Editing Salt (chemistry) (section)

===Acidity/basicity===
Ionic compounds containing [[hydrogen ion]]s (H<sup>+</sup>) are classified as [[acid]]s, and those containing [[electropositivity|electropositive]] cations<ref>{{cite web |url=http://www.wou.edu/las/physci/ch412/oxides.html |title=Periodic Trends and Oxides |access-date=2015-11-10 |url-status=live |archive-url=https://web.archive.org/web/20151229143840/http://www.wou.edu/las/physci/ch412/oxides.html |archive-date=2015-12-29 }}</ref> and basic anions ions [[hydroxide]] (OH<sup>−</sup>) or [[oxide]] (O<sup>2−</sup>) are classified as [[Base (chemistry)|bases]]. Other ionic compounds are known as salts and can be formed by [[Acid–base reaction#Arrhenius theory|acid–base reactions]].<ref>{{cite book |last1=Whitten |first1=Kenneth W. |last2=Galley |first2= Kenneth D.|last3=Davis|first3=Raymond E.| title=General Chemistry|url=https://archive.org/details/generalchemistry00whit_0 |url-access=registration |edition = 4th|year=1992 | publisher=Saunders | page=[https://archive.org/details/generalchemistry00whit_0/page/128 128]| isbn=978-0-03-072373-5}}</ref> Salts that produce [[hydroxide]] [[ions]] when dissolved in [[water]] are called [[alkali salt]]s, and salts that produce [[hydrogen]] [[ions]] when dissolved in [[water]] are called [[acid salt]]s. If the compound is the result of a reaction between a [[strong acid]] and a [[weak base]], the result is an [[acid salt]]. If it is the result of a reaction between a [[strong base]] and a [[weak acid]], the result is a [[base salt]]. If it is the result of a reaction between a strong acid and a strong base, the result is a neutral salt. Weak acids reacted with weak bases can produce ionic compounds with both the [[conjugate base]] ion and conjugate acid ion, such as [[ammonium acetate]].

Some ions are classed as [[Amphoterism|amphoteric]], being able to react with either an acid or a base.<ref>{{cite journal|last1=Davidson|first1=David|title=Amphoteric molecules, ions and salts|journal=Journal of Chemical Education|date=November 1955|volume=32|issue=11|page=550|doi=10.1021/ed032p550|bibcode=1955JChEd..32..550D}}</ref> This is also true of some compounds with ionic character, typically oxides or hydroxides of less-electropositive metals (so the compound also has significant covalent character), such as [[zinc oxide]], [[aluminium hydroxide]], [[aluminium oxide]] and [[lead(II) oxide]].<ref>{{cite book|first1=Mark|last1=Weller|first2=Tina|last2=Overton|first3=Jonathan|last3=Rourke|first4=Fraser|last4=Armstrong|title=Inorganic chemistry|date=2014|publisher=Oxford University Press|location=Oxford|isbn=978-0-19-964182-6|pages=129–130|edition=Sixth}}</ref>