Hidroksit hakkýnda bilgi
çeviri
...
çeviri
Hidroksit kimya biliminde,
oksijen ve
hidrojen atomlarý içeren diatomik
anyonun adýdýr. Genellikle bir
bazýn parçalanmasý sonucu ortaya çýkar. Bilinen en basit diatomik iyonlardan biridir.
Hidroksil grubu içeren
inorganik bileþikler hidroksitler olarak adlandýrýlýr. Baþlýca hidroksitler:
Sodyum hidroksit (NaOH)
Potasyum hidroksit (KOH)
Kalsiyum hidroksit (Ca(OH)<sub>2</sub>)
Amonyum hidroksit (NH<sub>4</sub>OH)
==Bir baz olarak hidroksit==
Hidroksit içeren çoðu bileþik baz yapýdadýr.
Sulu çözeltilerde çözündükçe hidroksit iyonu açýða çýkaran maddelere Arheniyus bazý denir. Örnek olarak Amonyak verilebilir. NH<sub>3</sub>:
NH<sub>3</sub>(g) + H<sub>2</sub>O(l) unicode|⇌ NH<sub>4</sub><sup>+</sup>(aq) + OH<sup>−</sup>(aq)
AÞAÄžIDAKÝ BÖLÜM ÇEVÝRÝ YAPILDIKÇA AÇILABÝLÝR
Thus, hydroxide ions are heavily involved in acid-base reactions as well as the special double displacement reaction called neutralization.
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 neutralisation reactions with acids. In general acid-alkali reactions can be simplified to
:OH<sup>−</sup> (aq) + H<sup>+</sup>(aq) → H<sub>2</sub>O (l)
by omitting spectator ions.
==Solubility==
Most inorganic hydroxide salts are insoluble in water, except for those with cations from Group I, NH<sub>4</sub><sup>+</sup>, Ba<sup>2+</sup>, Sr<sup>2+</sup>, Ca<sup>2+</sup> (little) or Tl<sup>+</sup>.
==Applications==
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 aluminium ore bauxite is composed largely of aluminium hydroxides.
==Ligand==
The hydroxide ion is a kind of ligand. It donates lone pairs of electrons, behaving as a Lewis base. Examples of complexes containing such a ligand include the aluminate ion Al(OH)<sub>4</sub><sup>−</sup> and aurate ion Au(OH)<sub>4</sub><sup>−</sup>.
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Ayrýca bakýnýz
Hidronyum
Oksit
Hidroksill
Hidroksi
==Notlar==
http://pubs3.acs.org/acs/journals/doilookup?in_doi=10.1021/j100016a003 Solvation and Transport of H<sub>3</sub>O<sup>+</sup> and OH<sup>−</sup> Ions in Water (JCP 99, 5749 (1995)
<references/>
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Ýlgili bilgi baþlýklarý
Ýlgili bilgiler: Amonyak Anyon Baz Hidrojen Hidroksil Kalsiyum hidroksit Kimya Oksijen Potasyum hidroksit Sodyum hidroksit
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