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|Molar mass||171.342 g/mol (anhydrous)|
189.36 g/mol (monohydrate)
315.46 g/mol (octahydrate)
|Solubility in other solvents||low|
|Std enthalpy of
|Except where noted otherwise, data are given for|
materials in their standard state
(at 25 °C, 100 kPa)
Infobox disclaimer and references
Barium hydroxide can be prepared by dissolving barium oxide (BaO) in water.
- BaO + 9H2O → Ba(OH)2·8H2O
It crystallises as the octahydrate, which converts to the monohydrate upon heating in air. At 100 °C in a vacuum, the monohydrate gives BaO.
Barium hydroxide is used in analytical chemistry for the titration of weak acids, particularly organic acids. Its clear aqueous solution is guaranteed to be free of carbonate, unlike those of sodium hydroxide and potassium hydroxide, as barium carbonate is insoluble in water. This allows the use of indicators such as phenolphthalein or thymolphthalein (with alkaline colour changes) without the risk of titration errors due to the presence of weakly basic carbonate ions.
It has been used to hydrolyse one of the two equivalent ester groups in dimethyl hendecanedioate.
- Under the name baryta it is used in homeopathic remedies.
- It is also used to clean up acid spills.
- Also under the name of baryta it is used in the production of photographic paper for printing.
Barium hydroxide presents the same hazards as other strong bases and as other water-soluble barium compounds: it is corrosive and toxic.
- Gmelins Handbuch der anorganischen Chemie (8. Aufl.), Weinheim:Verlag Chemie, 1960, p. 289.
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