Sulfuric Acid: 1 Molecule, 101 Uses - CORECHEM Inc.

H2SO4. Sulfuric Acid. Battery Acid. Vitriol.

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Whatever you call it, Sulfuric Acid is one of the most important chemicals, and plays some part in production of almost all manufactured goods!

The chemical properties of Sulfuric Acid are what make it a highly versatile chemical with a wide variety of applications. For one thing, it is a highly corrosive acid. Also, it has oxidizing and sanitizing properties. It is hygroscopic, meaning it pulls water out of the air. It functions as a dehydrating agent, or desiccant.

In addition to a wide range of chemical properties, this colorless, oily mineral acid is also very inexpensive- a core commodity chemical.

That means that Sulfuric Acid has an endless, diverse portfolio of applications. Since it is used in so many different things, it is commonly known as a barometric indicator of the overall health of the economy in a country. There is more Sulfuric Acid produced annually than any other manufactured chemical.

Here we have compiled a list of a mere 101 of them!

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101 Ways Sulfuric Acid Is Used

(These include both direct and indirect usage. May be used in the product or in the manufacture of the product.)

sulfuric acid, dense, colourless, oily, corrosive liquid; one of the most commercially important of all chemicals. Sulfuric acid is prepared industrially by the reaction of water with sulfur trioxide (see sulfur oxide), which in turn is made by chemical combination of sulfur dioxide and oxygen either by the contact process or the chamber process. In various concentrations the acid is used in the manufacture of fertilizers, pigments, dyes, drugs, explosives, detergents, and inorganic salts and acids, as well as in petroleum refining and metallurgical processes. In one of its most familiar applications, sulfuric acid serves as the electrolyte in lead–acid storage batteries.

Pure sulfuric acid has a specific gravity of 1.830 at 25 °C (77 °F); it freezes at 10.37 °C (50.7 °F). When heated, the pure acid partially decomposes into water and sulfur trioxide; the latter escapes as a vapour until the concentration of the acid falls to 98.3 percent. This mixture of sulfuric acid and water boils at a constant temperature of 338 °C (640 °F) at one atmosphere pressure. Sulfuric acid is commonly supplied at concentrations of 78, 93, or 98 percent.

Due to its affinity for water, pure anhydrous sulfuric acid does not exist in nature. Volcanic activity can result in the production of sulfuric acid, depending on the emissions associated with specific volcanoes, and sulfuric acid aerosols from an eruption can persist in the stratosphere for many years. These aerosols can then reform into sulfur dioxide (SO2), a constituent of acid rain, though volcanic activity is a relatively minor contributor to acid rainfall.

Sulfuric acid is a very strong acid; in aqueous solutions it ionizes completely to form hydronium ions (H3O+) and hydrogen sulfate ions (HSO4−). In dilute solutions the hydrogen sulfate ions also dissociate, forming more hydronium ions and sulfate ions (SO42−). In addition to being an oxidizing agent, reacting readily at high temperatures with many metals, carbon, sulfur, and other substances, concentrated sulfuric acid is also a strong dehydrating agent, combining violently with water; in this capacity, it chars many organic materials, such as wood, paper, or sugar, leaving a carbonaceous residue.

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