Manganese(II) sulfate

Manganese(II) sulfate monohydrate

Manganese(II) sulfate tetrahydrate

Names
IUPAC name

Manganese(II) sulfate

Identifiers

CAS Number

* 7785-87-7 Y
* 10034-96-5 (monohydrate) Y
* 10101-68-5 (tetrahydrate) Y

3D model (JSmol)

* Interactive image

ChEBI |

* CHEBI:86360

ChEMBL |

* ChEMBL1200557 N

ChemSpider |

* 22984 Y

EC Number |

* 232-089-9

PubChem CID

* 24580

RTECS number |

* OP1050000 (anhydrous)
OP0893500 (tetrahydrate)

UNII |

* IGA15S9H40 Y
* W00LYS4T26 (monohydrate) Y
* F46LH60L4M (tetrahydrate) Y

InChI

* InChI=1S/Mn.H2O4S/c;1-5(2,3)4/h;(H2,1,2,3,4)/q+2;/p-2 Y

Key: SQQMAOCOWKFBNP-UHFFFAOYSA-L Y

* InChI=1/Mn.H2O4S/c;1-5(2,3)4/h;(H2,1,2,3,4)/q+2;/p-2

Key: SQQMAOCOWKFBNP-NUQVWONBAV

SMILES

* [Mn+2].[O-]S([O-])(=O)=O

Properties

Chemical formula

| 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/cm3 (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)

Solubility in water

| 52 g/100 mL (5 °C)
70 g/100 mL (70 °C)
Solubility | Very slightly soluble in methanol
insoluble in ether and ethanol.

Magnetic susceptibility (χ)

| 1.3660×10−2 cm3/mol
Structure

Crystal structure

| orthogonal (anhydrous)
monoclinic (monohydrate)
monoclinic (tetrahydrate)
Hazards
Safety data sheet | ICSC 0290
GHS pictograms |
GHS Signal word | Warning

GHS hazard statements

| H373, H411

GHS precautionary statements

| P260, P273, P314, P391, P501
NFPA 704 (fire diamond)  |

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 YN ?)
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 260,000 tonnes of manganese(II) sulfate were produced worldwide in 2005. It is the precursor to manganese metal and many other chemical compounds. Manganese-deficient soil is remediated with this salt.[1]

## Contents

* 1 Structure
* 2 Applications and production
* 2.1 Electrolysis
* 3 Natural occurrence
* 4 References

## Structure

Coordination sphere for Mn and S in the monohydrate. The O6 coordination sphere is provided by four separate sulfate groups and a pair of mutually trans bridging aquo ligands.[2]

Like many metal sulfates, manganese sulfate forms a variety of hydrates: monohydrate, tetrahydrate, pentahydrate, and heptahydrate. All of these salts dissolve in water to give faintly pink solutions of the aquo complex [Mn(H2O)6]2+. The structure of MnSO4·H2O has been determined by X-ray crystallography (see figure). The tetrahydrate also features Mn(II) in an O6 coordination sphere provided by bridging two sulfate anions and four aquo ligands.[3]

## 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:[4]

MnO2 \+ SO2 \+ H2O → MnSO4(H2O)

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

Electrolysis of manganese sulfate reverses the above reaction yielding 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 nature and always occur as hydrates. The monohydrate is called szmikite; the tetrahydrate is called ilesite; the pentahydrate is called jōkokuite; the hexahydrate, the most rare, is called chvaleticeite; and the heptahydrate is called mallardite.[5]

## References

1. ↑ 1.0 1.1 1.2 Reidies, Arno H.. "Ullmann's Encyclopedia of Industrial Chemistry". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH.
2. ↑ Wildner, M.; Giester, G. (1991). "The Crystal Structures of Kieserite-type Compounds. I. Crystal Structures of Me(II)SO4*H2O (Me = Mn, Fe, Co, Ni, Zn) (English translation)". Neues Jahrbuch für Mineralogie - Monatshefte: 296-p306.
3. ↑ Held, Peter; Bohatý, Ladislav (2002). "Manganese(II) Sulfate Tetrahydrate (Ilesite)". Acta Crystallographica Section E 58 (12): i121–i123. doi:10.1107/S1600536802020962.
4. ↑ John R. Ruhoff (1936). "n-Heptanoic acid". Organic Syntheses 16: 39. doi:10.15227/orgsyn.016.0039.
5. ↑ "Home". http://www.mindat.org/.

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* t
* e

Manganese compounds

* MnO
* Mn3O4
* Mn5O8
* MnS
* MnS2
* MnSO4
* MnSe2
* MnSe
* MnTe
* Mn(NO3)2
* MnCO3
* MnCl2
* MnCl3
* MnCl4
* MnF2
* MnBr2
* MnI2
* MnTiO3
* MnMoO4
* Mn(CH3COO)2
* Mn2O3
* MnF3
* K6Mn2O6
* MnO2
* Mn(OH)2
* MnO3
* K3MnO4
* MnF4
* Na2MnO4
* K2MnO4
* Mn2O7
* NaMnO4
* KMnO4
* NH4MnO4
* AgMnO4
* Ca(MnO4)2
* Ba(MnO4)2
* MnH(CO)5
* Mn2(CO)10

* v
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* e

Compounds containing the sulfate group

H2SO4 |  |  |  | He

|
|
|
|

Li2SO4 | BeSO4 | B  | esters
ROSO3−
(RO)2SO2 | (NH4)2SO4
[N2H5]HSO4
(NH3OH)2SO4
NOHSO4 | HOSO4 | F  | Ne
Na2SO4
NaHSO4 | MgSO4 | Al2(SO4)3
Al2SO4(OAc)4 | Si  | P  | SO42−
HSO3HSO4
(HSO4)2 | Cl  | Ar
K2SO4
KHSO4 | CaSO4 | Sc2(SO4)3 | TiOSO4 | VSO4
V2(SO4)3
VOSO4 | CrSO4
Cr2(SO4)3 | MnSO4 | FeSO4
Fe2(SO4)3 | CoSO4 | NiSO4 | CuSO4
Cu2SO4
[Cu(NH3)4(H2O)]SO4 | ZnSO4 | Ga2(SO4)3 | Ge  | As  | Se  | Br  | Kr
RbHSO4
Rb2SO4 | SrSO4 | Y2(SO4)3 | Zr(SO4)2 | Nb  | Mo  | Tc  | Ru  | Rh2(SO4)3 | PdSO4 | Ag2SO4 | CdSO4 | In2(SO4)3 | SnSO4
Sn(SO4)2 | Sb2(SO4)3 | Te  | I  | Xe
Cs2SO4
CsHSO4 | BaSO4 |  | Hf  | Ta  | W  | Re  | Os  | Ir  | Pt  | AuSO4
Au2(SO4)3 | Hg2SO4
HgSO4 | Tl2SO4
Tl2(SO4)3 | PbSO4 | Bi2(SO4)3 | Po  | At  | Rn
Fr  | Ra  |  | Rf  | Db  | Sg  | Bh  | Hs  | Mt  | Ds  | Rg  | Cn  | Nh  | Fl  | Mc  | Lv  | Ts  | Og
| ↓  |  |
La  | Ce2(SO4)3
Ce(SO4)2 | Pr2(SO4)3 | Nd  | Pm  | Sm  | Eu  | Gd  | Tb  | Dy  | Ho  | Er  | Tm  | Yb2(SO4)3 | Lu
Ac  | Th  | Pa  | U(SO4)2
UO2SO4 | Np  | Pu  | Am  | Cm  | Bk  | Cf  | Es  | Fm  | Md  | No  | Lr

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