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Sulphate (SO42-) is one of the most common chemical compounds found as naturally occurring minerals on Earth. It is typically present in the environment due to atmospheric and terrestrial activities. Sulphur emitted from evaporite deposits, sulphide-containing rocks and minerals, and even volcanoes is an important source of sulphate.
Sulphate Structure
The sulphate ion is mostly made up of sulphur and oxygen atoms. Sulphur is the central element in this structure, surrounded by four oxygen atoms spaced evenly across the plane. In terms of bonding, two oxygen atoms make S=O bonds, while the other two form S-O- bonds. Because the oxygen atoms are in a -2 state, they are responsible for the anion’s negative charge (-2).
When we look at the structure or form of the molecule, we can see that it has a tetrahedral geometry, which is further supported by the VSEPR hypothesis. In layman’s words, the geometry of sulphate ion is star-shaped.
Physical Properties
- Ionic sulphates dissolve quickly in water.
- Strontium sulphate, calcium sulphate, barium sulphate, and lead (II) sulphate are some of the exceptions. They are poorly soluble.
- During reactions, they tend to create white precipitate.
Chemical Properties
- Sulfate has a unique chemical feature in that it may easily bond with metals.
- The sulphate ion functions as a ligand, linking two oxygens or one oxygen as a bridge.
- The sulphate ion is a conjugate base of bisulfate ion, HSO–4 (hydrogen sulphate), and sulfuric acid. Meanwhile, organic sulphate esters such as dimethyl sulphate are classified as esters of sulfuric acid and covalent molecules.
Sulphate Preparation
Sulfates are typically prepared in one of two ways.
- Metal sulphites and sulphides are oxidised. However, the creation of sulphate as the ultimate state of oxidation may be dictated by a series of processes that are highly reliant on other variables such as the catalyst, etc.
- Sulfuric acid is used to treat metal hydroxide, metal oxide, and pure metal.
Ba(ClO3)2 + H2SO4 → 2 HClO3 + BaSO4
Zn + H2SO4 → ZnSO4 + H2
Cu(OH)2 + H2SO4 → CuSO4 + 2 H2O
One thing to remember while making sulphate is that sulfuric acid should be deprotonated twice. If it happens only once, the ion hydrogen sulphate is formed.
Sulfates are abundant in nature and are also easily manufactured in industry. As a result, this chemical compound has a wide range of uses.
FAQs
Q. Why is sulfuric acid referred to as the “King of Acids,” despite the fact that hydrochloric acid is more concentrated?
ANS: Because of its direct and indirect applications in the synthesis of various chemicals, including fertilisers, sulphuric acid is known as the “king of acids.” To remove rust from steel rollers and soap, sulphuric acid is employed. It also dissolves the chemicals it contains. As a result, it is appropriate to refer to sulphuric acid as the “King of Chemicals.”
Q. Which procedure may be used to generate sulfuric acid from sulphur combustion or to regenerate wasted acid from alkylation plants?
ANS: The wet sulphuric acid method can be used to produce sulfuric acid from sulphur combustion or to regenerate wasted acid from alkylation units.
