EHSQL(Environment-Energy ,Health,Safety, Security and Social Ac. ,Quality-Lab) Technical services: Nitrate

Tuesday, 22 October 2013

Nitrate

Nitrate
Systematic name[hide] Nitrate
Properties
Molecular formula	NO− 3
Molar mass	62.0049 g mol^-1
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Infobox references

Nitrate is a polyatomic ion with the molecular formula NO₃⁻ and a molecular mass of 62.0049 g/mol. Nitrates also describe the organic functional group RONO₂. These nitrate esters are a specialized class of explosives.

     1 Structure
    2 Properties
    3 Occurrence
    4 Uses
        4.1 Other uses
    5 Detection
    6 Toxicity
        6.1 Toxicosis
        6.2 Human health effects
        6.3 Marine toxicity
    7 Nitrate overview
    8 See also
    9 References
    10 External links

Structure

The nitrate ion. The net charge of the whole ion s 1⁻.

The anion is the conjugate base of nitric acid, consisting of one central nitrogen atom surrounded by three identically bonded oxygen atoms in a trigonal planar arrangement. The nitrate ion carries a formal charge of -1. This 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 isoelectronic carbonate ion, the nitrate ion can be represented by resonance structures:

Canonical resonance structures for the nitrate ion

Properties

The nitrate ion with the partial charges shown

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).

Occurrence

Nitrate salts are found naturally on earth as large deposits, particularly of Chile saltpeter, a major source of sodium nitrate.
Nitrites are produced by a number of species of nitrifying bacteria, and the nitrate compounds for gunpowder were historically produced, in the absence of mineral nitrate sources, by means of various fermentation processes using urine and dung.

Uses

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

Other uses

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.

Detection

Free nitrate ions in solution can be detected by a nitrate ion selective electrode. Such electrodes function analogously to the pH selective electrode. This response is partially described by the Nernst equation.

Toxicity

Toxicosis

^{Nitrate toxicosis can occur through enterohepatic metabolism of nitrate to nitrite being an intermediate.[2] Nitrites oxidize the iron atoms in hemoglobin from ferrous iron (2+) to ferric iron (3+), rendering it unable to carry oxygen.[3] This process can lead to generalized lack of oxygen in organ tissue and a dangerous condition called methemoglobinemia. Although nitrite converts to ammonia, if there is more nitrite than can be converted, the animal slowly suffers from a lack of oxygen.[4]}

Human health effects

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. Methemoglobinemia in infants is known as blue baby syndrome. Although nitrates in drinking water were once thought to be a contributing factor, there are now significant scientific doubts as to whether there is a causal link.^[5]^[6] Blue baby syndrome is now thought to be the product of a number of factors, which can include any factor that causes gastric upset, such as diarrhoeal infection, protein intolerance, heavy metal toxicity etc., with nitrates playing a minor role. Nitrates, if a factor in a specific case, would most often be ingested by infants in high nitrate drinking water. However, nitrate exposure may also occur if eating, for instance, vegetables containing high levels of nitrate. Lettuce may contain elevated nitrate under growth conditions such as reduced sunlight, undersupply of the essential micronutrients molybdenum (Mo) and iron (Fe), or high concentrations of nitrate due to reduced assimilation of nitrate in the plant. High levels of nitrate fertilization also contribute to elevated levels of nitrate in the harvested plant.^[7]
Some adults can be more susceptible to the effects of nitrates than others. The methemoglobin reductase enzyme may be under-produced or absent in certain people that have an inherited mutation.^[8] Such individuals cannot break down methemoglobin as rapidly as those that do have the enzyme, leading to increased circulating levels of methemoglobin (the implication being that their blood is not as oxygen-rich). Those with insufficient stomach acid^[8] (including some vegetarians and vegans) may also be at risk. It is the increased consumption of green, leafy vegetables that typically accompany these types of diets may lead to increased nitrate intake. A wide variety of medical conditions, including food allergies, asthma,^[9] hepatitis, and gallstones may be linked with low stomach acid; these individuals may also be highly sensitive to the effects of nitrate.
Methemoglobinemia can be treated with methylene blue, which reduces ferric iron (3+) in affected blood cells back to ferrous iron (2+).^{[citation needed]}

Marine toxicity

Sea surface nitrate from the World Ocean Atlas.

In freshwater or estuarine systems close to land, nitrate can reach high levels that can potentially cause the death of fish. While nitrate is much less toxic than ammonia,^[10] levels over 30 ppm of nitrate can inhibit growth, impair the immune system and cause stress in some aquatic species.^[11] However, in light of inherent problems with past protocols on acute nitrate toxicity experiments, the extent of nitrate toxicity has been the subject of recent debate.^[12]
In most cases of excess nitrate concentrations in aquatic systems, the primary source is surface runoff from agricultural or landscaped areas that have received excess nitrate fertilizer. This is called eutrophication and can lead to algae blooms. As well as leading to water anoxia and dead zones, these blooms may cause other changes to ecosystem function, favouring some groups of organisms over others. As a consequence, as nitrate forms a component of total dissolved solids, they are widely used as an indicator of water quality.
Symptoms of nitrate poisoning 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:^[13]

Category	%NO₃	%NO₃-N	%KNO₃	Effects
1	<0.5	<0.12	<0.81	Generally safe for beef cattle and sheep
2	0.5-1.0	0.12-0.23	0.81-1.63	Caution - some subclinical symptoms may appear in pregnant horses, sheep and beef cattle
3	1.0	0.23	1.63	High nitrate problems - death losses and abortions can occur in beef cattle and sheep
4	<1.23	<0.28	<2.00	Maximum safe level for horses. Do not feed high nitrate forages to pregnant mares