| IUPAC name
| Other names
|Molar mass||197.34 g/mol|
|Melting point||811 °C (1,492 °F; 1,084 K) (polymorphic transformation)|
|Boiling point||1,450 °C (2,640 °F; 1,720 K) (decomposes)|
| 0.0016 g/100ml (8.8 °C)|
0.0022 g/100 ml (18 °C)
0.0024 g/100 ml (20 °C)
0.0024 g/100 ml (24.2 °C)
|Solubility|| Reacts with acids|
Insoluble in organic solvents
|Vapor pressure||~0 mmHg|
Std enthalpy of
|Safety data sheet||Sigma-Aldrich|
|Lethal dose or concentration (LD, LC):|
LD50 (Median dose)
|418 mg/kg (rat, oral)|
| Magnesium carbonate|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Barium carbonate is an insoluble barium salt of carbonic acid with the formula BaCO3, even less soluble than barium sulfate. Unlike BaSO4, barium carbonate reacts with acids and can serve as precursor to any barium salt.
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. Barium barbonate is quite dense, 4.286 g/cm3
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. This makes it a useful precursor to all barium compounds.
Barium carbonate is sold by chemical suppliers. Some rat poisons may contain barium carbonate.
Occasionally, pottery stores may sell barium carbonate.
It also occurs naturally as the mineral witherite.
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.
- Anything having to do with barium
- Make barium peroxide
Barium carbonate is safe to handle, unless ingested. Upon ingestion, it is acutely poisonous, as it reacts with gastric acid to form barium chloride which is soluble in water. In the event of accidental ingestion, immediately consume a soluble sulfate solution, like aqueous magnesium sulfate.
It can be stored anywhere and in anything. But places that may have acidic vapors are best avoided.
To neutralize barium carbonate, use sulfuric acid. The resulting inert barium sulfate can be dumped anywhere.