Cadmium sulfate

From Wikipedia, the free encyclopedia
Jump to navigation Jump to search
Cadmium sulfate
IUPAC name Cadmium(II) sulfate
Other names Sulfuric acid, cadmium salt (1:1),
CAS number 10124-36-4
PubChem 24962
EC number 233-331-6
RTECS number EV2700000
SMILES [Cd+2].[O-]S([O-])(=O)=O
Gmelin Reference 8295
Molecular 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)[1]
Melting point

1000 °C, 1273 K, 1832 °F

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)
76.7 g/100 mL (25 °C)
very soluble
Solubility slightly soluble in methanol, ethyl acetate
insoluble in ethanol
-59.2·10−6 cm3/mol
Refractive index (nD) 1.565
Crystal structure orthorhombic (anhydrous)
monoclinic (hepta & octahydrate)
Std enthalpy of
−935 kJ·mol−1[2]
Standard molar
123 J·mol−1·K−1[2]
NFPA 704

NFPA 704.svg

U.S. Permissible
exposure limit (PEL)
[1910.1027] TWA 0.005 mg/m3 (as Cd)[3]
Related compounds
Other anions Cadmium acetate,
Cadmium chloride,
Cadmium nitrate
Other cations Zinc sulfate,
Calcium sulfate,
Magnesium sulfate
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)

Cadmium sulfate is a chemical compound. Its chemical formula is CdSO4. It is made of cadmium and sulfate ions. The cadmium is in its +2 oxidation state.

Properties[change | change source]

Cadmium sulfate is a white solid. It easily dissolves in water. It is toxic and carcinogenic.

Preparation[change | change source]

Cadmium sulfate is made by dissolving cadmium carbonate, cadmium oxide, or cadmium metal in sulfuric acid.

Uses[change | change source]

Cadmium sulfate is used to electroplate cadmium on electronic circuits. It is also used to make cadmium sulfide, a pigment. It is used as an electrolyte in a certain battery used to make voltmeters accurate.

Related pages[change | change source]

References[change | change source]

  1. Lide, David R., ed. (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Press. ISBN 0-8493-0487-3.
  2. 2.0 2.1 Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A21. ISBN 0-618-94690-X.
  3. 3.0 3.1 "NIOSH Pocket Guide to Chemical Hazards #0087". National Institute for Occupational Safety and Health (NIOSH).