|Jmol 3D model||Interactive image|
|UN number||0222 – with > 0.2% combustible substances
1942 – with <= 0.2% combustible substances
2067 – fertilizers
2426 – liquid
|Molar mass||80.043 g/mol|
|Density||1.725 g/cm3 (20 °C)|
|Melting point||169.6 °C (337.3 °F; 442.8 K)|
|Boiling point||approx. 210 °C;decomposes|
|118 g/100 ml (0 °C)
150 g/100 ml (20 °C)
297 g/100 ml (40 °C)
410 g/100 ml (60 °C)
576 g/100 ml (80 °C)
1024 g/100 ml (100 °C)
|Shock sensitivity||very low|
|Friction sensitivity||very low|
|Detonation velocity||5270 m/s|
|Safety data sheet||ICSC 0216|
EU classification (DSD)
|Lethal dose or concentration (LD, LC):|
LD50 (median dose)
|2085–5300 mg/kg (oral in rats, mice)|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|what is ?)(|
Ammonium nitrate is a chemical compound, the nitrate salt of the ammonium cation. It has the chemical formula NH4NO3, simplified to N2H4O3. It is a white crystalline solid and is highly soluble in water. It is predominantly used in agriculture as a high-nitrogen fertilizer. Its other major use is as an explosive, in mining, quarrying, and civil construction. It is the main component of ANFO, a popular industrial explosive which accounts for 80% of explosives used in North America; similar formulations have been used in improvised explosive devices. It is being phased out of use in consumer applications in many countries due to concerns over its potential for misuse.
- 1 Occurrence
- 2 Production
- 3 Properties
- 4 Applications
- 5 Safety, handling, and storage
- 6 Health hazards
- 7 Disasters
- 8 References
- 9 External links
Ammonium nitrate is found as a natural mineral (ammonia nitre—the ammonium analogue of saltpetre and other nitre minerals such as sodium nitrate) in the driest regions of the Atacama Desert in Chile, often as a crust on the ground and/or in conjunction with other nitrate, chlorate, iodate, and halide minerals. Ammonium nitrate was mined there in the past, but virtually 100% of the chemical now used is synthetic.
- HNO3 + NH3 → NH4NO3
Ammonia is used in its anhydrous form (i.e., gas form) and the nitric acid is concentrated. This reaction is violent owing to its highly exothermic nature. After the solution is formed, typically at about 83% concentration, the excess water is evaporated to an ammonium nitrate (AN) content of 95% to 99.9% concentration (AN melt), depending on grade. The AN melt is then made into "prills" or small beads in a spray tower, or into granules by spraying and tumbling in a rotating drum. The prills or granules may be further dried, cooled, and then coated to prevent caking. These prills or granules are the typical AN products in commerce.
The ammonia required for this process is obtained by the Haber process from nitrogen and hydrogen. Ammonia produced by the Haber process is oxidized to nitric acid by the Ostwald process. Another production method is a variant of the Odda process:
Ammonium nitrate can also be made via metathesis reactions:
Ammonium nitrate reacts with metal hydroxides, releasing ammonia and forming alkali metal nitrate:
- NH4NO3 + MOH → NH3 + H2O + MNO3 (M = Na, K)
Ammonium nitrate leaves no residue when heated:
- NH4NO3 → N2O + 2H2O
Transformations of the crystal states due to changing conditions (temperature, pressure) affect the physical properties of ammonium nitrate. These crystalline states have been identified:
|System||Temperature (°C)||State||Volume change (%)|
|I||169.6 to 125.2||cubic||+2.1|
|II||125.2 to 84.2||tetragonal||−1.3|
|III||84.2 to 32.3||α-rhombic||+3.6|
|IV||32.3 to −16.8||β-rhombic||−2.9|
The type V crystal is a quasicubic form related to caesium chloride, the nitrogen atoms of the nitrate anions and the ammonium cations are at the sites in a cubic array where Cs and Cl would be in the CsCl lattice.
Ammonium nitrate is an important fertilizer with the NPK rating 34-0-0 (34% nitrogen). It is less concentrated than urea (46-0-0), giving ammonium nitrate a slight transportation disadvantage. Ammonium nitrate's advantage over urea is that it is more stable and does not rapidly lose nitrogen to the atmosphere. During warm weather it is best to apply urea soon before rain is expected or to cover it with soil to minimize nitrogen loss.
Mixture with fuel oil
ANFO is a mixture of 94% ammonium nitrate ("AN") and 6% fuel oil ("FO") widely used as a bulk industrial explosive.:1 It is used in coal mining, quarrying, metal mining, and civil construction in undemanding applications where the advantages of ANFO's low cost and ease of use matter more than the benefits offered by conventional industrial explosives, such as water resistance, oxygen balance, high detonation velocity, and performance in small diameters.:2
In November 2009, a ban on ammonium sulfate, ammonium nitrate, and calcium ammonium nitrate fertilizers was imposed in the former Malakand Division—comprising the Upper Dir, Lower Dir, Swat, Chitral, and Malakand districts of the North West Frontier Province (NWFP) of Pakistan—by the NWFP government, following reports that those chemicals were used by militants to make explosives. Due to these bans, "Potassium chlorate — the stuff that makes matches catch fire — has surpassed fertilizer as the explosive of choice for insurgents."
Safety, handling, and storage
Health and safety data are shown on the safety data sheets available from suppliers and found on the internet. In response to several explosions resulting in the deaths of numerous people, U.S. agencies of Environmental Protection (EPA), Occupational Health and Safety (OSHA) and the Bureau of Alcohol, Tobacco and Firearms jointly issued safety guidelines.
Heating or any ignition source may cause violent combustion or explosion. Ammonium nitrate reacts with combustible and reducing materials as it is a strong oxidant. Although it is mainly used for fertilizer, it can be used for explosives. It was sometimes used to blast away earth to make farm ponds. Ammonium nitrate is also used to modify the detonation rate of other explosives, such as trinitrotoluene in the form of amatol.
Numerous safety guidelines are available for storing and handling ammonium nitrate. It should not be stored near combustible substances. Ammonium nitrate is incompatible with certain substances such as chlorates, mineral acids and metal sulfides, contact with which can lead to vigorous or even violent decomposition.
Ammonium nitrate has a critical relative humidity of 59.4%, above which it will absorb moisture from the atmosphere. Therefore, it is important to store ammonium nitrate in a tightly sealed container. Otherwise, it can coalesce into a large, solid mass. Ammonium nitrate can absorb enough moisture to liquefy. Blending ammonium nitrate with certain other fertilizers can lower the critical relative humidity.
The potential for use of the material as an explosive has prompted regulatory measures. For example, in Australia, the Dangerous Goods Regulations came into effect in August 2005 to enforce licensing in dealing with such substances. Licenses are granted only to applicants (industry) with appropriate security measures in place to prevent any misuse. Additional uses such as education and research purposes may also be considered, but individual use will not. Employees of those with licenses to deal with the substance are still required to be supervised by authorized personnel and are required to pass a security and national police check before a license may be granted.
Acute health effects
|Area of exposure||Hazard level|
|Skin contact||Moderately hazardous (irritant)|
|Eye contact||Moderately hazardous|
Long-term health effects
||This section needs more medical references for verification or relies too heavily on primary sources. (August 2016)|
The toxicity of nitrates when ingested is due to in vivo conversion to nitrites. The material safety data sheet considers chronic ingestion of more than 5 mg/kg/day unacceptable. The primary overdose effects of chronic exposure are orthostatic hypotension and methemoglobinemia. Other common effects include: faintness, fatigue, weakness, depression, mental impairment, dizziness, shortness of breath, and reflex tachycardia; headache, nausea, vomiting, and nephritis may also occur.
|Types of effect||Effect level|
|Carcinogenic effects||Though no ammonium nitrate-specific studies are available, nitrates can be reduced to nitrites in the body, and the formed nitrites can subsequently react with amines to form N-nitrosamines, a class of chemicals suspected to be carcinogens.|
|Mutagenic effects||In general, nitrates and nitrites are genotoxic.|
|Developmental toxicity||Though not specific to ammonium nitrate, some studies have shown a link between birth defects (particularly neural tube defects) and nitrate-contaminated well water.|
|Prolonged exposure||Causes damage to lungs and mucous membranes and may also cause damage to blood and gastrointestinal tract. Chronic ingestion may also cause nephritis.|
Ammonium nitrate decomposes into the gases nitrous oxide and water vapor when heated (not an explosive reaction); however, it can be induced to decompose explosively by detonation. Large stockpiles of the material can be a major fire risk due to their supporting oxidation, and may also detonate, as happened in the Texas City disaster of 1947, which led to major changes in the regulations for storage and handling.
Two major classes of incidents resulting in explosions are:
- The explosion happens by the mechanism of shock-to-detonation transition. The initiation happens by an explosive charge going off in the mass, by the detonation of a shell thrown into the mass, or by detonation of an explosive mixture in contact with the mass. The examples are Kriewald, Morgan (present-day Sayreville, New Jersey), Oppau, and Tessenderlo.
- The explosion results from a fire that spreads into the ammonium nitrate itself (Texas City, Brest, Oakdale PA), or from a mixture of ammonium nitrate with a combustible material during the fire (Repauno, Cherokee, Nadadores). The fire must be confined at least to a degree for successful transition from a fire to an explosion (a phenomenon known as "deflagration-to-detonation transition"). Pure, compact AN is stable and very difficult to ignite, and numerous cases exist when even impure AN did not explode in a fire.
Ammonium nitrate was suspected as the explosive responsible for the fertilizer plant explosion in West, Texas on April 17, 2013. Investigators said they believe it exploded following a fire that began in the plant's office.
- Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
- Martel, B.; Cassidy, K. (2004). Chemical Risk Analysis: A Practical Handbook. Butterworth–Heinemann. p. 362. ISBN 1-903996-65-1.
- Karl-Heinz Zapp "Ammonium Compounds" in Ullmann's Encyclopedia of Industrial Chemistry 2012, Wiley-VCH, Weinheim. doi:10.1002/14356007.a02_243
- Int Panis, LLR (2008). "The Effect of Changing Background Emissions on External Cost Estimates for Secondary Particulates" (PDF). Open Environmental Sciences. 2: 47–53. doi:10.2174/1876325100802010047.
- Choi, C. S.; Prask, H. J. (1983). "The structure of ND4NO3 phase V by neutron powder diffraction". Acta Crystallographica B. 39 (4): 414–420. doi:10.1107/S0108768183002669.
- Nutrient Content of Fertilizer Materials
- Cook, Melvin A. (1974). The Science of Industrial Explosives. IRECO Chemicals. p. 1. ASIN B0000EGDJT.
- Potassium chlorate — the stuff that makes matches catch fire — has surpassed fertilizer as the explosive of choice for insurgents.
- Ammonium nitrate MSDS
- Chemical Advisory: Safe Storage, Handling, and Management of Ammonium Nitrate United States Environmental Protection Agency
- Pradyot Patnaik (2002). Handbook of Inorganic Chemicals. McGraw-Hill. ISBN 0-07-049439-8.
- Pothole pond
- Progressive Farmer Magazine
- Storing and handling ammonium nitrate
- Chemical Engineering Transactions
- Fertilizers Europe (2006). "Guidance for Compatibility of Fertilizer Blending Materials" (PDF).
- Dangerous Goods (HCDG) Regulations
- Ammonium Nitrate-Regulating its use, Balancing Access & Protection from "Worksafe Victoria".
- CF Industries. "Ammonium nitrate MSDS" (PDF).
- "Chemicalland21 – Ammonium Nitrate".
- "Ammonium Nitrate". Paton Fertilizers Pty Ltd. 2005.
- "Material Safety Data Sheet, Ammonium nitrate MSDS".
- Martel, B.; Cassidy, K. (2004). Chemical Risk Analysis: A Practical Handbook. Butterworth–Heinemann. ISBN 1-903996-65-1.
- Investigators blame ammonium nitrate in massive West explosion
- Properties: UNIDO and International Fertilizer Development Center (1998), Fertilizer Manual, Kluwer Academic Publishers, ISBN 0-7923-5032-4.
- International Chemical Safety Card 0216
- "Storing and Handling Ammonium Nitrate", United Kingdom Health and Safety Executive publication INDG230 (1986)
- Chemical Advisory: Safe Storage, Handling, and Management of Ammonium Nitrate United States Environmental Protection Agency
- Calculators: surface tensions, and densities, molarities and molalities of aqueous ammonium nitrate
|Salts and covalent derivatives of the Nitrate ion|