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Ferrous sulfate, also known as Iron (II) sulfate represents a spectrum of salts having the formula of FeSO4·H2O. Ferrous sulphate, green vitriol, Iron vitriol, Copperas, Melanterite, and Szomolnokite are some of the other names for Iron (II) sulphate. Iron sulfate is created when iron filings are added to a copper sulphate solution, the iron pushes the copper out of the way since it is more reactive. Iron (II) sulphate is a bluish-green chemical used in a variety of applications such as ink, dye, and medicine. Melanterite FeSO4H2O (blue-green) and Rozenite FeSO4H2O are two well-known mineral forms of ferrous sulphate (white, maybe a dehydrated version of melanterite).
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Ferrous Sulphate
Iron (II) Sulphate, often known as ferrous sulphate, is a salt that comes in a variety of forms. FeSO4·xH2O is the formula for salt. The most frequent type of salt is heptahydrate. Medically, the hydrated salt is used to treat iron deficiency. It can also be used in a variety of industrial settings. A similar aqua complex is formed when iron(II) sulphates dissolve in water. The geometry of this aqua complex is octahedral. [Fe(H2O)6]2+ is the formula for the aqua complex. It has a paramagnetic property.
Ferrous Sulphate
Properties of Ferrous Sulphate
- Chemical Formula- FeSO4
- Molar Mass- 151.908 g/mol
- Colour - Green
- Melting Point- 54-65° C
- Boiling Point- 330° C
- Solubility – Soluble in water
Production of Ferrous Sulphate
Steel is put through sulfuric acid baths before being coated or plated in the manufacturing process. As a by-product, a substantial amount of ferrous sulphate is produced.
Fe+H2SO4→FeSO4+H2
The sulphate procedure can be used to produce massive amounts of titanium dioxide from titanium-iron oxide rocks.
Formula for Ferrous Sulphate
By oxidising pyrite, ferrous sulphate can be produced commercially. Sulphuric acid and ferrous sulphate are generated in this process.
2FeS2+7O2+2H2O→2FeSO4+2H2SO4
Displacement of metals less reactive than Iron from their sulphates can also provide ferrous sulphate:
CuSO4+Fe→FeSO4+ Cu
Read More: Daniell CellReactions of Ferrous Sulphate
The metal aquo complex is formed when ferrous sulphate is dissolved in water [Fe(H2O)6]2+. It's a nearly colourless ion that's also paramagnetic.
When ferrous sulphate is heated, it loses its water of crystallisation first, then the actual green crystals become an anhydrous white solid. If the anhydrous solid is heated further, white fumes of sulphur trioxide and sulphur dioxide are released, leaving reddish-brown ferric oxide behind. When ferrous sulphate is virtually depleted, it begins to disintegrate at around 680oC.
2FeSO4→Fe2O3+SO2+SO3
Ferrous sulphate, like all other ferrous salts, is a reducing agent. It converts nitric acid to nitrogen monoxide and chlorine to chloride, for example:
FeSO4+HNO3 H2SO4→Fe2(SO4)3+H2O+NO
FeSO4+ Cl2→ Fe2(SO4)3+FeCl3
Read Also: Reduction Potential
Hydrates of Ferrous Sulphate
Iron(II) sulfate is available in several states of hydration, and some of these types occur in nature. Such as:
- FeSO4·H2O- Szomolnokite
- FeSO4·4H2O- Rozenite
- FeSO4·5H2O- Siderotil
- FeSO4·6H2O Ferro Hexahydrite
- FeSo4·7H2O Melanterite
Hydrates of Ferrous Sulphate
When the temperature of the aqueous solution exceeds an undefined control sequence degree, tetrahydrate becomes stable. At the Undefined control sequence degree, the solution generates both tetrahydrate and monohydrate.
All of the minerals listed have a connection to the oxidation zones of iron-bearing ore beds (marcasite) and the surrounding environment (like coal fire sites). Many are subjected to rapid dehydration and, on rare occasions, oxidation. In these conditions, copiapite is a good and common example of a more complex (either simple, hydrated, or with extra cations) Fe(II)-sulphate-bearing sulphate.
Read More: Uses of Carboxylic Acids
Uses of Ferrous Sulphate
Ferrous sulphate is primarily used in industry as a precursor to other iron components. It has a decreasing effect. It has been used as a dye fixative in the textile industry. It was also used as a component of ink and for blackening hides. The processing of sulphuric acid by the distillation of green vitriol (Iron(II) sulphate) is a well-known method for more than 700 years.
- Medical Uses: Ferrous sulphate is utilized to enhance food items for treating and avoiding anaemia that is caused by iron deficiency.Iron is a necessary heavy element that can be found in a variety of multivitamin and mineral supplements. Iron has little or no effect on the liver when ingested at the recommended daily intake or at the replacement dosage. Iron causes severe toxicity in large quantities and purposeful or inadvertent overdosages, one of which is abrupt liver failure.
Impheron and iron dextran are iron supplements that can be injected. Oral iron supplements include ferrous fumarate, ferrous gluconate, and ferrous sulphate. By far the safest and most affordable iron supplement is ferrous sulphate.
- Plant Use- Iron (II) sulphate or ferrous sulphate is a soil amendment that lowers the pH of high alkaline soils, allowing plants to absorb nutrients. In horticulture, it is used to cure iron chlorosis. Although it does not operate as quickly as ferric EDTA, its effects stay longer. It can be mixed with compost and buried into the ground to form a long-lasting store.
- Pigment and Craft- Ferrous sulphate can be used to colour concrete, as well as some limestones and sandstones, a yellowish rust. To give maple wood a silvery tone, woodworkers employ ferrous sulphate solutions. Green vitriol is also a good reagent for mushroom identification.
Points to Remember
- Ferrous Sulphate represents a category of salts that have the chemical formula of FeSO4·H2O.
- Ferrous sulphate occurs in a variety of hydrate forms which are Szomolnokite, Rozenite, Siderotil, Ferric Hexahydrate and Melanterite.
- Iron is very important in the making of medicine and as a resource for the body and hence ferrous sulphate is an active ingredient in many medicines all over the medical industry.
- Ferrous sulphate is a very important ingredient in ink and other dyes
Sample Questions
Ques: What are the benefits of ferrous sulphate? (3 Marks)
Ans. In the biological world, ferrous sulphate plays an important role. This mineral is essential to our health. It is used to treat and prevent anaemia caused by iron deficiency, which is a lack of RBCs (red blood corpuscles), or a lack of iron in the body.
Although ferrous sulphate is lighter, it has a high tensile strength. Some of the advantages of ferrous sulphate include high current conductivity (found in copper), zinc that is resistant to Corrosion, and magnetic force tolerance. These ferrous metals are either converted into intermediate metals or completed products.
Ques: What are the adverse effects of ferrous sulphate overdose? (1 Mark)
Ans. People most commonly experience various sorts of gastrointestinal distress, such as nausea, diarrhoea, vomiting, stomach pain, constipation, and black or discoloured faeces.
Ques: What is the color of ferrous sulphate crystals? How does this color change after heating? Name the products formed on strongly heating ferrous sulphate crystals. What type of chemical reaction occurs in this type of change. (3 Marks)
Ans. Ferrous sulphate crystals are green in colour.
Water molecules can be found in ferrous sulphate crystals (FeSO4·7H2O). When ferrous sulphate crystals are heated, they lose water and anhydrous ferrous sulphate (FeSO4) is created. As a result, their colour shifts from bright green to white.
Anhydrous ferrous sulphate decomposes further on heating to create ferric oxide (Fe2O3), sulphur dioxide (SO2), and sulphur trioxide (SO3). As a result, the released gas smells like burning sulphur.
The single ingredient FeSO4 decomposes into three distinct products in this reaction. As a result, the reaction is classified as a decomposition reaction.
Ques: What is the substance that is left in the test tube after heating ferrous sulphate? (4 Marks)
Ans. The blue-green heptahydrate (hydrate with 7 water particles) is the most well-known variety of the substance. In water, all of the iron (II) sulphates break down to form the corresponding aquo complex [Fe(H2O)6]2+, which has octahedral molecular geometry and is paramagnetic. The name copperas comes from the time when copper (II) sulphate was referred to as blue copperas, and iron (II) and zinc sulphate were referred to separately as green and white copperas.
When ferrous sulphate is heated in a test tube, the following reaction occurs:
FeSO4·7H2O→FeSO4+7H2O
2FeSO4→Fe2O3+SO2+SO3
Both SO2 (sulphur dioxide) and SO3 (sulphur trioxide) are colourless gases that are emitted.
Only Fe2O3, or ferric oxide, which is reddish brown in colour, remains in the test tube.
As a result, Fe2O3, or ferric oxide, which is reddish brown in colour, remains in a test tube after heating ferrous sulphate.
Ques: 2g of ferrous sulphate crystals are heated in a dry boiling tube. (3 Marks)
- List any two observations.
- Name the type of chemical reaction taking place.
- ‘Write the chemical equation for the reaction
Ans.
- Two observations:
- When heated, the colour changes from pale green to brown or reddish brown, indicating a change in state and colour.
- Gas evolution.
- Reaction of decomposition
- The chemical equation is as follows:
2FeSO4(s) +Heat Fe2O3(s) + SO2(g) + SO3(g)
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