Calcium carbonate

Calcium carbonate

  Calcium, Ca
  Carbon, C
  Oxygen, O
Names
IUPAC name
Calcium carbonate
Other names
Identifiers
3D model (JSmol)
ChEBI
ChEMBL
ChemSpider
DrugBank
ECHA InfoCard 100.006.765 Edit this at Wikidata
EC Number
  • 207-439-9
E number E170 (colours)
KEGG
RTECS number
  • FF9335000
UNII
  • InChI=1S/CH2O3.Ca/c2-1(3)4;/h(H2,2,3,4);/q;+2/p-2 checkY
    Key: VTYYLEPIZMXCLO-UHFFFAOYSA-L checkY
  • InChI=1/CH2O3.Ca/c2-1(3)4;/h(H2,2,3,4);/q;+2/p-2
    Key: VTYYLEPIZMXCLO-NUQVWONBAS
  • [Ca+2].[O-]C([O-])=O
  • C(=O)([O-])[O-].[Ca+2]
Properties
CaCO3
Molar mass 100.0869 g/mol
Appearance Fine white powder or colorless crystals; chalky taste
Odor odorless
Density 2.711 g/cm3 (calcite)
2.83 g/cm3 (aragonite)
Melting point 1,339 °C (2,442 °F; 1,612 K) (calcite)
825 °C (1,517 °F; 1,098 K) (aragonite)[4][5]
Boiling point decomposes
0.013 g/L (25 °C)[1][2]
3.3×10−9[3]
Solubility in dilute acids soluble
Acidity (pKa) 9.0
−3.82×10−5 cm3/mol
1.59
Structure
Trigonal
32/m
Thermochemistry
93 J/(mol·K)[6]
−1207 kJ/mol[6]
Pharmacology
A02AC01 (WHO) A12AA04 (WHO)
Hazards
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 0: Exposure under fire conditions would offer no hazard beyond that of ordinary combustible material. E.g. sodium chlorideFlammability 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
0
0
0
Lethal dose or concentration (LD, LC):
6450 mg/kg (oral, rat)
NIOSH (US health exposure limits):
PEL (Permissible)
 TWA 15 mg/m3 (total) TWA 5 mg/m3 (resp)[7]
Safety data sheet (SDS) ICSC 1193
Related compounds
Other anions
 Calcium bicarbonate
Other cations
Related compounds
 Calcium sulfate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Crystal structure of calcite

Calcium carbonate is a chemical compound with the chemical formula CaCO3. It is a common substance found in rocks as the minerals calcite and aragonite, most notably in chalk and limestone, eggshells, gastropod shells, shellfish skeletons and pearls. Materials containing much calcium carbonate or resembling it are described as calcareous. Calcium carbonate is the active ingredient in agricultural lime and is produced when calcium ions in hard water react with carbonate ions to form limescale. It has medical use as a calcium supplement or as an antacid, but excessive consumption can be hazardous and cause hypercalcemia and digestive issues.[8]

  1. ^ Aylward, Gordon; Findlay, Tristan (2008). SI Chemical Data Book (4th ed.). John Wiley & Sons Australia. ISBN 978-0-470-81638-7.
  2. ^ Rohleder, J.; Kroker, E. (2001). Calcium Carbonate: From the Cretaceous Period Into the 21st Century. Springer Science & Business Media. ISBN 978-3-7643-6425-0.
  3. ^ Benjamin, Mark M. (2002). Water Chemistry. McGraw-Hill. ISBN 978-0-07-238390-4.
  4. ^ "Occupational safety and health guideline for calcium carbonate" (PDF). US Dept. of Health and Human Services. Archived (PDF) from the original on 30 April 2011. Retrieved 31 March 2011.
  5. ^ "CRC Handbook of Chemistry and Physics" (PDF). Archived from the original (PDF) on 29 October 2018. Retrieved 29 October 2018.
  6. ^ a b Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A21. ISBN 978-0-618-94690-7.
  7. ^ NIOSH Pocket Guide to Chemical Hazards. "#0090". National Institute for Occupational Safety and Health (NIOSH).
  8. ^ Strumińska-Parulska, DI (2015). "Determination of 210Po in calcium supplements and the possible related dose assessment to the consumers". Journal of Environmental Radioactivity. 150: 121–125. doi:10.1016/j.jenvrad.2015.08.006. PMID 26318774.