Cadmium sulfate

Cadmium sulfate is the name of a series of related inorganic compounds with the formula CdSO4·xH2O. 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.

Cadmium sulfate
Names
IUPAC name
Cadmium(II) sulfate
Other names
Sulfuric acid, cadmium salt (1:1),
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
ECHA InfoCard 100.030.288
EC Number
  • 233-331-6
8295
RTECS number
  • EV2700000
UNII
UN number 2570
Properties
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 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)
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
-59.2·10−6 cm3/mol
1.565
Structure
orthorhombic (anhydrous)
monoclinic (hepta & octahydrate)
Thermochemistry
123 J·mol−1·K−1[2]
−935 kJ·mol−1[2]
Hazards
Safety data sheet
GHS pictograms
GHS Signal word Danger
H301, H330, H340, H350, H360, H372, H400, H410
P201, P202, P260, P264, P270, P271, P273, P281, P284, P301+310, P304+340, P308+313, P310, P314, P320, P321, P330, P391, P403+233, P405, P501
NFPA 704 (fire diamond)
Flammability code 1: Must be pre-heated before ignition can occur. Flash point over 93 °C (200 °F). E.g. canola oilHealth code 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasReactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
1
3
0
Lethal dose or concentration (LD, LC):
280 mg/kg (oral, rat)
NIOSH (US health exposure limits):
PEL (Permissible)
 [1910.1027] TWA 0.005 mg/m3 (as Cd)[3]
REL (Recommended)
 Ca[3]
IDLH (Immediate danger)
 Ca [9 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 otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is YN ?)
Infobox references

Structure, preparation, and occurrence

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.[4]

Cadmium sulfate octohydrate 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 is prepared using sodium persulfate:

Cd + Na2S2O8 → CdSO4 + Na2SO4

Pure cadmium sulfate occurs as very 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
  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. Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A21. ISBN 978-0-618-94690-7.
  3. NIOSH Pocket Guide to Chemical Hazards. "#0087". National Institute for Occupational Safety and Health (NIOSH).
  4. Theppitak, C/; Chainok, K. "Crystal structure of CdSO4(H2O): A Redetermination" Acta Crystallographica, Section E. Structure Reports Online 2015, volume 71, pi8-pi9. doi:10.1107/S2056989015016904
Compounds containing the sulfate group (SO2−
4)
H2SO4 He
Li2SO4 BeSO4 B2S2O9 esters
ROSO3−
(RO)2SO2		 (NH4)2SO4
[N2H5]HSO4
(NH3OH)2SO4
NOHSO4		 HOSO4 F Ne
Na2SO4
NaHSO4		 MgSO4 Al2(SO4)3
Al2SO4(OAc)4		 Si P SO42−
HSO3HSO4
(HSO4)2		 Cl Ar
K2SO4
KHSO4		 CaSO4 Sc2(SO4)3 TiOSO4 VSO4
V2(SO4)3
VOSO4		 CrSO4
Cr2(SO4)3		 MnSO4 FeSO4
Fe2(SO4)3		 CoSO4
Co2(SO4)3		 NiSO4
Ni2(SO4)3		 CuSO4
Cu2SO4
[Cu(NH3)4(H2O)]SO4		 ZnSO4 Ga2(SO4)3 Ge As Se Br Kr
RbHSO4
Rb2SO4		 SrSO4 Y2(SO4)3 Zr(SO4)2 Nb MoSO4
Mo2(SO4)3
Mo(SO4)2
Mo(SO4)2
Mo(SO4)3		 Tc Ru(SO4)2 RhSO4
Rh2(SO4)3		 PdSO4 Ag2SO4
AgSO4		 CdSO4 In2(SO4)3 SnSO4
Sn(SO4)2		 Sb2(SO4)3 Te I Xe
Cs2SO4
CsHSO4		 BaSO4   Hf Ta W Re OsSO4
Os2(SO4)3
Os(SO4)2		 IrSO4
Ir2(SO4)3		 PtSO4
Pt(SO4)2		 AuSO4
Au2(SO4)3		 Hg2SO4
HgSO4		 Tl2SO4
Tl2(SO4)3		 PbSO4
Pb(SO4)2		 Bi2(SO4)3 PoSO4
Po(SO4)2		 At Rn
Fr Ra   Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og
↓
La2(SO4)3 Ce2(SO4)3
Ce(SO4)2		 Pr2(SO4)3 Nd2(SO4)3 Pm2(SO4)3 Sm2(SO4)3 Eu2(SO4)3 Gd2(SO4)3 Tb2(SO4)3 Dy2(SO4)3 Ho2(SO4)3 Er2(SO4)3 Tm2(SO4)3 Yb2(SO4)3 Lu2(SO4)3
Ac2(SO4)3 Th(SO4)2 Pa U2(SO4)3
U(SO4)2
UO2SO4		 Np(SO4)2 Pu(SO4)2 Am2(SO4)3 Cm2(SO4)3 Bk Cf Es Fm Md No Lr
This article is issued from Wikipedia. The text is licensed under Creative Commons - Attribution - Sharealike. Additional terms may apply for the media files.