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For sodium in the diet, see salt.
{{Chembox new| Name = Sodium chloride| ImageFile = Halite(Salt)USGOV.jpg| ImageFile1 = Sodium-chloride-3D-ionic.png| IUPACName = Sodium chloride| OtherNames = Common salt; halite;
table salt| Section1 = {{Chembox Identifiers| CASNo = 7647-14-5| RTECS = VZ4725000 -->
| Section2 = {{Chembox Properties| Formula = SodiumChlorine| MolarMass = 58.442 g/mol| Appearance = white and crystalized| Density = 2.16 g/cm³, solid| Solubility = 35.9 g/100 mL (25 °C)| MeltingPt = 801 °C| BoilingPt = 1465 °C (1738 K)| Index of Refraction = 1.544 (589 nm) -->
| Section3 = {{Chembox Structure| Coordination = Octahedral| Structure = Cubic crystal system -->
| Section7 = {{Chembox Hazards| MainHazards = Irritant and Might Sting| NFPA-H = 1| NFPA-F =| NFPA-R =| FlashPt = Non-flammable| RPhrases = 36| SPhrases = none -->
| Section8 = {{Chembox Related| OtherAnions =
Sodium fluoride, Sodium bromide,
Sodium iodide| OtherCations =
Lithium chloride, Potassium chloride, Rubidium chloride,
Caesium chloride,
Magnesium chloride,
Calcium chloride| Function = salts] -->
-->
Sodium chloride, also known as
common salt,
table salt, or halite, is a
chemical compound with the chemical formula
SodiumChlorine. Sodium chloride is the
salt (chemistry) most responsible for the salinity of the
ocean and of the
extracellular fluid of many multicellular organisms. As the main 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 g of chlorine.
Production and use
Salt is currently produced by
evaporation of
seawater or
brine from other sources, such as brine wells and salt lake (geography)s, and by
salt mine 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).Susan R. Feldman. Sodium chloride.
Kirk-Othmer Encyclopedia of Chemical Technology. John Wiley & Sons, Inc. Published online
2005.
While most people are familiar with the many uses of salt in cooking, they might be unaware that salt is used in a plethora of applications, from
manufacturing pulp and paper to setting dyes in textiles and fabric, to producing
soaps and detergents. In most of Canada and the northern USA, 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)..Image:Dead-Sea---Salt-Evaporation-Ponds.jpg]ian and Israeli salt evaporation ponds at the south end of the Dead SeaImage:Piles of Salt Salar de Uyuni Bolivia Luca Galuzzi 2006 a.jpg],
Bolivia.
Image:Salt mine 0096.jpg].Image:Aigues-Mortes2.jpg|Evaporation lagoons, Aigues-Mortes, France{] || 36|-|
Ammonia || 3.02|-| Methanol ] || 5.2|-| Sulfolane ] || 0.0003|-|
Acetone ] || 9.4|-|
Dimethylformamide || 0.04|-| align="center" colspan="2" | 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
Polyvinyl chloride 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 Downs 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.
Food Uses
Salt is commonly used as a flavour enhancer and
preservative for
food and has been identified as one of the
basic tastes. Unfortunately, given its history, this has resulted in large sections of the developed world ingesting salt massively in excess of the required intake. . This causes elevated levels of blood pressure (
hypertension) in some, which in turn is associated with increased risks of myocardial infarction and
stroke. Consuming salt in excess can also dehydrate the human body. Salt also has a practical use in cooking in that it raises the boiling point of water, thus allowing a food to cook slower and more thoroughly on a slow boil.
Biological uses
Many microorganisms cannot live in an overly salty environment: water is drawn out of their
cell (biology) by
osmosis. For this reason salt is used to
Food preservation 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. In medieval times salt would be rubbed into household surfaces as a cleansing agent.
Crystal structure
Sodium chloride forms crystals with cubic
symmetry. In these, the larger
Chlorine 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 blue 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 crystal system (ccp).
It is held together with an ionic bond and electrostatic forces.
Salt is also known in the chemical world as a nuclear additive.
Road salt
De-icing
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 deicing roads in winter, both in
grit bins and spread by winter service vehicles. This works because salt and water form an eutectic mixture. For a solution of table salt (sodium chloride, NaCl) in water, the freezing temperature becomes -21 °C (-6 °F) under controlled lab conditions. In practice, however, sodium chloride can melt ice only down to about -9 °C (15 °F).
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. In 1924 trace amounts of
iodine in form of sodium iodide, potassium iodide or potassium iodate were first added, creating iodized salt to reduce the incidence of simple
Goitre.
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. Addingsalt lowers the freezing point of the water, which allows the liquid to bestable 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.
See also
References
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
For sodium in the diet, see salt.
{{Chembox new| Name = Sodium chloride| ImageFile = Halite(Salt)USGOV.jpg| ImageFile1 = Sodium-chloride-3D-ionic.png| IUPACName = Sodium chloride| OtherNames = Common salt; halite;
table salt| Section1 = {{Chembox Identifiers| CASNo = 7647-14-5| RTECS = VZ4725000 -->
| Section2 = {{Chembox Properties| Formula = SodiumChlorine| MolarMass = 58.442 g/mol| Appearance = white and crystalized| Density = 2.16 g/cm³, solid| Solubility = 35.9 g/100 mL (25 °C)| MeltingPt = 801 °C| BoilingPt = 1465 °C (1738 K)| Index of Refraction = 1.544 (589 nm) -->
| Section3 = {{Chembox Structure| Coordination = Octahedral| Structure =
Cubic crystal system -->
| Section7 = {{Chembox Hazards| MainHazards = Irritant and Might Sting| NFPA-H = 1| NFPA-F =| NFPA-R =| FlashPt = Non-flammable| RPhrases = 36| SPhrases = none -->
| Section8 = {{Chembox Related| OtherAnions = Sodium fluoride, Sodium bromide,
Sodium iodide| OtherCations =
Lithium chloride,
Potassium chloride, Rubidium chloride,
Caesium chloride, Magnesium chloride, Calcium chloride| Function =
salts] -->
-->
Sodium chloride, also known as
common salt,
table salt, or
halite, is a chemical compound with the chemical formula SodiumChlorine. Sodium chloride is the salt (chemistry) most responsible for the salinity of the
ocean and of the extracellular fluid of many multicellular
organisms. As the main 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 g of chlorine.
Production and use
Salt is currently produced by evaporation of seawater or
brine from other sources, such as brine wells and
salt lake (geography)s, and by salt mine
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).Susan R. Feldman. Sodium chloride.
Kirk-Othmer Encyclopedia of Chemical Technology. John Wiley & Sons, Inc. Published online
2005.
While most people are familiar with the many uses of salt in cooking, they might be unaware that salt is used in a plethora of applications, from
manufacturing pulp and paper to setting dyes in textiles and fabric, to producing soaps and detergents. In most of Canada and the northern USA, 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)..Image:Dead-Sea---Salt-Evaporation-Ponds.jpg]ian and
Israeli salt evaporation ponds at the south end of the Dead SeaImage:Piles of Salt Salar de Uyuni Bolivia Luca Galuzzi 2006 a.jpg], Bolivia.
Image:Salt mine 0096.jpg].Image:Aigues-Mortes2.jpg|Evaporation lagoons,
Aigues-Mortes, France{] || 36|-| Ammonia || 3.02|-| Methanol ] || 5.2|-|
Sulfolane ] || 0.0003|-| Acetone ] || 9.4|-| Dimethylformamide || 0.04|-| align="center" colspan="2" | 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 Polyvinyl chloride 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 Downs 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.
Food Uses
Salt is commonly used as a flavour enhancer and
preservative for
food and has been identified as one of the
basic tastes. Unfortunately, given its history, this has resulted in large sections of the developed world ingesting salt massively in excess of the required intake. . This causes elevated levels of blood pressure (
hypertension) in some, which in turn is associated with increased risks of
myocardial infarction and stroke. Consuming salt in excess can also dehydrate the human body. Salt also has a practical use in cooking in that it raises the boiling point of water, thus allowing a food to cook slower and more thoroughly on a slow boil.
Biological uses
Many
microorganisms cannot live in an overly salty environment: water is drawn out of their cell (biology) by
osmosis. For this reason salt is used to Food preservation 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. In
medieval times salt would be rubbed into household surfaces as a cleansing agent.
Crystal structure
Sodium chloride forms
crystals with cubic symmetry. In these, the larger Chlorine 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 blue 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 crystal system (ccp).
It is held together with an ionic bond and
electrostatic forces.
Salt is also known in the chemical world as a nuclear additive.
Road salt
De-icing
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 deicing roads in winter, both in grit bins and spread by winter service vehicles. This works because salt and water form an
eutectic mixture. For a solution of table salt (sodium chloride, NaCl) in water, the freezing temperature becomes -21 °C (-6 °F) under controlled lab conditions. In practice, however, sodium chloride can melt ice only down to about -9 °C (15 °F).
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. In 1924 trace amounts of iodine in form of sodium iodide, potassium iodide or
potassium iodate were first added, creating iodized salt to reduce the incidence of simple
Goitre.
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. Addingsalt lowers the freezing point of the water, which allows the liquid to bestable 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.
See also
- Biosalinity
- Black salt
- Edible salt
- Halite, the mineral form of sodium chloride
- Salinity
- Soap
- Salting the earth
References
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
Sodium chloride - Wikipedia, the free encyclopedia
For sodium chloride in the diet, see salt.
Safety (MSDS) data for sodium chloride
Safety (MSDS) data for sodium chloride. Safety data for sodium chloride Click here for data on sodium chloride in student-friendly format, from the HSci project
Chemical Safety Data: Sodium Chloride
Chemical Safety Data: Sodium Chloride ... Common synonyms: Salt, table salt, sea salt, rock salt, common salt: Formula
Category:Sodium chloride - Wikimedia Commons
Media in category "Sodium chloride" The following 51 files are in this category, out of 51 total.
Definition: sodium chloride from Online Medical Dictionary
The Online Medical Dictionary is a searchable dictionary of definitions from medicine, science and technology.
Medicines
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SODIUM CHLORIDE
1. Product Identification Synonyms: Salt; Rock Salt; Saline; Table Salt CAS No.: 7647-14-5 Molecular Weight: 58.44 Chemical Formula: ...
Food Standards Agency - Eat well, be well - Sodium chloride
Sodium chloride is commonly known as salt. ... Sodium chloride. Sodium chloride is commonly known as salt. Salt is found naturally at low levels in all foods, but high levels are ...
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sodium chloride
Environmental Fate - Ecotoxicology - Human Health - A to Z Index - Home . GENERAL INFORMATION . Description: A inorganic salt for use as a total herbicide ...
