Sulphuric Acid Plant
Your Professional Sulphuric Acid Plant Supplier
Our company are specialized in overseas project contracting, particularly in chemicals fields including chlor-alkali(caustic soda, calcium chloride, PVC, etc.) and fertilizer industry (Sulfuric acid, phosphoric acid , potassium and phosphate fertilizer-SOP, TSP, DCP, MCP, MKP, MAP and etc.).
Why Choose us
Rich Experience
We have accumulated very rich experiences after completing many project successfully, including technology know-how, machinery procurement, erection/fabrication, commissioning/start-up, training, etc.
Powerful Supplier
Years of development have made us a powerful supplier of traditional chemical plants with good cost-effectiveness.
Production Market
We have contracted projects in South Korea, Jordan, Bangladesh, Vietnam, Indonesia, Malaysia, Egypt, and etc .
Chemical Properties of Sulphuric Acid
Dissociation
H₂SO₄, when heated, undergoes dissociation into steam (H₂O) and SO₃.
H₂SO₄ ⇌ H₂O + SO₃
Acidic nature
The aqueous solution of the acid behaves as a strong dibasic acid since it ionises in two stages and gives two H⁺ ions. For instance,
H₂SO₄ ⇌ 2H⁺ + SO₄⁻
Oxidising agent
Hot concentrated sulphuric acid acts as a powerful oxidising agent. It is due to the reason that H₂SO₄ can lose nascent oxygen quite readily. When H₂SO₄ oxidises any substance, it is reduced to SO₂. These oxidising properties are not possible with diluting H₂SO₄.
H₂SO₄ → H₂O + SO₂ + [O]
Dehydrating agent
Concentrated H₂SO₄ dissolves in water and forms sulphuric acid hydrates, H₂SO₄.nH₂O. Due to this property, concentrated H₂SO₄ shows dehydrating properties. For instance,
(COOH)₂ + H₂SO₄ → CO + CO₂ + [H₂SO₄.H₂O]
Precipitation reaction
When the aqueous solutions of calcium, barium, lead, etc. salts are treated with dilute H₂SO₄, white precipitates of their corresponding metal sulphates are formed. For instance,
BaCl₂ + H₂SO₄ → BaSO₄ ↓ + 2HCl
Electrolysis
When 50% H₂SO₄ is electrolysed, peroxydisulfuric acid (H₂S₂O₈) is obtained at the anode in the solution.
Action on salts
H₂SO₄ is a strong acid that decomposes the salts of more volatile acids such as carbonates, sulfites, nitrates, chlorides, etc. The more volatile acid is liberated in each case. For instance,
2NaCl + H₂SO₄ → Na₂SO₄ + 2HCl
Application of Sulphuric Acid Plant
One of the primary uses of sulphuric acid is in manufacturing. It is a key component in the production of lead-acid batteries, which are commonly found in vehicles. These batteries are not just about starting cars; they play a pivotal role in ensuring the smooth operation of many vehicle functions. From providing power to lights to supporting the vehicle’s electrical system, lead-acid batteries are foundational to modern transportation. Their reliability and efficiency are, in part, thanks to the role sulphuric acid plays in their composition.
The metal finishing industry heavily relies on sulphuric acid, especially for processes like electroplating and sulphuric acid anodizing. Anodizing stands out as a transformative technique, increasing the thickness of the natural oxide layer on metal surfaces. This isn’t just about giving metals a shiny finish; it’s about equipping them with a shield against wear, corrosion, and environmental factors. As industries strive for products that last longer and perform better, the role of sulphuric acid in metal finishing becomes even more paramount.
Agriculture is another sector where sulphuric acid plays a significant role. Here, sulphuric acid emerges as an unsung hero, underpinning many processes that boost agricultural productivity. Sulphuric acid is a pivotal component in the production of phosphatic fertilizers, such as the superphosphate of lime and ammonium sulfate. But why does this matter? These fertilizers play a crucial role in soil health, enriching it with essential nutrients that plants crave. By enhancing nutrient uptake, they pave the way for plant growth and bountiful yields.
Apart from its primary uses, sulphuric acid plays a foundational role in producing various other chemicals. As a powerful dehydrating agent, it facilitates the creation of concentrated substances and essential lab reagents, including oleum and concentrated nitric acid.
Sulphuric acid’s potent acidic properties position it as a go-to ingredient in many cleaning solutions. Whether it’s clearing clogged drains or combating rust, this acid proves effective against tough challenges. Beyond these uses, sulphuric acid is also a key component in descaling agents. These agents combat the build-up of limescale and similar mineral deposits, ensuring surfaces remain clean and functional.
Sulphuric acid (H₂SO₄) has a tetrahedral geometry around the sulfur atom. The molecule consists of one sulfur atom centrally bonded to four oxygen atoms. Two of these oxygen atoms are bonded via double bonds, and the remaining two are bonded as hydroxyl groups (–OH).
The bond length of the sulfur-oxygen double bonds is shorter than that of the sulfur-oxygen single bonds (–OH groups). As a result, the oxygen atoms exert greater repulsion on the –OH groups. This leads to a larger bond angle in the sulfur-oxygen double bonds than in the sulfur-oxygen single bonds.
Common Sulphuric Acid Reactions
Oxidizing Agent: Hot concentrated sulphuric acid acts as an oxidising agent, oxidising metals and non-metals while itself being reduced to sulfur dioxide:
Oxidation of Copper: Cu(s) + 2H2SO4(hot) → CuSO4(aq) + SO2(g) + 2H2O(l)
Oxidation of Carbon: C(s) + 2H2SO4(hot, conc.) → CO2(g) + 2SO2(g) + 2H2O(l)
Reactions with Alkalis: Sulphuric acid neutralises alkalis to form bisulfates and sulfates:
Formation of Sodium Bisulfate: H2SO4(conc.) + 2NaOH(aq)→2NaHSO4(aq)+H2O(l)
Formation of Sodium Sulfate: H2SO4(conc.) + 2NaOH(aq)→Na2SO4(aq)+2H2O(l)
Preparation of Volatile Acids: Sulphuric acid is used to liberate more volatile acids from their salts:
From sodium chloride, concentrated sulphuric acid produces hydrogen chloride: NaCl + H2SO4(conc) → NaHSO4 + HCl
From calcium fluoride, concentrated sulphuric acid produces hydrogen fluoride: CaF2 + H2SO4(conc) → CaSO4 + 2HF
Dehydrating Agent: Sulphuric acid is a potent dehydrating agent that dries gases and removes water from organic compounds. Sulphuric acid converts glucose, sugar, and starch to carbon.
Dehydration of Sugars: C12H22O11 + H2SO4(conc.) →12C+11H2O
FAQ
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