Manganese(II) sulfate

Manganese(II) sulfate

Manganese(II) sulfate monohydrate

Manganese(II) sulfate tetrahydrate
Names
IUPAC name
Manganese(II) sulfate
Identifiers
3D model (JSmol)
ChEMBL
ChemSpider
ECHA InfoCard 100.029.172
EC Number 232-089-9
RTECS number OP1050000 (anhydrous)
OP0893500 (tetrahydrate)
UNII
Properties
MnSO4
Molar mass 151.001 g/mol (anhydrous)
169.02 g/mol (monohydrate)
223.07 g/mol (tetrahydrate)
277.11 g/mol (heptahydrate)
Appearance white crystals (anhydrous)
pale pink solid (hydrates)
Density 3.25 g/cm 3 (anhydrous)
2.95 g/cm3 (monohydrate)
2.107 g/cm3 (tetrahydrate)
Melting point 710 °C (1,310 °F; 983 K) (anhydrous)
27 °C (tetrahydrate)
Boiling point 850 °C (1,560 °F; 1,120 K) (anhydrous)
52 g/100 mL (5 °C)
70 g/100 mL (70 °C)
Solubility Very slightly soluble in methanol
insoluble in ether and ethanol.
+13,660·10−6 cm3/mol
Structure
orthogonal (anhydrous)
monoclinic (monohydrate)
monoclinic (tetrahydrate)
Hazards
Safety data sheet ICSC 0290
Harmful (Xn)
Dangerous for the environment (N)
R-phrases (outdated) R48/20/22, R51/53
S-phrases (outdated) (S2), S22, S61
NFPA 704
Flammability code 0: Will not burn. E.g., waterHealth code 1: Exposure would cause irritation but only minor residual injury. E.g., turpentineReactivity code 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g., calciumSpecial hazards (white): no codeNFPA 704 four-colored diamond
0
1
1
Related compounds
Other cations
 Chromium(III) sulfate
Iron(II) sulfate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is ☑Y☒N ?)
Infobox references

Manganese(II) sulfate usually refers to the inorganic compound with the formula MnSO4·H2O. This pale pink deliquescent solid is a commercially significant manganese(II) salt. Approximately 260 thousand tonnes of manganese(II) sulfate were produced worldwide in 2005. It is the precursor to manganese metal and many other chemical compounds. Mn-deficient soil is remediated with this salt.[1]

Structure

Like many metal sulfates, manganese sulfate forms a variety of hydrates: monohydrate, tetrahydrate, pentahydrate, and heptahydrate. The monohydrate is most common. All of these salts dissolve to give faintly pink solutions of the aquo complex [Mn(H2O)6]2+. The pale pink colour of Mn(II) salts is highly characteristic.

Applications and production

Typically, manganese ores are purified by their conversion to manganese(II) sulfate. Treatment of aqueous solutions of the sulfate with sodium carbonate leads to precipitation of manganese carbonate, which can be calcined to give the oxides MnOx. In the laboratory, manganese sulfate can be made by treating manganese dioxide with sulfur dioxide:[2]

MnO2 + SO2 → MnSO4

It can also be made by mixing potassium permanganate with sodium bisulfate and hydrogen peroxide.

Manganese sulfate is a by-product of various industrially significant oxidations that use manganese dioxide, including the manufacture of hydroquinone and anisaldehyde.[1]

Electrolysis of manganese sulfate yields manganese dioxide, which is called EMD for electrolytic manganese dioxide. Alternatively oxidation of manganese sulfate with potassium permanganate yields the so-called chemical manganese dioxide (CMD). These materials, especially EMD, are used in dry-cell batteries.[1]

Natural occurrence

Manganese(II) sulfate minerals are very rare in the nature and always occur as hydrates. The monohydrate is called szmikite; tetrahydrate = ilesite; hexahydrate (the most rare) = chvaleticeite; pentahydrate = jôkokuite; heptahydrate = mallardite.[3]

References

  1. 1 2 3 Arno H. Reidies "Manganese Compounds" Ullmann's Encyclopedia of Chemical Technology 2007; Wiley-VCH, Weinheim. doi:10.1002/14356007.a16_123
  2. ↑ John R. Ruhoff (1943). "n-Heptanoic acid". Organic Syntheses. ; Collective Volume, 2, p. 315
  3. ↑ www.mindat.org
This article is issued from Wikipedia. The text is licensed under Creative Commons - Attribution - Sharealike. Additional terms may apply for the media files.