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Manganese(II) carbonate

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Title: Manganese(II) carbonate  
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Subject: Manganese, Carbonates, Manganese(II) nitrate, Manganese compounds, Chalybeate
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Manganese(II) carbonate

Manganese(II) carbonate
Impure sample of MnCO3
Names
IUPAC name
Manganese(II) carbonate
Identifiers
 Y
ChemSpider  Y
EC number 209-942-9
Jmol-3D images Image
PubChem
UNII  Y
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
2.24 x 10−11
Solubility soluble in dilute acid, CO2
insoluble in alcohol, ammonia
1.597 (20 °C, 589 nm)
Structure
hexagonal-rhombohedral
Thermochemistry
94.8 J/mol·K[2]
109.5 J/mol·K[2]
-881.7 kJ/mol[2]
-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).
 Y  (: Y/N?)

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]

Contents

  • Production and uses 1
  • Toxicity 2
  • See also 3
  • References 4

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 is essential for aerobic life and its compounds are not highly toxic. Manganese poisoning, also known as manganism, may be caused by long-term exposure to manganese dust or fumes.

See also

References

  1. ^ Sigma-Aldrich Co., Manganese(II) carbonate. Retrieved on 2014-05-06.
  2. ^ a b c d e http://chemister.ru/Database/properties-en.php?dbid=1&id=3854
  3. ^ a b Arno H. Reidies "Manganese Compounds" Ullmann's Encyclopedia of Chemical Technology 2007; John Wiley
  4. ^ "How To Stain Concrete with Manganese"
Carbonates
H2CO3 He
LiCO3 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
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