exclusion of any other added substance (also used for fertilizer), Hazard Class: 5.1; Labels: 5.1-Oxidizer. UN3375 Ammonium nitrate emulsion or Ammonium nitrate suspension or Ammonium nitrate gel, intermediate for blasting explosives, Hazard Class: 5.1; Labels: 5.1-Oxidizer. UN2072 Ammonium nitrate fertilizer, n.o.s., doesn’t appear in the 49 CFR Hazmat Table, refer to UN1942, above). UN2071 Ammonium nitrate based fertilizer, Hazard class: 9; Labels: 9-Miscellaneous hazardous material. UN2426/140 Ammonium nitrate, liquid (hot concentrated solution), Hazard Class: 5.1; Labels: 5.1-Oxidizer.

Purification Methods

It is crystallised twice from distilled water (1mL/g) by adding EtOH, or from warm water (0.5mL/g) by cooling in an ice-salt bath. Dry it in air, then under vacuum. After 3 recrystallisations of ACS grade, it contained Li and B at 0.03 and 0.74 ppm, respectively. It is deliquescent. [Early & Lowry J Chem Soc 115 1387 1919, 121 963 1922, Hendricks et al. J Am Chem Soc 54 2766 1932.]

Incompatibilities

A strong oxidizer. Reducing agents; combustible materials; organic materials; finely divided (powdered) metals may form explosive mixtures or cause fire and explosions. When contaminated with oil, charcoal or flammable liquids, can be considered an explosive which can be detonated by combustion or shock.

Waste Disposal

Pretreatment involves addition of sodium hydroxide to liberate ammonia and form the soluble sodium salt. The liberated ammonia can be recovered and sold. After dilution to the permitted provisional limit, the sodium salt can be discharged into a stream or sewer.

InChI:InChI=1/HNO3.H3N/c2-1(3)4;/h(H,2,3,4);1H3