Sodium hydrosulfide

Sodium hydrosulfide
Names
	IUPAC name Sodium hydrosulfide
	Other names Sodium bisulfide; Sodium sulfhydrate; Sodium hydrogen sulfide
Identifiers
CAS Number	16721-80-5 ; 207683-19-0 (hydrate) ;
3D model (JSmol)	Interactive image;
ChEMBL	ChEMBL1644699 ;
ChemSpider	26058 ;
ECHA InfoCard	100.037.056
EC Number	240-778-0;
IUPHAR/BPS	6278;
PubChem CID	28015;
RTECS number	WE1900000;
UNII	FWU2KQ177W ;
UN number	2922 2318
CompTox Dashboard (EPA)	DTXSID3029738 ;
	InChI InChI=1S/Na.H2S/h;1H2/q+1;/p-1 Key: HYHCSLBZRBJJCH-UHFFFAOYSA-M ; InChI=1/Na.H2S/h;1H2/q+1;/p-1 Key: HYHCSLBZRBJJCH-REWHXWOFAV;
	SMILES [Na+].[SH-];
Properties
Chemical formula	NaSH
Molar mass	56.063 g/mol
Appearance	off-white solid, deliquescent
Density	1.79 g/cm3
Melting point	350.1 °C (662.2 °F; 623.2 K) (anhydrous) ; 55 °C (dihydrate) ; 22 °C (trihydrate)
Solubility in water	50 g/100 mL (22 °C)
Solubility	Soluble in alcohol, ether
Structure
Crystal structure	rhombohedral
Hazards
	Occupational safety and health (OHS/OSH):
Main hazards	Flammable solid, stench, reacts with acids to release hydrogen sulfide
	GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H226, H251, H290, H301, H314, H400
Precautionary statements	P210, P233, P234, P235+P410, P240, P241, P242, P243, P260, P264, P270, P273, P280, P301+P310, P301+P330+P331, P303+P361+P353, P304+P340, P305+P351+P338, P310, P321, P330, P363, P370+P378, P390, P391, P403+P235, P404, P405, P407, P413, P420, P501
NFPA 704 (fire diamond)	3 2
Flash point	90 °C (194 °F; 363 K)
Safety data sheet (SDS)	TDC MSDS
Related compounds
Other anions	Sodium hydroxide; Sodium amide
Other cations	Ammonium hydrosulfide
Related compounds	Sodium sulfide
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). verify (what is ?) Infobox references

Sodium hydrosulfide is the chemical compound with the formula NaSH. This compound is the product of the half-neutralization of hydrogen sulfide (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 H₂S owing to hydrolysis by atmospheric moisture. In contrast with sodium sulfide (Na₂S), which is insoluble in organic solvents, NaSH, being a 1:1 electrolyte, is more soluble.

Structure and properties

Crystalline NaHS undergoes two phase transitions. At temperatures above 360 K, NaSH adopts the NaCl structure, which implies that the HS⁻ behaves as a spherical anion owing to its rapid rotation, leading to equal occupancy of eight equivalent positions. Below 360 K, a rhombohedral structure forms, and the HS⁻ sweeps out a discoidal shape. Below 114 K, the structure becomes monoclinic. The analogous rubidium and potassium compounds behave similarly.^[1]

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, NaSH·2H₂O and 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:^[2]

NaOCH₂CH₃ + H₂S → NaSH + CH₃CH₂OH

An alternative method involves reaction of sodium with hydrogen sulfide.^[3]

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 flotation agent in copper mining where it is used to activate oxide mineral species, and in the leather industry for the removal of hair from hides.^[4]

References

↑ Haarmann, F.; Jacobs, H.; Roessler, E.; Senker, J. (2002). "Dynamics of anions and cations in hydrogensulfides of alkali metals (NaHS, KHS, RbHS): A proton nuclear magnetic resonance study". J. Chem. Phys. 117 (3): 1269–1276. Bibcode:2002JChPh.117.1269H. doi:10.1063/1.1483860.
↑ Eibeck, R. I. (1963). "Sodium Hydrogen Sulfide". Inorganic Syntheses. Inorganic Syntheses. Vol. 7. pp. 128–31. doi:10.1002/9780470132388.ch35. ISBN 9780470132388.
↑ Pavlik, Jeffrey W.; Noll, Bruce C.; Oliver, Allen G.; Schulz, Charles E.; Scheidt, W. Robert (2010). "Hydrosulfide (HS⁻) Coordination in Iron Porphyrinates". Inorganic Chemistry. 49 (3): 1017–1026. doi:10.1021/ic901853p. PMC 2811220. PMID 20038134.
↑ Butts, David; Bush, David R.; Updated By Staff (2013). "Sodium Sulfates and Sulfides". Kirk-Othmer Encyclopedia of Chemical Technology. doi:10.1002/0471238961.1915040902212020.a01.pub3. ISBN 978-0471238966.

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[1] Haarmann, F.; Jacobs, H.; Roessler, E.; Senker, J. (2002). "Dynamics of anions and cations in hydrogensulfides of alkali metals (NaHS, KHS, RbHS): A proton nuclear magnetic resonance study". J. Chem. Phys. 117 (3): 1269–1276. Bibcode:2002JChPh.117.1269H. doi:10.1063/1.1483860.

[2] Eibeck, R. I. (1963). "Sodium Hydrogen Sulfide". Inorganic Syntheses. Inorganic Syntheses. Vol. 7. pp. 128–31. doi:10.1002/9780470132388.ch35. ISBN 9780470132388.

[3] Pavlik, Jeffrey W.; Noll, Bruce C.; Oliver, Allen G.; Schulz, Charles E.; Scheidt, W. Robert (2010). "Hydrosulfide (HS⁻) Coordination in Iron Porphyrinates". Inorganic Chemistry. 49 (3): 1017–1026. doi:10.1021/ic901853p. PMC 2811220. PMID 20038134.

[4] Butts, David; Bush, David R.; Updated By Staff (2013). "Sodium Sulfates and Sulfides". Kirk-Othmer Encyclopedia of Chemical Technology. doi:10.1002/0471238961.1915040902212020.a01.pub3. ISBN 978-0471238966.

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