Is no3 organic or inorganic

Is no3 organic or inorganic DEFAULT

Nitrate and Nitrite Compounds, Inorganic

There are 63 chemical datasheets assigned to this reactive group.



These compounds are explosive.


Compounds in this group can act as exceedingly potent oxidizing agents, and mixtures with reducing agents or reduced materials such as organic substances can be explosive. However, compounds such as ammonium nitrate will explode even with virtually no reduced material present. Generally, for these explosions to occur a significant amount of initiating energy must be supplied.

In general, nitrate and nitrite salts with redox-active cations are more reactive with organic materials and reducing agents at ambient conditions. Redox-active cations are transition metals and the metals in group 3a, 4a, and 5a of the periodic table as well as the ammonium cation [NH4]+. In general, nitrate and nitrite salts with non-redox active cations (also called spectator cations) are less reactive at ambient conditions. These include the alkali metals and alkaline earth salts.

Because of the wide range of reactivity with these salts, this tool will be conservative and generally predict a high hazard with other materials, especially organics. However, in many cases, as explained above, some mixtures may be perfectly benign. Consequently, inadvertent mixtures with inorganic nitrate or nitrite salts need to be vetted carefully on an individual basis. Caution should be used before proceeding. Further research of comparable examples in the literature or very small scale, carefully controlled experiments may be needed to fully assess compatibility.


Humans are subject to nitrate toxicity, with infants being especially vulnerable to methemoglobinemia due to nitrate metabolizing triglycerides present at higher concentrations than at other stages of development.

Other Characteristics

The nitrate ion is a polyatomic ion with the molecular formula [NO3]- and is the conjugate base of nitric acid. Almost all inorganic nitrate salts are soluble in water at standard temperature and pressure. A common example of an inorganic nitrate salt is potassium nitrate (saltpeter). Nitrate compounds have a wide range of uses which rely on their activity as oxidizing agents, the presence of freely available nitrogen, or their high solubility. Potassium nitrate and sodium nitrate are widely used as strong oxidizing agents, most notably in explosives where the rapid decomposition of nitrate into its constituent elements frees up large volumes of reactive oxygen. Nitrates are widely used in very large quantities as fertilizers in agriculture because of their readiness to decompose and release nitrogen for plant growth and because of their ready solubility ensuring that nitrate ions can be absorbed by plant root hairs. Nitrate compounds are widely used as industrial feedstock where an oxidizing agent or source of nitrate ion is required.


Aluminum nitrate, barium nitrate, didymium nitrate, nickel nitrite, potassium nitrate, sodium nitrite, uranyl nitrate.

Reactivity Documentation

Use the links below to find out how this reactive group interacts with any of the reactive groups in the database.

The predicted hazards and gas byproducts for each reactive group pair will be displayed, as well as documentation and references that were used to make the reactivity predictions.

Mix Nitrate and Nitrite Compounds, Inorganic with:

  • Acetals, Ketals, Hemiacetals, and Hemiketals
  • Acids, Carboxylic
  • Acids, Strong Non-oxidizing
  • Acids, Strong Oxidizing
  • Acids, Weak
  • Acrylates and Acrylic Acids
  • Acyl Halides, Sulfonyl Halides, and Chloroformates
  • Alcohols and Polyols
  • Aldehydes
  • Alkynes, with Acetylenic Hydrogen
  • Alkynes, with No Acetylenic Hydrogen
  • Amides and Imides
  • Amines, Aromatic
  • Amines, Phosphines, and Pyridines
  • Anhydrides
  • Aryl Halides
  • Azo, Diazo, Azido, Hydrazine, and Azide Compounds
  • Bases, Strong
  • Bases, Weak
  • Carbamates
  • Carbonate Salts
  • Chlorosilanes
  • Conjugated Dienes
  • Cyanides, Inorganic
  • Diazonium Salts
  • Epoxides
  • Esters, Sulfate Esters, Phosphate Esters, Thiophosphate Esters, and Borate Esters
  • Ethers
  • Fluoride Salts, Soluble
  • Fluorinated Organic Compounds
  • Halogenated Organic Compounds
  • Halogenating Agents
  • Hydrocarbons, Aliphatic Saturated
  • Hydrocarbons, Aliphatic Unsaturated
  • Hydrocarbons, Aromatic
  • Insufficient Information for Classification
  • Isocyanates and Isothiocyanates
  • Ketones
  • Metal Hydrides, Metal Alkyls, Metal Aryls, and Silanes
  • Metals, Alkali, Very Active
  • Metals, Elemental and Powder, Active
  • Metals, Less Reactive
  • Nitrate and Nitrite Compounds, Inorganic
  • Nitrides, Phosphides, Carbides, and Silicides
  • Nitriles
  • Nitro, Nitroso, Nitrate, and Nitrite Compounds, Organic
  • Non-Redox-Active Inorganic Compounds
  • Not Chemically Reactive
  • Organometallics
  • Oxidizing Agents, Strong
  • Oxidizing Agents, Weak
  • Oximes
  • Peroxides, Organic
  • Phenolic Salts
  • Phenols and Cresols
  • Polymerizable Compounds
  • Quaternary Ammonium and Phosphonium Salts
  • Reducing Agents, Strong
  • Reducing Agents, Weak
  • Salts, Acidic
  • Salts, Basic
  • Siloxanes
  • Sulfides, Inorganic
  • Sulfides, Organic
  • Sulfite and Thiosulfate Salts
  • Sulfonates, Phosphonates, and Thiophosphonates, Organic
  • Thiocarbamate Esters and Salts/Dithiocarbamate Esters and Salts
  • Water and Aqueous Solutions


Type of ion, commonly found in explosives and fertilisers

For the functional group –ONO
2, see Nitrate ester. For that functional group in medicine, see Nitrovasodilator.

Not to be confused with NO
2, nitrite.

Chemical compound

Nitrate is a polyatomic ion with the chemical formulaNO
3. Salts containing this ion are called nitrates. Nitrates are common components of fertilizers and explosives.[1] Almost all inorganic nitrates are soluble in water. An example of an insoluble nitrate is bismuth oxynitrate.


The nitrate ion with the partial charges shown

The ion is the conjugate base of nitric acid, consisting of one central nitrogenatom surrounded by three identically bonded oxygen atoms in a trigonal planar arrangement. The nitrate ion carries a formal charge of −1. This charge results from a combination formal charge in which each of the three oxygens carries a −2⁄3 charge, whereas the nitrogen carries a +1 charge, all these adding up to formal charge of the polyatomic nitrate ion. This arrangement is commonly used as an example of resonance. Like the isoelectroniccarbonate ion, the nitrate ion can be represented by resonance structures:

Canonical resonance structures for the nitrate ion

Dietary nitrates[edit]

A rich source of inorganic nitrate in the human diets come from leafy green foods, such as spinach and arugula. NO
3 (inorganic nitrate) is the viable active component within beetroot juice and other vegetables. Drinking water is also a dietary source.[2]

Dietary nitrate supplementation delivers positive results when testing endurance exercise performance.[3]

Ingestion of large doses of nitrate either in the form of pure sodium nitrate or beetroot juice in young healthy individuals rapidly increases plasma nitrate concentration by a factor of 2 to 3, and this elevated nitrate concentration can be maintained for at least 2 weeks. Increased plasma nitrate stimulates the production of nitric oxide. Nitric oxide is important physiological signalling molecule that is used in, among other things, regulation of muscle blood flow and mitochondrial respiration.[4]

Cured meats[edit]

Nitrite consumption is primarily determined by the amount of processed meats eaten, and the concentration of nitrates in these meats. Although nitrites are the nitrogen compound chiefly used in meat curing, nitrates are used as well. Nitrates lead to the formation of nitrosamines.[5] The production of carcinogenic nitrosamines may be inhibited by the use of the antioxidants vitamin C and the alpha-tocopherol form of vitamin E during curing.[6]

Anti-hypertensive diets, such as the DASH diet, typically contain high levels of nitrates, which are first reduced to nitrite in the saliva, as detected in saliva testing, prior to forming nitric oxide.[2]

Occurrence and production[edit]

Nitrate salts are found naturally on earth as large deposits, particularly of nitratine, a major source of sodium nitrate.

Nitrates are produced by a number of species of nitrifying bacteria in the natural environment using ammonia or urea as a source of nitrogen. Nitrate compounds for gunpowder were historically produced, in the absence of mineral nitrate sources, by means of various fermentation processes using urine and dung.

Lightning strikes in earth's nitrogen-oxygen rich atmosphere produce a mixture of oxides of nitrogen which form nitrous ions and nitrate ions which are washed from the atmosphere by rain or in occult deposition.

Nitrates are produced industrially from nitric acid.[1]


Nitrates are mainly produced for use as fertilizers in agriculture because of their high solubility and biodegradability. The main nitrate fertilizers are ammonium, sodium, potassium, calcium, and magnesium salts. Several million kilograms are produced annually for this purpose.[1]

The second major application of nitrates is as oxidizing agents, most notably in explosives where the rapid oxidation of carbon compounds liberates large volumes of gases (see gunpowder for an example). Sodium nitrate is used to remove air bubbles from molten glass and some ceramics. Mixtures of the molten salt are used to harden some metals.[1]

Nitrate was also used as a film stock through nitrocellulose. Due to its high combustibility, the studios swapped to acetate safety film in 1950.


Almost all methods for detection of nitrate rely on its conversion to nitrite followed by nitrite-specific tests. The reduction of nitrate to nitrite is effected by copper-cadmium material. The sample is introduced with a flow injection analyzer, and the resulting nitrite-containing effluent is then combined with a reagent for colorimetric or electrochemical detection. The most popular of these assays is the Griess test, whereby nitrite is converted to a deeply colored azo dye, suited for UV-vis spectroscopic analysis. The method exploits the reactivity of nitrous acid derived from acidification of nitrite. Nitrous acid selectively reacts with aromatic amines to give diazonium salts, which in turn couple with a second reagent to give the azo dye. The detection limit is 0.02 to 2 μM.[7] Methods have been highly adapted to biological samples.[8]


The acute toxicity of nitrate is low. "Substantial disagreement" exists about the long-term risks of nitrate exposure. The two areas of possible concern are that (i) nitrate could be a precursor to nitrite in the lower gut, and nitrite is a precursor to nitrosamines, which are implicated in carcinogenesis, and (ii) nitrate is implicated in methemoglobinemia, a disorder of red blood cells hemoglobin.[9][10]


Nitrates do not affect infants and pregnant women.[11][12] Blue baby syndrome is caused by a number of other factors such as gastric upset, such as diarrheal infection, protein intolerance, heavy metal toxicity etc., with nitrates playing a minor role.[13]

Drinking water standards[edit]

Through the Safe Drinking Water Act, the United States Environmental Protection Agency has set a maximum contaminant level of 10 mg/L or 10 ppm of nitrates in drinking water.[14]

An acceptable daily intake (ADI) for nitrate ions was established in the range of 0–3.7 mg (kg body weight)−1 day−1 by the Joint FAO/WHO Expert Committee on Food additives (JEFCA).[15]

Aquatic toxicity[edit]

In freshwater or estuarine systems close to land, nitrate can reach concentrations that are lethal to fish. While nitrate is much less toxic than ammonia,[16] levels over 30 ppm of nitrate can inhibit growth, impair the immune system and cause stress in some aquatic species.[17] Nitrate toxicity remains the subject of debate.[18]

In most cases of excess nitrate concentrations in aquatic systems, the primary sources are wastewater discharges, as well as surface runoff from agricultural or landscaped areas that have received excess nitrate fertilizer. The resulting eutrophication and algae blooms result in anoxia and dead zones. As a consequence, as nitrate forms a component of total dissolved solids, they are widely used as an indicator of water quality.

Domestic animal feed[edit]

Symptoms of nitrate poisoning in domestic animals include increased heart rate and respiration; in advanced cases blood and tissue may turn a blue or brown color. Feed can be tested for nitrate; treatment consists of supplementing or substituting existing supplies with lower nitrate material. Safe levels of nitrate for various types of livestock are as follows:[19]

1< 0.5< 0.12< 0.81Generally safe for beef cattle and sheep
20.5–1.00.12–0.230.81–1.63Caution: some subclinical symptoms may appear in pregnant horses, sheep and beef cattle nitrate problems: death losses and abortions can occur in beef cattle and sheep
4< 1.23< 0.28< 2.00Maximum safe level for horses. Do not feed high nitrate forages to pregnant mares

The values above are on a dry (moisture-free) basis.

Salts and covalent derivatives[edit]

Nitrate formation with elements of the periodic table.

Salts and covalent derivatives of the nitrate ion

See also[edit]


  1. ^ abcdLaue W, Thiemann M, Scheibler E, Wiegand KW (2006). "Nitrates and Nitrites". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a17_265.
  2. ^ abHord NG, Tang Y, Bryan NS (July 2009). "Food sources of nitrates and nitrites: the physiologic context for potential health benefits". The American Journal of Clinical Nutrition. 90 (1): 1–10. doi:10.3945/ajcn.2008.27131. PMID 19439460.
  3. ^McMahon NF, Leveritt MD, Pavey TG (April 2017). "The Effect of Dietary Nitrate Supplementation on Endurance Exercise Performance in Healthy Adults: A Systematic Review and Meta-Analysis"(PDF). Sports Medicine (Auckland, N.Z.). 47 (4): 735–756. doi:10.1007/s40279-016-0617-7. PMID 27600147. S2CID 207494150.
  4. ^Maughan, Ronald J (2013). Food, Nutrition and Sports Performance III. New York: Taylor & Francis. p. 63. ISBN .
  5. ^Bingham SA, Hughes R, Cross AJ (November 2002). "Effect of white versus red meat on endogenous N-nitrosation in the human colon and further evidence of a dose response". The Journal of Nutrition. 132 (11 Suppl): 3522S–3525S. doi:10.1093/jn/132.11.3522S. PMID 12421881.
  6. ^Parthasarathy DK, Bryan NS (November 2012). "Sodium nitrite: the "cure" for nitric oxide insufficiency". Meat Science. 92 (3): 274–9. doi:10.1016/j.meatsci.2012.03.001. PMID 22464105.
  7. ^Moorcroft, M.; Davis, J.; Compton, R. G. (2001). "Detection and determination of nitrate and nitrite: A review". Talanta. 54 (5): 785–803. doi:10.1016/S0039-9140(01)00323-X. PMID 18968301.
  8. ^Ellis, Graham; Adatia, Ian; Yazdanpanah, Mehrdad; Makela, Sinikka K. (1998). "Nitrite and Nitrate Analyses: A Clinical Biochemistry Perspective". Clinical Biochemistry. 31 (4): 195–220. doi:10.1016/S0009-9120(98)00015-0. PMID 9646943.
  9. ^Powlson, David S.; Addiscott, Tom M.; Benjamin, Nigel; Cassman, Ken G.; De Kok, Theo M.; Van Grinsven, Hans; l'Hirondel, Jean-Louis; Avery, Alex A.; Van Kessel, Chris (2008). "When Does Nitrate Become a Risk for Humans?". Journal of Environmental Quality. 37 (2): 291–5. doi:10.2134/jeq2007.0177. PMID 18268290.
  10. ^"Nitrate and Nitrite Poisoning: Introduction". The Merck Veterinary Manual. Retrieved 2008-12-27.
  11. ^Addiscott, T.M.; Benjamin, N. (2006). "Nitrate and human health". Soil Use and Management. 20 (2): 98–104. doi:10.1111/j.1475-2743.2004.tb00344.x.
  12. ^A. A. Avery: Infant Methemoglobinemia - Reexamining the Role of Drinking Water Nitrates, Environmental Health Perspectives, Volume 107, Number 7, July 1999.
  13. ^Manassaram DM, Backer LC, Messing R, Fleming LE, Luke B, Monteilh CP (October 2010). "Nitrates in drinking water and methemoglobin levels in pregnancy: a longitudinal study". Environmental Health. 9 (1): 60. doi:10.1186/1476-069x-9-60. PMC 2967503. PMID 20946657.
  14. ^"4. What are EPA's drinking water regulations for nitrate?". Ground Water & Drinking Water. Retrieved 2018-11-13.
  15. ^Bagheri, H.; Hajian, A.; Rezaei, M.; Shirzadmehr, A. (2017). "Composite of Cu metal nanoparticles-multiwall carbon nanotubes-reduced graphene oxide as a novel and high performance platform of the electrochemical sensor for simultaneous determination of nitrite and nitrate". Journal of Hazardous Materials. 324 (Pt B): 762–772. doi:10.1016/j.jhazmat.2016.11.055. PMID 27894754.
  16. ^Romano N, Zeng C (September 2007). "Acute toxicity of sodium nitrate, potassium nitrate, and potassium chloride and their effects on the hemolymph composition and gill structure of early juvenile blue swimmer crabs(Portunus pelagicus Linnaeus, 1758) (Decapoda, Brachyura, Portunidae)". Environmental Toxicology and Chemistry. 26 (9): 1955–62. doi:10.1897/07-144r.1. PMID 17705664.
  17. ^Sharpe, Shirlie. "Nitrates in the Aquarium". Retrieved October 30, 2013.
  18. ^Romano N, Zeng C (December 2007). "Effects of potassium on nitrate mediated alterations of osmoregulation in marine crabs". Aquatic Toxicology. 85 (3): 202–8. doi:10.1016/j.aquatox.2007.09.004. PMID 17942166.
  19. ^"Nitrate Risk in Forage Crops - Frequently Asked Questions". Agriculture and Rural Development. Government of Alberta. Retrieved October 30, 2013.

External links[edit]

Nitric oxidesignalingmodulators

NO donors
  • Indirect/downstream NO modulators:ACE inhibitors/AT-II receptor antagonists (e.g., captopril, losartan)
  • ETB receptor antagonists (e.g., bosentan)
  • L-Type calcium channelblockers (e.g., dihydropyridines: nifedipine)
  • Nebivolol (beta blocker)
  • PDE5 inhibitors (e.g., sildenafil)
  • non-selective PDE inhibitors (e.g., caffeine)
  • PDE9 inhibitors (e.g., paraxanthine)
  • cGMP preferring PDE inhibitors (e.g., sildenafil, paraxanthine, tadalafil)
  • Statins (e.g., simvastatin)

See also:Receptor/signaling modulators

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A comparison of organic and inorganic nitrates/nitrites

Although both organic and inorganic nitrates/nitrites mediate their principal effects via nitric oxide, there are many important differences. Inorganic nitrate and nitrite have simple ionic structures and are produced endogenously and are present in the diet, whereas their organic counterparts are far more complex, and, with the exception of ethyl nitrite, are all medicinally synthesised products. These chemical differences underlie the differences in pharmacokinetic properties allowing for different modalities of administration, particularly of organic nitrates, due to the differences in their bioavailability and metabolic profiles. Whilst the enterosalivary circulation is a key pathway for orally ingested inorganic nitrate, preventing an abrupt effect or toxic levels of nitrite and prolonging the effects, this is not used by organic nitrates. The pharmacodynamic differences are even greater; while organic nitrates have potent acute effects causing vasodilation, inorganic nitrite's effects are more subtle and dependent on certain conditions. However, in chronic use, organic nitrates are considerably limited by the development of tolerance and endothelial dysfunction, whereas inorganic nitrate/nitrite may compensate for diminished endothelial function, and tolerance has not been reported. Also, while inorganic nitrate/nitrite has important cytoprotective effects against ischaemia-reperfusion injury, continuous use of organic nitrates may increase injury. While there are concerns that inorganic nitrate/nitrite may induce carcinogenesis, direct evidence of this in humans is lacking. While organic nitrates may continue to dominate the therapeutic arena, this may well change with the increasing recognition of their limitations, and ongoing discovery of beneficial effects and specific advantages of inorganic nitrate/nitrite.

Difference between Organic and Inorganic Compounds

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Inorganic is or no3 organic

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BCLN - Organic and Inorganic Compounds

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