Zinc nitrate

Zinc nitrate
Names
	IUPAC name Zinc nitrate
	Other names Zinc dinitrate
Identifiers
CAS Number	7779-88-6 ; 19154-63-3 (tetrahydrate) ; 10196-18-6 (hexahydrate) ;
3D model (JSmol)	Interactive image;
ChemSpider	22926 ;
ECHA InfoCard	100.029.039
EC Number	231-943-8;
PubChem CID	24518;
RTECS number	ZH4772000;
UNII	EDO66F5U49 ;
UN number	1514
CompTox Dashboard (EPA)	DTXSID10890636 ;
	InChI InChI=1S/2NO3.Zn/c22-1(3)4;/q2-1;+2 Key: ONDPHDOFVYQSGI-UHFFFAOYSA-N ; InChI=1/2NO3.Zn/c22-1(3)4;/q2-1;+2 Key: ONDPHDOFVYQSGI-UHFFFAOYAQ;
	SMILES [N+](=O)([O-])[O-].[N+](=O)([O-])[O-].[Zn+2];
Properties
Chemical formula	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)
Solubility in water	327 g/100 mL, 40 °C (trihydrate) ; 184.3 g/100 mL, 20 °C (hexahydrate)
Solubility	very soluble in alcohol
Magnetic susceptibility (χ)	−63.0·10−6 cm3/mol
Hazards
Main hazards	Oxidant, may explode on heating
Safety data sheet (SDS)	ICSC 1206
	GHS labelling:
Pictograms
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 otherwise noted, data are 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 salt 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[]

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 + H₂O

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[]

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[]

^ 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.
^ 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.