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About Sulphuric Acid
Manufacture of Sulphuric Acid
Contact Process
Lead Chamber Process
Physical Properties of Sulphuric Acid
Chemical Properties of Sulphuric Acid
Example of Sulphuric Acid
Uses of Sulphuric Acid
Sulphuric acid, H2SO4 is an odorless, colorless, oily liquid that is extremely corrosive It was at first called Oil of Vitriol.
It occurs in both combined and free state.
It is framed close to the sulfide beds.
In the joined frame, it happens as metallic sulfates (salts in minerals).
Fig. 1: A molecule of sulphuric acid
Fig. 2: Structure of sulfuric acid
Commercially, Sulphuric Acid can be prepared by two techniques that are as follows:
Lead chamber process
Contact process
The contact process includes three steps:
Step – I: Production of Sulphur Dioxide: This can be made by smoldering sulfur or sulfide ores, for example, iron pyrites in abundance of air.
S (Sulphur) + O2 (Oxygen) + Δ (Heating) → SO2 (Sulphur dioxide) 4FeS (Iron pyrites) + 7O2 (Oxygen) + Δ (heating) → 2Fe2O3 (Ferric Oxide) + 4SO2(Sulphur dioxide)
Step -II:
Formation of Sulphur Trioxide:
Sulphur dioxide is oxidized to sulphur trioxide with atmospheric oxygen within the sight of V2O5 as a catalyst.
2SO2 (Sulphur dioxide) + O2 (Oxygen) + V2O5 (Catalyst) → SO3 (Sulphurtriioxide)
Step -III
Conversion of Sulphur Trioxide into Sulphuric Acid: The sulfur trioxide shaped in the second step is broken up in 98% sulphuric acid to give pyrosulphuric acid or oleum. Oleum is then diluted or weakened with water to give sulphuric acid of the concentration that is required.
SO3 (Sulphur trioxide) + H2SO4 (Sulphuric acid-98%) → H2S2O7 (Pyrosulphuric acid -Oleum) H2S2O7 (Pyrosulphuric acid -Oleum) + H2O (Dilution ) → 2H2SO4(Sulphuric acid)
Fig. 3: A schematic diagram of a contact-process sulfuric acid converter
Fig. 4: Reactions and steps involved in the Contact Process
Lead Chamber process is one of the sulphuric acid manufacturing strategies which give just around 50-60 B grade acids. The fundamental standard of the procedure is that the wet SO2 (Sulfur Dioxide) in the nearness of nitrogenous oxides (dynamic impetus) is oxidized to sulfur trioxide with the oxygen exhibit in air. Sulfur trioxide is made to react with water to create sulphuric acid. The reactions would resemble beneath:
2SO2 + O2 → 2SO3
SO3 + H2O → H2SO4
Fig. 5: Lead chamber process
Sulphuric acid is a thick, colourless, oily fluid with a specific gravity of 1.84 at 298 K.
The boiling point is 611 K. The high boiling point and thick nature is because of hydrogen bonding.
Concentrated sulphuric acid has a strong water affinity. A lot of heat is created when the acid is blended with water.
The acid is constantly diluted by adding it to water gradually with steady blending.
Remember - Never add water to Sulphuric Acid.
Fig. 6: Physical properties of Sulphuric Acid
Fig. 7: Chemical properties of Sulphuric Acid
Sulphuric Acid is a very strong dibasic acid. It ionizes in two stages in aqueous solution:
Step 1: H2SO4(aq) + H2O(I) → H3O+(aq) + HSO4-(aq); Ka1 = very large (Ka1 > 10) Step 2: HSO4(aq) + H2O(I) → H3O+(aq) + SO42-(aq); Ka2 = 1.2 x 10-2
Example:
Concentrated sulphuric acid reacts with sodium hydroxide and structures sodium bisulphate and sodium sulfate.
H2SO4 (Conc.Sulphuric acid) + 2NaOH (Sodium hydroxide)→ 2NaHSO4 (Sodium bisulphate) + H2O (Water) H2SO4 (Conc.Sulphuric acid) + 2NaOH (Sodium hydroxide) → Na2SO4 (Sodium sulphate) + 2H2O (Water)
CaF2 (Calcium fluoride)+ H2SO4 (Conc. Sulphuric acid) → CaSO4(Calcium sulphate) + 2HF (Hydrogen floride)
C12H22O11(Cane sugar) + (H2SO4) → 12C (Carbon) + 11H2O (Water)
Hot concentrated sulphuric acid oxidizes copper to copper sulfate. Similarly, it oxidizes non-metallic carbon to carbon dioxide.
Cu (Copper) + 2H2SO4 (Hot suphuric acid) → CuSO4 (Copper sulphate) + SO2 (Sulphur dioxide) + H2O (Water) C (Carbon) + 2H2SO4 (Hot suphuric acid) → CO2 (Carbon dioxide) + 2SO2 (Sulphur dioxide) + 2H2O (Water)
Example: Concentrated sulphuric acid liberates hydrogen chloride from sodium chloride and hydrogen fluoride from calcium fluoride.
CaF2 (Calcium fluoride)+ H2SO4 (Conc. Sulphuric acid) →
CaSO4 (Calcium sulphate) + 2HF (Hydrogen floride)
C12H22O11 (Cane sugar) + (H2SO4) → 12C (Carbon) + 11H2O (Water)
Hot concentrated sulphuric acid oxidizes copper to copper sulfate .Similarly, it oxidizes non-metallic carbon to carbon dioxide.
Sulphuric acid, on account of its wide applications, is alluded as the King of Chemicals.
It is utilized as a part in the preparation of:
Fertilisers like ammonium sulfate and superphosphate
Dyes, shades, and paints
Explosives, for example, TNT
Other imperative chemicals like hydrochloric acid, phosphoric acid, nitric acid, and sodium carbonate
It is utilized as a part of the refining of petroleum
As a pickling agent
As a laboratory agent, and an oxidizing and dehydrating agent
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Sulphuric Acid
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