Iron III nitrate is a chemical compound. It is formed by combining iron ions with nitrate ions. It is commonly used in industrial applications and as a laboratory reagent.
| IUPAC Name | Iron(III) Nitrate |
| Molecular Formula | Fe(NO3)3 |
| CAS Number | 10421-48-4 |
| Synonyms | Ferric nitrate, Iron trinitrate, Nitric acid iron(III) salt |
| InChI | InChI=1S/Fe.3NO3/c;32-1(3)4/q+3;3-1 |
Iron(III) Nitrate Properties
Iron(III) Nitrate Formula
The formula for Iron III nitrate is Fe(NO3)3. It consists of one iron (Fe) ion and three nitrate (NO3) ions. This formula represents the combination of the iron cation with the nitrate anions.
Iron(III) Nitrate Molar Mass
The molar mass of Iron nitrate can be calculated by adding the atomic masses of its constituent elements. Iron (Fe) has a molar mass of 55.845 g/mol, while each nitrate (NO3) ion has a molar mass of 62.0049 g/mol. Adding these values together gives a molar mass of approximately 241.86 g/mol for Iron nitrate.
Iron(III) Nitrate Boiling Point
Iron nitrate does not have a specific boiling point. Upon heating, it decomposes into various nitrogen oxides and eventually forms iron oxide. The decomposition temperature depends on factors such as the concentration and presence of other substances.
Iron(III) Nitrate Melting Point
The melting point of Iron nitrate is approximately 47 °C (117 °F). At this temperature, the solid compound transforms into a liquid state. It is important to note that the melting point may vary slightly depending on factors such as impurities or the exact composition of the compound.
Iron(III) Nitrate Density g/mL
The density of Fe(NO3)3 is approximately 1.68 g/mL. Density represents the mass per unit volume of a substance. In this case, it indicates the mass of Fe(NO3)3 per milliliter of the compound.
Iron(III) Nitrate Molecular Weight
The molecular weight of Iron nitrate is approximately 241.86 g/mol. Molecular weight refers to the sum of the atomic weights of all the atoms in a molecule.
Iron(III) Nitrate Structure
Iron nitrate has a crystal structure in its solid form. It consists of Fe3+ cations surrounded by coordinated nitrate (NO3-) anions. The iron cations are held together by ionic bonds, while the nitrate anions are attracted to the cations through electrostatic forces.
Iron(III) Nitrate Solubility
Iron nitrate is highly soluble in water. It readily dissolves in water to form a clear, pale yellow solution. The solubility of Iron nitrate in other solvents or substances may vary.
| Appearance | Pale yellow crystals |
| Specific Gravity | 1.68 |
| Color | Pale yellow |
| Odor | Odorless |
| Molar Mass | 241.86 g/mol |
| Density | 1.68 g/mL |
| Melting Point | 47 °C (117 °F) |
| Boiling Point | Decomposes |
| Flash Point | Not applicable |
| Water Solubility | Highly soluble |
| Solubility | Soluble in water and polar solvents |
| Vapor Pressure | Not available |
| Vapor Density | Not available |
| pKa | Not available |
| pH | Acidic |
Iron(III) Nitrate Safety and Hazards
Iron nitrate poses certain safety hazards and precautions should be taken when handling it. It is considered an irritant to the skin, eyes, and respiratory system. Direct contact with the compound should be avoided, and protective equipment such as gloves and goggles should be worn. Ingestion or inhalation of Iron nitrate can cause harmful effects, and therefore, it should not be ingested or inhaled. It is important to work with this compound in a well-ventilated area to minimize the risk of inhalation. In case of accidental exposure or ingestion, immediate medical attention should be sought. Proper storage and handling practices should be followed to ensure safety.
| Hazard Symbols | Xi, O |
| Safety Description | Causes skin and eye irritation. May cause respiratory irritation. Harmful if swallowed. |
| UN IDs | UN 1466 (Anhydrous) |
| HS Code | 28342990 |
| Hazard Class | 5.1 (Oxidizing Agent) |
| Packing Group | II |
| Toxicity | Moderate toxicity |
Iron(III) Nitrate Synthesis Methods
One can synthesize Iron nitrate through various methods, with a common method involving dissolving iron(III) oxide (Fe2O3) in concentrated nitric acid (HNO3). This reaction results in the formation of Iron nitrate, as represented by the equation:
Concentrated nitric acid dissolves iron(III) oxide, yielding Fe(NO3)3 along with the production of water:
Fe2O3 + 6HNO3 → 2Fe(NO3)3 + 3H2O.
Another method entails combining iron metal with a mixture of nitric acid and hydrogen peroxide, which oxidizes the iron to form Iron nitrate. The well-known reaction earns the name “aqua regia” method.
The addition of iron metal to a mixture of nitric acid and hydrogen peroxide leads to the production of Iron nitrate and water:
2Fe + 8HNO3 + 6H2O2 → 2Fe(NO3)3 + 6H2O.
It is crucial to exercise caution while carrying out these reactions due to the corrosive and oxidizing nature of the chemicals involved. It is necessary to follow proper safety measures, such as wearing protective equipment and working in a well-ventilated area.
Reputable chemical suppliers offer commercially available Iron nitrate, guaranteeing a consistent and reliable source of the compound for various applications in industries and laboratories.
Iron(III) Nitrate Uses
Iron nitrate has several practical uses in various industries and laboratory settings. Here are some key applications of Iron nitrate:
- Industrial Catalyst: Several industrial processes, including the production of nylon and other polymers, use Iron nitrate as a catalyst.
- Dyeing and Pigments: The dyeing and pigmentation industry employs Iron nitrate as a mordant to fix dyes to fabrics and enhance colorfastness.
- Etching Agent: Metalworking and electronics industries use Iron nitrate as an etching agent to create intricate patterns and designs on metal surfaces.
- Laboratory Reagent: Iron nitrate serves as a common laboratory reagent for various chemical reactions and experiments, especially for synthesizing other compounds.
- Oxidizing Agent: Iron nitrate acts as an oxidizing agent in chemical reactions, including organic synthesis, due to its strong oxidizing properties.
- Water Treatment: Iron nitrate is useful in water treatment processes for removing impurities, such as phosphates and sulfides, from industrial wastewater.
- Photography: Certain photographic processes, particularly the preparation of iron-based photographic emulsions, utilize Iron nitrate.
- Analytical Chemistry: Iron nitrate finds application in analytical chemistry techniques, such as colorimetric analysis, to detect and quantify specific substances.
- Preservation of Wood: Wood preservation treatments utilize Iron nitrate as an active ingredient to safeguard wood from fungal decay and insect infestation.
- Pharmaceutical Applications: The formulation of certain pharmaceutical products and medicines involves the use of Iron nitrate.
It is important to note that proper handling and safety precautions should be followed when working with Iron nitrate due to its corrosive and oxidizing nature.
Questions:
Q: Is iron(III) nitrate flammable?
A: No, iron nitrate is not flammable.
Q: What are some of the safety and handling concerns with iron(III) nitrate?
A: Safety concerns include skin, eye, and respiratory irritation, hence it should be handled with proper protective equipment and precautions.
Q: Which formula represents iron(III) nitrate?
A: The formula for iron nitrate is Fe(NO3)3.
Q: What is the formula of iron(III) nitrate?
A: The formula of iron(III) nitrate is Fe(NO3)3.
Q: What is the molar mass of iron(III) nitrate?
A: The molar mass of Fe(NO3)3 is approximately 241.86 g/mol.
Q: Is iron hydroxide soluble in water?
A: Iron hydroxide is sparingly soluble in water.
Q: Does Ca react with iron(III) nitrate?
A: No, calcium (Ca) does not typically react with Fe(NO3)3.
Q: What part of aspirin does iron(III) nitrate react with?
A: Iron(III) nitrate reacts with the carboxylate group (-COO-) present in the aspirin molecule.
Q: What is the molecular mass of iron(III) nitrate?
A: The molecular mass of Fe(NO3)3 is approximately 241.86 g/mol.
Q: Does Al react with iron(III) nitrate?
A: Yes, aluminum (Al) can react with Fe(NO3)3 to form aluminum nitrate and iron metal.
Q: How many moles of nitrate are dissolved in 50.0 g of water in a 3.80 M iron(III) nitrate solution?
A: To determine the moles of nitrate, the volume of the solution is needed, as only molarity and mass of water are provided.