Zinc nitrate

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Zinc nitrate
IUPAC name
Zinc nitrate
Other names
Nitric acid, zinc salt
Zinc(II) nitrate
Zinc dinitrate
Zn(NO3)2 (anhydrous)
Zn(NO3)2·6 H2O (hexahydrate)
Molar mass 189.36 g/mol (anhydrous)
297.49 g/mol (hexahydrate)
Appearance Colorless crystalline solid, hygroscopic
Density 2.065 g/cm3 (hexahydrate)
Melting point 110 °C (230 °F; 383 K) (anhydrous)
45.5 °C (113.9 °F; 318.65 K) (trihydrate)
36.4 °C (97.52 °F; 309.55 K) (hexahydrate)
Boiling point 125 °C (257 °F; 398 K) (decomposes) (hexahydrate)
327 g/100 ml (40 °C)
184.3 g/100 ml (20 °C)
Solubility Soluble in ethanol, methanol
Vapor pressure ~0 mmHg
Safety data sheet Sigma-Aldrich (hydrate)
Flash point Non-flammable
Lethal dose or concentration (LD, LC):
1,400 mg/kg (rat, female, oral)
1,558.7 mg/kg (rat, male, oral)
241.3 mg/kg (mouse ,male, oral)
Related compounds
Related compounds
Cadmium nitrate
Mercury(II) nitrate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Zinc nitrate is a salt of zinc with the formula Zn(NO3)2. Zinc nitrate is highly deliquescent and is typically encountered as a hexahydrate, Zn(NO3)2·6H2O, though a trihydrate is also known.



When heated, zinc nitrate decomposes to give off nitrogen dioxide and oxygen gasses, leaving behind zinc oxide.

Zn(NO3)2 → ZnO + 2 NO2 + ½ O2


Zinc nitrate is an odorless hygroscopic solid, soluble in water and alcohols.


Zinc nitrate is available as Zn+N fertilizer, though not always as pure substance.

Zinc nitrate is sold by chemical suppliers, most of the time as hexahydrate. It can also be purchased on eBay and Amazon.


Zinc nitrate can be produced by dissolving zinc oxide, zinc hydroxide or zinc carbonate in nitric acid.

ZnO + 2 HNO3 → Zn(NO3)2 + H2
Zn(OH)2 + 2 HNO3 → Zn(NO3)2 + 3 H2
ZnCO3 + 2 HNO3 → Zn(NO3)2 + H2 + CO2

If zinc metal is used, diluted nitric acid should be used, as reaction of zinc metal with concentrated nitric acid also produces ammonium nitrate.

Zn + 2 HNO3 (dil.) → Zn(NO3)2 + H2
4 Zn + 10 HNO3 (conc.) → 4 Zn(NO3)2 + NH4NO3 + 3 H2O


  • Make flash powders
  • Make nitrogen dioxide and nitric acid
  • Compound collecting



Zinc nitrate is irritant and a strong oxidizer, though it's hygroscopicity limits its oxidizing power.


Should be stored in closed, air-tight containers, away from flammable materials.


Addition of a soluble carbonate will precipitate zinc carbonate.

Unless contaminated with heavy metals, diluted solutions of zinc nitrate can be used as fertilizer.


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