Difference between revisions of "Barium carbonate"
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| − | '''Barium carbonate''' is an insoluble barium salt of [[carbonic acid]] with the formula BaCO<sub>3</sub>, even less soluble than barium sulfate. It, however, reacts with acids and can serve as precursor to any barium salt. | + | '''Barium carbonate''' is an insoluble barium salt of [[carbonic acid]] with the formula '''BaCO<sub>3</sub>''', even less soluble than barium sulfate. It, however, reacts with acids and can serve as precursor to any barium salt. |
== Properties == | == Properties == | ||
=== Physical === | === Physical === | ||
| − | Barium carbonate is a white chalk-like powder, insoluble in water and virtually all solvents, though it dissolves in acids, releasing carbon dioxide. When heated to 811 °C, it undergoes polymorphic transformation and starting from 1360-1,450 °C it decomposes to release carbon dioxide. It is quite dense, 4.286 g/cm<sup>3</sup> | + | Barium carbonate is a white chalk-like powder, insoluble in water and virtually all solvents, though it dissolves in acids, releasing [[carbon dioxide]]. When heated to 811 °C, it undergoes polymorphic transformation and starting from 1360-1,450 °C it decomposes to release carbon dioxide. It is quite dense, 4.286 g/cm<sup>3</sup> |
=== Chemical === | === Chemical === | ||
| − | + | Heat causes it to decompose, liberating carbon dioxide and turning into the oxide [[Barium oxide|BaO]]. | |
| − | Heat causes it to decompose, liberating carbon dioxide and turning into the oxide BaO. | + | |
It reacts with all acids, resulting in barium salts and carbon dioxide. | It reacts with all acids, resulting in barium salts and carbon dioxide. | ||
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Some pottery stores may sell barium carbonate. | Some pottery stores may sell barium carbonate. | ||
| − | It also occurs naturally as the mineral witherite. | + | It also occurs naturally as the mineral ''witherite''. |
== Preparation == | == Preparation == | ||
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[[Category:Barium compounds]] | [[Category:Barium compounds]] | ||
[[Category:Carbonates]] | [[Category:Carbonates]] | ||
| + | [[Category:Materials unstable in acidic solution]] | ||
Revision as of 10:26, 15 August 2016
Barium carbonate is an insoluble barium salt of carbonic acid with the formula BaCO3, even less soluble than barium sulfate. It, however, reacts with acids and can serve as precursor to any barium salt.
Contents
Properties
Physical
Barium carbonate is a white chalk-like powder, insoluble in water and virtually all solvents, though it dissolves in acids, releasing carbon dioxide. When heated to 811 °C, it undergoes polymorphic transformation and starting from 1360-1,450 °C it decomposes to release carbon dioxide. It is quite dense, 4.286 g/cm3
Chemical
Heat causes it to decompose, liberating carbon dioxide and turning into the oxide BaO.
It reacts with all acids, resulting in barium salts and carbon dioxide.
Availability
Barium carbonate is sold by chemical suppliers. Some rat poisons may contain barium carbonate.
Some pottery stores may sell barium carbonate.
It also occurs naturally as the mineral witherite.
Preparation
Barium carbonate is prepared from barium sulfate by lengthy boiling under reflux with sodium carbonate. This reaction is sometimes called the Curie reaction, because Marie Curie prepared radium carbonate the same way.
The reaction is very long.
Projects
- Anything having to do with barium
Handling
Safety
Barium carbonate is safe unless ingested. Upon ingestion, it is acutely poisonous, as it reacts with gastric acid to form barium chloride which is soluble in water.
Storage
It can be stored anywhere and in anything. But places that may have acidic vapors are best avoided.
Disposal
To neutralize barium carbonate, use sulfuric acid. The resulting inert barium sulfate can be dumped anywhere.
