Zinc nitrate

Zinc nitrate  Zinc nitrate

Names
IUPAC name

Zinc nitrate

Other names

Zinc dinitrate

Identifiers

CAS Number

* 7779-88-6 Y
* 19154-63-3 (tetrahydrate) N
* 10196-18-6 (hexahydrate) N

3D model (JSmol)

* Interactive image

ChEBI |

* CHEBI:231504

ChemSpider |

* 22926 Y

ECHA InfoCard | 100.029.038
EC Number |

* 231-943-8

PubChem CID

* 24518

RTECS number |

* ZH4772000

UNII |

* EDO66F5U49 Y

UN number | 1514

CompTox Dashboard (EPA)

* DTXSID10890636

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

Magnetic susceptibility (χ)

| −63.0·10−6 cm3/mol
Hazards
Occupational safety and health (OHS/OSH):

Main hazards

| Oxidant, may explode on heating
GHS labelling:

Pictograms

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).

N verify (what is YN ?)

Infobox references

Chemical compound

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

[edit]

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

[edit]

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

Aqueous zinc nitrate contains aquo complexes [Zn(H2O)6]2+ and [Zn(H2O)4]2+.[3] and, thus, this reaction may be better written as the reaction of the aquated ion with hydroxide through donation of a proton, as follows.

## Applications

[edit]

Zinc nitrate has no large scale application but is used on a laboratory scale for the synthesis of coordination polymers.[4] Its controlled decomposition to zinc oxide has also been used for the generation of various ZnO based structures, including nanowires.[5]

It is used as a corrosion inhibitor. [6]

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. ^ 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. ^ Sze, Yu-Keung, and Donald E. Irish. "Vibrational spectral studies of ion-ion and ion-solvent interactions. I. Zinc nitrate in water." Journal of Solution Chemistry 7.6 (1978): 395-415.
4. ^ 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)00121-8.1–2&rft.pages=145-168&rft.date=2003-11&rft_id=info:doi/10.1016/S0010-8545(03)00121-8&rft.aulast=Barnett&rft.aufirst=Sarah+A&rft.au=Champness,+Neil+R&rfr_id=info:sid/en.wikipedia.org:Zinc+nitrate" class="Z3988">
5. ^ 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.
6. ^ "Zinc nitrate uses". Amizara Speciality Chemicals LLP. 10 March 2025.

* v
* t
* e

Zinc compounds

Zinc(I)|

| Organozinc(I) compounds|

* Zn2(C5(CH3)5)2

|

Zinc(II)|

* Zn(acac)2
* Zn(N3)2
* ZnBr2
* ZnCO3
* Zn(CN)2
* ZnCl2
* Zn(ClO3)2
* ZnCrO4
* ZnF2
* ZnH2
* ZnI2
* ZnMoO4
* Zn(NO3)2
* ZnO
* ZnO2
* Zn(ClO

* Zn(OH)2
* ZnS
* ZnSO4
* ZnSe
* ZnTe
* Zn2P2O7
* Zn3Sb2
* Zn3As2
* Zn3N2
* Zn3P2
* ZnP2
* Zn3(PO4)2

| Organozinc(II) compounds|

* Zn(CH3)2
* Zn(C2H5)2
* Zn(CH3COO)2
* Zn(CH(CH3)2)2
* Zn(C(CH3)3)2
* Zn(C6H5)2
* Zn(C3H5O3)2
* ZnICH2I
* C
24H
46ZnO

|

* v
* t
* e

Salts and covalent derivatives of the nitrate ion

| HNO3 |  |  |  | He

|
|
|
|

LiNO3 | Be(NO3)2 | B(NO3)−4 | RONO2
+CO3
+C2O4 | NO3−
NH4NO3 | HOONO2 | FNO3
+F | Ne
NaNO3 | Mg(NO3)2 | Al(NO3)3
Al(NO3)−4 | Si  | P  | +SO4 | ClONO2
+Cl | 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  | +SeO3 | BrNO3
+Br | Kr
RbNO3 | Sr(NO3)2 |  | Y(NO3)3 | Zr(NO3)4 | NbO(NO3)3 | MoO2(NO3)2 | Tc  | Ru  | Rh(NO3)3 | Pd(NO3)2 | AgNO3 | Cd(NO3)2 | In(NO3)3 | Sn(NO3)4 | Sb4O4(OH)2(NO3)2 | Te  | INO3
+IO3 | Xe(NO3)2
CsNO3 | Ba(NO3)2 | *  | Lu(NO3)3 | Hf(NO3)4 | TaO(NO3)3 | WO2(NO3)2 | ReO3NO3 | Os  | Ir3O(NO3)10 | Pt  | Au(NO3)−4 | 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 | **  | Lr  | 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
**  | Ac(NO3)3 | Th(NO3)4 | PaO(NO3)3 | UO2(NO3)2 | Np(NO3)4 | Pu(NO3)4 | Am(NO3)3 | Cm(NO3)3 | Bk(NO3)3 | Cf(NO3)3 | Es  | Fm  | Md  | No
*[CID]: Compound ID
*[EPA]: U.S. Environmental Protection Agency
*[v]: View this template
*[t]: Discuss this template
*[e]: Edit this template