Sodium chloride (NaCl)
Common salt (or table salt) is one of the most important sodium compounds, indispensable for living organisms.
sodium chloride, table salt, common salt, ionic compound, ionic crystal lattice, anion, cation, crystal lattice, salty water, inorganic chemistry, chemistry
Sodium chloride, table salt NaCl
Molar mass: 58.44 g/mol
Melting point: 801 °C
Boiling point: 1,413 °C
Density: 2.165 g/cm³
Hardness: 2 (on the Mohs scale of mineral hardness)
Sodium chloride, commonly known as table salt, is a white, odourless, crystalline material. It is an ionic compound; its ions form a face-centred cubic lattice. It dissolves well in water; the solution has a neutral pH.
Biologically important sodium and chloride ions are consumed as NaCl. It plays an important role in maintaining osmotic pressure in the body, but excessive consumption may cause high blood pressure. In medicine, a solution of 0.90% w/v of NaCl, called saline solution, is used in intravenous drips.
Occurrence and production
It is the third most common compound of sodium. It occurs in large quantities in seawater, brine wells and enclosed, dried-out coastal areas. It can be obtained through mining or evaporation.
Sodium chloride is used as table salt and as a preservative, as well as in the production of sodium compounds.
Common salt is dissolved by water: polar water molecules form a coat around the ions.
A yellow-green toxic gas with a strong odour, one of the halogens.
The face-centred cubic metal lattice allows the closest fit of metal atoms.
The desalination process produces drinking water from seawater.
Used in the production of beryllium and as a catalyst.
A white, crystalline compound which breaks down when exposed to light.
A white, crystalline compound that breaks down when affected by light.
A light yellow compound formed in the reaction of silver nitrate and potassium iodide.