Hydroxylammonium sulfate

Hydroxylammonium sulfate
Names
	Other names Hydroxylamine sulfate
Identifiers
CAS Number	10039-54-0 ;
3D model (JSmol)	Interactive image;
ChEMBL	ChEMBL3183215;
ChemSpider	23229 ;
ECHA InfoCard	100.030.095
EC Number	233-118-8;
PubChem CID	24846;
RTECS number	NC5425000;
UNII	49KP498D4O ;
UN number	2865
CompTox Dashboard (EPA)	DTXSID2025424 ;
	InChI InChI=1S/2H4NO.H2O4S/c21-2;1-5(2,3)4/h22H,1H3;(H2,1,2,3,4)/q2+1;/p-2 Key: VGYYSIDKAKXZEE-UHFFFAOYSA-L ; InChI=1/2H4NO.H2O4S/c21-2;1-5(2,3)4/h22H,1H3;(H2,1,2,3,4)/q2+1;/p-2 Key: VGYYSIDKAKXZEE-NUQVWONBAN;
	SMILES [O-]S([O-])(=O)=O.O[NH3+].O[NH3+];
Properties
Chemical formula	H8N2O6S
Molar mass	164.14 g/mol
Appearance	white crystalline to fine product, slightly hygroscopic
Density	1.88 g/cm3
Melting point	120 °C (248 °F; 393 K) decomposes
Solubility in water	58.7 g/100 ml (20 °C)
Structure
Crystal structure	Monoclinic
Space group	P21/c
Lattice constant	a = 7.932±0.002 Å, b = 7.321±0.002 Å, c = 10.403±0.003 Å α = 90°, β = 106.93±0.03°, γ = 90°
Formula units (Z)	4
Hazards
	GHS labelling:
Pictograms
Signal word	Warning
Hazard statements	H290, H302, H312, H315, H317, H319, H351, H373, H400, H412
Precautionary statements	P201, P202, P234, P260, P261, P264, P270, P272, P273, P280, P281, P301+P312, P302+P352, P305+P351+P338, P308+P313, P312, P314, P321, P322, P330, P332+P313, P333+P313, P337+P313, P362, P363, P390, P391, P404, P405, P501
NFPA 704 (fire diamond)	3 1 2
Safety data sheet (SDS)	External MSDS
Related compounds
Other anions	Hydroxylammonium nitrate; Hydroxylammonium chloride
Other cations	Ammonium sulfate; Hydrazinium sulfate
Related compounds	Hydroxylamine
	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

Hydroxylammonium sulfate is the inorganic compound with the formula [NH₃OH]₂SO₄. A colorless solid, it is the sulfate salt of hydroxylamine. It is primarily used as an easily handled form of hydroxylamine, which is a volatile liquid.^[2]

Production

Hydroxylammonium sulfate is prepared industrially by protonation of hydroxylamine. The latter is produced by the hydrogenation of nitric oxide using a platinum catalyst:^[2]

2 NO + 3 H₂ + H₂SO₄ → [NH₃OH]₂[SO₄]

Another route to NH₂OH is the Raschig process: aqueous ammonium nitrite is reduced by HSO−3 and SO₂ at 0 °C to yield a hydroxylamido-N,N-disulfonate anion::^[3]

[NH₄]⁺[NO₂]⁻ + 2 SO₂ + NH₃ + H₂O → [NH₄]₂[HON(SO₃)₂]

This ammonium hydroxylamine disulfonate anion is then hydrolyzed to give hydroxylammonium sulfate:

[NH₄]₂[HON(SO₃)₂] + 2 H₂O → [HONH₃]₂SO₄

Applications

Almost all hydroxylamine and its salts are used to make precursors to nylons via cyclohexanone oxime.^[2] Many aldehydes and ketones undergo the same conversion to oximes. carboxylic acids and their derivatives (e.g. esters) convert to hydroxamic acids. Isocyanates to N-hydroxyureas. Nitriles react to give amidoximes. Hydroxylammonium sulfate is also used to generate hydroxylamine-O-sulfonic acid from oleum or from chlorosulfuric acid.

Hydroxylammonium sulfate is used in the production of anti-skinning agents, pharmaceuticals, rubber, textiles, plastics and detergents. It is a radical scavenger that terminates radical polymerization reactions and serves as an antioxidant in natural rubber. (NH₃OH)₂SO₄ is a starting material for some insecticides, herbicides and growth regulators. It is used in photography as a stabiliser for colour developers and as an additive in photographic emulsions in colour film.

Structure

Hydroxylammonium sulfate exists as tetrahedral NH₃OH⁺ cations and sulfate anions.

Safety

Hydroxylamine, which occurs widely in nature, has low toxicity. The compound is stable below 120 °C.^[2]

References

^ Mirceva, A.; Golic, L. (15 May 1995). "Hydroxylammonium Sulfate". Acta Crystallographica Section C Crystal Structure Communications. 51 (5): 798–800. Bibcode:1995AcCrC..51..798M. doi:10.1107/S0108270194013351.
^ ^a ^b ^c ^d Ritz, Josef; Fuchs, Hugo; Perryman, Howard G. (2000). "Hydroxylamine". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a13_527. ISBN 3527306730.
^ Oblath, S. B.; Markowitz, S. S.; Novakov, T.; Chang, S. G. (December 1982). "Kinetics of the initial reaction of nitrite ion in bisulfite solutions" (PDF). The Journal of Physical Chemistry. 86 (25): 4853–4857. doi:10.1021/j100222a005.

External links

International Chemical Safety Card 0898

[1] Mirceva, A.; Golic, L. (15 May 1995). "Hydroxylammonium Sulfate". Acta Crystallographica Section C Crystal Structure Communications. 51 (5): 798–800. Bibcode:1995AcCrC..51..798M. doi:10.1107/S0108270194013351.

[Ullmann-2] Ritz, Josef; Fuchs, Hugo; Perryman, Howard G. (2000). "Hydroxylamine". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a13_527. ISBN 3527306730.

[3] Oblath, S. B.; Markowitz, S. S.; Novakov, T.; Chang, S. G. (December 1982). "Kinetics of the initial reaction of nitrite ion in bisulfite solutions" (PDF). The Journal of Physical Chemistry. 86 (25): 4853–4857. doi:10.1021/j100222a005.

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