Acids questions

Hydrofluoric acid is a precursor to almost all fluorine compounds, including: fluoxetine (Prozac), PTFE (Teflon).It is a colourless solution that is highly corrosive, capable of dissolving many materials, especially oxides. Because of its high reactivity toward glass and moderate reactivity toward many metals, hydrofluoric acid is usually stored in plastic containers.

It is a formic acid formula.

With the same central atom, acid strength increases as the number of oxygens attached to it increases, so perchloric acid (HClO4) is the strongest.

Sulfoxylic acid (H2SO2) (also known as hyposulfurous acid or sulfur dihydroxide)) is an unstable oxoacid of sulfur in an intermediate oxidation state between hydrogen sulfide and dithionous acid. It consists of two hydroxy groups attached to a sulfur atom.

Acetic acid (CH3COOH) has a carboxylic group (COOH). Carbonic acid (H2CO3), nitric acid (HNO3) and hydrochloric acid (HCL) of this group do not.

The most important gas which leads to acidification is sulfur dioxide, coming from fossil fuel combustion and industry (and, in lesser amounts, from volcanoes and wildfires). In recent years, emissions of nitrogen oxides which are oxidized to form nitric acid are of increasing importance due to stricter controls on emissions of sulfur containing compounds.

World production of sulfuric acid in 2004 was about 180 million tonnes. About 60% of this amount is consumed for fertilizers, particularly superphosphates, ammonium phosphate and ammonium sulfates. Similarily, 75–80% of the 26M tons of nitric acid produced annually is used to produce ammonium nitrate fertilizer.

Nitric acid is the primary reagent used for nitration - the addition of a nitro group. Nitration reactions are notably used for the production of explosives, for example synthesis of nitroglycerine, the conversion of guanidine to nitroguanidine and the conversion of toluene to trinitrotoluene (TNT).

Fluoroantimonic acid is an ionic liquid created by reacting hydrogen fluoride with antimony pentafluoride in stoichiometrically equivalent amounts. The 1:1 combination forms the strongest known superacid, 10^16 (10 quadrillion) times stronger than 100% sulfuric acid.

Pure water is about 7 at 25 °C; this value decreases with increasing temperatures. At 50 °C, it is 6.55. It is also worth to note, that water that has been exposed to air is mildly acidic, because it absorbs carbon dioxide from the air.