Calcium nitrate is a chemical compound with the formula Ca(NO3)2. It is a colorless and odorless solid that is highly soluble in water. Calcium nitrate is commonly used as a fertilizer and in wastewater treatment. It is also used in the production of concrete, as a component of explosives, and in the manufacture of various other chemicals.
| IUPAC Name | Calcium dinitrate |
| Molecular Formula | Ca(NO3)2 |
| CAS Number | 10124-37-5 |
| Synonyms | Calcium nitrate tetrahydrate, Nitric acid calcium salt, Nitrocalcite, Norwegian saltpeter, Lime saltpeter, Norgessalpeter |
| InChI | InChI=1S/Ca.2NO3/c;22-1(3)4/q+2;2-1 |
Calcium Nitrate Formula
The formula for calcium nitrate is Ca(NO3)2. This means that each unit of calcium nitrate contains one calcium ion (Ca²⁺) and two nitrate ions (NO3⁻). The formula for calcium nitrate is often used to determine the molar mass and other properties of the compound.
Calcium Nitrate Molar Mass
Calcium nitrate has a molar mass of 164.088 g/mol. It is a salt composed of Ca+2 and NO3- ions, with the formula, Ca(NO3)2. The molar mass of a compound is the mass in grams of one mole of that compound, which is equal to its formula weight. In the case of Ca(NO3)2, the formula weight is the sum of the atomic weights of all the atoms in the compound.
Calcium Nitrate Boiling Point
Ca(NO3)2 has a relatively high boiling point of 132 degrees Celsius. This means that it requires a significant amount of energy to convert the solid compound into a gas. The high boiling point of Ca(NO3)2 is due to its ionic nature, which results in strong electrostatic interactions between the Ca+2 and NO3- ions.
Calcium Nitrate Melting Point
The melting point of Ca(NO3)2 is 561 degrees Celsius. This is relatively high for a salt, and once again reflects the strong ionic interactions between the Ca+2 and NO3- ions. The melting point of Ca(NO3)2 makes it a useful compound for high-temperature applications, such as in the manufacture of fertilizers or explosives.
Calcium Nitrate Density g/ml
The density of Ca(NO3)2 varies depending on its form. For example, the density of anhydrous Ca(NO3)2 is approximately 2.5 g/cm³, while the density of the tetrahydrate (Ca(NO3)2·4H2O) is about 1.82 g/cm³. These values make Ca(NO3)2 a relatively dense compound compared to many other salts.
Calcium Nitrate Molecular Weight
The molecular weight of Ca(NO3)2 is 164.088 g/mol. This value is the sum of the atomic weights of all the atoms in the compound, which includes two nitrogen atoms, six oxygen atoms, and one calcium atom.
Calcium Nitrate Structure
Ca(NO3)2 has an ionic structure, with the calcium ion (Ca²⁺) surrounded by six oxygen atoms in an octahedral arrangement. The NO3- ion is also present in the crystal lattice, with each oxygen atom of the NO3- ion forming a coordinate bond with the Ca+2 ion. The structure of Ca(NO3)2 is similar to that of other ionic compounds, such as sodium chloride.
| Appearance | White crystals or powder |
| Specific Gravity | 2.5 (anhydrous); 1.82 (tetrahydrate) |
| Color | Colorless (anhydrous); White (tetrahydrate) |
| Odor | Odorless |
| Molar Mass | 164.088 g/mol |
| Density | 2.5 g/cm³ (anhydrous); 1.82 g/cm³ (tetrahydrate) |
| Melting Point | 561 °C (anhydrous); 45 °C (tetrahydrate) |
| Boiling Point | 132 °C (decomposes) |
| Flash Point | Not applicable |
| Water Solubility | 121.2 g/100 mL (0 °C); 126.7 g/100 mL (20 °C); 179.6 g/100 mL (100 °C) |
| Solubility | Soluble in water, ethanol, methanol |
| Vapor Pressure | Negligible (anhydrous) |
| Vapor Density | Not applicable |
| pKa | Not applicable |
| pH | 4.5-7.5 (10% solution) |
Calcium Nitrate Safety and Hazards
Calcium nitrate (Ca(NO3)2) may pose several hazards if not handled properly. It is a strong oxidizing agent and can cause fire or explosion if it comes in contact with combustible materials. The compound can also cause skin and eye irritation upon contact, and inhalation of dust can cause respiratory irritation. Ca(NO3)2 should be stored in a cool, dry place away from sources of heat and should not be mixed with other chemicals without proper precautions. Personal protective equipment such as gloves and eye protection should be worn when handling Ca(NO3)2 to avoid contact with the skin or eyes. In case of accidental ingestion, medical attention should be sought immediately.
| Hazard Symbols | Oxidizing Agent (GHS05), Irritant (GHS07) |
| Safety Description | S22: Do not breathe dust/fume/gas/mist/vapours/spray. S26: In case of contact with eyes, rinse immediately with plenty of water and seek medical advice. S36/37/39: Wear suitable protective clothing, gloves and eye/face protection. |
| UN Ids | UN1454 (Calcium nitrate, anhydrous), UN1455 (Calcium nitrate tetrahydrate) |
| HS Code | 283429 |
| Hazard Class | 5.1 (Oxidizing agents) |
| Packing Group | III |
| Toxicity | Oral (LD50): 3,420 mg/kg (rat); Dermal (LD50): >5,000 mg/kg (rabbit); Inhalation (LC50): >4.8 mg/l/4h (rat) |
Calcium Nitrate Synthesis Methods
Various methods exist for synthesizing Ca(NO3)2 based on the specific application and desired purity.
One common method involves reacting calcium carbonate with nitric acid to produce Ca(NO3)2 and carbon dioxide:
CaCO3 + 2HNO3 → Ca(NO3)2 + CO2 + H2O
Another method involves reacting calcium hydroxide with nitric acid:
Ca(OH)2 + 2HNO3 → Ca(NO3)2 + 2H2O
The reaction between nitric acid and calcium oxide yields Ca(NO3)2:
CaO + 2HNO3 → Ca(NO3)2 + H2O
The resulting Ca(NO3)2 can be further purified by recrystallization or by adding a small amount of sulfuric acid to remove impurities such as iron and aluminum.
Manufacturers can produce Ca(NO3)2 by reacting calcium metal with nitric acid or by reacting calcium hydroxide with ammonium nitrate. However, they use these methods less commonly due to the higher cost or safety concerns associated with reactive metals or ammonium nitrate.
Calcium Nitrate Uses
- Used as a fertilizer in agriculture to provide plants with calcium and nitrogen nutrients for growth.
- Used as a component in several types of concrete and cement to improve their strength and durability.
- Used as an additive in the production of wastewater treatment chemicals to help remove phosphorus and nitrogen compounds from the water.
- Used in the production of several types of explosives and fireworks due to its oxidizing properties.
- Used as a source of calcium and nitrogen in the production of various chemicals such as nylon and other synthetic fibers.
- Used as a corrosion inhibitor for metals such as aluminum and steel in industrial applications.
- Used in the preservation of meats and as a food additive to improve the quality of certain food products.
- Used in the production of smoke bombs and signal flares for military and civilian applications.
- Used in the manufacturing of some fertilizers. Also used in combination with other compounds to provide a balanced nutrient supply for crops.
- Used as a component in some specialized aquarium fertilizers to provide essential nutrients to aquatic plants.
Questions:
Q: What is the name of Ca(NO3)2?
A: The name of Ca(NO3)2 is calcium nitrate.
Q: Is Ca(NO3)2 soluble in water?
A: Yes, Ca(NO3)2 is highly soluble in water. At room temperature, 100 grams of water can dissolve up to 121 grams of calcium nitrate.
Q: Where to buy calcium nitrate?
A: Ca(NO3)2 can be purchased from a variety of chemical suppliers, both online and in-store. Some common places to buy Ca(NO3)2 include scientific supply companies, agricultural supply stores, and home and garden centers. It is important to ensure that the supplier is reputable and that the product is of high quality and suitable for the intended application.