Cadmium nitrate

Cadmium nitrate describes any of the related members of a family of inorganic compounds with the general formula , the most commonly encountered form being the tetrahydrate. The anhydrous form is volatile, but the others are colourless crystalline solids that are deliquescent, tending to absorb enough moisture from the air to form an aqueous solution. Like other cadmium compounds, cadmium nitrate is known to be carcinogenic.

Cadmium nitrate
Names
IUPAC name
Cadmium(II) nitrate
Other names
Nitric acid, cadmium salt
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
ECHA InfoCard 100.030.633
EC Number
  • 233-710-6
UNII
UN number 3087, 2570
Properties
Cd(NO3)2
Molar mass 236,42
Appearance White crystals, hygroscopic
Odor Odorless
Density 3.6 g/cm3 (anhydrous)
2.45 g/cm3 (tetrahdyrate)[1]
Melting point 360 °C (680 °F; 633 K)
at 760 mmHg (anhydrous)
59.5 °C (139.1 °F; 332.6 K)
at 760 mmHg (tetrahydrate)[1]
Boiling point 132 °C (270 °F; 405 K)
at 760 mmHg (tetrahydrate)[2]
109.7 g/100 mL (0 °C)
126.6 g/100 mL (18 °C)
139.8 g/100 mL (30 °C)
320.9 g/100 mL (59.5 °C)[3]
Solubility Soluble in acids, ammonia, alcohols, ether, acetone
5 g/L in methanol
−5.51·10−5 cm3/mol (anhydrous)
−1.4·10−4 cm3/mol (tetrahydrate)[1]
Structure
Cubic (anhydrous)
Orthorhombic (tetrahydrate)[1]
Fdd2, No. 43 (tetrahydrate)[4]
mm2 (tetrahydrate)[4]
α = 90°, β = 90°, γ = 90°
Hazards
GHS pictograms [5]
GHS Signal word Danger
H301, H330, H340, H350, H360, H372, H410[5]
P201, P260, P273, P284, P301+310, P310[5]
NFPA 704 (fire diamond)
Lethal dose or concentration (LD, LC):
300 mg/kg (rats, oral)[2]
NIOSH (US health exposure limits):
PEL (Permissible)
 [1910.1027] TWA 0.005 mg/m3 (as Cd)[6]
REL (Recommended)
 Ca[6]
IDLH (Immediate danger)
 Ca [9 mg/m3 (as Cd)][6]
Related compounds
Other anions
 Cadmium acetate
Cadmium chloride
Cadmium sulfate
Other cations
 Zinc nitrate
Calcium nitrate
Magnesium nitrate
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

Uses

Cadmium nitrate is used for coloring glass and porcelain[7] and as a flash powder in photography.

Preparation

Cadmium nitrate is prepared by dissolving cadmium metal or its oxide, hydroxide, or carbonate, in nitric acid followed by crystallization:

CdO + 2HNO3 → Cd(NO3)2 + H2O
CdCO3 + 2 HNO3 → Cd(NO3)2 + CO2 + H2O
Cd + 4 HNO3 → 2 NO2 + 2 H2O + Cd(NO3)2

Reactions

Thermal dissociation at elevated temperatures produces cadmium oxide and oxides of nitrogen. When hydrogen sulfide is passed through an acidified solution of cadmium nitrate, yellow cadmium sulfide is formed. A red modification of the sulfide is formed under boiling conditions.

When with caustic soda solution, cadmium oxide forms precipitate of cadmium hydroxide. Many insoluble cadmium salts are obtained by such precipitation reactions.

References
  1. Lide, David R., ed. (2009). CRC Handbook of Chemistry and Physics (90th ed.). Boca Raton, Florida: CRC Press. ISBN 978-1-4200-9084-0.
  2. "MSDS of Cadmium nitrate tetrahydrate". www.fishersci.ca. Fisher Scientific. Retrieved 2014-06-25.
  3. Seidell, Atherton; Linke, William F. (1919). Solubilities of Inorganic and Organic Compounds (2nd ed.). New York: D. Van Nostrand Company. p. 178.
  4. James, D. W.; Carrick, M. T.; Leong, W. H. (1978). "Raman spectrum of cadmium nitrate". Australian Journal of Chemistry. 31 (6): 1189. doi:10.1071/CH9781189.
  5. Sigma-Aldrich Co., Cadmium nitrate tetrahydrate. Retrieved on 2014-06-25.
  6. NIOSH Pocket Guide to Chemical Hazards. "#0087". National Institute for Occupational Safety and Health (NIOSH).
  7. Karl-Heinz Schulte-Schrepping, Magnus Piscator "Cadmium and Cadmium Compounds" in Ullmann's Encyclopedia of Industrial Chemistry, 2007 Wiley-VCH, Weinheim. doi:10.1002/14356007.a04_499.
Salts and covalent derivatives of the nitrate ion
HNO3 He
LiNO3 Be(NO3)2 B(NO
3)−
4		 RONO2 NO−
3
NH4NO3		 HOONO2 FNO3 Ne
NaNO3 Mg(NO3)2 Al(NO3)3 Si P S ClONO2 Ar
KNO3 Ca(NO3)2 Sc(NO3)3 Ti(NO3)4 VO(NO3)3 Cr(NO3)3 Mn(NO3)2 Fe(NO3)2
Fe(NO3)3		 Co(NO3)2
Co(NO3)3		 Ni(NO3)2 CuNO3
Cu(NO3)2		 Zn(NO3)2 Ga(NO3)3 Ge As Se Br Kr
RbNO3 Sr(NO3)2 Y(NO3)3 Zr(NO3)4 Nb Mo Tc Ru(NO3)3 Rh(NO3)3 Pd(NO3)2
Pd(NO3)4		 AgNO3
Ag(NO3)2		 Cd(NO3)2 In(NO3)3 Sn Sb(NO3)3 Te INO3 Xe(NO3)2
CsNO3 Ba(NO3)2   Hf(NO3)4 Ta W Re Os Ir Pt(NO3)2
Pt(NO3)4		 Au(NO3)3 Hg2(NO3)2
Hg(NO3)2		 TlNO3
Tl(NO3)3		 Pb(NO3)2 Bi(NO3)3
BiO(NO3)		 Po(NO3)4 At Rn
FrNO3 Ra(NO3)2   Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og
↓
La(NO3)3 Ce(NO3)3
Ce(NO3)4		 Pr(NO3)3 Nd(NO3)3 Pm(NO3)3 Sm(NO3)3 Eu(NO3)3 Gd(NO3)3 Tb(NO3)3 Dy(NO3)3 Ho(NO3)3 Er(NO3)3 Tm(NO3)3 Yb(NO3)3 Lu(NO3)3
Ac(NO3)3 Th(NO3)4 PaO2(NO3)3 UO2(NO3)2 Np(NO3)4 Pu(NO3)4 Am(NO3)3 Cm(NO3)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.