Zinc nitrate

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Zinc nitrate
Zinc nitrate
Dusičnan zinečnatý.JPG
Names
IUPAC name
Zinc nitrate
Identifiers
7779-88-6 YesY
19154-63-3 (tetrahydrate)
10196-18-6 (hexahydrate)
ChemSpider 22926 YesY
EC number 231-943-8
Jmol-3D images Image
PubChem 24518
RTECS number ZH4772000
UN number 1514
Properties
Zn(NO3)2
Molar mass 189.36 g/mol (anhydrous)
297.49 g/mol (hexahydrate)
Appearance colorless, deliquescent crystals
Density 2.065 g/cm3 (hexahydrate)
Melting point 110 °C (230 °F; 383 K) (anhydrous)
45.5 °C (trihydrate)
36.4 °C (hexahydrate)
Boiling point ~ 125 °C (257 °F; 398 K) decomposes (hexahydrate)
327 g/100 mL, 40 °C (trihydrate)
184.3 g/100 ml, 20 °C (hexahydrate)
Solubility very soluble in alcohol
Hazards
MSDS ICSC 1206
Main hazards Oxidant, may explode on heating
EU Index Not listed
Flash point Non-flammable
Related compounds
Other anions
Zinc sulfate
Zinc chloride
Other cations
Cadmium nitrate
Mercury(II) nitrate
Related compounds
Copper(II) nitrate
Except where noted otherwise, data is given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
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Infobox references

Zinc nitrate is an inorganic chemical compound with the formula Zn(NO3)2 . This white, crystalline solid is highly deliquescent and is typically encountered as a hexahydrate Zn(NO3)2•6H2O. It is soluble in both water and alcohol.

Synthesis and reactions[edit]

Zinc nitrate is usually prepared by dissolving zinc in nitric acid, this reaction is concentration dependent, with a reaction in concentrated acid also forming ammonium nitrate:

Zn + 2 HNO3 (diluted) → Zn(NO3)2 + H2
4 Zn + 10 HNO3 (concentrated) → 4 Zn(NO3)2 + NH4NO3 + 3 H2O

On heating, it undergoes thermal decomposition to form zinc oxide, nitrogen dioxide and oxygen.

2 Zn(NO3)2 → 2 ZnO + 4 NO2 + O2

Applications[edit]

Zinc nitrate has no large scale application but is used on a laboratory scale for the synthesis of coordination polymers,[1] its controlled decomposition to zinc oxide has also been used for the generation of various ZnO based structures, including nanowires.[2]

It can be used as a mordant in dyeing. An example reaction gives a precipitate of zinc carbonate:

Zn(NO3)2 + Na2CO3 → ZnCO3 + 2 NaNO3.

References[edit]

  1. ^ Barnett, Sarah A; Champness, Neil R (November 2003). "Structural diversity of building-blocks in coordination framework synthesis—combining M(NO3)2 junctions and bipyridyl ligands". Coordination Chemistry Reviews 246 (1-2): 145–168. doi:10.1016/S0010-8545(03)00121-8. 
  2. ^ Greene, Lori E.; Yuhas, Benjamin D.; Law, Matt; Zitoun, David; Yang, Peidong (September 2006). "Solution-Grown Zinc Oxide Nanowires". Inorganic Chemistry 45 (19): 7535–7543. doi:10.1021/ic0601900. 
Salts and the ester of the Nitrate ion
HNO3 He
LiNO3 Be(NO3)2 B(NO3)4 RONO2 NO3
NH4NO3
O 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)3 Co(NO3)2,
Co(NO3)3
Ni(NO3)2 Cu(NO3)2 Zn(NO3)2 Ga(NO3)3 Ge As Se Br Kr
RbNO3 Sr(NO3)2 Y Zr(NO3)4 Nb Mo Tc Ru Rh Pd(NO3)2 AgNO3 Cd(NO3)2 In Sn Sb Te I XeFNO3
CsNO3 Ba(NO3)2   Hf Ta W Re Os Ir Pt Au Hg2(NO3)2,
Hg(NO3)2
Tl(NO3)3 Pb(NO3)2 Bi(NO3)3 Po At Rn
Fr Ra   Rf Db Sg Bh Hs Mt Ds Rg Cn Uut Fl Uup Lv Uus Uuo
La Ce(NO3)x Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
Ac Th Pa UO2(NO3)2 Np Pu Am Cm Bk Cf Es Fm Md No Lr