Agatos Sulphuric Acid H2SO4.

Sulfuric acid (alternative spelling sulphuric acid) is a strong mineral acid with the molecular formula H2SO4. Its historical name is oil of vitriol. Pure sulfuric acid is a highly corrosive, colorless, viscous liquid. The salts of sulfuric acid are called sulfates. Sulfuric acid is soluble in water at all concentrations.

Sulfuric acid has many applications, and is a central substance in the chemical industry. Principal uses include lead-acid batteries for cars and other vehicles, ore processing,fertilizer manufacturing, oil refining, wastewater processing, and chemical synthesis.

Grades of sulfuric acid

Although nearly 99% sulfuric acid can be made, this loses SO3 at the boiling point to produce 98.3% acid. The 98% grade is more stable in storage, and is the usual form of what is described as "concentrated sulfuric acid." Other concentrations are used for different purposes. Some common concentrations are

Oleum (Latin oleum = "oil"), or fuming sulfuric acid refers to a solution of various compositions of sulfur trioxide in sulfuric acid or sometimes more specifically to disulfuric acid(also known as pyrosulfuric acid).

Oleums can be described by the formula ySO3.H2O where y is the total molar sulfur trioxide content. The value of y can be varied, to include different oleums. They can also be described by the formula H2SO4.xSO3 where x is now defined as the molar free sulfur trioxide content. Oleum is generally assayed according to the free SO3 content by weight. It can also be expressed as a percentage of sulfuric acid strength; for oleum concentrations, that would be over 100%. For example, 10% Oleum can also be expressed as H2SO4.0.1SO3,1.0225SO3.H2O or 102.25% Sulfuric Acid. The conversion between % acid and % oleum is: % Acid = 100 + 18/80 * % Oleum

Sulfur dioxide (also sulphur dioxide) is the chemical compound with the formula SO2. It is released by volcanoes and in various industrial processes. Since coal and petroleumoften contain sulfur compounds, their combustion generates sulfur dioxide unless the sulfur compounds are removed before burning the fuel. Further oxidation of SO2, usually in the presence of a catalyst such as NO2, forms H2SO4, and thus acid rain.[2] Sulfur dioxide emissions are also a precursor to particulates in the atmosphere. Both of these impacts are cause for concern over the environmental impact of these fuels