Calcium nitrate
chemical compound
Calcium nitrate, also known as Norwegian saltpeter, is a chemical compound. Its chemical formula is Ca(NO3)2. It contains calcium and nitrate ions.
| Names | ||
|---|---|---|
| Other names Kalksalpeter, nitrocalcite, Norwegian saltpeter, lime nitrate | ||
| Identifiers | ||
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3D model (JSmol) | ||
| ChemSpider | ||
| ECHA InfoCard | 100.030.289 | |
PubChem CID | ||
| RTECS number |
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| UNII | ||
| UN number | 1454 | |
CompTox Dashboard (EPA) | ||
SMILES
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| Properties | ||
| Ca(NO3)2 | ||
| Molar mass | 164.088 g/mol (anhydrous) 236.15 g/mol (tetrahydrate) | |
| Appearance | colorless solid hygroscopic | |
| Density | 2.504 g/cm3 (anhydrous) 1.896 g/cm3 (tetrahydrate) | |
| Melting point | 561 °C (1,042 °F; 834 K) (anhydrous) 42.7 °C (109 °F; 316 K) (tetrahydrate) | |
| Boiling point | decomposes (anhydrous) 132 °C (270 °F; 405 K) (tetrahydrate) | |
| anhydrous: 1212 g/L (20 °C) 2710 g/L (40 °C) tetrahydrate: 1050 g/L (0 °C) 1290 g/L (20 °C) 3630 g/L (100 °C) | ||
| Solubility | soluble in ammonia almost insoluble in nitric acid | |
| Solubility in ethanol | 51.4 g/100 g (20 °C) 62.9 g/100 g (40 °C)[1] | |
| Solubility in methanol | 134 g/100 g (10 °C) 144 g/100 g (40 °C) 158 g/100 g (60 °C)[1] | |
| Solubility in acetone | 16.8 g/kg (20 °C)[1] | |
| Acidity (pKa) | 6.0 | |
| -45.9·10−6 cm3/mol | ||
| Structure | ||
| cubic (anhydrous) monoclinic (tetrahydrate) | ||
| Hazards | ||
| NFPA 704 |
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| R-phrases | R22, R41 | |
| Flash point | Non-flammable | |
| Related compounds | ||
| Other anions | Calcium sulfate Calcium chloride | |
| Other cations | Magnesium nitrate Strontium nitrate Barium nitrate | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | ||
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| Infobox references | ||
Properties
Calcium nitrate is a colorless solid. It is an oxidizing agent. It absorbs water from the air. It decomposes to make nitrogen dioxide and calcium oxide when heated.
Preparation
Calcium nitrate is made by reacting calcium hydroxide or calcium carbonate with nitric acid. It is made when nitric acid reacts with calcium phosphate. It can be made by reacting ammonium nitrate and calcium hydroxide.
Uses
Calcium nitrate is used in fertilizers to add nitrogen to the soil. It can be complexed with urea to make a different nitrogen fertilizer.
References
Related pages
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