|Jmol 3D model||Interactive image|
|Molar mass||84.9947 g/mol|
|Appearance||White powder or colorless crystals|
|Density||2.257 g/cm3, solid|
|Melting point||308 °C (586 °F; 581 K)|
|Boiling point||380 °C (716 °F; 653 K) decomposes|
|73 g/100 mL (0 °C)
91.2 g/100 mL (25 °C)
180 g/100 mL (100 °C)
|Solubility||very soluble in ammonia, hydrazine
soluble in alcohol
slightly soluble in pyridine
insoluble in acetone
Refractive index (nD)
|Viscosity||2.85 cP (317 °C)|
|trigonal and rhombohedral|
|93.05 J/(mol K)|
|116 J/(mol K)|
Std enthalpy of
Gibbs free energy (ΔfG˚)
|Main hazards||Oxidant, irritant|
|Safety data sheet||ICSC 0185|
EU classification (DSD)
|Lethal dose or concentration (LD, LC):|
LD50 (median dose)
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|what is ?)(|
Sodium nitrate is the chemical compound with the formula NaNO3. This alkali metal nitrate salt is also known as Chile saltpeter or Peru saltpeter (due to the large deposits found in the Atacama desert in these countries) 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 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.
The first shipment of Chile saltpeter to Europe arrived in England in 1820 or 1825, but did not find any buyers and was dumped at sea in order to avoid customs toll. With time, however, the mining of South American saltpeter became a profitable business (in 1859, England alone consumed 47,000 metric tons). Chile fought against the allies Peru and Bolivia in the War of the Pacific 1879-1884 and took over the richest deposits. In 1919, Ralph Walter Graystone Wyckoff determined its crystal structure using X-ray crystallography.
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. 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. 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. 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.
- 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
- NH4NO3 + NaOH → NaNO3 + NH4OH
- NH4NO3 + NaHCO3 → NaNO3 + NH4HCO3
- 2NH4NO3 + Na2CO3 → 2NaNO3 + (NH4)2CO3
Sodium nitrate was used extensively as a fertilizer and a raw material for the manufacture of gunpowder in the late 19th century. It can be combined with iron hydroxide to make a synthetic resin.
Sodium nitrate can be combined with sulfuric acid and nitric acid distilled off. At lower pressure the lower temperature needed results in less decomposition. The theoretical 2 moles of nitric acid per 1 mole of sulfuric acid results in a very high end temperature, much decomposition and a solid neutral sulfate that is difficult to remove. When this reaction was important industrially, it was common practice to operate with sulfuric acid in excess to end on a mostly bisulfate product poured molten out of the retort.
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, USA and Australia and New Zealand. Sodium nitrate should not be confused with sodium nitrite, which is also a common food additive and preservative used, for example, in deli meats.
Sodium nitrate is used together with potassium nitrate and calcium nitrate for heat storage and, more recently, for heat transfer in solar power plants. A mixture of sodium nitrate, calcium nitrate and potassium nitrate is used as energy-storage material in prototype plants, such as Andasol Solar Power Station and the Archimedes project.
It is also used in the wastewater industry for facultative microorganism respiration. Nitrosomonas, a genus of microorganisms, consumes nitrate in preference to oxygen, enabling it to grow more rapidly in the wastewater to be treated.
Sodium nitrate is also sometimes used by marine aquarists who utilize carbon-dosing techniques. It is used to increase nitrate levels in the water and promote bacterial growth.
Studies have shown a link between increased levels of nitrates and increased deaths from certain diseases including Alzheimer's, diabetes mellitus, Gastric Cancer, and Parkinson's: possibly through the damaging effect of nitrosamines on DNA, however, little is done to control for other possible causes in the epidemiological results. Nitrosamines, formed in cured meats containing sodium nitrate and nitrite, have been linked to gastric cancer and oesophageal cancer. Sodium nitrate and nitrite are associated with a higher risk of colorectal cancer. World Cancer Research Fund UK, states that one of the reasons that processed meat increases the risk of colon cancer is its content of nitrate. 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 NOCs (nitroso compounds). NOCs can be formed either when meat is cured or in the body as meat is digested.
For most people, the highest dietary source of nitrates is from fruits and vegetables and no studies have conclusively linked nitrates and nitrites to cancer or any other form of diseases. On the contrary, some research has hinted to beneficial properties of nitrites such as lowering blood pressure by slightly expanding arteries. The only reason nitrates and nitrites came under such legal scrutiny is when the US Food and Drug Administration presented a brief report which stated that some adverse effect was observed on mice (“depression of growth”) when their intake of nitrites was up to 90% of daily diet.[clarification needed]
- War of the Pacific, also known as "the Saltpeter War".
Notes and references
- Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A23. ISBN 0-618-94690-X.
- S. H. Baekeland "Några sidor af den kemiska industrien" (1914) Svensk Kemisk Tidskrift, p. 140.
- Friedrich Georg Wieck, Uppfinningarnas bok (1873, Swedish translation of Buch der Erfindungen), vol. 4, p. 473.
- Stephen R. Bown, A Most Damnable Invention: Dynamite, Nitrates, and the Making of the Modern World, Macmillan, 2005, ISBN 0-312-32913-X, p. 157.
- UK Food Standards Agency: "Current EU approved additives and their E Numbers". Retrieved 2011-10-27.
- US Food and Drug Administration: "Listing of Food Additives Status Part II". Retrieved 2011-10-27.
- Australia New Zealand Food Standards Code"Standard 1.2.4 - Labelling of ingredients". Retrieved 2011-10-27.
- Albert A. Robbins "Chemical freezing package" U.S. Patent 2,898,744, Issue date: August 1959.
- De La Monte, SM; Neusner, A; Chu, J; Lawton, M (2009). "Epidemilogical trends strongly suggest exposures as etiologic agents in the pathogenesis of sporadic Alzheimer's disease, diabetes mellitus, and non-alcoholic steatohepatitis". Journal of Alzheimer's disease : JAD. 17 (3): 519–29. doi:10.3233/JAD-2009-1070 (inactive 2015-02-02). PMID 19363256.
- Cross, AJ; Ferrucci, LM; Risch, A; Graubard, BI; Ward, MH; Park, Y; Hollenbeck, AR; Schatzkin, A; Sinha, R (2010). "A large prospective study of meat consumption and colorectal cancer risk: An investigation of potential mechanisms underlying this association". Cancer Research. 70 (6): 2406–14. doi:10.1158/0008-5472.CAN-09-3929. PMC . PMID 20215514.
- "Why does processed meat increase bowel cancer risk?", World Cancer Research Fund (2010) accessdate 2010-03-06
- Hord NG, Tang Y, Bryan NS. Food sources of nitrates and nitrites: the physiologic context for potential health benefits. Am J Clin Nutr 2009;90:1–10 
- Lehman AJ. Quarterly reports to the editor on topics of current interest - Nitrates and nitrites in meat products. Quarterly Bulletin Association of Food and Drug Officials of the United States 1958;22:136–8.
- Barnum, Dennis (2003). "Some History of Nitrates". Journal of Chemical Education. 80: 1393–. doi:10.1021/ed080p1393.
- 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
|Salts and covalent derivatives of the Nitrate ion|