Sulfuric acid
Sulfuric acid, also known as sulphuric acid, is a strong acid. It is a chemical compound. Its chemical formula is H2SO4. It was known as "Oil of Vitriol" in ancient times.
Properties
It is a dense (thick), clear, corrosive liquid that can dissolve in water. It can also melt through some weak substances.
History
It was once known as "oil of vitriol". This name was created by Jabir ibn Hayyan, the person who discovered it. It used to be prepared by the reaction of potassium nitrate with sulfur. This reaction would produce sulfur trioxide which would dissolve in steam to produce sulfuric acid. Then this reaction was done in lead containers. The contact process, the most common process, was invented in 1831 and is still used today.
Production
It is made by reacting sulfur trioxide with sulfuric acid to produce oleum. Then oleum is dissolved in water to produce more sulfuric acid. The sulfur trioxide is produced by burning sulfur to produce sulfur dioxide, which was then oxidized to sulfur trioxide with a catalyst. This process is called the contact process.
Uses
Sulfuric acid has many uses. World production in 2001 was 165 million tons, worth about $8 billion US dollars. Uses include ore processing, fertilizer manufacturing, oil refining, wastewater processing, lead acid batteries, and combining chemicals for scientific reasons. For example, phosphate rocks are reacted with sulfuric acid to produce soluble phosphates, useful in fertilizers. This reaction is also used to make phosphoric acid, useful in soda. Potassium compounds are dissolved in sulfuric acid to produce potassium sulfate, useful in fertilizers. Ammonia is also reacted with sulfuric acid to produce ammonium sulfate. These three chemicals are solids and provide the three main minerals needed in plants. Lead acid batteries use sulfuric acid as their electrolyte.
Reactions and safety
Sulfuric acid is very poisonous because of its acidity and corrosiveness. When it is mixed with sugar, it turns it into carbon.[1] When it is dissolved in water, it becomes less harmful but is still corrosive like normal acids. It reacts with metals to produce hydrogen and the metal sulfate. Some metals, such as tin, make sulfur dioxide and tin(II) sulfate. It reacts with sodium chloride to make hydrogen chloride.
Related pages
References
- ↑ Reaction
Sulfuric Acid Media
An experiment that demonstrates the dehydration properties of concentrated sulfuric acid. When concentrated sulfuric acid comes into contact with sucrose, slow carbonification of the sucrose takes place. The reaction is accompanied by the evolution of gaseous products that contribute to the formation of the foamy carbon pillar that rises above the beaker.
Drops of concentrated sulfuric acid rapidly decompose a piece of cotton towel by dehydration.
Solid state structure of the [D
3SO
4]+
ion present in [D
3SO
4]+
[SbF
6]−
, synthesized by using DF in place of HF.
sulfonation of benzene
Rio Tinto with its highly acidic water
Sulfuric acid production in 2000
Domestic acidic drain cleaners usually contain sulfuric acid at a high concentration which turns a piece of pH paper red and chars it instantly, demonstrating both the strong acidic nature and dehydrating property.
Domestic acidic drain cleaners can be used to dissolve grease, hair and even tissue paper inside water pipes.
John Dalton's 1808 sulfuric acid molecule shows a central sulfur atom bonded to three oxygen atoms, or sulfur trioxide, the anhydride of sulfuric acid.
Archived 2009-02-11 at the Wayback Machine, retrieved 1 November 2010, chemistry.about.com
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