Manganese(II) sulfate: Difference between revisions

| Verifiedfields = changed

| Watchedfields = changed

| verifiedrevid = 400106050

| ImageCaption = Manganese(II) sulfate monohydrate

| ImageSize1 =

| ImageCaption1 = Manganese(II) sulfate tetrahydrate

|Section1={{Chembox Identifiers

| CASNo = 7785-87-7

| CASNo_Ref = {{cascite|correct|CAS}}

| CASNo2_Ref = {{cascite|correct|CAS}}

| CASNo2 = 10034-96-5

| CASNo2_Comment = (monohydrate)

| CASNo3_Ref = {{cascite|correct|CAS}}

| CASNo3 = 10101-68-5

| CASNo3_Comment = (tetrahydrate)

| ChEBI = 86360

| ChEMBL_Ref = {{ebicite|changed|EBI}}

| ChEMBL = 1200557

| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}

| PubChem = 24580

| EINECS = 232-089-9

| RTECS = OP1050000 (anhydrous) <br /> OP0893500 (tetrahydrate)

| UNII1_Ref = {{fdacite|correct|FDA}}

| UNII1 = W00LYS4T26

| UNII1_Comment = (monohydrate)

| UNII2_Ref = {{fdacite|correct|FDA}}

| UNII2 = F46LH60L4M

| UNII2_Comment = (tetrahydrate)

| StdInChI_Ref = {{stdinchicite|correct|chemspider}}

| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}

|Section2={{Chembox Properties

| Formula = MnSO₄

| MolarMass = 151.001 g/mol (anhydrous) <br /> 169.02 g/mol (monohydrate) <br /> 223.07 g/mol (tetrahydrate) <br /> 277.11 g/mol (heptahydrate)

| Appearance = white crystals (anhydrous) <br /> pale pink solid (hydrates)

| Density = 3.25 g/cm³ (anhydrous) <br /> 2.95 g/cm³ (monohydrate) <br /> 2.107 g/cm³ (tetrahydrate)

| Solubility = 52 g/100 mL (5&nbsp;°C) <br /> 70 g/100 mL (70 °C)

| SolubleOther = Very slightly soluble in [[methanol]] <br /> insoluble in [[diethyl ether|ether]] and [[ethanol]].

| MeltingPtC = 710

| MeltingPt_notes = (anhydrous) <br /> 27&nbsp;°C (tetrahydrate)

| BoilingPtC = 850

| BoilingPt_notes = (anhydrous)

| MagSus = {{val|1.3660e-2|u=cm³/mol}}

|Section3={{Chembox Structure

| Coordination =

| CrystalStruct = orthogonal (anhydrous) <br /> monoclinic (monohydrate) <br /> monoclinic (tetrahydrate)

| Dipole =

|Section7={{Chembox Hazards

| ExternalSDS = [http://www.inchem.org/documents/icsc/icsc/eics0290.htm ICSC 0290]

| NFPA-H = 1

| NFPA-F = 0

| NFPA-R = 1

| GHSPictograms = {{GHS08}}{{GHS09}}

| GHSSignalWord = Warning

| HPhrases = {{H-phrases|373|411}}

| PPhrases = {{P-phrases|260|273|314|391|501}}

|Section8={{Chembox Related

| OtherAnions =

| OtherCations = [[Chromium(III) sulfate]]<br />[[Iron(II) sulfate]]

| OtherCompounds =

}}

'''Manganese(II) sulfate''' usually refers to the [[inorganic compound]] with the [[Chemical formula|formula]] MnSO₄·H₂O. This pale pink [[deliquescent]] solid is a commercially significant manganese(II) salt. Approximately 260,000 [[tonne]]s 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 (chemistry)|salt]].<ref name=Reidies>{{ullmann|first1=Arno H. |last1=Reidies |title=Manganese Compounds |date=2007 |DOI=10.1002/14356007.a16_123}}</ref>

==Structure==

[[File:MnSO4(aq).png|thumb|left|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 ligand]]s.<ref>{{cite journal|journal=Neues Jahrbuch für Mineralogie - Monatshefte|year=1991|author=Wildner, M.|author2=Giester, G.|page=296-p306|title=The Crystal Structures of Kieserite-type Compounds. I. Crystal Structures of Me(II)SO₄*H₂O (Me = Mn, Fe, Co, Ni, Zn) (English translation)}}</ref>]]

Like many metal [[sulfate]]s, manganese sulfate forms a variety of [[Water of hydration|hydrates]]: monohydrate, tetrahydrate, pentahydrate, and heptahydrate. All of these salts dissolve in water to give faintly pink solutions of the [[Metal aquo complex|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 ligand]]s.<ref>{{cite journal |doi=10.1107/S1600536802020962|title=Manganese(II) Sulfate Tetrahydrate (Ilesite) |year=2002 |last1=Held |first1=Peter |last2=Bohatý |first2=Ladislav |journal=Acta Crystallographica Section E |volume=58 |issue=12 |pages=i121–i123 |s2cid=62599961 |doi-access=free }}</ref>

Typically, [[:Category:Manganese minerals|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 [[Manganese(II) oxide|MnO]]_''x''. In the laboratory, manganese sulfate can be made by treating [[manganese dioxide]] with [[sulfur dioxide]]:<ref>{{cite journal | author = John R. Ruhoff | title = ''n''-Heptanoic acid | journal = Organic Syntheses | volume = 16 | pages = 39 | year = 1936 | doi = 10.15227/orgsyn.016.0039}}</ref>

:{{chem2 | MnO2 + SO2 + H2O -> MnSO4(H2O) }}

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

=== Electrolysis ===

[[Electrolysis]] of manganese sulfate reverses the above reaction [[yield (chemistry)|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 battery|dry-cell batteries]].<ref name="Reidies" />

==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.<ref name=Mindat>{{cite web |url=http://www.mindat.org/ |title=Home |website=mindat.org}}</ref>

{{Reflist}}

{{Sulfates}}

[[Category:Manganese(II) compounds]]

[[Category:Deliquescent materials]]