The Environmental Protection Agency (EPA) and Comprehensive Environmental Response, Compensation, and Liability Act of 1980 categories the most hazardous wastes in the nation and ammonia has approximately 8% toxic (“ammonium nitrate”, 2016). Although ammonium nitrate has many advantages such as being used as a fertilizer, instant ice pack, or explosive, there are different occasions of explosions involving the substance. Because of such incidents, the government is improving chemical risk management and protecting human health and the environment through different emergency planning, and safety emergency response education. This essay will discuss the uses, effects, and sampling of ammonia nitrate. Nitrate of Ammonia is a commercially available chemical substance both as a colorless solid and powder for different applications. It has exceptional properties such as its ability not to burn unless contaminated with other materials and high nitrogen levels which make it great in its usage. It is used in safety explosives, as a freezing mixture, and as a fertilizer. However, ammonium nitrate decomposes to release ammonia ions and nitrous fumes which are harmful to the human body and to the environment. Its dilution may cause water pollution, while inhaling, ingesting or contact with the skin may cause severe body injury, burns or deaths. An overall view on the toxicology of ammonium nitrate is important to the interested individuals, public health officials and physicians to prevent possible effects from exposure of the chemical.
Scientists believe that the Germans developed ammonium nitrate to use it as fertilizer since it was cheaper compared to Chilean Nitrates. Ammonium nitrate has the following chemical names; Nitram, ammonium saltpeter, ammonium nitric, nitric acid ammonium salt, and herco prills among others. Scientists have ammonium nitrate chemical formula as NH4NO3. Ammonia nitrate has two nitrogen atoms, three oxygen atoms, and four hydrogen atoms. It also contains two ions, nitrate ion (NO3-) and ammonium ion (NH4+) forming the ionic bond. This chemical substance appears in white crystalline form but when at room temperature it is colorless. Ammonium nitrate is a white solid. It can either take the bead or crystalline bond. The ammonium nitrate melting point is 169.6 degrees Celsius or 337.3 degrees Fahrenheit while its melting point is 170 degrees Celsius. Ammonium nitrate ph level is 5.4, and it is known as a strong oxidizer as it can react violently with other materials which are not incompatible. It is also highly soluble in water, heating its water solution leads to its decomposition and production of nitrous oxide (laughing gas) ( Cameo Chemicals) .
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Ammonium nitrate a salt of nitric acid and ammonia has different industrial uses mostly in explosives, as blasting agents and as fertilizers because of its availability, low price, readily explosive if subjected to heat, and its high nitrogen content. Below are the common uses.
Fertilizer
Ammonium nitrate is an important chemical in agriculture, and it’s a component in fertilizers sold in pellets forms coated with clay. Nitrogen is important to plant nutrient as it helps in the growth of plants and other processes such as photosynthesis. It happens that ammonium nitrate has high nitrogen content from ammonia and the nitrate thus providing a ready supply of nitrogen. Besides, ammonium nitrate is odorless and very affordable, and farmers continue to use it in large-scale agricultural fields and gardens to promote plant growth since the 1940’s. Ammonium nitrate formation is from the reaction between nitric acid and ammonia gas which produces heat. It then fused with ammonium sulfate since it is volatile to minimize its volatility. Farmers mix Ammonium nitrate, as it is high soluble, with other fertilizers to make foliar sprays. Its advantages in using it as fertilizer are that it increases the production capacity of fruits, plants produce quality green leafy vegetables, and yield fast growth of plants. However, when exposed to heat, it may lead to an explosion since it is sensitive to heat (Grant, 2016).
Explosives
Ammonium nitrate is the primary ingredient in the manufacturing explosives, ANFO (ammonium nitrate fuel oil). ANFO is a mixture of fuel oil (6%) and ammonium nitrate (94%) which is the oxidizing agent for fuel. ANFO is highly stable and cheap and is common in North America. Amatol is also an explosive material with a mixture of ammonium nitrate and trinitrotoluene. During World War, I and II Amatol were popular in various military weapons such as shells and aircraft bombs. Because of ammonium nitrate’s low cost and availability, people use it to make homemade bombs, construction sites, and the mining industry. It is easy to make improvised explosive devices as ammonium nitrate is hygroscopic, that is it can collect water molecules from the surroundings quickly. However, ammonium nitrate should not be kept in humid places as water can undermine its explosive abilities. Ammonium nitrate modifies the ignition of explosives such as ammonia dynamites or in ammonals as the oxidizing agent, as a mixture of powdered aluminum and ammonium nitrate. The government is regulating ammonium nitrates shipment and storage because of its explosive decomposition if exposed to heat in a confined space (Casablanca, 2015).
Instant cold packs
Instant cold packs are a convenient replacement for ice bag to reduce bruises, swelling, or inflammation as a result of sports injury. People make instant cold packs using dry ammonium nitrate bag and water bag. Ammonium nitrate quickly dissolves if exposed to water in an endothermic reaction. Therefore, to lower the temperature of the pack to 2 to 3 degree Celsius in a short time, the barrier separating the two bags is ruptured causing an endothermic reaction. The cold pack is used to attend to the bruises and inflammation. Ammonium nitrate has many advantages, but it also has its lethal downside. The chemical substance is stable in its molten, solid or solution. However, it can become less resistant to initiation. The following can result in the instability of ammonium nitrate; exposure to contaminants such as metals or chlorides, increased acidity, and bubble formation in its molten form. Ammonium nitrate may also explode due to exposure to high temperatures or strong shocks. Ammonium nitrate does not burn, but if it comes in contact with heat, it is likely to explode violently. The explosive force results when solid ammonium nitrate decomposes to nitrous oxide and water vapor. Other times it may explode from contamination or react with hydrocarbons, which ARE fuels. An example of the deadliest industrial accident as result of ammonium nitrate exposure happened in Texas City in 1947 in the port. The ship was transporting ammonium nitrate in paper sacks of 2,300 tons, and a cigarette was tossed carelessly towards the ship starting a fire. The chemical exploded causing a powerful knockout of the people around to the ground about 16 kilometers away. Ammonium nitrate accelerates burning when exposed to a fire. In this case, the ignition caused a nearby ship transporting ammonium nitrate too to explode. Chemical tanks and oil refineries surrounding the port caught fire causing the death of 581 people. Another example of exposure limit of ammonium nitrate happened in Bali in 2002. The chemical was used to kill 202 people in nightclub bombing. Other cases of Ammonium nitrate usage in terrorist attacks, and its regulation is in most places. The Department of Homeland Security has set rules to limit the sale of ammonium nitrate since most are using it as an explosive in the mining industries and construction sites. A mixture of aluminum powder and ammonium nitrate is used as explosive, If ammonium nitrate is heated in an enclosed space excessively it results in an explosion (Lallanilla, 2013). If an individual ingests the chemical substance, inhales or gets in contact with the skin or eyes, it may cause severe burns, injury or death. Runoff from dilution water or fire control may cause pollution while fire may produce toxic, corrosive or irritating gasses. When heated it melts, decomposes releasing toxic gasses that are nitrogen oxides and ammonia gas ( Nortech Laboratories, 2011). Ammonium nitrate has little Molecular Weight of 80.043 and high water solubility. Therefore, there is an expectation of logpow high absorption from the gastrointestinal tract. However, ammonium nitrate decreases this absorption when gets in contact with a fluid. Therefore, 50% of the intake is oral, inhaled, and dermal exposed. Ammonium nitrate dissociates into nitrate and ammonium nitrate since it is a soluble salt. This dissociation impairs the passage of the gastrointestinal wall. if ammonium nitrate is absorbed it is distributed widely through the body causing a reaction to the body. AN excretion is through urine as urea, through the production of sweat, in expired air, and in the feces. Exposure of Ammonium nitrate to inhalation or respiratory is dangerous as it is not available for inhalation as a vapor because of its pressure. However, an individual may inhale the particles during its use, and the deposition of ammonium nitrate particles in the nasopharyngeal. The highest percentage of the inhaled ammonium nitrate is retained in the upper respiratory tract and is ultimately eliminated in expired air. These particles are either sneezed or coughed out of the body or swallowed. Ammonium nitrate particles below 10um can reach the pulmonary regions or the tracheobronchial regions. Ammonium nitrate is highly soluble and will, therefore, dissolve in the aqueous pores and mucous lining of the respiratory tract. The chemical substance has the potential of absorption in the dermal because of the availability of the surface moisture of the skin. Besides, its molecular weight and high water solubility makes its favorable for the dermal uptake. Ammonia ion is produced in the human intestines by bacteria degradation of ingested food with nitrogenous compounds and through the usage of amino acids as glutamine deamination. Ammonia ion is present in the blood, and the body maintains a low concentration of it to maintain a steady metabolic state ( OMICS International, 2014). Exposure to ammonium nitrate for a short period to the skin, eyes or through inhalation and ingestion can cause symptoms such as Minor skin irritation and gastric irritation, nausea, vomiting, headaches, hypertension, dizziness, and c hronic effects. Nitrates are toxic if ingested especially if it is more than 5mg per day. An overdose of ammonium nitrate causes methemoglobinemia and orthostatic hypotension. When an individual inhales ammonium nitrate in high concentration, it may cause respiratory tract irritation while if swallowed in high level may cause bloody diarrhea, vomiting, abdominal pain, tingling sensation, convulsions, suffocation, and headaches. Other effects include nephritis as a result of chronic ingestion, reflex tachycardia, and shortness of breath, depression, fatigue and mental dizziness. If the individual is exposed to ammonia nitrate for an extended period, he/she may experience damaged mucous membranes and lungs. This effect may cause harm to the gastrointestinal tract (OMICS International, 2014).
Following its chemical and physical properties, industrial hygiene sampling includes:
Storage in tightly closed containers.
One should not store the chemical near flammable materials.
Keep away from clothing, eyes, and skin.
Avoid breathing ammonium nitrate dust.
Use the dust in open ventilations.
Wash your hands thoroughly after handling.
After use remove and wash the contaminated clothing immediately.
Store below 30C.
In the case of a spill or accidental discharge, the fire department should collect the discharge and store in suitable containers for future use or dispose of the spilled solid.
An individual exposed to Ammonium nitrate should take the following precautions.
For eye contact:
The individual should flush the eyes with running water immediately for not less than 15 minutes. During the whole process, the individual should keep the eyelids open.
If the irritation persists, the person should seek medical attention.
For skin contact:
Clean the irritated skin with soap and water.
Dry and apply the affected part with a quality dermatological skin care lotion.
Seek medical attention if the irritation persists.
In the case of inhalation, take the individual to fresh air and for any breathing difficulty get medical treatment ( EPA, OSHA, and ATF, 2015).
Conclusion
There are many reports of deaths resulting from using ammonium nitrate as an explosive or from inhalation of this chemical substance. Ammonium nitrate toxicity is fatal in humans when they are exposed to it. Humans risks chemical burns, skin irritation, convulsions, headaches, respiratory effects to the extent of immediate deaths, as from inhaling, swallowing or their skin getting in contact with this chemical substance. Besides, the negative effects of ammonium nitrate, it is has some advantages such as its usage as a fertilizers. Farmers will still use it because of its efficiency, availability and low price. However, to the stay on the safe side, individuals should handle ammonium nitrate with precaution and follow the protocols for industrial handling of the substance. The government is already its part of providing safety by limiting the use and sale of ammonium nitrate; this ensures it does not land in the hands of terrorists who use the chemical substance for bombings.
References
“Ammonium nitrate.” (2016). State of Queensland . Retrieved from https://www.worksafe.qld.gov.au/injury-prevention-safety/hazardous-chemicals/specific-hazardous-chemicals/ammonium-nitrate
Cameo Chemicals. Ammonium nitrate, liquid (hot concentrated solution). Retrieved from https://cameochemicals.noaa.gov/chemical/5397#section6
Casablanca, P. (2015). Uses of Ammonium Nitrate. Knowsumo. Retrieved from http://www.knowsumo.com/uses-of-ammonium-nitrate/
EPA, OSHA, and ATF. (2015). Safe storage, handling, and management of solid ammonium nitrate prills. Retrieved from https://www.epa.gov/sites/production/files/2015-06/documents/an_advisory_6-5-15.pdf
Grant, L.B. (2016). Ammonium Nitrate Fertilizer: How To Use Ammonium Nitrate in Gardens. Retrieved from http://www.gardeningknowhow.com/garden-how-to/soil-fertilizers/ammonium-nitrate-fertilizer.htm
Lallanilla, M. (2013). What Causes Fertilizer Explosions? Retrieved from http://www.livescience.com/28841-fertilizer-explosions-ammonium-nitrate.html
Nortech Laboratories. (2011). The hazards and Dangers of Ammonium nitrate. Retrieved from http://www.nortechlabs.com/hazards-ammonium-nitrate.html
OMICS International. (2014). Ammonium Nitrate. Retrieved from http://research.omicsgroup.org/index.php/Ammonium_nitrate
