Sodium nitrate

Sodium nitrate

Names
IUPAC name Sodium nitrate
Other names Peru saltpeter Soda niter cubic niter
Identifiers
CAS Number	7631-99-4 Y
3D model (JSmol)	Interactive image
ChEMBL	ChEMBL1644698 N
ChemSpider	22688 Y
ECHA InfoCard	100.028.686
EC Number	231-554-3
E number	E251 (preservatives)
PubChem CID	24268
RTECS number	WC5600000
UNII	8M4L3H2ZVZ Y
UN number	1498
CompTox Dashboard (EPA)	DTXSID6020937
show InChI InChI=1S/NO3.Na/c2-1(3)4;/q-1;+1 Y Key: VWDWKYIASSYTQR-UHFFFAOYSA-N Y InChI=1/NO3.Na/c2-1(3)4;/q-1;+1 Key: VWDWKYIASSYTQR-UHFFFAOYAL
show SMILES [Na+].[O-][N+]([O-])=O
Properties
Chemical formula	NaNO3
Molar mass	84.9947 g/mol
Appearance	White powder or colorless crystals
Odor	sweet
Density	2.257 g/cm3, solid
Melting point	308 °C (586 °F; 581 K)
Boiling point	380 °C (716 °F; 653 K) decomposes
Solubility in water	73 g/100 g water (0 °C) 91.2 g/100 g water (25 °C)[1][2] 180 g/100 g water (100 °C)
Solubility	very soluble in ammonia, hydrazine soluble in alcohol slightly soluble in pyridine insoluble in acetone
Magnetic susceptibility (χ)	−25.6·10−6 cm3/mol
Refractive index (nD)	1.587 (trigonal) 1.336 (rhombohedral)
Viscosity	2.85 cP (317 °C)
Structure
Crystal structure	trigonal and rhombohedral
Thermochemistry
Heat capacity (C)	93.05 J/(mol K)
Std molar entropy (So298)	116 J/(mol K)[3]
Std enthalpy of formation (ΔfH⦵298)	−467 kJ/mol[3]
Gibbs free energy (ΔfG˚)	−365.9 kJ/mol
Hazards
Main hazards	Harmful (Xn) Oxidant (O)
Safety data sheet	ICSC 0185
GHS pictograms
NFPA 704 (fire diamond)	1 0 0 OX
Flash point	Non-flammable
Lethal dose or concentration (LD, LC):
LD50 (median dose)	3236 mg/kg
Related compounds
Other anions	Sodium nitrite
Other cations	Lithium nitrate Potassium nitrate Rubidium nitrate Caesium nitrate
Related compounds	Sodium sulfate Sodium chloride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N  (what is YN ?)
Infobox references

Advertisement for sodium nitrate fertilizer from Chile on a wall of a village in the Algarve area of Portugal

Sodium nitrate is the chemical compound with the formula NaNO
₃. This alkali metal nitrate salt is also known as Chile saltpeter (large deposits of which were historically mined in Chile)^[4][5] to distinguish it from ordinary saltpeter, potassium nitrate. The mineral form is also known as nitratine, nitratite or soda niter.

Sodium nitrate is a white deliquescent solid very soluble in water. It is a readily available source of the nitrate anion (NO₃⁻), which is useful in several reactions carried out on industrial scales for the production of fertilizers, pyrotechnics and smoke bombs, glass and pottery enamels, food preservatives (esp. meats), and solid rocket propellant. It has been mined extensively for these purposes.

History[]

The first shipment of saltpeter to Europe arrived in England from Peru in 1820 or 1825, right after that country's independence from Spain, but did not find any buyers and was dumped at sea in order to avoid customs toll.^[6][7] With time, however, the mining of South American saltpeter became a profitable business (in 1859, England alone consumed 47,000 metric tons^[7]). Chile fought the War of the Pacific (1879–1884) against the allies Peru and Bolivia and took over their richest deposits of saltpeter. In 1919, Ralph Walter Graystone Wyckoff determined its crystal structure using X-ray crystallography.

Occurrence[]

The largest accumulations of naturally occurring sodium nitrate are found in Chile and Peru, where nitrate salts are bound within mineral deposits called caliche ore.^[8] Nitrates accumulate on land through marine-fog precipitation and sea-spray oxidation/desiccation followed by gravitational settling of airborne NaNO₃, KNO₃, NaCl, Na₂SO₄, and I, in the hot-dry desert atmosphere.^[9] El Niño/La Niña extreme aridity/torrential rain cycles favor nitrates accumulation through both aridity and water solution/remobilization/transportation onto slopes and into basins; capillary solution movement forms layers of nitrates; pure nitrate forms rare veins. For more than a century, the world supply of the compound was mined almost exclusively from the Atacama desert in northern Chile until, at the turn of the 20th century, German chemists Fritz Haber and Carl Bosch developed a process for producing ammonia from the atmosphere on an industrial scale (see Haber process). With the onset of World War I, Germany began converting ammonia from this process into a synthetic Chilean saltpeter, which was as practical as the natural compound in production of gunpowder and other munitions. By the 1940s, this conversion process resulted in a dramatic decline in demand for sodium nitrate procured from natural sources.

Chile still has the largest reserves of caliche, with active mines in such locations as Pedro de Valdivia, María Elena and Pampa Blanca, and there it used to be called white gold.^[4][5] Sodium nitrate, potassium nitrate, sodium sulfate and iodine are all obtained by the processing of caliche. The former Chilean saltpeter mining communities of Humberstone and Santa Laura were declared Unesco World Heritage sites in 2005.

Synthesis[]

Sodium nitrate is also synthesized industrially by neutralizing nitric acid with sodium carbonate or sodium bicarbonate:

2 HNO₃ + Na₂CO₃ → 2 NaNO₃ + H₂O + CO₂

HNO₃ + NaHCO₃ → NaNO₃ + H₂O + CO₂

or also by neutralizing it with sodium hydroxide (however, this reaction is very exothermic):

HNO₃ + NaOH → NaNO₃ + H₂O

or by mixing stoichiometric amounts of ammonium nitrate and sodium hydroxide, sodium bicarbonate or sodium carbonate:

NH₄NO₃ + NaOH → NaNO₃ + NH₄OH

NH₄NO₃ + NaHCO₃ → NaNO₃ + NH₄HCO₃

2NH₄NO₃ + Na₂CO₃ → 2NaNO₃ + (NH₄)₂CO₃

Uses[]

Most sodium nitrate is used in fertilizers, where it supplies a water soluble form of nitrogen. Its use, which is mainly outside of the Western World, is attractive since it doess not alter the pH of the soil. Another major use is as a complement to ammonium nitrate in explosives. Molten sodium nitrate and its solutions with potassium nitrate have good thermal stability (up to 600 °C) and high heat capacities. These properties are suitable for thermally annealing metals and for storing thermal energy in solar applications.^[10]

Food[]

Sodium nitrate is also a food additive used as a preservative and color fixative in cured meats and poultry; it is listed under its INS number 251 or E number E251. It is approved for use in the EU,^[11] US^[12] and Australia and New Zealand.^[13] Sodium nitrate should not be confused with sodium nitrite, which is also a common food additive and preservative used, for example, in deli meats.

Thermal storage[]

Sodium nitrate has also been investigated as a phase-change material for thermal energy recovery, owing to its relatively high melting enthalpy of 178 J/g.^[14][15] Examples of the applications of sodium nitrate used for thermal energy storage include solar thermal power technologies and direct steam generating parabolic troughs.^[14]

Health concerns[]

Studies have shown a link between increased levels of nitrates and increased deaths from certain diseases including Alzheimer's disease, diabetes mellitus, stomach cancer, and Parkinson's disease: possibly through the damaging effect of nitrosamines on DNA; however, little has been done to control for other possible causes in the epidemiological results.^[16] Nitrosamines, formed in cured meats containing sodium nitrate and nitrite, have been linked to gastric cancer and esophageal cancer.^[17] Sodium nitrate and nitrite are associated with a higher risk of colorectal cancer.^[18]

Substantial evidence in recent decades, facilitated by an increased understanding of pathological processes and science, exists in support of the theory that processed meat increases the risk of colon cancer and that this is due to the nitrate content. A small amount of the nitrate added to meat as a preservative breaks down into nitrite, in addition to any nitrite that may also be added. The nitrite then reacts with protein-rich foods (such as meat) to produce carcinogenic NOCs (nitroso compounds). NOCs can be formed either when meat is cured or in the body as meat is digested.^[19]

However, several things complicate the otherwise straightforward understanding of "nitrates in food raise your risk of cancer": Commonly consumed plants are well known to be rich sources of nitrates. In fact, exposure of nitrates from plants may even be higher than meat for most people. Processed meats have no fiber, vitamins, or phytochemical antioxidants, are high in sodium, may contain high fat, and are often fried or cooked at a temperature sufficient to degrade protein into nitrosamines, and typically not consumed as part of a nutritious, balanced diet with high fiber, vitamins, minerals, and the like. Nitrates are key intermediates and effectors in the primary vasculature signaling which is necessary for all mammals to survive.^[20]

See also[]

• Sodium nitrite

References[]

Further reading[]

• Archer, Donald G. (2000). "Thermodynamic properties of the NaNO₃ + H₂O system". Journal of Physical and Chemical Reference Data. 29 (5): 1141–1156. doi:10.1063/1.1329317. ISSN 0047-2689.
• Barnum, Dennis (2003). "Some history of nitrates". Journal of Chemical Education. 80 (12): 1393–. Bibcode:2003JChEd..80.1393B. doi:10.1021/ed080p1393.
• Mullin, J. W. (1997). Crystallization. Butterworth-Heinemann. ISBN 978-0-7506-3759-6.

External links[]

• ATSDR – Case Studies in Environmental Medicine – Nitrate/Nitrite Toxicity U.S. Department of Health and Human Services (public domain)
• FAO/WHO report
• Calculators: surface tensions, and densities, molarities and molalities of aqueous sodium nitrate