Manganese(II) carbonate
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_Carbonate.jpg) |
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| Names | |
|---|---|
| IUPAC name
Manganese(II) carbonate
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| Identifiers | |
598-62-9  |
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| ChemSpider | 11233 |
| EC Number | 209-942-9 |
| Jmol 3D model | Interactive image |
| PubChem | 11726 |
| UNII | 9ZV57512ZM |
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| Properties | |
| MnCO3 | |
| Appearance | White to faint pink solid |
| Density | 3.12 g/cm3 |
| Melting point | 200–300 °C (392–572 °F; 473–573 K) decomposes[1][2] |
| negligible | |
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Solubility product (Ksp)
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2.24 x 10−11 |
| Solubility | soluble in dilute acid, CO2 insoluble in alcohol, ammonia |
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Refractive index (nD)
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1.597 (20 °C, 589 nm) |
| Structure | |
| hexagonal-rhombohedral | |
| Thermochemistry | |
| 94.8 J/mol·K[2] | |
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Std molar
entropy (S |
109.5 J/mol·K[2] |
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Std enthalpy of
formation (ΔfH |
-881.7 kJ/mol[2] |
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Gibbs free energy (ΔfG˚)
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-811.4 kJ/mol[2] |
| Vapor pressure | {{{value}}} |
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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| Infobox references | |
Manganese carbonate is a compound with the chemical formula MnCO3. Manganese carbonate occurs naturally as the mineral rhodochrosite. Approximately 20,000 metric tonnes were produced in 2005.[3]
Production and uses
Treatment of aqueous solutions of manganese(II) salts with alkali metal carbonates leads to precipitation of this faintly pink solid. The carbonate is insoluble in water but, like most carbonates, hydrolyses upon treatment with acids to give water-soluble salts.
Manganese carbonate decomposes with release of carbon dioxide at 200 °C to give manganese(II) oxide:
- MnCO3 → MnO + CO2
This method is sometimes employed in the production of manganese dioxide for dry-cell batteries and for ferrites.[3]
Manganese carbonate is widely used as an additive to plant fertilizers to cure manganese deficient crops. It is also used in health foods, in ceramics as a glaze colorant and flux, and in concrete stains.[4]
It is used in medicine as a hematinic.
Toxicity
Manganese poisoning, also known as manganism, may be caused by long-term exposure to manganese dust or fumes.
See also
References
- ↑ Sigma-Aldrich Co., Manganese(II) carbonate. Retrieved on 2014-05-06.
- ↑ 2.0 2.1 2.2 2.3 2.4 http://chemister.ru/Database/properties-en.php?dbid=1&id=3854
- ↑ 3.0 3.1 Arno H. Reidies "Manganese Compounds" Ullmann's Encyclopedia of Chemical Technology 2007; John Wiley
- ↑ "How To Stain Concrete with Manganese"
| H2CO3 | He | ||||||||||||||||
| Li2CO3 | 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 | Uut | Fl | Uup | Lv | Uus | Uuo | |
| ↓ | |||||||||||||||||
| La2(CO3)3 | Ce | 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 | |||
