Zinc nitrate

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Zinc nitrate
Zinc nitrate
Names
IUPAC name
Zinc nitrate
Other names
Zinc dinitrate
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.029.038 Edit this at Wikidata
EC Number
  • 231-943-8
RTECS number
  • ZH4772000
UNII
UN number 1514
  • InChI=1S/2NO3.Zn/c2*2-1(3)4;/q2*-1;+2 checkY
    Key: ONDPHDOFVYQSGI-UHFFFAOYSA-N checkY
  • InChI=1/2NO3.Zn/c2*2-1(3)4;/q2*-1;+2
    Key: ONDPHDOFVYQSGI-UHFFFAOYAQ
  • [N+](=O)([O-])[O-].[N+](=O)([O-])[O-].[Zn+2]
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
−63.0·10−6 cm3/mol
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 Oxidant, may explode on heating
GHS labelling:
GHS03: OxidizingGHS07: Exclamation mark
Flash point Non-flammable
Safety data sheet (SDS) ICSC 1206
Related compounds
Other anions
 Zinc sulfate
Zinc chloride
Other cations
 Cadmium nitrate
Mercury(II) nitrate
Related compounds
 Copper(II) nitrate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Zinc nitrate is an inorganic chemical compound with the formula Zn(NO3)2. This colorless, crystalline salt is highly deliquescent. It is typically encountered as a hexahydrate Zn(NO3)2·6H2O. It is soluble in both water and alcohol.

Synthesis

Zinc nitrate is usually prepared by dissolving zinc metal, zinc oxide, or related materials in nitric acid:

Zn + 2 HNO3 → Zn(NO3)2 + H2
ZnO + 2 HNO3 → Zn(NO3)2 + H2O

These reactions are accompanied by the hydration of the zinc nitrate.

The anhydrous salt arises by the reaction of anhydrous zinc chloride with nitrogen dioxide:[1]

ZnCl2 + 4 NO2 → Zn(NO3)2 + 2 NOCl

Reactions

Treatment of zinc nitrate with acetic anhydride gives zinc acetate.[2]

On heating, zinc nitrate undergoes thermal decomposition to form zinc oxide, nitrogen dioxide and oxygen:

2 Zn(NO3)2 → 2 ZnO + 4 NO2 + 1 O2

Applications

Zinc nitrate has no large scale application but is used on a laboratory scale for the synthesis of coordination polymers.[3] Its controlled decomposition to zinc oxide has also been used for the generation of various ZnO based structures, including nanowires.[4]

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

  1. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 455. ISBN 978-0-08-037941-8.
  2. ^ O. F. Wagenknecht; R. Juza (1963). "Zinc Acetate". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. Vol. 2. NY, NY: Academic Press. p. 1087.
  3. ^ 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.
  4. ^ 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. PMID 16961338.


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