Chemistry:Cadmium sulfate
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| Names | |
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| IUPAC name
Cadmium(II) sulfate
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| Other names
Sulfuric acid, cadmium salt (1:1),
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| Identifiers | |
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3D model (JSmol)
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| ChEBI |
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| ChemSpider | |
| EC Number |
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| 8295 | |
PubChem CID
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| RTECS number |
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| UNII | |
| UN number | 2570 |
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| Properties | |
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| Molar mass |
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| Appearance | White hygroscopic solid |
| Odor | odorless |
| Density |
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| Melting point |
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| Solubility in methanol | slightly soluble |
| Solubility in ethyl acetate | slightly soluble |
| −59.2×10−6 cm3/mol | |
Refractive index (nD)
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1.565 |
| Viscosity |
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| Structure | |
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| Thermochemistry | |
Std molar
entropy (S |
123 J⋅mol−1·K-1[2] |
Std enthalpy of
formation (ΔfH⦵298) |
−935 kJ⋅mol−1[2] |
| Hazards[4] | |
| Safety data sheet | |
| GHS pictograms |   
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| GHS Signal word | Danger |
| H301, H330, H340, H350, H360, H372, H410 | |
| P201, P202, P260, P264, P270, P271, P273, P280, P284, P301+310+330Script error: No such module "Preview warning".Category:GHS errors, P304+340+310, P308+313, P403+233, P405, P501 | |
| NFPA 704 (fire diamond) | |
Threshold limit value (TLV)
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| Lethal dose or concentration (LD, LC): | |
LD50 (median dose)
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107 mg/kg (oral, rat, analgous compound) |
LC50 (median concentration)
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0.75 mg/L (goldfish, analgous compound) |
| NIOSH (US health exposure limits):Template:Chembox NIOSH (set)/formatPocketGuideLink | |
PEL (Permissible)
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TWA 0.005 mg/m3 (as Cd) |
REL (Recommended)
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TWA 0.005 mg/m3 (as Cd) |
IDLH (Immediate danger)
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9 mg/m3 (as Cd) |
| Related compounds | |
Other anions
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Other cations
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
 verify (what is   ?)
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| Infobox references | |
Cadmium sulfate is the name of a series of related inorganic compounds with the formula CdSO
4 · xH
2O. The most common form is the monohydrate CdSO
4 · H2O, but two other forms are known: the octahydrate (3CdSO
4 · 8H2O) and the anhydrous salt (CdSO
4). All salts are colourless and highly soluble in water.
Preparation
Cadmium sulfate hydrate can be prepared by the reaction of cadmium metal or its oxide or hydroxide with dilute sulfuric acid:[citation needed]
- CdO + H
2SO
4 → CdSO
4 + H
2O - Cd + H
2SO
4 → CdSO
4 + H
2
The anhydrous material can be prepared using sodium persulfate:[citation needed]
- Cd + Na
2S
2O
8 → CdSO
4 + Na
2SO
4
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.[citation needed]
Structure
X-ray crystallography shows that CdSO
4 · 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.[6]
Occurrence
Cadmium sulfates occur as the following rare minerals drobecite (CdSO
4 · 4H2O),[contradictory] voudourisite (monohydrate), and lazaridisite (the octahydrate).[citation needed]
Safety
Cadmium sulfate (along with cadmium and its compounds) are classified as group 1 (human carcinogens) by IARC and have been identified as causing lung and prostate cancer as well as mutagenic effects in humans.[7]
References
- ↑ Lide, David R., ed (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Press. ISBN 0-8493-0487-3.
- ↑ 2.0 2.1 Zumdahl, Steven S. (2009). Chemical Principles 6th Ed.. Houghton Mifflin Company. p. A21. ISBN 978-0-618-94690-7.
- ↑ 3.0 3.1 "Safety Data Sheet - Cadmium Sulfate". ThermoFisher Scientific. 28 December 2021. p. 3. https://www.fishersci.com/store/msds?partNumber=AC447755000&productDescription=CADMIUM+SULFATE+ACS+REA+500GR&vendorId=VN00032119&countryCode=US&language=en.
- ↑ 4.0 4.1 "Safety Data Sheet - Cadmium Sulfate". Sigma-Aldrich. 20 May 2025. https://www.sigmaaldrich.com/US/en/sds/sigald/383082?userType=anonymous.
- ↑ 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. doi:10.1524/zkri.1980.0011. Bibcode: 1980ZK....153..121A.
- ↑ Theppitak, C.; Chainok, K. (2015). "Crystal Structure of CdSO4(H2O): A Redetermination"". Acta Crystallographica Section E 71 (10): i8–pi9. doi:10.1107/S2056989015016904. PMID 26594423.
- ↑ "Cadmium". Beryllium, Cadmium, Mercury, and Exposures in the Glass Manufacturing Industry. Lyon, France: World Health Organization - International Agency for Research on Cancer. February 1993. p. 210. ISBN 92-832-1258-4. https://publications.iarc.who.int/_publications/media/download/1954/ed5ada49ff1536d1474abdb982ee69583dbf1bc2.pdf. Retrieved 21 October 2025.
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