Sodium chloride

"NaCl" redirects here. For the Google technology, see Google Native Client.

This article is about the chemical compound. For sodium chloride in the diet, see Salt. For sodium chloride as a mineral, see Halite.

Sodium chloride
IUPAC name Sodium chloride
Other names Common salt Halite Rock salt Saline Sodium chloric Table salt
Identifiers
CAS number	7647-14-5 Y
PubChem	5234
ChemSpider	5044 Y
UNII	451W47IQ8X Y
EC number	231-598-3
KEGG	D02056 Y
MeSH	Sodium+chloride
ChEBI	CHEBI:26710 Y
ChEMBL	CHEMBL1200574 N
RTECS number	VZ4725000
ATC code	A12CA01,B05CB01, B05XA03
Beilstein Reference	3534976
Gmelin Reference	13673
Jmol-3D images	Image 1
SMILES [Na+].[Cl-]
InChI InChI=1S/ClH.Na/h1H;/q;+1/p-1 Y Key: FAPWRFPIFSIZLT-UHFFFAOYSA-M Y InChI=1/ClH.Na/h1H;/q;+1/p-1 Key: FAPWRFPIFSIZLT-REWHXWOFAE
Properties
Molecular formula	NaCl
Molar mass	58.44 g mol−1
Exact mass	57.958622382 g mol−1
Appearance	Colorless crystals
Odor	Odorless
Density	2.165 g cm−3
Melting point	801 °C, 1074 K, 1474 °F
Boiling point	1413 °C, 1686 K, 2575 °F
Solubility in water	359 g L−1
Solubility in ammonia	21.5 g L−1
Solubility in methanol	14.9 g L−1
Acidity (pKa)	6.7–7.3
Basicity (pKb)	6.7–7.3
Refractive index (nD)	1.5442 (at 589 nm)
Structure
Crystal structure	Face-centered cubic (see text), cF8
Space group	Fm3m, No. 225
Lattice constant	a = 564.02 pm
Coordination geometry	Octahedral (Na+) Octahedral (Cl–)
Thermochemistry
Std enthalpy of formation ΔfHo298	-411.12 kJ mol−1
Standard molar entropy So298	72.11 J K−1 mol−1
Specific heat capacity, C	36.79 J K−1 mol−1
Hazards
MSDS	External MSDS
NFPA 704	0 0 0
LD50	3000–8000 mg/kg (oral in rats, mice, rabbits)[1]
Related compounds
Other anions	Sodium fluoride Sodium bromide Sodium iodide
Other cations	Lithium chloride Potassium chloride Rubidium chloride Caesium chloride
Supplementary data page
Structure and properties	n, εr, etc.
Thermodynamic data	Phase behaviour Solid, liquid, gas
Spectral data	UV, IR, NMR, MS
N (verify) (what is: Y/N?) Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Infobox references

Sodium chloride, also known as salt, common salt, table salt or halite, is an inorganic compound with the formula NaCl. Sodium chloride is the salt most responsible for the salinity of the ocean and of the extracellular fluid of many multicellular organisms. As the major ingredient in edible salt, it is commonly used as a condiment and food preservative.

Chemistry of solid and dissolved sodium chloride

Solid sodium chloride

See also: Cubic crystal system

In solid sodium chloride, each ion is surrounded by six ions of the opposite charge as expected on electrostatic grounds. The surrounding ions are located at the vertices of a regular octahedron. In the language of close-packing, the larger chloride ions are arranged in a cubic array whereas the smaller sodium ions fill all the cubic gaps (octahedral voids) between them. This same basic structure is found in many other compounds and is commonly known as the halite or rock-salt crystal structure. It can be represented as a face-centered cubic (fcc) lattice with a two-atom basis or as two interpenetrating face centered cubic lattices. The first atom is located at each lattice point, and the second atom is located half way between lattice points along the fcc unit cell edge.

Thermal conductivity of NaCl as a function of temperature has a maximum of 2.03 W/(cm K) at 8 K and decreases to 0.069 at 314 K (41 °C). It also decreases with doping.^[2]

Aqueous solutions

The attraction between the Na⁺ and Cl^- ions in the solid is so strong that only highly polar solvents like water dissolve NaCl well.

Solubility of NaCl in various solvents (g NaCl / 1 kg of solvent at 25 °C)[3]
H2O	360
Formamide	94
glycerin	83
propylene glycol	71
Formic acid	52
Liquid ammonia	30.2
Methanol	14
Ethanol	0.65
Dimethylformamide	0.4
1-propanol	0.124
Sulfolane	0.05
1-butanol	0.05
2-propanol	0.03
1-pentanol	0.018
Acetonitrile	0.003
Acetone	0.00042

When dissolved in water, the sodium chloride framework disintegrates as the Na⁺ and Cl^- ions become surrounded by the polar water molecules. These solutions consist of metal aquo complex with the formula [Na(H₂O)_x]⁺, where x is 8 with the Na-O distance of 250 pm. The chloride ions are also strongly solvated, each being surrounded by an average of 6 molecules of water.^[4] Solutions of sodium chloride have very different properties from pure water. The freezing point is −21.12 °C for 23.31 wt% of salt, and the boiling point of saturated salt solution is near 108.7 °C.^[5] From cold solutions, salt crystallises as the dihydrate NaCl^.2H₂O.

Occurrence

Small particles of sea salt are the dominant cloud condensation nuclei well out at sea, which allow the formation of clouds in otherwise non-polluted air.^[6]

Production

Modern rock salt mine near Mount Morris^{[disambiguation needed ]}, New York, United States

Salt is currently mass-produced by evaporation of seawater or brine from brine wells and salt lakes. mining of rock salt is also a major source. China is the world's main supplier of salt.^[7] In 2010, world production was estimated at 270 million tonnes, the top five producers (in million tonnes) being China (60.0), United States (45.0), Germany (16.5), India (15.8) and Canada (14.0).^[8]

Uses

In addition to the familiar domestic uses of salt, more dominant applications of the approximately 250 megatons/year production (2008 data) include chemicals and de-icing.^[9]

Chemicals production

Salt is the source, directly or indirectly, for the production of many chemicals, which consume most of the world's production.^[7]

Chlor-alkali industry

It is the starting point for the Chloralkali process, which provides the world with chlorine and sodium hydroxide according to the chemical equation:

2 NaCl + 2 H₂O → Cl₂ + H₂ + 2 NaOH

This electrolysis is conducted in a Down's cell in which sodium chloride is mixed with calcium chloride to lower the melting point below 700 °C. As calcium is more electropositive than sodium, no calcium will be formed at the cathode. This method is less expensive than the previous method of electrolyzing sodium hydroxide. Some application of chlorine include PVC, disinfectants, and solvents. From sodium hydroxide enables industries that produce paper, soap, and aluminium.

Soda ash industry

Via the Solvay process, sodium chloride is used to produce sodium carbonate and calcium chloride. Sodium carbonate is used to produce glass, sodium bicarbonate, and dyes as well as myriad other chemicals. In the Mannheim process and in the Hargreaves process, it is used for the production of sodium sulfate and hydrochloric acid.

Miscellaneous industrial uses

Sodium chloride is heavily used, so even miscellaneous applications can consume massive quantities. In oil and gas exploration, salt is an important component of drilling fluids in well drilling. It is used to flocculate and increase the density of the drilling fluid to overcome high downwell gas pressures. Whenever a drill hits a salt formation, salt is added to the drilling fluid to saturate the solution and to minimize the dissolution within the salt stratum.^[9]

Salt is also used to increase the curing of concrete in cemented casings.^[7] In textiles and dyeing, salt is used as a brine rinse to separate organic contaminants, to promote “salting out” of dyestuff precipitates, and to blend with concentrated dyes to standardize them. One of its main roles is to provide the positive ion charge to promote the absorption of negatively charged ions of dyes.^[7]

In metal processing, salt is used in concentrating uranium ore into uranium oxide (yellow cake). It also is used in processing aluminium, beryllium, copper, steel and vanadium. In the pulp and paper industry, salt is used to bleach wood pulp. It also is used to make sodium chlorate, which is added along with sulfuric acid and water to manufacture chlorine dioxide, an excellent oxygen-based bleaching chemical. The chlorine dioxide process, which originated in Germany after World War I, is becoming more popular because of environmental pressures to reduce or eliminate chlorinated bleaching compounds. In tanning and leather treatment, salt is added to animal hides to inhibit microbial activity on the underside of the hides and to attract moisture back into the hides.^[7]

In rubber manufacture, salt is used to make buna, neoprene and white rubber types. Salt brine and sulfuric acid are used to coagulate an emulsified latex made from chlorinated butadiene.^[9][7]

Salt also is added to secure the soil and to provide firmness to the foundation on which highways are built. The salt acts to minimize the effects of shifting caused in the subsurface by changes in humidity and traffic load.^[7]

Water softening

Hard water contains calcium and magnesium ions that interfere with action of soap and contribute to the buildup of a scale or film of alkaline mineral deposits in household and industrial equipment and pipes. Commercial and residential water-softening units use ion exchange resins to remove the offending ions that cause the hardness. These resins are generated and regenerated using sodium chloride.^[9][7]

Road salt

Phase diagram of water-NaCl mixture.

The second major application of salt is for deicing and anti-icing of roads, both in grit bins and spread by winter service vehicles. In anticipation of snowfall, roads are optimally "anti-iced" with brine (concentrated solution of salt in water), which prevents bonding between the snow-ice and the road surface. This procedures precludes the heavy use of salt after the snowfall. For de-icing, mixtures of brine and salt are used, sometimes with additional agents such as calcium and magnesium chloride. The use of salt or brine becomes ineffective below -10 °C.

Salt for de-icing in the United Kingdom predominantly comes from a single mine in Winsford in Cheshire. Prior to distribution it is mixed with <100 ppm of sodium hexacyanoferrate(II) as an anti-caking agent, which enables rock salt to flow freely out of the gritting vehicles despite being stockpiled prior to use. In recent years this additive has also been used in table salt. Other additives had been used in road salt to reduce the total costs. For example, in the US, a byproduct carbohydrate solution from sugar beet processing was mixed with rock salt and adhered to road surfaces about 40% better than loose rock salt alone. Because it stayed on the road longer, the treatment did not have to be repeated several times, saving time and money.^[7]

In the technical terms of physical chemistry, the minimum freezing point of a water-salt mixture is −21.12 °C for 23.31 wt% of salt. Freezing near this concentration is however so slow that the eutectic point of −22.4 °C can be reached with about 25 wt% of salt.^[5]

Environmental effect

Road salt ends up in fresh water bodies and could harm aquatic plants and animals by disrupting their osmoregulation ability.^[10] The omnipresence of salt poses a problem in any coastal coating application, as trapped salts cause great problems in adhesion. Naval authorities and ship builders monitor the salt concentrations on surfaces during construction. Maximum salt concentrations on surfaces are dependent on the authority and application. The IMO regulation is mostly used and sets salt levels to a maximum of 50 mg/m² soluble salts measured as sodium chloride. These measurements are done by means of a Bresle test.

In highway deicing, salt has been associated with corrosion of bridge decks, motor vehicles, reinforcement bar and wire, and unprotected steel structures used in road construction. Surface runoff, vehicle spraying, and windblown actions also affect soil, roadside vegetation, and local surface water and groundwater supplies. Although evidence of environmental loading of salt has been found during peak usage, the spring rains and thaws usually dilute the concentrations of sodium in the area where salt was applied.^[7]

Food industry, medicine and agriculture

Main article: Salt

Many micro organisms cannot live in an overly salty environment: water is drawn out of their cells by osmosis. For this reason salt is used to preserve some foods, such as smoked bacon or fish. It can also be used to detach leeches that have attached themselves to feed. It is also used to disinfect wounds.

Salt is added in most food items, by the food processor or by the consumer, as a flavor enhancer, preservative, binder, fermentation-control additive, texture-control agent and color developer. The salt consumption in the food industry is subdivided, in descending order of consumption, into other food processing, meat packers, canning, baking, dairy and grain mill products. Salt is added to promote color development in bacon, ham and other processed meat products. As a preservative, salt inhibits the growth of bacteria. Salt acts as a binder in sausages to form a binding gel made up of meat, fat, and moisture. Salt also acts as a flavor enhancer and as a tenderizer.^[7]

In the dairy industry, salt is added to cheese as a color-, fermentation-, and texture-control agent. The dairy subsector includes companies that manufacture creamery butter, condensed and evaporated milk, frozen desserts, ice cream, natural and processed cheese, and specialty dairy products. In canning, salt is primarily added as a flavor enhancer and preservative. It also is used as a carrier for other ingredients, dehydrating agent, enzyme inhibitor and tenderizer. In baking, salt is added to control the rate of fermentation in bread dough. It also is used to strengthen the gluten (the elastic protein-water complex in certain doughs) and as a flavor enhancer, such as a topping on baked goods. The food-processing category also contains grain mill products. These products consist of milling flour and rice and manufacturing cereal breakfast food and blended or prepared flour. Salt is also used a seasoning agent, e.g. in potato chips, pretzels, cat and dog food.^[7]

Sodium chloride is used in veterinary medicine as emesis causing agent. It is given as warm saturated solution. Emesis can also be caused by pharyngeal placement of small amount of plain salt or salt crystals.

Firefighting

A class D fire extinguisher for various metals

Sodium chloride is the principal extinguishing agent in fire extinguishers (Met-L-X, Super D) used on combustible metal fires such as magnesium, potassium, sodium, and NaK alloys (Class D). Thermoplastic powder is added to the mixture, along with waterproofing (metal stearates) and anti-caking materials (tricalcium phosphate) to form the extinguishing agent. When it is applied to the fire, the salt acts like a heat sink, dissipating heat from the fire, and also forms an oxygen-excluding crust to smother the fire. The plastic additive melts and helps the crust maintain its integrity until the burning metal cools below its ignition temperature. This type of extinguisher was invented in the late 1940s in the cartridge-operated type shown here, although stored pressure versions are now popular. Common sizes are 30 lb portable and 350 lb wheeled.

Cleanser

Since at least medieval times, people have used salt as a cleansing agent rubbed on household surfaces. It is also used in many brands of shampoo, toothpaste and popularly to de-ice driveways and patches of ice.

Biological functions

For further information about sodium chloride in the diet, see Salt.

In humans, a high-salt intake has long been suspected to generally raise blood pressure.^{[citation needed]} More recently, it was demonstrated to attenuate nitric oxide production. Nitric oxide (NO) contributes to vessel homeostasis by inhibiting vascular smooth muscle contraction and growth, platelet aggregation, and leukocyte adhesion to the endothelium.^[11][12]

• 

  Jordanian and Israeli salt evaporation ponds at the south end of the Dead Sea.

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  Mounds of salt, Salar de Uyuni, Bolivia.

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  Evaporation lagoons, Aigues-Mortes, France.

See also

• Biosalinity
• Kala Namak
• Halite, the mineral form of sodium chloride
• Salinity
• Salt
• Soap
• Salting the earth

References

 This article incorporates public domain material from the United States Geological Survey document "Salt".

1. ^ Martel, B.; Cassidy, K. (2004). Chemical Risk Analysis: A Practical Handbook. Butterworth–Heinemann. p. 369. ISBN 1903996651. 
2. ^ Dinker B. Sirdeshmukh, Lalitha Sirdeshmukh, K. G. Subhadra (2001). Alkali halides: a handbook of physical properties. Springer. pp. 65, 68. ISBN 3540421807. http://books.google.com/books?id=X-yL7EgMK6wC&pg=PA68. 
3. ^ Burgess, J. (1978). Metal Ions in Solution. New York: Ellis Horwood. ISBN 0-85312-027-7. 
4. ^ S. F. Lincoln, D. T. Richens, A. G. Sykes "Metal Aqua Ions" Comprehensive Coordination Chemistry II Volume 1, Pages 515-555. doi:10.1016/B0-08-043748-6/01055-0
5. ^ ^{a b} Elvers, B. et al. (ed.) (1991) Ullmann's Encyclopedia of Industrial Chemistry, 5th ed. Vol. A24, Wiley, ISBN 978-3527201242 p. 319
6. ^ B. J. Mason (2006-12-19). "The role of sea-salt particles as cloud condensation nuclei over the remote oceans". The Quarterly Journal of the Royal Meteorological Society 127 (576): 2023–32. doi:10.1002/qj.49712757609. http://www3.interscience.wiley.com/journal/114028130/abstract. 
7. ^ ^{a b c d e f g h i j k l} Dennis S. Kostick Salt, U.S. Geological Survey, 2008 Minerals Yearbook
8. ^ Salt, U.S. Geological Survey
9. ^ ^{a b c d} Gisbert Westphal, Gerhard Kristen, Wilhelm Wegener, Peter Ambatiello, Helmut Geyer, Bernard Epron, Christian Bonal, Georg Steinhauser, Franz Götzfried "Sodium Chloride" in Ullmann's Encyclopedia of Industrial Chemistry, 2002, Wiley-VCH, Weinheim doi:10.1002/14356007.a24_317.pub4
10. ^ Does road salt harm the environment?
11. ^ Osanai T, Fujiwara N, Saitoh M, et al. (2002). "Relationship between salt intake, nitric oxide and asymmetric dimethylarginine and its relevance to patients with end-stage renal disease". Blood Purif. 20 (5): 466–8. doi:10.1159/000063555. PMID 12207094. http://content.karger.com/produktedb/produkte.asp?typ=fulltext&file=bpu20466. 
12. ^ McCarron, David A. (2008). "Dietary sodium and cardiovascular and renal disease risk factors: dark horse or phantom entry?". Nephrol Dial Transplant 23 (7): 2133–7. doi:10.1093/ndt/gfn312. PMC 2441768. PMID 18587159. http://www.pubmedcentral.nih.gov/articlerender.fcgi?tool=pmcentrez&artid=2441768. 

External links

• The Salt Manufacturers Association website
• Salt Archive website
• Salt United States Geological Survey Statistics and Information
• "Using Salt and Sand for Winter Road Maintenance". Road Management Journal. December 1997. http://www.usroads.com/journals/p/rmj/9712/rm971202.htm. 
• Dejima Y, Fukuda S, Ichijoh Y, Takasaka K, Ohtsuka R (June 1996). "Cold-induced salt intake in mice and catecholamine, renin and thermogenesis mechanisms". Appetite 26 (3): 203–19. doi:10.1006/appe.1996.0016. PMID 8800478. http://linkinghub.elsevier.com/retrieve/pii/S0195-6663(96)90016-1.  — Salt Intake in Cold Weather
• Oxford MSDS
• JtBaker MSDS