Sodium chloride

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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
Halite(Salt)USGOV.jpg
Sodium-chloride-3D-ionic.png
IUPAC name
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Sodium chloride
Other names Common salt; halite; table salt; rock salt
Identifiers
CAS number 7647-14-5 Yes check.svgY
PubChem 5234
ChemSpider ID 5044
RTECS number VZ4725000
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 35.6 g/100 mL (0 °C)
35.9 g/100 mL (25 °C)
39.1 g/100 mL (100 °C)
Solubility soluble in glycerol, ethylene glycol, formic acid
insoluble in HCl
Solubility in methanol 1.49 g/100 mL
Solubility in ammonia 2.15 g/100 mL
Acidity (pKa) 6.7-7.3
Refractive index (nD) 1.5442 (589 nm)
Structure
Crystal structure Cubic (see text), cF8
Space group Fm3m, No. 225
Lattice constant a = 564.02 pm
Coordination
geometry Octahedral (Na+)
Octahedral (Cl−)
Hazards
MSDS External MSDS
EU Index Not listed
NFPA 704
NFPA 704.svg
0
1
0

Flash point Non-flammable
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
Yes check.svgY (what is this?) (verify)
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Infobox references
Close up view of NaCl crystals.

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
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* 1 Production and use
o 1.1 Synthetic uses
o 1.2 Biological uses
o 1.3 Optical uses
o 1.4 Optical data
o 1.5 Household uses
o 1.6 Firefighting uses
o 1.7 In weather
* 2 Biological functions
* 3 Crystal structure
* 4 Road salt
o 4.1 Additives
* 5 Alternative names
* 6 See also
* 7 References
* 8 Further reading
* 9 External links

[edit] 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 tons, the top five producers (in million tonnes) being the United States (40.3), China (32.9), Germany (17.7), India (14.5) and Canada (12.3).[2]

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; as it draws water out of bacteria through osmotic pressure preventing them from reproducing and causing food to spoil. 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, United States.


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
[edit] Synthetic uses

Sodium chloride is also the raw material used to produce chlorine which itself is required for sterilization and the production of many modern materials including 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

2NaCl + 2H2O → Cl2 + H2 + 2NaOH

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.
[edit] 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.
[edit] Optical uses

Pure NaCl crystal is an optical compound with a wide transmission range from 200 nm to 20 um. It was often used in the infrared spectrum range and it is still used sometimes.

NaCl crystal is soft, hygroscopic and inexpensive. This limits its application to protected environment or for short term uses (prototyping). Exposed to free air NaCl optics will "rot".

Today tougher crystals like ZnSe are used instead of NaCl (for the IR spectral range).
[edit] Optical data

* Transmitivity: 92% (from 400 nm to 13μm)
* Refractive Index: 1.494 @ 10μm
* Reflection Loss: 7.5% @ 10μm (2 surfaces)
* dN/dT: -36.2 x 10-6/°C @ 0.7μm

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.

At one time salt water was used to clean teeth.
[edit] Firefighting uses
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.
[edit] In weather
Clouds above the Pacific

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.[3] 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 salt as well as other chloride-based chemicals to eliminate snow from road surfaces and sidewalks.[4]
[edit] 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.[5][6]
[edit] Crystal structure
The crystal structure of sodium chloride. Each ion has six nearest neighbors, with octahedral geometry.
Main article: Cubic crystal system

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.
[edit] Road salt

Magnesium chloride

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. It 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 (1000g) water, and the freezing temperatures are as follows.
S(g/kg) 0 10 20 24.7 30 35
T(freezing) (C) 0 -0.5 -1.08 -1.33 -1.63 -1.91
[edit] 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.[7] 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.[8]

Salt for de-icing in the UK predominantly comes from a single mine in Winsford in Cheshire [[1]]. Prior to distribution it has an anti-caking agent added, sodium hexacyanoferrate(II) at less than 100ppm, 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.

Alternative names

* NaCl, Sodium monochloride
* Table salt, Sal Culinare or Sal Culinaris
* Common Salt, Sal Commune
* Muriate of soda, Muriate of natrium, Chloride of Sodium, Hydrochlorate of Soda (older names)
* Sodii Chloridum, SodAe Hydro-chloras, SodAe Murias (ancient names)
* Nat Mur for Natrum Muriaticum, Natrum Muriatica, or even Natrium Muriate (homeopathic/Biochemic cell salts)