Zinc nitrate
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| UN number | 1514 |
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| Template:Longitem | Template:Chem2 |
| Molar mass | 189.36 g/mol (anhydrous) 297.49 g/mol (hexahydrate) |
| Appearance | colorless, deliquescent crystals |
| Density | 2.065 g/cm3 (hexahydrate) |
| Melting point | Template:Chembox CalcTemperatures |
| Boiling point | Template:Chembox CalcTemperatures |
| Solubility | very soluble in alcohol |
| Template:Longitem | −63.0·10−6 cm3/mol |
| Flash point | Template:Chembox CalcTemperatures |
| Template:Longitem | Zinc sulfate Zinc chloride |
| Template:Longitem | Cadmium nitrate Mercury(II) nitrate |
| Template:Longitem | Copper(II) nitrate |
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Zinc nitrate is an inorganic chemical compound with the formula Template:Chem2. This colorless, crystalline salt is highly deliquescent. It is typically encountered as a hexahydrate Template:Chem2. 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:
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]
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:
Aqueous zinc nitrate contains aquo complexes Template:Chem2.[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
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- ↑ 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.
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