Zinc nitrate
| Names | |
|---|---|
| IUPAC name
Zinc nitrate
| |
| Other names
Celloxan
Nitric acid, zinc salt Zinc(II) nitrate Zinc dinitrate | |
| Properties | |
| 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) |
| trihydrate 327 g/100 ml (40 °C) hexahydrate 184.3 g/100 ml (20 °C) | |
| Solubility | Soluble in ethanol, methanol |
| Vapor pressure | ~0 mmHg |
| Hazards | |
| Safety data sheet | Sigma-Aldrich (hydrate) |
| Flash point | Non-flammable |
| Lethal dose or concentration (LD, LC): | |
| LD50 (Median dose)
|
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.
Contents
Properties
Chemical
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
Physical
Zinc nitrate is an odorless hygroscopic solid, soluble in water and alcohols.
Availability
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.
Preparation
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
Projects
- Make flash powders
- Make nitrogen dioxide and nitric acid
- Compound collecting
Handling
Safety
Zinc nitrate is irritant and a strong oxidizer, though it's hygroscopicity limits its oxidizing power.
Storage
Should be stored in closed, air-tight containers, away from flammable materials.
Disposal
Addition of a soluble carbonate will precipitate zinc carbonate.
Unless contaminated with heavy metals, diluted solutions of zinc nitrate can be used as fertilizer.
