Chemistry:Magnesium carbonate
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3D model (JSmol)
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| ChEBI | |
| ChEMBL | |
| ChemSpider | |
PubChem CID
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| Properties | |
| MgCO 3 | |
| Molar mass | 84.3139 g/mol (anhydrous) |
| Appearance | Colourless crystals or white solid Hygroscopic |
| Odor | Odorless |
| Density | 2.958 g/cm3 (anhydrous) 2.825 g/cm3 (dihydrate) 1.837 g/cm3 (trihydrate) 1.73 g/cm3 (pentahydrate) |
| Melting point | 350 °C (662 °F; 623 K) decomposes (anhydrous) 165 °C (329 °F; 438 K) (trihydrate) |
| Anhydrous: 0.0139 g/100 ml (25 °C) 0.0063 g/100 ml (100 °C)[1] | |
Solubility product (Ksp)
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10−7.8[2] |
| Solubility | Soluble in acid, aqueous CO 2 Insoluble in acetone, ammonia |
| −32.4·10−6 cm3/mol | |
Refractive index (nD)
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1.717 (anhydrous) 1.458 (dihydrate) 1.412 (trihydrate) |
| Structure | |
| Trigonal | |
| R3c, No. 167[3] | |
| Thermochemistry | |
Heat capacity (C)
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75.6 J/mol·K[1] |
Std molar
entropy (S |
65.7 J/mol·K[1][4] |
Std enthalpy of
formation (ΔfH⦵298) |
−1113 kJ/mol[4] |
Gibbs free energy (ΔfG˚)
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−1029.3 kJ/mol[1] |
| Pharmacology | |
| 1=ATC code }} | A02AA01 (WHO) A06AD01 (WHO) |
| Hazards | |
| Safety data sheet | ICSC 0969 |
| NFPA 704 (fire diamond) | |
| Flash point | Non-flammable |
| NIOSH (US health exposure limits): | |
PEL (Permissible)
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| Related compounds | |
Other anions
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Magnesium bicarbonate |
Other cations
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Beryllium carbonate Calcium carbonate Strontium carbonate Barium carbonate Radium carbonate |
Related compounds
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Artinite Hydromagnesite Dypingite |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
 verify (what is   ?)
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| Infobox references | |
Magnesium carbonate, MgCO
3 (archaic name magnesia alba), is an inorganic salt that is a colourless or white solid. Several hydrated and basic forms of magnesium carbonate also exist as minerals.
Forms
The most common magnesium carbonate forms are the anhydrous salt called magnesite (MgCO
3), and the di, tri, and pentahydrates known as barringtonite (MgCO
3 · 2H2O), nesquehonite (MgCO
3 · 3H2O), and lansfordite (MgCO
3 · 5H2O), respectively.[6] Some basic forms such as artinite (Mg
2CO
3(OH)
2 · 3H2O), hydromagnesite (Mg
5(CO
3)
4(OH)
2 · 4H2O), and dypingite (Mg
5(CO
3)
4(OH)
2 · 5H2O) also occur as minerals. All of those minerals are colouress or white.
Magnesite consists of colourless or white trigonal crystals. The anhydrous salt is practically insoluble in water, acetone, and ammonia. All forms of magnesium carbonate react with acids. Magnesite crystallizes in the calcite structure wherein Mg2+ is surrounded by six oxygen atoms.[3]
| Carbonate coordination | Magnesium coordination | Unit cell |
|---|---|---|
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The dihydrate has a triclinic structure, while the trihydrate has a monoclinic structure.
References to "light" and "heavy" magnesium carbonates actually refer to the magnesium hydroxy carbonates hydromagnesite and dypingite, respectively.[7]
Preparation
Magnesium carbonate is ordinarily obtained by mining the mineral magnesite. Seventy percent of the world's supply is mined and prepared in China.[8]
Magnesium carbonate can be prepared in laboratory by reaction between any soluble magnesium salt and sodium bicarbonate:
- MgCl2(aq) + 2 NaHCO3(aq) → MgCO3(s) + 2 NaCl(aq) + H2O(l) + CO2(g)
If magnesium chloride (or sulfate) is treated with aqueous sodium carbonate, a precipitate of basic magnesium carbonate – a hydrated complex of magnesium carbonate and magnesium hydroxide – rather than magnesium carbonate itself is formed:
- 5 MgCl2(aq) + 5 Na2CO3(aq) + 5 H2O(l) → Mg4(CO3)3(OH)2·3H2O(s) + Mg(HCO3)2(aq) + 10 NaCl(aq)
High purity industrial routes include a path through magnesium bicarbonate, which can be formed by combining a slurry of magnesium hydroxide and carbon dioxide at high pressure and moderate temperature.[6] The bicarbonate is then vacuum dried, causing it to lose carbon dioxide and a molecule of water:
- Mg(OH)
2 + 2 CO
2 → Mg(HCO
3)
2 - Mg(HCO
3)
2 → MgCO
3 + CO
2 + H
2O
Chemical properties
With acids
Like many common group 2 metal carbonates, magnesium carbonate reacts with aqueous acids to release carbon dioxide and water:
- MgCO
3 + 2 HCl → MgCl
2 + CO
2 + H
2O - MgCO
3 + H
2SO
4 → MgSO
4 + CO
2 + H
2O
Decomposition
At high temperatures MgCO3 decomposes to magnesium oxide and carbon dioxide. This process is important in the production of magnesium oxide.[6] This process is called calcining:
- MgCO
3 → MgO + CO
2 (ΔH = +118 kJ/mol)
The decomposition temperature is given as 350 °C (662 °F).[9][10] However, calcination to the oxide is generally not considered complete below 900 °C due to interfering readsorption of liberated carbon dioxide.
The hydrates of the salts lose water at different temperatures during decomposition.[11] For example, in the trihydrate MgCO
3 · 3H2O, which molecular formula may be written as Mg(HCO
3)(OH) · 2H2O, the dehydration steps occur at 157 °C and 179 °C as follows:[11]
- Mg(HCO
3)(OH) · 2(H
2O) → Mg(HCO
3)(OH) · (H
2O) + H
2O at 157 °C - Mg(HCO
3)(OH) · (H
2O) → Mg(HCO
3)(OH) + H
2O at 179 °C
Uses
The primary use of magnesium carbonate is the production of magnesium oxide by calcining. Magnesite and dolomite minerals are used to produce refractory bricks.[6] MgCO
3 is also used in flooring, fireproofing, fire extinguishing compositions, cosmetics, dusting powder, and toothpaste. Other applications are as filler material, smoke suppressant in plastics, a reinforcing agent in neoprene rubber, a drying agent, and colour retention in foods.
Because of its low solubility in water and hygroscopic properties, MgCO
3 was first added to salt in 1911 to make it flow more freely. The Morton Salt company adopted the slogan "When it rains it pours", meaning that its salt containing MgCO
3 would not stick together in humid weather.[12] Magnesium carbonate, most often referred to as "chalk", is also used as a drying agent on athletes' hands in rock climbing, gymnastics, weightlifting and other sports in which a firm grip is necessary.[8]
As a food additive, magnesium carbonate is known as E504. Its only known side effect is that it may work as a laxative in high concentrations.[13]
Magnesium carbonate is used in taxidermy for whitening skulls. It can be mixed with hydrogen peroxide to create a paste, which is spread on the skull to give it a white finish.
Magnesium carbonate is used as a matte white coating for projection screens.[14]
Medical use
It is a laxative to loosen the bowels.
In addition, high purity magnesium carbonate is used as an antacid and as an additive in table salt to keep it free flowing. Magnesium carbonate can do this because it does not dissolve in water, only in acid, where it will effervesce (bubble).[15]
Safety
Magnesium carbonate is non-toxic and non-flammable.
Compendial status
See also
- Calcium acetate/magnesium carbonate
- Upsalite, a reported amorphous form of magnesium carbonate
Notes and references
- ↑ 1.0 1.1 1.2 1.3 "Magnesium carbonate". http://chemister.ru/Database/properties-en.php?dbid=1&id=634.
- ↑ Bénézeth, Pascale; Saldi, Giuseppe D.; Dandurand, Jean-Louis; Schott, Jacques (2011). "Experimental determination of the solubility product of magnesite at 50 to 200 °C". Chemical Geology 286 (1–2): 21–31. doi:10.1016/j.chemgeo.2011.04.016. Bibcode: 2011ChGeo.286...21B.
- ↑ 3.0 3.1 Ross, Nancy L. (1997). "The equation of state and high-pressure behavior of magnesite". Am. Mineral. 82 (7–8): 682–688. doi:10.2138/am-1997-7-805. Bibcode: 1997AmMin..82..682R.
- ↑ 4.0 4.1 Zumdahl, Steven S. (2009). Chemical Principles 6th Ed.. Houghton Mifflin Company. p. A22. ISBN 978-0-618-94690-7.
- ↑ NIOSH Pocket Guide to Chemical Hazards. "#0373". National Institute for Occupational Safety and Health (NIOSH). https://www.cdc.gov/niosh/npg/npgd0373.html.
- ↑ 6.0 6.1 6.2 6.3 Margarete Seeger; Walter Otto; Wilhelm Flick; Friedrich Bickelhaupt; Otto S. Akkerman. "Ullmann's Encyclopedia of Industrial Chemistry". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a15_595.pub2.
- ↑ Botha, A.; Strydom, C.A. (2001). "Preparation of a magnesium hydroxy carbonate from magnesium hydroxide". Hydrometallurgy 62 (3): 175. doi:10.1016/S0304-386X(01)00197-9. Bibcode: 2001HydMe..62..175B.
- ↑ 8.0 8.1 Allf, Bradley (2018-05-21). "The Hidden Environmental Cost of Climbing Chalk". Cruz Bay Publishing. https://www.climbing.com/gear/the-hidden-environmental-cost-of-climbing-chalk/. "In fact, China produces 70 percent of the world’s magnesite. Most of that production—both mining and processing—is concentrated in a small corner of Liaoning, a hilly industrial province in northeast China between Beijing and North Korea."
- ↑ "IAState MSDS". http://avogadro.chem.iastate.edu/MSDS/MgCO3_anhydrous.htm.
- ↑ Weast, Robert C. (1978). CRC Handbook of Chemistry and Physics (59th ed.). West Palm Beach, FL: CRC Press. p. B-133. ISBN:0-8493-0549-8. https://archive.org/details/crchandbookofche00clev.
- ↑ 11.0 11.1 "Conventional and Controlled Rate Thermal analysis of nesquehonite Mg(HCO3)(OH)·2(H2O)". http://core.kmi.open.ac.uk/download/pdf/10883918.pdf.
- ↑ "Her Debut - Morton Salt". http://www.mortonsalt.com/heritage-era/her-first-appearance/.
- ↑ "Food-Info.net : E-numbers : E504: Magnesium carbonates". http://www.food-info.net/uk/e/e504.htm. 080419 food-info.net
- ↑ Noronha, Shonan (2015). Certified Technology Specialist-Installation. McGraw Hill Education. pp. 256. ISBN 978-0071835657.
- ↑ "What Is Magnesium Carbonate?" (in en). https://sciencing.com/magnesium-carbonate-5626269.html.
- ↑ British Pharmacopoeia Commission Secretariat (2009). "Index, BP 2009". http://www.pharmacopoeia.co.uk/pdf/2009_index.pdf.
- ↑ "Japanese Pharmacopoeia, Fifteenth Edition". 2006. http://jpdb.nihs.go.jp/jp15e/JP15.pdf.
External links
| H2CO3 | He | ||||||||||||||||
| Li2CO3, LiHCO3 |
BeCO3 | B | C | (NH4)2CO3, NH4HCO3 |
O | F | Ne | ||||||||||
| Na2CO3, NaHCO3, Na3H(CO3)2 |
MgCO3, Mg(HCO3)2 |
Al2(CO3)3 | Si | P | S | Cl | Ar | ||||||||||
| K2CO3, KHCO3 |
CaCO3, Ca(HCO3)2 |
Sc | Ti | V | Cr | MnCO3 | FeCO3 | CoCO3 | NiCO3 | CuCO3 | ZnCO3 | Ga | Ge | As | Se | Br | Kr |
| Rb2CO3 | SrCO3 | Y | Zr | Nb | Mo | Tc | Ru | Rh | Pd | Ag2CO3 | CdCO3 | In | Sn | Sb | Te | I | Xe |
| Cs2CO3, CsHCO3 |
BaCO3 | Hf | Ta | W | Re | Os | Ir | Pt | Au | Hg | Tl2CO3 | PbCO3 | (BiO)2CO3 | Po | At | Rn | |
| Fr | Ra | Rf | Db | Sg | Bh | Hs | Mt | Ds | Rg | Cn | Nh | Fl | Mc | Lv | Ts | Og | |
| ↓ | |||||||||||||||||
| La2(CO3)3 | Ce2(CO3)3 | Pr | Nd | Pm | Sm | Eu | Gd | Tb | Dy | Ho | Er | Tm | Yb | Lu | |||
| Ac | Th | Pa | UO2CO3 | Np | Pu | Am | Cm | Bk | Cf | Es | Fm | Md | No | Lr | |||
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