Hydroxide

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Hydroxide
Space-filling model of the hydroxide ion
General
Systematic name[1] hydroxide
oxidanide
hydridooxygenate(1−)
Molecular formula OH
Molar mass 19.02 g/mol
CAS number [14280-30-9]
Except where noted otherwise, data are given for
materials in their standard state (at 25 °C, 100 kPa)
Infobox disclaimer and references
Pellets of sodium hydroxide.

In chemistry, hydroxide is the most common name for the diatomic anion OH, consisting of oxygen and hydrogen atoms. It is one of the simplest diatomic ions known. The term "hydroxide" also refers to the class of compounds that contain the hydroxide ion. Common examples are sodium hydroxide, potassium hydroxide, and ammonium hydroxide.

Hydroxide compounds and ions are relatively common in nature. Several mineral ores, such as bauxite and limonite, are hydroxides. In addition, hydroxides are widely used in human activities. For example, sodium hydroxide (lye) is useful as a strong base in industry, and potassium hydroxide is used in agriculture.

Contents

Hydroxide as a base

Most compounds containing the hydroxide ion are chemical bases. Thus, hydroxide ions are involved in numerous acid-base reactions, including the reaction known as neutralization.

A substance that produces hydroxide ions when dissolved in aqueous solution is called an Arrhenius base. One example is ammonia (NH3):

NH3(g) + H2O(l) NH4+(aq) + OH(aq)

Salts containing hydroxide are called base salts. Base salts will dissociate into a cation and one or more hydroxide ions in water, making the solution basic. Base salts will undergo neutralization reactions with acids. In general, an acid-alkali reactions can be simplified to

OH(aq) + H+(aq) → H2O(l)

Ions that do not participate in this reaction are called spectator ions and are not shown here.

Solubility

Most inorganic hydroxide salts are insoluble in water. Important exceptions are salts in which the cations are alkali metal ions and or NH4+, Ba2+, Sr2+, Ca2+, or Tl+ ions.

Behavior as a ligand

The hydroxide ion is a type of ligand. Each oxygen atom in the OH ion has a "lone pair" (unshared pairs) of electrons in the outermost shell, and it forms bonds by donating this pair of electrons to an appropriate receiving atom. In this manner, a hydroxide ion behaves as a Lewis base. Examples include the aluminate ion [Al(OH)4], and aurate ion [Au(OH)4].

Uses of hydroxide

Hydroxides and hydroxide ions are relatively common. Many useful chemicals and chemical processes involve hydroxides or hydroxide ions. Sodium hydroxide (lye) is used in industry as a strong base, potassium hydroxide is used in agriculture, and iron hydroxide minerals such as goethite and limonite have been used as low grade brown iron ore. The aluminum ore bauxite is composed largely of aluminum hydroxides.

See also

Notes

  1. http://www.iupac.org/reports/provisional/abstract04/RB-prs310804/TableIX-3.04.pdf

References

  • Cotton, F. Albert, and Geoffrey Wilkinson. 1980. Advanced Inorganic Chemistry. 4th ed. New York: Wiley. ISBN 0471027758.
  • McMurry, J., and R.C. Fay. 2004. Chemistry. 4th ed. Upper Saddle River, NJ: Prentice Hall. ISBN 0131402080.

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