en Cadmium sulfate

Cadmium sulfate
Names
	IUPAC name Cadmium(II) sulfate
	Other names Sulfuric acid, cadmium salt (1:1),
Identifiers
CAS Number	10124-36-4 ; 7790-84-3 (octahydrate) ; 13477-21-9 (tetrahydrate) ;
3D model (JSmol)	Interactive image;
ChEBI	CHEBI:50292 ; CHEBI:86157 (octahydrate);
ChemSpider	23335 ;
ECHA InfoCard	100.030.288
EC Number	233-331-6;
Gmelin Reference	8295
PubChem CID	24962 (anhydrous); 23618914 (tetrahydrate); 16211218 (octahydrate);
RTECS number	EV2700000;
UNII	947UNF3Z6O ;
UN number	2570
CompTox Dashboard (EPA)	DTXSID1020229 ;
	InChI InChI=1S/Cd.H2O4S/c;1-5(2,3)4/h;(H2,1,2,3,4)/q+2;/p-2 Key: QCUOBSQYDGUHHT-UHFFFAOYSA-L ; InChI=1/Cd.H2O4S/c;1-5(2,3)4/h;(H2,1,2,3,4)/q+2;/p-2 Key: QCUOBSQYDGUHHT-NUQVWONBAG;
	SMILES [Cd+2].[O-]S([O-])(=O)=O;
Properties
Chemical formula	CdSO4 ; CdSO4·H2O (monohydrate) ; 3CdSO4·8H2O (octahydrate)
Molar mass	208.47 g/mol (anhydrous) ; 226.490 g/mol (monohydrate) ; 769.546 g/mol (octahydrate)
Appearance	White hygroscopic solid
Odor	odorless
Density	4.691 g/cm3 (anhydrous) ; 3.79 g/cm3 (monohydrate) ; 3.08 g/cm3 (octahydrate)
Melting point	1,000 °C (1,830 °F; 1,270 K) (anhydrous) ; 105 °C (monohydrate) ; 40 °C (octahydrate)
Boiling point	(decomposes to basic sulfate and then oxide)
Solubility in water	anhydrous: ; 75 g/100 mL (0 °C) ; 76.4 g/100 mL (25 °C) ; 58.4 g/100 mL (99 °C) monohydrate: ; 76.7 g/100 mL (25 °C) octahydrate: ; very soluble
Solubility	slightly soluble in methanol, ethyl acetate ; insoluble in ethanol
Magnetic susceptibility (χ)	-59.2·10−6 cm3/mol
Refractive index (nD)	1.565
Structure
Crystal structure	orthorhombic (anhydrous) ; monoclinic (hepta & octahydrate)
Thermochemistry
Std molar; entropy (S⦵298)	123 J·mol−1·K−1
Std enthalpy of; formation (ΔfH⦵298)	−935 kJ·mol−1
Hazards
	GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H301, H330, H340, H350, H360, H372, H410
Precautionary statements	P201, P202, P260, P264, P270, P271, P273, P281, P284, P301+P310, P304+P340, P308+P313, P310, P314, P320, P321, P330, P391, P403+P233, P405, P501
NFPA 704 (fire diamond)	3 1 0
	Lethal dose or concentration (LD, LC):
LD50 (median dose)	280 mg/kg (oral, rat)
	NIOSH (US health exposure limits):
PEL (Permissible)	[1910.1027] TWA 0.005 mg/m3 (as Cd)
REL (Recommended)	Ca
IDLH (Immediate danger)	Ca [9 mg/m3 (as Cd)]
Safety data sheet (SDS)	[1]
Related compounds
Other anions	Cadmium acetate,; Cadmium chloride,; Cadmium nitrate
Other cations	Zinc sulfate,; Calcium sulfate,; Magnesium sulfate
	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

Cadmium sulfate is the name of a series of related inorganic compounds with the formula CdSO₄· $x$ H₂O. The most common form is the monohydrate CdSO₄·H₂O, but two other forms are known CdSO₄·8⁄3H₂O and the anhydrous salt (CdSO₄). All salts are colourless and highly soluble in water.

Structure, preparation, and occurrence

Portion of structure of CdSO4 illustrating the distorted tetrahedral geometry at Cd (dark blue spheres).^[4]

X-ray crystallography shows that CdSO₄·H₂O is a typical coordination polymer. Each Cd²⁺ center has octahedral coordination geometry, being surrounded by four oxygen centers provided by four sulfate ligands and two oxygen centers from the bridging water ligands.^[5]

Cadmium sulfate hydrate can be prepared by the reaction of cadmium metal or its oxide or hydroxide with dilute sulfuric acid:

CdO + H₂SO₄ → CdSO₄ + H₂O

Cd + H₂SO₄ → CdSO₄ + H₂

The anhydrous material can be prepared using sodium persulfate:^{[citation needed]}

Cd + Na₂S₂O₈ → CdSO₄ + Na₂SO₄

Cadmium sulfates occur as the following rare minerals drobecite (CdSO₄·4H₂O), voudourisite (monohydrate), and lazaridisite (the 8/3-hydrate).

Applications

Cadmium sulfate is used widely for the electroplating of cadmium in electronic circuits. It is also a precursor to cadmium-based pigment such as cadmium sulfide. It is also used for electrolyte in a Weston standard cell as well as a pigment in fluorescent screens.

References

^ Lide, David R., ed. (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Press. ISBN 0-8493-0487-3.
^ ^a ^b Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A21. ISBN 978-0-618-94690-7.
^ ^a ^b ^c NIOSH Pocket Guide to Chemical Hazards. "#0087". National Institute for Occupational Safety and Health (NIOSH).
^ Aurivillius, Karin; Stålhandske, Claes (1980). "A Reinvestigation of the Crystal Structures of HgSO₄ and CdSO₄". Zeitschrift für Kristallographie - Crystalline Materials. 153 (1–2): 121–129. Bibcode:1980ZK....153..121A. doi:10.1524/zkri.1980.0011.
^ Theppitak, C.; Chainok, K. (2015). "Crystal Structure of CdSO₄(H₂O): A Redetermination"". Acta Crystallographica Section E. 71 (10): i8–pi9. doi:10.1107/S2056989015016904. PMC 4647421. PMID 26594423.

[1] Lide, David R., ed. (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Press. ISBN 0-8493-0487-3.

[b1-2] Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A21. ISBN 978-0-618-94690-7.

[PGCH-3] NIOSH Pocket Guide to Chemical Hazards. "#0087". National Institute for Occupational Safety and Health (NIOSH).

[4] Aurivillius, Karin; Stålhandske, Claes (1980). "A Reinvestigation of the Crystal Structures of HgSO₄ and CdSO₄". Zeitschrift für Kristallographie - Crystalline Materials. 153 (1–2): 121–129. Bibcode:1980ZK....153..121A. doi:10.1524/zkri.1980.0011.

[5] Theppitak, C.; Chainok, K. (2015). "Crystal Structure of CdSO₄(H₂O): A Redetermination"". Acta Crystallographica Section E. 71 (10): i8–pi9. doi:10.1107/S2056989015016904. PMC 4647421. PMID 26594423.

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