Iron Iii Nitrate Formula
Iron III Nitrate Formula
Iron III Nitrate , also known as ferric nitrate or iron(3+) salt, is a deliquescent salt that is most frequently seen in nonahydrate form with the Iron III Nitrate Formula Fe(NO3)3. Additionally, the crystalline iron source is highly soluble in water and suitable for usage with nitrates and lower (acidic) pH levels. Additionally, it crystallises in a colourless to pale violet range when dissolved and turns yellow as a result of hydrolysis.
Properties Of Iron (III) Nitrate
Although the Iron III Nitrate Formula is noncombustible and has the appearance of a violet crystalline solid, it can quicken the burning of items that are combustible. Its nonahydrate has a density of 1.6429g/cm3, whereas its hexahydrate weighs 1.68g/cm3. Its boiling point is 125oC, and it also has a 47oC melting point. It is barely soluble in cold concentrated HNO3 nitric acid but perfectly soluble in water, acetone, and alcohol.
Iron III Nitrate Formula and Structure
Iron III Nitrate has the molecular formula FeN3O9 and the Iron III Nitrate Formula is Fe(NO3)3. Its molecular weight is 241.857 g/mol as well. The iron ion (Fe3+) and the NO nitric oxide ion (NO3) have positive and negative charges, respectively, in Iron III Nitrate. Additionally, iron metal powder is treated with nitric acid to produce Iron III Nitrate.
Occurrence of Iron III Nitrate
Iron III Nitrate occurs in its nonahydrate form Fe(NO3)39H2O because it is deliquescent, which means it attracts and holds water molecules either through adsorption or absorption. The Iron III Nitrate crystallises in this as colourless to pale violet particles.
Preparation of Iron III Nitrate
Iron metal powder is treated with nitric acid to produce the Iron III Nitrate Formula.
Properties of Iron III Nitrate
The Iron III Nitrate Formula is Fe(NO3)3 (or) FeN3O9 with the IUPAC name, Iron(III) Nitrate. The other chemical names are Ferric Nitrate, Nitric Acid, Iron(3+) salt, and Iron Trinitrate. It appears as pale violet crystals with a molecular weight of 241.857 g/mol (Anhydrous). The Iron III Nitrate Formula has a density of 1.68 g/cm3 (hexahydrate) and 1.6429 g/cm3(nonahydrate). It melts at 47.2 °C and boils at 125 °C. It is soluble in water, alcohol, and acetone and is slightly soluble in cold concentrated nitric acid. In order to learn more about this topic, students are recommended to visit the Extramarks website.
Uses of Iron III Nitrate
The Iron III Nitrate Formula is the preferred catalyst in chemical laboratories for producing sodium amide from sodium in an ammonia solution
It has been demonstrated that certain clays impregnated with ferric nitrate are effective oxidants for organic synthesis. It is employed by metalworkers and jewellers to etch silver and silver alloys.
The Iron III Nitrate Formula is used in industries as a non-pesticide, an intermediary, a panting agent, and a surface treatment agent in agriculture. Additionally, it can also be employed as a corrosion inhibitor, a weighting agent for silks, a mordant in dyeing, and a component of analytical chemistry.
Safety and Health Hazard of Iron III Nitrate
- The nose and throat become irritated when exposed to Ferric Nitrate dust.
- The lips and stomach may become irritated after consuming Iron (III) Nitrate.
- It might irritate the skin and the eyes with prolonged contact. The liver may be impacted by repeated exposure.
- It is a potent oxidiser, and when it comes into touch with organic material, there is a risk of a hazardous fire. Fires can produce dangerous nitrogen oxides and nitric acid vapours.
Solved Example for You
Question: Describe a process for making Iron III Nitrate.
Solution: Here is how Iron III Nitrate is made:
Reason: The combined 30 ml of water and 50 g of iron filings or fine turnings with 100 ml of pure nitric acid. Additionally, the reaction might be controlled by gradually raising the temperature of the mixture, keeping it below 70oC, and the pace at which iron is added.
Additionally, after the iron particles practically dissolve, the solution is filtered and set it away to crystallise. Due to the fact that colloidal basic nitrates are present, filtrate often has a dark tint. As these nitrates gradually transform into regular nitrate, their colour lightens considerably.
Most importantly, since the crystals are slightly less soluble in nitric acid than in water, crystallisation can begin by adding strong nitric acid if none have formed after standing.