Zinc nitrate

Zinc nitrate

Zinc nitrate
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Names
IUPAC name Zinc nitrate
Identifiers
CAS Number	7779-88-6 Y 19154-63-3 (tetrahydrate) N 10196-18-6 (hexahydrate) N
ChemSpider	22926 Y
EC Number	231-943-8
Jmol 3D model	Interactive image
PubChem	24518
RTECS number	ZH4772000
UN number	1514
InChI InChI=1S/2NO3.Zn/c2*2-1(3)4;/q2*-1;+2 Y Key: ONDPHDOFVYQSGI-UHFFFAOYSA-N Y InChI=1/2NO3.Zn/c2*2-1(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
Vapor pressure	{{{value}}}
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).
N verify (what is YN ?)
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

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

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

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

Salts and covalent derivatives of the Nitrate ion
HNO3																	He
LiNO3	Be(NO3)2											B(NO3)4−	C	N	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	Xe(NO3)2
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)3, Ce(NO3)4	Pr	Nd	Pm	Sm	Eu	Gd(NO3)3	Tb	Dy	Ho	Er	Tm	Yb	Lu
		Ac	Th	Pa	UO2(NO3)2	Np	Pu	Am	Cm	Bk	Cf	Es	Fm	Md	No	Lr