Difference between revisions of "Sodium chloride"
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| verifiedrevid = 262758507 | | verifiedrevid = 262758507 | ||
| Name = Sodium chloride | | Name = Sodium chloride | ||
| − | | ImageFile = | + | | ImageFile = Sodiumchloride crystal 01.jpg |
| ImageFile1 = Sodium-chloride-3D-ionic.png | | ImageFile1 = Sodium-chloride-3D-ionic.png | ||
| IUPACName = Sodium chloride | | IUPACName = Sodium chloride | ||
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| ChemSpiderID = 5044 | | ChemSpiderID = 5044 | ||
| RTECS = VZ4725000 | | RTECS = VZ4725000 | ||
| − | + | }} | |
| Section2 = {{Chembox Properties | | Section2 = {{Chembox Properties | ||
| Formula = [[Sodium|Na]][[Chlorine|Cl]] | | Formula = [[Sodium|Na]][[Chlorine|Cl]] | ||
| Line 32: | Line 32: | ||
| RefractIndex = 1.5442 (589 nm) | | RefractIndex = 1.5442 (589 nm) | ||
| pKa = 6.7–7.3 | | pKa = 6.7–7.3 | ||
| − | + | }} | |
| Section3 = {{Chembox Structure | | Section3 = {{Chembox Structure | ||
| CrystalStruct = Face-centered cubic <br>(''see text''), [[Pearson symbol|cF8]] | | CrystalStruct = Face-centered cubic <br>(''see text''), [[Pearson symbol|cF8]] | ||
| Line 38: | Line 38: | ||
| Coordination = Octahedral (Na<sup>+</sup>)<br/>Octahedral (Cl<sup>–</sup>) | | Coordination = Octahedral (Na<sup>+</sup>)<br/>Octahedral (Cl<sup>–</sup>) | ||
| LattConst_a = 564.02 pm | | LattConst_a = 564.02 pm | ||
| − | + | }} | |
| Section7 = {{Chembox Hazards | | Section7 = {{Chembox Hazards | ||
| ExternalMSDS = | | ExternalMSDS = | ||
| Line 49: | Line 49: | ||
| SPhrases = | | SPhrases = | ||
| LD50 = 3000–8000 mg/kg (oral in rats, mice, rabbits)<ref>{{Cite book|author = Martel, B.; Cassidy, K.|title = Chemical Risk Analysis: A Practical Handbook|publisher = Butterworth–Heinemann|year = 2004|page = 369|isbn = 1903996651|postscript = <!--None-->}}</ref> | | LD50 = 3000–8000 mg/kg (oral in rats, mice, rabbits)<ref>{{Cite book|author = Martel, B.; Cassidy, K.|title = Chemical Risk Analysis: A Practical Handbook|publisher = Butterworth–Heinemann|year = 2004|page = 369|isbn = 1903996651|postscript = <!--None-->}}</ref> | ||
| − | + | }} | |
| Section8 = {{Chembox Related | | Section8 = {{Chembox Related | ||
| OtherAnions = [[Sodium fluoride]]<br/>[[Sodium bromide]]<br/>[[Sodium iodide]] | | OtherAnions = [[Sodium fluoride]]<br/>[[Sodium bromide]]<br/>[[Sodium iodide]] | ||
| OtherCations = [[Lithium chloride]]<br/>[[Potassium chloride]]<br/>[[Rubidium chloride]]<br/>[[Caesium chloride]] | | OtherCations = [[Lithium chloride]]<br/>[[Potassium chloride]]<br/>[[Rubidium chloride]]<br/>[[Caesium chloride]] | ||
| − | + | }} | |
}} | }} | ||
'''Sodium chloride''', also known as '''salt''', ''' common salt''', '''table salt''', or [[halite]], is an [[ionic compound]] with the [[chemical formula|formula]] [[Sodium|Na]][[Chloride|Cl]]. Sodium chloride is the [[salt (chemistry)|salt]] most responsible for the salinity of the [[ocean]] and of the [[extracellular fluid]] of many multicellular [[organism]]s. As the major ingredient in [[edible salt]], it is commonly used as a [[condiment]] and food [[preservative]]. | '''Sodium chloride''', also known as '''salt''', ''' common salt''', '''table salt''', or [[halite]], is an [[ionic compound]] with the [[chemical formula|formula]] [[Sodium|Na]][[Chloride|Cl]]. Sodium chloride is the [[salt (chemistry)|salt]] most responsible for the salinity of the [[ocean]] and of the [[extracellular fluid]] of many multicellular [[organism]]s. As the major ingredient in [[edible salt]], it is commonly used as a [[condiment]] and food [[preservative]]. | ||
| + | |||
| + | ==Properties== | ||
| + | [[Thermal conductivity]] of pure 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.<ref>Dinker B. Sirdeshmukh, Lalitha Sirdeshmukh, K. G. Subhadra [http://books.google.com/books?id=X-yL7EgMK6wC&pg=PA68 Alkali halides: a handbook of physical properties], Springer, 2001 ISBN 3540421807 pp. 65, 68</ref> | ||
==Production and use== | ==Production and use== | ||
| − | [[ | + | [[File:Salt mine 0096.jpg|thumb|left|Modern rock salt mine near [[Mount Morris, New York|Mount Morris]], [[New York]], [[United States]]]] |
| − | Salt is currently [[Mass production|mass-produced]] by [[evaporation]] of [[seawater]] or [[brine]] from other sources, such as [[brine well]]s and [[salt lake (geography)|salt lake]]s, and by [[salt mine|mining]] '''rock salt''', called [[halite]]. In | + | Salt is currently [[Mass production|mass-produced]] by [[evaporation]] of [[seawater]] or [[brine]] from other sources, such as [[brine well]]s and [[salt lake (geography)|salt lake]]s, and by [[salt mine|mining]] '''rock salt''', called [[halite]]. In 2009, world production was estimated at 260 million [[metric ton]]s, the top five producers (in million tonnes) being China (60.0), United States (46.0), Germany (16.5), India (15.8) and Canada (14.0).<ref>[http://minerals.usgs.gov/minerals/pubs/commodity/salt/mcs-2010-salt.pdf Salt], U.S. Geological Survey</ref> |
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 [[soap]]s, [[detergent]]s, and other bath products. It is the major source of industrial chlorine and [[sodium hydroxide]], and used in almost every industry. | 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 [[soap]]s, [[detergent]]s, and other bath products. It is the major source of industrial chlorine and [[sodium hydroxide]], and used in almost every industry. | ||
| − | Sodium chloride is sometimes used as a cheap and safe [[desiccant]] because it appears to have [[hygroscopic]] properties, making [[Salting (food)|salting]] an effective method of [[food preservation]] historically; the salt draws water out of bacteria through [[osmotic pressure]] | + | Sodium chloride is sometimes used as a cheap and safe [[desiccant]] because it appears to have [[hygroscopic]] properties, making [[Salting (food)|salting]] an effective method of [[food preservation]] historically; the salt draws water out of bacteria through [[osmotic pressure]], keeping it from reproducing, a major source of food spoilage. Even though more effective desiccants are available, few are safe for humans to ingest. |
{| class="toccolours" border="1" align="left" style="margin: 1em; border-collapse: collapse;" | {| class="toccolours" border="1" align="left" style="margin: 1em; border-collapse: collapse;" | ||
| − | ! {{chembox header}}|Solubility of NaCl in various solvents<br/ >(g NaCl / 1 kg of solvent at 25 °C)<ref>Burgess, J. ''Metal Ions in Solution'' (Ellis Horwood, New York, 1978) ISBN 0-85312-027-7</ref> | + | ! {{chembox header}}|Solubility of NaCl in various solvents<br/ >(g NaCl / 1 kg of solvent at 25 °C)<ref>Burgess, J. ''Metal Ions in Solution'' (Ellis Horwood, New York, 1978) ISBN 0-85312-027-7</ref> |
|- | |- | ||
| [[Water (molecule)|H<sub>2</sub>O]] || 360 | | [[Water (molecule)|H<sub>2</sub>O]] || 360 | ||
| Line 125: | Line 128: | ||
*Transmitivity: 92% (from 400 nm to 13 μm) | *Transmitivity: 92% (from 400 nm to 13 μm) | ||
| − | * Refractive Index: 1.494 at 10 μm | + | *Refractive Index: 1.494 at 10 μm |
| − | * Reflection Loss: 7.5% at 10 μm (2 surfaces) | + | *Reflection Loss: 7.5% at 10 μm (2 surfaces) |
| − | * dN/dT: −36.2×10<sup>−6</sup>/°C at 0.7 μm | + | *dN/dT: −36.2×10<sup>−6</sup>/°C at 0.7 μm |
===Household uses=== | ===Household uses=== | ||
| Line 133: | Line 136: | ||
===Firefighting uses=== | ===Firefighting uses=== | ||
| − | [[ | + | [[File:Metlx.jpg|thumb|left|upright|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. | 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. | ||
===In weather=== | ===In weather=== | ||
| − | [[ | + | [[File:Clouds from above.JPG|thumb|Clouds above the [[Pacific]]]] |
| − | Small particles of [[sea salt]] are the dominant [[cloud condensation nuclei]] well out at sea, which allow the formation of [[cloud]]s in otherwise non-polluted [[air]].<ref>{{cite journal|url=http://www3.interscience.wiley.com/journal/114028130/abstract|title=The role of sea-salt particles as cloud condensation nuclei over the remote oceans|author=B. J. Mason|journal=The Quarterly Journal of the Royal Meteorological Society|volume=127|issue=576|pages=2023–2032|date=2006-12-19|accessdate=2009-07-08}}</ref> [[Snow removal]] by addition of salt (salting) is done to make travel easier and safer, and decrease the long term impact of a heavy [[snow]]fall on human populations. This process is done by both individual households and by governments and institutions and utilizes salts to eliminate snow from road surfaces and sidewalks.<ref>{{cite book|url=http://books.google.com/?id=I3gxuwTE5_MC&pg=PA10&lpg=PA10&dq=effect+of+snowfall+on+infrastructure|title=Managing roadway snow and ice control operations|author=David A. Kuemmel|page=10|isbn=9780309056663|publisher=Transportation Research Board|year=1994|accessdate=2009-07-08}}</ref> | + | Small particles of [[sea salt]] are the dominant [[cloud condensation nuclei]] well out at sea, which allow the formation of [[cloud]]s in otherwise non-polluted [[air]].<ref>{{cite journal|doi=10.1002/qj.49712757609|url=http://www3.interscience.wiley.com/journal/114028130/abstract|title=The role of sea-salt particles as cloud condensation nuclei over the remote oceans|author=B. J. Mason|journal=The Quarterly Journal of the Royal Meteorological Society|volume=127|issue=576|pages=2023–2032|date=2006-12-19|accessdate=2009-07-08}}</ref> [[Snow removal]] by addition of salt (salting) is done to make travel easier and safer, and decrease the long term impact of a heavy [[snow]]fall on human populations. This process is done by both individual households and by governments and institutions and utilizes salts to eliminate snow from road surfaces and sidewalks.<ref>{{cite book|url=http://books.google.com/?id=I3gxuwTE5_MC&pg=PA10&lpg=PA10&dq=effect+of+snowfall+on+infrastructure|title=Managing roadway snow and ice control operations|author=David A. Kuemmel|page=10|isbn=9780309056663|publisher=Transportation Research Board|year=1994|accessdate=2009-07-08}}</ref> |
==Biological functions== | ==Biological functions== | ||
| − | In humans, a high-salt intake has long been | + | {{for|further information about sodium chloride in the diet|Salt}} |
| + | In humans, a high-salt intake has long been suspected to generally raise blood pressure. 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]].<ref>[http://content.karger.com/ProdukteDB/produkte.asp?Aktion=ShowPDF&ProduktNr=223997&Ausgabe=228460&ArtikelNr=63555 Relationship between Salt Intake, Nitric Oxide and Asymmetric Dimethylarginine and Its Relevance to Patients with End-Stage]</ref><ref>{{Cite journal |first=David A. |last=McCarron |title=Dietary sodium and cardiovascular and renal disease risk factors: dark horse or phantom entry? |journal=Nephrol Dial Transplant |year=2008 |volume=23 |issue=7 |pages=2133–2137 |doi=10.1093/ndt/gfn312 |pmid=18587159 |pmc=2441768 |postscript=<!--None-->}}.</ref> | ||
==Crystal structure== | ==Crystal structure== | ||
| − | [[ | + | [[File:NaCl polyhedra.png|thumb|The crystal structure of sodium chloride. Each ion has six nearest neighbors, with [[octahedral geometry]].]] |
| − | [[ | + | [[File:Close Up View Of Sodium Chloride Crystals.jpg|thumb|Close up view of NaCl crystals]] |
{{main|Cubic crystal system}} | {{main|Cubic crystal system}} | ||
Sodium chloride forms [[crystal]]s with face-centered cubic [[symmetry]]. In these, the larger [[Chlorine|chloride]] [[ion]]s, 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 all the cubic gaps between them. Each ion is surrounded by six ions of the other kind; the surrounding ions are located at the vertices of a regular [[octahedron]]. | Sodium chloride forms [[crystal]]s with face-centered cubic [[symmetry]]. In these, the larger [[Chlorine|chloride]] [[ion]]s, 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 all the cubic gaps between them. Each ion is surrounded by six ions of the other kind; the surrounding ions are located at the vertices of a regular [[octahedron]]. | ||
| Line 212: | Line 216: | ||
Road salt ends up in fresh water bodies and could harm aquatic plants and animals by disrupting their [[osmoregulation]] ability.<ref>[http://www.slate.com/id/2244156 Does road salt harm the environment?]</ref> An alternative is to spread rough sand on ice so the surface is not slippery. | Road salt ends up in fresh water bodies and could harm aquatic plants and animals by disrupting their [[osmoregulation]] ability.<ref>[http://www.slate.com/id/2244156 Does road salt harm the environment?]</ref> An alternative is to spread rough sand on ice so the surface is not slippery. | ||
| − | The omnipresence of salt posts a problem in any coastal coating application, as trapped salts cause great problems in adhesion. Costs can reach staggering amounts. Naval authorities and ship builders keep a close eye on salt concentrations on surfaces during construction. Maximum salt concentrations on surfaces are dependent on the authority and application. The [[International Maritime Organization|IMO]] regulation is mostly used and sets salt levels to a maximum of 50 mg/ | + | The omnipresence of salt posts a problem in any coastal coating application, as trapped salts cause great problems in adhesion. Costs can reach staggering amounts. Naval authorities and ship builders keep a close eye on salt concentrations on surfaces during construction. Maximum salt concentrations on surfaces are dependent on the authority and application. The [[International Maritime Organization|IMO]] regulation is mostly used and sets salt levels to a maximum of 50 mg/m<sup>2</sup> soluble salts measured as sodium chloride. These measurements are done by means of a [[Bresle test]]. |
| − | <gallery> | + | <gallery widths=220px heights=180px> |
| − | + | File:Dead-Sea---Salt-Evaporation-Ponds.jpg| [[Israel]]i and [[Jordan]]ian salt evaporation ponds at the south end of the [[Dead Sea]]. | |
| − | + | File:Piles of Salt Salar de Uyuni Bolivia Luca Galuzzi 2006 a.jpg|Mounds of salt, [[Salar de Uyuni]], [[Bolivia]]. | |
| − | + | File:Aigues-Mortes2.jpg|Evaporation lagoons, [[Aigues-Mortes]], [[France]]. | |
</gallery> | </gallery> | ||
==See also== | ==See also== | ||
{{Cookbook|Salt}} | {{Cookbook|Salt}} | ||
| + | {{colbegin}} | ||
*[[Biosalinity]] | *[[Biosalinity]] | ||
*[[Kala Namak]] | *[[Kala Namak]] | ||
| Line 229: | Line 234: | ||
*[[Soap]] | *[[Soap]] | ||
*[[Salting the earth]] | *[[Salting the earth]] | ||
| + | {{colend}} | ||
==References== | ==References== | ||
{{reflist|2}} | {{reflist|2}} | ||
| − | |||
| − | |||
| − | |||
| − | |||
==External links== | ==External links== | ||
| Line 273: | Line 275: | ||
[[eo:Natria klorido]] | [[eo:Natria klorido]] | ||
[[eu:Sodio kloruro]] | [[eu:Sodio kloruro]] | ||
| − | [[fa: | + | [[fa:کلرید سدیم]] |
[[fr:Chlorure de sodium]] | [[fr:Chlorure de sodium]] | ||
[[gl:Cloruro de sodio]] | [[gl:Cloruro de sodio]] | ||
| Line 304: | Line 306: | ||
[[th:โซเดียมคลอไรด์]] | [[th:โซเดียมคลอไรด์]] | ||
[[uk:Хлорид натрію]] | [[uk:Хлорид натрію]] | ||
| − | [[vi:Natri | + | [[vi:Natri clorua]] |
[[fiu-vro:Keedosuul]] | [[fiu-vro:Keedosuul]] | ||
[[zh:氯化钠]] | [[zh:氯化钠]] | ||
[[Category:2Fix]] | [[Category:2Fix]] | ||
Latest revision as of 15:51, 27 September 2010
| Sodium chloride | |
|---|---|
| File:Sodiumchloride crystal 01.jpg | |
| File:Sodium-chloride-3D-ionic.png | |
| Sodium chloride | |
| Other names Common salt, halite, table salt, rock salt, saline, hyposaline, sodium monochloride, sodium chloric, saltex[1] | |
| style="background: #F8EABA; text-align: center;" colspan="2" | Identifiers | |
| CAS number | 7647-14-5 
|
| PubChem | 5234 |
| ChemSpider | 5044 |
| RTECS number | VZ4725000 |
| style="background: #F8EABA; text-align: center;" colspan="2" | Properties | |
| Molecular formula | NaCl |
| Molar mass | 58.443 g/mol |
| Appearance | Colorless/white crystalline solid |
| Odor | Odorless |
| Density | 2.165 g/cm3 |
| Melting point |
801 °C, 1074 K, 1474 °F |
| Boiling point |
1413 °C, 1686 K, 2575 °F |
| Solubility in water | 356 g/L (0 °C) 359 g/L (25 °C) 391 g/L (100 °C) |
| Solubility | soluble in glycerol, ethylene glycol, formic acid insoluble in HCl |
| Solubility in methanol | 14.9 g/L |
| Solubility in ammonia | 21.5 g/L |
| Acidity (pKa) | 6.7–7.3 |
| Refractive index (nD) | 1.5442 (589 nm) |
| style="background: #F8EABA; text-align: center;" colspan="2" | Structure | |
| Crystal structure | Face-centered cubic (see text), cF8 |
| Space group | Fm3m, No. 225 |
| Lattice constant | a = 564.02 pm |
| Octahedral (Na+) Octahedral (Cl–) | |
| style="background: #F8EABA; text-align: center;" colspan="2" | Hazards | |
| EU Index | Not listed |
| NFPA 704 | |
| Flash point | Non-flammable |
| LD50 | 3000–8000 mg/kg (oral in rats, mice, rabbits)[2] |
| style="background: #F8EABA; text-align: center;" colspan="2" | Related compounds | |
| Other anions | Sodium fluoride Sodium bromide Sodium iodide |
| Other cations | Lithium chloride Potassium chloride Rubidium chloride Caesium chloride |
 (what is this?) (verify)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 ionic 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.
Contents
Properties
Thermal conductivity of pure 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.[3]
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 2009, world production was estimated at 260 million metric tons, the top five producers (in million tonnes) being China (60.0), United States (46.0), Germany (16.5), India (15.8) and Canada (14.0).[4]
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. It is the major source of industrial chlorine and sodium hydroxide, and used in almost every industry.
Sodium chloride is sometimes used as a cheap and safe desiccant because it appears to have hygroscopic properties, making salting an effective method of food preservation historically; the salt draws water out of bacteria through osmotic pressure, keeping it from reproducing, a major source of food spoilage. Even though more effective desiccants are available, few are safe for humans to ingest.
| style="background: #F8EABA; text-align: center;" colspan="2"|Solubility of NaCl in various solvents (g NaCl / 1 kg of solvent at 25 °C)[5] | |
|---|---|
| H2O | 360 |
| Liquid ammonia | 30.2 |
| glycerin | 83 |
| propylene glycol | 71 |
| Methanol | 14 |
| Ethanol | 0.65 |
| 1-propanol | 0.124 |
| 2-propanol | 0.03 |
| 1-butanol | 0.05 |
| 1-pentanol | 0.018 |
| Sulfolane | 0.05 |
| Formic acid | 52 |
| Acetone | 0.00042 |
| Formamide | 94 |
| Acetonitrile | 0.003 |
| Dimethylformamide | 0.4 |
Synthetic uses
Uses of chlorine include PVC, pesticides and epoxy resins. 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
- 2 NaCl + 2 H2O → Cl2 + H2 + 2 NaOH
Sodium metal is produced commercially through the electrolysis of liquid sodium chloride. This is now 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 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.
Optical uses
Pure NaCl crystal is an optical compound with a wide transmission range from 200 nm to 20 µm. It was often used in the infrared spectrum range and it is still used sometimes.
While inexpensive, NaCl crystal is soft and hygroscopic. When exposed to free air, NaCl optics gradually covers with "frost". This limits application of NaCl to protected environments or for short-term uses such as prototyping.
Today tougher crystals like zinc selenide (ZnSe) are used instead of NaCl (for the IR spectral range).
Optical data
- Transmitivity: 92% (from 400 nm to 13 μm)
- Refractive Index: 1.494 at 10 μm
- Reflection Loss: 7.5% at 10 μm (2 surfaces)
- dN/dT: −36.2×10−6/°C at 0.7 μm
Household uses
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, and popularly to de-ice driveways and patches of ice.
Firefighting uses
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.
In weather
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] Snow removal by addition of salt (salting) is done to make travel easier and safer, and decrease the long term impact of a heavy snowfall on human populations. This process is done by both individual households and by governments and institutions and utilizes salts to eliminate snow from road surfaces and sidewalks.[7]
Biological functions
In humans, a high-salt intake has long been suspected to generally raise blood pressure. 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.[8][9]
Crystal structure
Sodium chloride forms crystals with face-centered 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 all the cubic gaps between them. Each ion is surrounded by six ions of the other kind; the surrounding ions are located at the vertices of a regular octahedron.
This same basic structure is found in many other minerals 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. 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.
It is held together by an ionic bond which is produced by electrostatic forces arising from the difference in charge between the ions.
Road salt
While salt was once a scarce commodity in history, industrialized production has now made salt plentiful. Approximately 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. Calcium chloride is preferred over sodium chloride, since CaCl2 releases energy upon forming a solution with water, heating any ice or snow it is in contact with. It also lowers the freezing point, depending on the concentration. NaCl does not release heat upon solution; however, it does lower the freezing point. Calcium chloride is thought to be more environmentally friendly than sodium chloride when used to de-ice roads, however a drawback is that it tends to promote corrosion (of vehicles) more so than sodium chloride. NaCl is also more readily available and does not have any special handling or storage requirements, unlike calcium chloride. The salinity (S) of water is measured as grams salt per kilogram of water, and the freezing temperatures are as follows.
| S (g/kg) | 0 | 15 | 30 | 45 | 59 | 75 | 90 | 106 | 123 | 140 | 157 | 175 | 193 | 212 | 231 | 250 | 269 | 290 | 311 | 331 | 353 |
| T (°C) | 0 | −0.8 | −1.7 | −2.7 | −3.6 | −4.6 | −5.5 | −6.6 | −7.8 | −9.1 | −10.4 | −11.8 | −13.2 | −14.6 | −16.2 | −17.8 | −19.4 | −21.1 | −17.3 | −11.1 | −2.7 |
Additives
Most 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.[10] 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.[11]
Salt for de-icing in the United Kingdom predominantly comes from a single mine in Winsford in Cheshire. Prior to distribution it has an anti-caking agent added: sodium hexacyanoferrate(II) at less than 100 ppm. This treatment 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.
Environmental impact
Road salt ends up in fresh water bodies and could harm aquatic plants and animals by disrupting their osmoregulation ability.[12] An alternative is to spread rough sand on ice so the surface is not slippery.
The omnipresence of salt posts a problem in any coastal coating application, as trapped salts cause great problems in adhesion. Costs can reach staggering amounts. Naval authorities and ship builders keep a close eye on 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.
- Piles of Salt Salar de Uyuni Bolivia Luca Galuzzi 2006 a.jpg
Mounds of salt, Salar de Uyuni, Bolivia.
- Aigues-Mortes2.jpg
Evaporation lagoons, Aigues-Mortes, France.
See also
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- Biosalinity
- Kala Namak
- Halite, the mineral form of sodium chloride
- Salinity
- Salt
- Soap
- Salting the earth
References
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<references />, or <references group="..." />External links
| 40x40px | Wikimedia Commons has media related to Sodium chloride. |
- The Salt Manufacturers Association website
- Salt Institute website
- Salt Archive website
- Salt United States Geological Survey Statistics and Information
- US Road Management website
- Salt Intake in Cold Weather
- Oxford MSDS
- JtBaker MSDS
ar:كلوريد الصوديوم az:Natrium Xlorid bn:সোডিয়াম ক্লোরাইড bs:Natrijum hlorid bg:Натриев хлорид ca:Clorur de sodi cs:Chlorid sodný cy:Halen da:Natriumklorid de:Natriumchlorid et:Naatriumkloriid es:Cloruro de sodio eo:Natria klorido eu:Sodio kloruro fa:کلرید سدیم fr:Chlorure de sodium gl:Cloruro de sodio ko:염화 나트륨 hy:Նատրիումի քլորիդ hr:Natrijev klorid id:Natrium klorida is:Borðsalt it:Cloruro di sodio he:מלח בישול ka:ნატრიუმქლორიდი la:Natrii chloridum lv:Nātrija hlorīds lt:Natrio chloridas hu:Nátrium-klorid ms:Natrium klorida nl:Natriumchloride ja:塩化ナトリウム no:Koksalt nds:Natriumchlorid pl:Chlorek sodu pt:Cloreto de sódio qu:Yanuna kachi ru:Хлорид натрия scn:Cloruru di sodiu simple:Table salt sk:Chlorid sodný sr:Кухињска со sv:Natriumklorid th:โซเดียมคลอไรด์ uk:Хлорид натрію vi:Natri clorua fiu-vro:Keedosuul
zh:氯化钠- ↑ National Institute of Standards and Technology: Sodium Chloride
- ↑ Martel, B.; Cassidy, K. (2004). Chemical Risk Analysis: A Practical Handbook. Butterworth–Heinemann. p. 369. ISBN 1903996651.
- ↑ Dinker B. Sirdeshmukh, Lalitha Sirdeshmukh, K. G. Subhadra Alkali halides: a handbook of physical properties, Springer, 2001 ISBN 3540421807 pp. 65, 68
- ↑ Salt, U.S. Geological Survey
- ↑ Burgess, J. Metal Ions in Solution (Ellis Horwood, New York, 1978) ISBN 0-85312-027-7
- ↑ 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): 2023–2032. doi:10.1002/qj.49712757609. Retrieved 2009-07-08.
- ↑ David A. Kuemmel (1994). Managing roadway snow and ice control operations. Transportation Research Board. p. 10. ISBN 9780309056663. Retrieved 2009-07-08.
- ↑ Relationship between Salt Intake, Nitric Oxide and Asymmetric Dimethylarginine and Its Relevance to Patients with End-Stage
- ↑ McCarron, David A. (2008). "Dietary sodium and cardiovascular and renal disease risk factors: dark horse or phantom entry?". Nephrol Dial Transplant. 23 (7): 2133–2137. doi:10.1093/ndt/gfn312. PMC 2441768 Freely accessible. PMID 18587159..
- ↑ "Morton Salt FAQ". Retrieved 2007-05-12.
- ↑ 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. doi:10.2105/AJPH.77.2.219. PMC 1646845 Freely accessible. PMID 3541654.
- ↑ Does road salt harm the environment?
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