Barium carbonate

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Barium carbonate
Skeletal formula of barium carbonate Barium carbonate.png
Skeletal formula of barium carbonate
Powder of barium carbonate Uhlicitan barnaty.JPG
Powder of barium carbonate
Barium-carbonate-3D-vdW.png
Names
Other names
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
ECHA InfoCard 100.007.426 OOjs UI icon edit-ltr-progressive.svg
EC Number
  • 208-167-3
PubChem CID
RTECS number
  • CQ8600000
UNII
UN number 1564
  • InChI=1S/CH2O3.Ba/c2-1(3)4;/h(H2,2,3,4);/q;+2/p-2 Yes check.svgY
    Key: AYJRCSIUFZENHW-UHFFFAOYSA-L Yes check.svgY
  • InChI=1/CH2O3.Ba/c2-1(3)4;/h(H2,2,3,4);/q;+2/p-2
    Key: AYJRCSIUFZENHW-NUQVWONBAT
  • [Ba+2].[O-]C([O-])=O
  • C(=O)([O-])[O-].[Ba+2]
Properties
BaCO3
Molar mass 197.335 g·mol−1
Appearancewhite crystals
Odor odorless
Density 4.286 g/cm3
Melting point 811 °C (1,492 °F; 1,084 K) polymorphic transformation
Boiling point 1,450 °C (2,640 °F; 1,720 K) decomposes [1] from 1,360 °C (2,480 °F; 1,630 K)
  • 16 mg/L (8.8 °C (47.8 °F; 281.9 K))
  • 22 mg/L (18 °C (64 °F; 291 K))
  • 24 mg/L (20 °C (68 °F; 293 K))
  • 24 mg/L (24.2 °C (75.6 °F; 297.3 K)) [1]
2.58×10−9
Solubility in acid decomposes
−58.9×10−6 cm3/mol
1.676
Structure
orthorhombic
Thermochemistry
85.35 J/mol·K [1]
Std molar
entropy
(S298)
112 J/mol·K [2]
−1219 kJ/mol [2]
−1139 kJ/mol [1]
Hazards
GHS labelling: [3]
GHS-pictogram-exclam.svg
Warning
H302
P264, P270, P301+P312+P330, P501
NFPA 704 (fire diamond)
[4]
NFPA 704.svgHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
2
0
0
Flash point Non-flammable
Lethal dose or concentration (LD, LC):
418 mg/kg, oral (rat) [3]
NIOSH (US health exposure limits): [3]
REL (Recommended)
0.5 mg/m3
Safety data sheet (SDS)Sigma-Aldrich [3]
Related compounds
Other anions
Other cations
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
X mark.svgN  verify  (what is  Yes check.svgYX mark.svgN ?)

Barium carbonate is the inorganic compound with the formula BaCO3. Like most alkaline earth metal carbonates, it is a white salt that is poorly soluble in water. It occurs as the mineral known as witherite. In a commercial sense, it is one of the most important barium compounds. [5]

Contents

Preparation

Barium carbonate is made commercially from barium sulfide by treatment with sodium carbonate at 60 to 70 °C (140 to 158 °F) (soda ash method) or, more commonly carbon dioxide at 40 to 90 °C (104 to 194 °F): [5]

BaS + H2O + CO2 → BaCO3 + H2S

Reactions

Barium carbonate reacts with acids such as hydrochloric acid to form soluble barium salts, such as barium chloride:

BaCO3 + 2 HCl → BaCl2 + CO2 + H2O

Pyrolysis of barium carbonate gives barium oxide. [6]

Uses

It is mainly used to remove sulfate impurities from feedstock of the chlor-alkali process. Otherwise it is a common precursor to barium-containing compounds such as ferrites. [5]

Other uses

Barium carbonate is widely used in the ceramics industry as an ingredient in glazes. It acts as a flux, a matting and crystallizing agent and combines with certain colouring oxides to produce unique colours not easily attainable by other means. Its use is somewhat controversial since it can leach from glazes into food and drink. To reduce toxicity concerns, it is often substituted with strontium carbonate, which behaves in a similar way in glazes but is of lower toxicity.

In the brick, tile, earthenware and pottery industries barium carbonate is added to clays to precipitate soluble salts (calcium sulfate and magnesium sulfate) that cause efflorescence.

It is sometimes used as an "energiser" in the Case-hardening process.

References

  1. 1 2 3 4 "Barium carbonate". Archived from the original on 2014-05-06. Retrieved 2014-05-06.
  2. 1 2 Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. ISBN   978-0-618-94690-7.
  3. 1 2 3 4 Sigma-Aldrich Co., Barium carbonate. Retrieved on 2014-05-06.
  4. "Fisher SDS - Barium Carbonate". www.fishersci.com. Fisher Scientific. 29 March 2025. Retrieved 18 September 2025.
  5. 1 2 3 Kresse, Robert; Baudis, Ulrich; Jäger, Paul; Riechers, H. Hermann; Wagner, Heinz; Winkler, Jochen; Wolf, Hans Uwe (2007). "Barium and Barium Compounds". Ullmann's Encyclopedia of Industrial Chemistry . Weinheim: Wiley-VCH. doi:10.1002/14356007.a03_325.pub2. ISBN   978-3527306732.
  6. P. Ehrlich (1963). "Barium Oxide". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. Vol. 1. NY, NY: Academic Press. pp. 933–944.