Manganese oxalate is an inorganic compound with the chemical formula MnC2O4.[3][4] Solid samples are pale pink and insoluble in water. At least two hydrates have been observed.[5] It occurs naturally as the mineral Lindbergite.[6]

Synthesis

Exchange reaction between sodium oxalate and manganese chloride:

MnCl2 + Na2C2O4 + 2 H2O → MnC2O4·2H2O + 2 NaCl

The dihydrate can also be prepared hydrothermally.[1]

Physical properties

Manganese oxalate forms light pink crystals. The crystalline hydrates have the composition MnC2O4•n H2O, where n = 2 and 3.[7] The dihydrate forms light pink crystals of the orthorhombic system, space group P212121, cell parameters a = 0.6262 nm, b = 1.3585 nm, c = 0.6091 nm, Z = 4, melts in its own crystallization water at 100 °C.[8][9]

It does not dissolve in water, pKsp = 6.8.

Chemical properties

Manganese oxalate is a precursor various manganese oxides, such as MnO, Mn
2O
3, and Mn
3O
4. it decomposes at 215 °C:[10]

MnC2O4 → MnO + CO2 + CO

See also

References

  1. ^ a b Lethbridge, Zoe A.D.; Congreve, Aileen F.; Esslemont, Emma; Slawin, Alexandra M.Z.; Lightfoot, Philip (2003). "Synthesis and structure of three manganese oxalates: MnC2O4·2H2O, [C4H8(NH2)2][Mn2(C2O4)3] and Mn2(C2O4)(OH)2". Journal of Solid State Chemistry. 172: 212–218. doi:10.1016/S0022-4596(03)00035-5.
  2. ^ John Rumble (June 18, 2018). CRC Handbook of Chemistry and Physics (99 ed.). CRC Press. pp. 5–188. ISBN 978-1138561632.
  3. ^ Lunge, Georg (1924). Lunge and Keane's Technical Methods of Chemical Analysis. 2d Ed., Edited by Charles A. Keane ...and P.C.L. Thorne. Gurney and Jackson. p. 61. Retrieved 5 August 2021.
  4. ^ Young, Philena Anne (1928). The Volumetric Determination of Vanadium and Chromium in Special Alloy Steels: Ceric Sulfate as a Volumetric Oxidizing Agent. Mack Printing Company. p. 74. Retrieved 5 August 2021.
  5. ^ Donkova, B.; Mehandjiev, D. (2004). "Mechanism of decomposition of manganese(II) oxalate dihydrate and manganese(II) oxalate trihydrate". Thermochimica Acta. 421 (1–2): 141–149. Bibcode:2004TcAc..421..141D. doi:10.1016/j.tca.2004.04.001. ISSN 0040-6031. Retrieved 5 August 2021.
  6. ^ Atencio, Daniel; Coutinho, José M.V.; Graeser, Stefan; Matioli, Paulo A.; Menezes Filho, Luiz A.D. (2004). "Lindbergite, a new Mn oxalate dihydrate from Boca Rica mine, Galiléia, Minas Gerais, Brazil, and other occurrences". American Mineralogist. 89 (7): 1087–1091. Bibcode:2004AmMin..89.1087A. doi:10.2138/am-2004-0721. ISSN 1945-3027. S2CID 100604132. Retrieved 1 December 2021.
  7. ^ Nedyalkova, Miroslava; Antonov, Vladislav (1 January 2018). "Manganese oxalates - structure-based Insights". Open Chemistry. 16 (1): 1176–1183. doi:10.1515/chem-2018-0123. ISSN 2391-5420. S2CID 104343447.
  8. ^ Puzan, Anna N.; Baumer, Vyacheslav N.; Lisovytskiy, Dmytro V.; Mateychenko, Pavel V. (1 April 2018). "Structure disordering and thermal decomposition of manganese oxalate dihydrate, MnC2O4·2H2O". Journal of Solid State Chemistry. 260: 87–94. Bibcode:2018JSSCh.260...87P. doi:10.1016/j.jssc.2018.01.022. ISSN 0022-4596.
  9. ^ Donkova, Borjana; Avdeev, Georgi (1 August 2015). "Synthesis and decomposition mechanism of γ-MnC2O4·2H2O rods under non-isothermal and isothermal conditions". Journal of Thermal Analysis and Calorimetry. 121 (2): 567–577. doi:10.1007/s10973-015-4590-4. ISSN 1588-2926. S2CID 97032400.
  10. ^ Ahmad, Tokeer; Ramanujachary, Kandalam V.; Lofland, Samuel E.; Ganguli, Ashok K. (24 November 2004). "Nanorods of manganese oxalate: a single source precursor to different manganese oxide nanoparticles (MnO, Mn2O3, Mn3O4)". Journal of Materials Chemistry. 14 (23): 3406–3410. doi:10.1039/B409010A. ISSN 1364-5501.
Allikas: https://en.wikipedia.org/wiki/Manganese_oxalate
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