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:''For sodium in the diet, see salt.''
'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 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.
Salt is currently 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]
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).
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.
Main articles: Salt
Salt is commonly used as a flavour enhancer 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 heart attack and stroke. Consuming salt in excess can also dehydrate the human body.
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. In medieval times salt would be rubbed into household surfaces as a cleansing agent.
'energetic sector.'
Its high heat of fusion value is 25.2 kj/mol (259 kwh/m3!).
It's practically possible to store 259 kwh/m3 of thermal energy at constant temperature...
It's potentially a great business!
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 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 close packed'' (ccp).
It is held together with an ionic bond and electrostatic forces.
Salt is also known in the chemical world as a nuclear additive.
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 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).
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, creating iodized salt 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.
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 CaCl[1][2].
★ Biosalinity
★ Black salt
★ Edible salt
★ Halite, the mineral form of sodium chloride
★ Salinity
★ Soap
★ Salting the earth
1. Susan R. Feldman. Sodium chloride. ''Kirk-Othmer Encyclopedia of Chemical Technology''. John Wiley & Sons, Inc. Published online '2005'.
2. Morton Salt FAQ
3. "When it rains it pours": endemic goiter, iodized salt, and David Murray Cowie, MD, Markel H, , , American journal of public health, 1987
★ 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 | |
|---|---|
USGOV.jpg) Sodium chloride  Sodium chloride | |
| General | |
| Systematic name | Sodium chloride |
| Other names | Common salt, halite, table salt |
| Chemical formula | NaCl |
| Molar mass | 58.442 g/mol |
| Appearance | white and crystalized |
| CAS number | [7647-14-5] |
| Properties | |
| Density and phase | 2.16 g/cm³, solid |
| Solubility in water | 35.9 g/100 ml (25 °C) |
| Melting point | 801 °C (1074 K) |
| Boiling point | 1465 °C (1738 K) |
| Structure | |
| Coordination geometry | Octahedral |
| Crystal structure | Face centered cubic |
| Hazards | |
| MSDS | External MSDS |
| Main hazards | Irritant and Might Sting |
| NFPA 704 | |
| Flash point | Non-flammable |
| R/S statement | R: 36 S: none |
| RTECS number | VZ4725000 |
| Supplementary data page | |
| Structure and properties | ''n'', εr, etc. |
| Thermodynamic data | Phase behaviour Solid, liquid, gas |
| Spectral data | UV, IR, NMR, MS |
| Related compounds | |
| Other anions | NaF, NaBr, NaI |
| Other cations | LiCl, KCl, RbCl, CsCl, MgCl2, CaCl2 |
| Related salts | Sodium acetate |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) | |
'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 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.
| Contents |
| Production and use |
| Synthetic uses |
| Flavour enhancer |
| Biological uses |
| Possible uses |
| Crystal structure |
| Road salt |
| De-icing |
| Additives |
| Common chemicals |
| See also |
| References |
| External Links |
Production and use
Salt is currently 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]
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).
| Solubility of NaCl in various solvents (g NaCl / 100 g of solvent at 25 °C) | |
|---|---|
| H2O | 36 |
| Liquid ammonia | 3.02 |
| Methanol | 1.4 |
| Formic acid | 5.2 |
| Sulfolane | 0.005 |
| Acetonitrile | 0.0003 |
| Acetone | 0.000042 |
| Formamide | 9.4 |
| 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.
Flavour enhancer
Main articles: Salt
Salt is commonly used as a flavour enhancer 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 heart attack and stroke. Consuming salt in excess can also dehydrate the human body.
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. In medieval times salt would be rubbed into household surfaces as a cleansing agent.
Possible uses
'energetic sector.'
Its high heat of fusion value is 25.2 kj/mol (259 kwh/m3!).
It's practically possible to store 259 kwh/m3 of thermal energy at constant temperature...
It's potentially a great business!
Crystal structure
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 blue spheres, fill the octahedral gaps between them.
The crystal structure of sodium chloride. Each atom has six nearest neighbors, with octahedral geometry.
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 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 de-ice 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. [2] 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 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 CaCl[1][2].
See also
★ Biosalinity
★ Black salt
★ Edible salt
★ Halite, the mineral form of sodium chloride
★ Salinity
★ Soap
★ Salting the earth
References
1. Susan R. Feldman. Sodium chloride. ''Kirk-Othmer Encyclopedia of Chemical Technology''. John Wiley & Sons, Inc. Published online '2005'.
2. Morton Salt FAQ
3. "When it rains it pours": endemic goiter, iodized salt, and David Murray Cowie, MD, Markel H, , , American journal of public health, 1987
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
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