Chemistry:Zinc nitrate
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| Names | |
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| IUPAC name
Zinc nitrate
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| Other names
Zinc dinitrate
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| Identifiers | |
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3D model (JSmol)
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PubChem CID
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| UNII | |
| UN number | 1514 |
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| Properties | |
| Zn(NO 3) 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 | |
| Main hazards | Oxidant, may explode on heating |
| Safety data sheet | ICSC 1206 |
| GHS pictograms |  
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| Flash point | Non-flammable |
| Related compounds | |
Other anions
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Zinc sulfate Zinc chloride |
Other cations
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Cadmium nitrate Mercury(II) nitrate |
Related compounds
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Copper(II) nitrate |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
 verify (what is   ?)
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| Infobox references | |
Zinc nitrate is an inorganic chemical compound with the formula Zn(NO
3)
2. This colorless, crystalline salt is highly deliquescent. It is typically encountered as a hexahydrate Zn(NO
3)
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 HNO
3 → Zn(NO
3)
2 + H
2 - ZnO + 2 HNO
3 → Zn(NO
3)
2 + H
2O
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]
- ZnCl
2 + 4 NO
2 → Zn(NO
3)
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(NO
3)
2 → 2 ZnO + 4 NO
2 + 1 O
2
Aqueous zinc nitrate contains aquo complexes [Zn(H
2O)
6]2+ and [Zn(H
2O)
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
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:
References
- ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 455. ISBN 978-0-08-037941-8.
- ↑ O. F. Wagenknecht; R. Juza (1963). "Zinc Acetate". in G. Brauer. Handbook of Preparative Inorganic Chemistry, 2nd Ed.. 2. NY, NY: Academic Press. p. 1087.
- ↑ 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.
- ↑ 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. PMID 16961338.
- ↑ "Zinc nitrate uses". Amizara Speciality Chemicals LLP. 10 March 2025. https://amizaraspecialitychemicals.co.in/product/zinc-nitrate/.
| HNO3 | He | ||||||||||||||||
| LiNO3 | Be(NO3)2 | B(NO3)−4 | C | NO−3, 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, Fe(NO3)2 |
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(NO3)3 | Zr(NO3)4 | Nb | Mo | Tc | Ru | Rh | Pd(NO3)2 | AgNO3 | Cd(NO3)2 | In | Sn | Sb(NO3)3 | 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, TlNO3 |
Pb(NO3)2 | Bi(NO3)3 BiO(NO3) |
Po | At | Rn | |
| FrNO3 | Ra(NO3)2 | 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 | Nd(NO3)3 | Pm | Sm | Eu(NO3)3 | Gd(NO3)3 | Tb(NO3)3 | Dy | Ho | Er | Tm | Yb | Lu | |||
| Ac(NO3)3 | Th(NO3)4 | Pa | UO2(NO3)2 | Np | Pu | Am | Cm | Bk | Cf | Es | Fm | Md | No | Lr | |||
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