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|3D model (Jmol)||Interactive image|
|Molar mass||58.44 g mol−1|
|Melting point||801 °C (1,474 °F; 1,074 K)|
|Boiling point||1,413 °C (2,575 °F; 1,686 K)|
|Solubility in ammonia||21.5 g/L|
|Solubility in methanol||14.9 g/L|
Refractive index (nD)
|1.5442 (at 589 nm)|
(see text), cF8
|Fm3m, No. 225|
a = 564.02 pm
|36.79 J K−1 mol−1|
|72.11 J K−1 mol−1|
Std enthalpy of
|−411.12 kJ mol−1|
|A12CA01 (WHO) B05CB01 (WHO), B05XA03 (WHO), S01XA03 (WHO)|
|Safety data sheet||See: data page|
|Lethal dose or concentration (LD, LC):|
LD50 (median dose)
|3 g/kg (oral, rats)|
|Supplementary data page|
Refractive index (n),
Dielectric constant (εr), etc.
|UV, IR, NMR, MS|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|what is ?)(|
Sodium chloride / /, also known as salt or halite, is an ionic compound with the chemical formula NaCl, representing a 1:1 ratio of sodium and chloride ions. Sodium chloride is the salt most responsible for the salinity of seawater and of the extracellular fluid of many multicellular organisms. In the form of edible or table salt it is commonly used as a condiment and food preservative. Large quantities of sodium chloride are used in many industrial processes, and it is a major source of sodium and chlorine compounds used as for further chemical syntheses. A second major application of sodium chloride is de-icing of roadways in sub-freezing weather.
In addition to the familiar domestic uses of salt, more dominant applications of the approximately 250 megatons/year production (2008 data) include chemicals and de-icing.
Salt is used, directly or indirectly, in the production of many chemicals, which consume most of the world's production.
|Solubility of NaCl in various solvents
(g NaCl / 1 kg of solvent at 25 °C, 77 °F)
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