Editing Barium chloride (section)

==Preparation==
On an industrial scale, barium chloride is prepared via a two step process from [[barite]] ([[barium sulfate]]).<ref>{{Greenwood&Earnshaw2nd}}</ref> The first step requires high temperatures.
:{{chem2|BaSO4 + 4 C → BaS + 4 CO}}
The second step requires reaction between [[barium sulfide]] and [[hydrogen chloride]]:
:{{chem2|BaS + 2 HCl → BaCl2 + H2S}}
or between [[barium sulfide]] and [[calcium chloride]]:
:{{chem2|BaS + CaCl2 → CaS + BaCl2}}<ref name="sciencedirect"></ref>
In place of HCl, [[chlorine]] can be used.<ref name="Ullman2005"/> Barium chloride is extracted out from the mixture with water. From water solutions of barium chloride, its dihydrate ({{chem2|BaCl2*2H2O}}) can be crystallized as colorless crystals.<ref name="sciencedirect"></ref>

Barium chloride can in principle be prepared by the reaction between [[barium hydroxide]] or [[barium carbonate]] with [[hydrogen chloride]]. These basic salts react with [[hydrochloric acid]] to give hydrated barium chloride.
:{{chem2|Ba(OH)2 + 2 HCl → BaCl2 + 2 H2O}}
:{{chem2|BaCO3 + 2 HCl → BaCl2 + H2O + CO2}}