Manganese(II) carbonate
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Names | |
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IUPAC name
Manganese(II) carbonate | |
Identifiers | |
3D model (JSmol) |
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ChemSpider | |
ECHA InfoCard | 100.009.040 |
EC Number | 209-942-9 |
PubChem CID |
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UNII | |
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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 | |
Solubility product (Ksp) |
2.24 x 10−11 |
Solubility | soluble in dilute acid, CO2 insoluble in alcohol, ammonia |
+11,400·10−6 cm3/mol | |
Refractive index (nD) |
1.597 (20 °C, 589 nm) |
Structure | |
hexagonal-rhombohedral | |
Thermochemistry | |
Heat capacity (C) |
94.8 J/mol·K[2] |
Std molar entropy (S |
109.5 J/mol·K[2] |
Std enthalpy of formation (ΔfH |
-881.7 kJ/mol[2] |
Gibbs free energy (ΔfG˚) |
-811.4 kJ/mol[2] |
Hazards | |
Flash point | Non-flammable |
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 but it is typically produced industrially. It is a pale pink, water-insoluble solid. Approximately 20,000 metric tonnes were produced in 2005.[3]
Structure and production
MnCO3 adopts a structure like calcite, consisting of manganese(II) ions in an octahedral coordination geometry.[4]
Treatment of aqueous solutions of manganese(II) nitrate with ammonia and carbon dioxide leads to precipitation of this faintly pink solid. The side product, ammonium nitrate is used as fertilizer.
![](../I/m/Rhodochrosite-Pyrite-Calcite-219228.jpg)
Reactions and uses
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, i.e. calcining, at 200 °C to give MnO1.88:
- MnCO3 + 0.44 O2 → MnO1.8 + CO2
This method is sometimes employed in the production of manganese dioxide, which is used in 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.[5]
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.
- 1 2 3 4 5 http://chemister.ru/Database/properties-en.php?dbid=1&id=3854
- 1 2 Arno H. Reidies (2007). "Manganese Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a16_123.
- ↑ Pertlik, F. (1986). "Structures of hydrothermally synthesized cobalt(II) carbonate and nickel(II) carbonate". Acta Crystallographica Section C. 42: 4–5. doi:10.1107/S0108270186097524.
- ↑ "How To Stain Concrete with Manganese"
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 |