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20-September-2008 09:55:50 - Sodium chloride For sodium chloride in the diet, see salt. Sodium chloride IUPAC name Sodium chloride Other names Common salt; halite; table salt Identifiers CAS number 7647-14-5 RTECS number VZ4725000 Properties Molecular formula NaCl Molar mass 58.44277 g/mol Appearance White or colorless crystals or powder Density 2.16 g/cm³, solid Melting point 801 °C Boiling point 1465 °C 1738 K Solubility in water 35.9 g/100 mL 25 °C Structure Crystal structure Face centered cubic Coordination geometry Octahedral Hazards MSDS External MSDS Main hazards Might sting eyes, prolonged exposure to flame and air liberates strong acid NFPA 704 0 1 1 R-phrases R36 S-phrases S15,S25,S47 Flash point Non-flammable Related compounds Other anions NaF, NaBr, NaI Other cations LiCl, KCl, RbCl, CsCl, MgCl2, CaCl2 Related salts Sodium acetate Supplementary data page Structure and properties n, εr, etc. Thermodynamic data Phase behaviour Solid, liquid, gas Spectral data UV, IR, NMR, MS 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 common salt, table salt, or halite, is a chemical 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. In one gram of sodium chloride, there are approximately 0.3933 grams of sodium, and 0.6067 grams of chlorine. Contents 1 Production and use 1.1 Synthetic uses 1.2 Biological uses 1.3 Household uses 2 Biological functions 3 Crystal structure 4 Road salt 4.1 Additives 4.2 Common chemicals 5 See also 6 References 7 External links Production and use Salt is currently mass-produced by evaporation of seawater or brine from other sources, such as brine wells and salt lakes, and by mining rock salt, called halite. In 2002, world production was estimated at 210 million metric tonnes, the top five producers being the United States 40.3 million tonnes, China 32.9, Germany 17.7, India 14.5, and Canada 12.3.1 As well as the familiar uses of salt in cooking, salt is used in many applications, from manufacturing pulp and paper to setting dyes in textiles and fabric, to producing soaps, detergents, and other bath products. In cold countries, large quantities of rock salt are used to help clear highways of ice during winter, although Road Salt loses its melting ability at temperatures below -15°C to -20°C 5°F to -4°F. Sodium chloride is sometimes used as a cheap and safe desiccant due to its hygroscopic properties, making salting an effective method of food preservation historically. Even though more effective desiccants are available, few are safe for humans to ingest. Israeli and Jordanian salt evaporation ponds at the south end of the Dead Sea Mounds of salt, Salar de Uyuni, Bolivia. Modern rock salt mine near Mount Morris, New York. Evaporation lagoons, Aigues-Mortes, France Solubility of NaCl in various solvents g NaCl / 100 g of solvent at 25 °C H2O 36 Liquid ammonia 3.02 Methanol 1.4 Sulfolane 0.005 Formic acid 5.2 Acetone 0.000042 Formamide 9.4 Acetonitrile 0.0003 Dimethylformamide 0.04 Reference: Burgess, J. Metal Ions in Solution Ellis Horwood, New York, 1978 ISBN 0-85312-027-7 Synthetic uses Salt is also the raw material used to produce chlorine which itself is required for the production of many modern materials including PVC and pesticides. Industrially, elemental chlorine is usually produced by the electrolysis of sodium chloride dissolved in water. Along with chlorine, this chloralkali process yields hydrogen gas and sodium hydroxide, according to the chemical equation 2NaCl + 2H2O → Cl2 + H2 + 2NaOH Sodium metal is produced commercially through the electrolysis of liquid sodium chloride. This is done 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. Sodium chloride is used in other chemical processes for the large-scale production of compounds containing sodium or chlorine. In the Solvay process, sodium chloride is used for producing sodium carbonate and calcium chloride. In the Mannheim process and in the Hargreaves process, it is used for the production of sodium sulfate and hydrochloric acid. Biological uses Many microorganisms 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 and can also be used to detach leeches that have attached themselves to feed. It has also been used to disinfect wounds. Household uses Since at least medieval times, people have used salt as a cleansing agent rubbed on household surfaces. Biological functions In humans, a high-salt intake has long been known to generally raise blood pressure, especially in certain individuals. 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 1 Dietary sodium and cardiovascular and renal disease risk factors: dark horse or phantom entry? http://ndt.oxfordjournals.org/cgi/reprint/23/7/2133 Crystal structure The crystal structure of sodium chloride. Each atom has six nearest neighbors, with octahedral geometry. The crystal structure of sodium chloride. Each atom has six nearest neighbors, with octahedral geometry. Sodium chloride forms crystals with cubic symmetry. In these, the larger chloride ions, shown to the right as green spheres, are arranged in a cubic close-packing, while the smaller sodium ions, shown to the right as silver spheres, fill the octahedral gaps between them. Each ion is surrounded by six ions of the other kind. This same basic structure is found in many other minerals, and is known as the halite structure. This arrangement is known as cubic close packed ccp. It can be represented as two interpenetrating face-centered cubic fcc lattices, or one fcc lattice with a two atom basis. It is most commonly known as the rocksalt crystal structure. It is held together with an ionic bond and electrostatic forces. Road salt While salt was once a scarce commodity in history, industrialized production has now made salt plentiful. About 51% of world output is now used by cold countries to de-ice roads in winter, both in grit bins and spread by winter service vehicles. This works because salt and water form a eutectic mixture. Adding salt to water will lower the freezing temperature of the water, depending on the concentration. The salinity S of water is measured as grams salt per kilogram 1000g water, and the freezing temperatures are as follows. Sg/kg 0 10 20 24.7 30 35 Tfreezing C 0 -0.5 -1.08 -1.33 -1.63 -1.91 Additives Table salt sold for consumption today is not pure sodium chloride. In 1911 magnesium carbonate was first added to salt to make it flow more freely.2 In 1924 trace amounts of iodine in form of sodium iodide, potassium iodide or potassium iodate were first added, to reduce the incidence of simple goiter.3 Salt for de-icing in the UK typically contains sodium hexacyanoferrate II at less than 100ppm as an anti-caking agent. In recent years this additive has also been used in table salt. Common chemicals Chemicals used in de-icing salts are mostly found to be sodium chloride NaCl or calcium chloride CaCl2. Both are similar and are effective in de-icing roads. When these chemicals are produced, they are mined/made, crushed to fine granules, then treated with an anti-caking agent. Adding salt lowers the freezing point of the water, which allows the liquid to be stable at lower temperatures and allows the ice to melt. Alternative de-icing chemicals have also been used. Chemicals such as calcium magnesium acetate and potassium formate are being produced. These chemicals have few of the negative chemical effects on the environment commonly associated with NaCl and CaCl2.45 See also Wikibooks Wikibooks Cookbook has an article on Salt Wikimedia Commons has media related to: Sodium chloride Biosalinity Black salt Edible salt Halite, the mineral form of sodium chloride Salinity Soap Salting the earth References ^ Susan R. Feldman. Sodium chloride. Kirk-Othmer Encyclopedia of Chemical Technology. John Wiley Sons, Inc. Published online 2005. doi:10.1002/0471238961.1915040902051820.a01.pub2 ^ Morton Salt FAQ. ^ Markel H 1987. When it rains it pours: endemic goiter, iodized salt, and David Murray Cowie, MD. American journal of public health 77 2: 219-29. PMID 3541654. ^ Finnish Environment Institute 1/9/2007. Migration of alternative de-icing chemicals in aquifers MIDAS. Press release. ^ Finnish Environment Institute 2/10/2004. Alternative de-icer found. Press release. External links The Salt Manufacturers Association website Salt Institute website Salt Archive website Video of rotating rock salt unit cell divx, 378kb Salt United States Geological Survey Statistics and Information US Road Management website Salt Intake in Cold Weather Retrieved from http://en..org/wiki/Sodium_chloride Categories: Chlorides | Sodium compounds | Edible salt | Metal halides | Salts | Granular materials | Preservatives | Antiseptics | Snow removal Views Article Discussion this page History Personal tools Log in / create account Navigation Main page Contents Featured content Current events Random article Search Go Search Interaction Community portal Recent changes Contact Donate to Help Toolbox What links here Related changes Upload file Special pages Printable version Permanent link Cite this page Languages አማáˆáŠ› العربية AzÉ™rbaycan БългарÑ?ки Català Česky Cymraeg Dansk Deutsch Eesti Español Esperanto Ù?ارسی Français Galego í•œêµì–´ Hrvatski Bahasa Indonesia Ã?slenska Italiano עברית Latina LatvieÅ¡u Lietuvių Magyar Bahasa Melayu Nederlands 日本語 ქáƒ?რთული ‪Norsk bokmÃ¥l‬ Nouormand Plattdüütsch Polski Português Runa Simi РуÑ?Ñ?кий Sicilianu Simple English SlovenÄ?ina СрпÑ?ки / Srpski Suomi Svenska ไทย Tiếng Việt УкраїнÑ?ька ä¸æ–‡ This page was last modified on 3 August 2008, at 18:0
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