Wikipedia:WikiProject Chemicals/Chembox validation/VerifiedDataSandbox and Sodium hydrosulfide: Difference between pages

{{not to be confused with|sodium hydrosulfite}}

|Verifiedfields = changed

|Watchedfields = changed

|verifiedrevid = 476996639

|ImageFile = Sodium-hydrosulfide-LT-xtal-1991-CM-3D-balls.png

|ImageSize = 250

|IUPACName = Sodium hydrosulfide

|OtherNames = Sodium bisulfide<br/>Sodium sulfhydrate<br/>Sodium hydrogen sulfide

|Section1 = {{Chembox Identifiers

|CASNo = 16721-80-5

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

|CASNo2_Ref = {{cascite|changed|??}}

|CASNo2 = 207683-19-0

|CASNo2_Comment = (hydrate)

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

|ChemSpiderID = 26058

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

|ChEMBL = 1644699

|IUPHAR_ligand = 6278

|PubChem = 28015

|RTECS = WE1900000

|EINECS = 240-778-0

| UNNumber = 2922 2318

|UNII_Ref = {{fdacite|correct|FDA}}

|UNII = FWU2KQ177W

|InChI = 1/Na.H2S/h;1H2/q+1;/p-1

|InChIKey = HYHCSLBZRBJJCH-REWHXWOFAV

|SMILES = [Na+].[SH-]

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

|StdInChI = 1S/Na.H2S/h;1H2/q+1;/p-1

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

|StdInChIKey = HYHCSLBZRBJJCH-UHFFFAOYSA-M

}}

|Section2 = {{Chembox Properties

|Formula = NaSH

|MolarMass = 56.063 g/mol

|Appearance = off-white solid, [[deliquescent]]

|Density = 1.79 g/cm³

|Solubility = 50 g/100 mL (22 °C)

|SolubleOther = Soluble in [[ethanol|alcohol]], [[diethyl ether|ether]]

|MeltingPtC = 350.1

|MeltingPt_notes = (anhydrous) <br> 55 °C (dihydrate) <br> 22 °C (trihydrate)

|Section3 = {{Chembox Structure

|CrystalStruct = rhombohedral

}}

|Section7 = {{Chembox Hazards

| ExternalSDS = [http://genesisenergy.com/wp-content/uploads/Sodium-Hydrosulfide-Solution-SDS_US-English.pdf TDC MSDS]

| GHSPictograms = {{GHS02}}{{GHS05}}{{GHS06}}{{GHS09}}

| GHSSignalWord = Danger

| HPhrases = {{H-phrases|226|251|290|301|314|400}}

| PPhrases = {{P-phrases|210|233|234|235+410|240|241|242|243|260|264|270|273|280|301+310|301+330+331|303+361+353|304+340|305+351+338|310|321|330|363|370+378|390|391|403+235|404|405|407|413|420|501}}

| MainHazards = Flammable solid, stench, reacts with acids to release [[hydrogen sulfide]]

| NFPA-H = 3

| NFPA-F = 2

| FlashPtC = 90

}}

|Section8 = {{Chembox Related

|OtherAnions = [[Sodium hydroxide]]<br/>[[Sodium amide]]

|OtherCations = [[Ammonium hydrosulfide]]

|OtherCompounds = [[Sodium sulfide]]

}}

}}

'''Sodium hydrosulfide''' is the [[chemical compound]] with the formula NaSH. This compound is the product of the half-neutralization of [[hydrogen sulfide]] ({{chem2|H2S}}) with [[sodium hydroxide]] (NaOH). NaSH and sodium sulfide are used industrially, often for similar purposes. Solid NaSH is colorless. The solid has an odor of {{chem2|H2S}} owing to hydrolysis by atmospheric moisture. In contrast with [[sodium sulfide]] ({{chem2|Na2S}}), which is insoluble in organic solvents, NaSH, being a 1:1 electrolyte, is more soluble.

==Structure and properties==

Crystalline NaHS undergoes two [[phase transition]]s. At temperatures above 360&nbsp;K, NaSH adopts the NaCl structure, which implies that the {{chem2|HS−}} behaves as a spherical anion owing to its rapid rotation, leading to equal occupancy of eight equivalent positions. Below 360&nbsp;K, a [[rhombohedral]] structure forms, and the {{chem2|HS−}} sweeps out a discoidal shape. Below 114&nbsp;K, the structure becomes [[monoclinic]]. The analogous [[rubidium]] and [[potassium]] compounds behave similarly.<ref>{{cite journal |author1=Haarmann, F. |author2=Jacobs, H. |author3=Roessler, E. |author4=Senker, J. | journal = [[J. Chem. Phys.]] | year = 2002 | volume = 117 | pages = 1269–1276 | doi = 10.1063/1.1483860 | title = Dynamics of anions and cations in hydrogensulfides of alkali metals (NaHS, KHS, RbHS): A proton nuclear magnetic resonance study | issue = 3|bibcode=2002JChPh.117.1269H | doi-access = free }}</ref>

NaSH has a relatively low melting point of 350 °C. In addition to the aforementioned anhydrous forms, it can be obtained as two different hydrates, {{chem2|NaSH*2H2O}} and {{chem2|NaSH*3H2O}}. These three species are all colorless and behave similarly, but not identically. It can be used to precipitate other metal hydrosulfides, by treatment of aqueous solutions of their salts with sodium hydrosulfide. It is analogous to sodium hydroxide, and is a strong base.

==Preparation==

One laboratory synthesis entails treatment of [[sodium ethoxide]] (NaOEt) with [[hydrogen sulfide]]:<ref>{{cite book | last = Eibeck | first = R. I. | title = Inorganic Syntheses | chapter = Sodium Hydrogen Sulfide | series = [[Inorganic Syntheses]] | volume = 7 | pages = 128–31 | year = 1963 | doi = 10.1002/9780470132388.ch35 | isbn = 9780470132388 }}</ref>

:{{chem2|NaOCH2CH3 + H2S → NaSH + CH3CH2OH}}

An alternative method involves reaction of sodium with hydrogen sulfide.<ref>{{cite journal|doi=10.1021/ic901853p|title=Hydrosulfide (HS⁻) Coordination in Iron Porphyrinates|year=2010|last1=Pavlik|first1=Jeffrey W.|last2=Noll|first2=Bruce C.|last3=Oliver|first3=Allen G.|last4=Schulz|first4=Charles E.|last5=Scheidt|first5=W. Robert|journal=Inorganic Chemistry|volume=49|issue=3|pages=1017–1026|pmid=20038134|pmc=2811220}}</ref>

==Applications==

Thousands of tons of NaSH are produced annually. Its main uses are in cloth and paper manufacture as a makeup chemical for [[sulfur]] used in the [[kraft process]], as a [[froth flotation|flotation]] agent in [[Copper extraction|copper mining]] where it is used to activate oxide [[mineral]] species, and in the leather industry for the removal of hair from hides.<ref>{{cite book |doi=10.1002/0471238961.1915040902212020.a01.pub3|chapter=Sodium Sulfates and Sulfides|title=Kirk-Othmer Encyclopedia of Chemical Technology|year=2013|last1=Butts|first1=David|last2=Bush|first2=David R.|last3=Updated By Staff|isbn=978-0471238966}}</ref>

==References==

{{reflist}}

{{sulfur compounds}}

{{Sodium compounds}}

[[Category:Sodium compounds]]

[[Category:Hydrosulfides]]