Difference between revisions of "Barium carbonate"

Revision as of 11:41, 20 December 2015

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.

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 will 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.

References

Relevant Sciencemadness threads

• BariumCarbonate from BariumSulfate + Soda