Bisulfaatin

Bisulfaatin, or bisulfate, refers to the bisulfate ion HSO4− and the salts that contain it. It is formed by partial neutralization of sulfuric acid (H2SO4), yielding species such as sodium bisulfate (NaHSO4), potassium bisulfate (KHSO4), and ammonium bisulfate ((NH4)HSO4). Bisulfate is chemically distinct from bisulfite (HSO3−), which derives from sulfurous acid.

Chemical properties and structure: In water, HSO4− acts as an acid and can dissociate further to SO4^2−, releasing a proton. The salts are typically highly soluble in water and often occur as hydrates. They are usually hygroscopic and can be corrosive, capable of causing irritation to skin, eyes, and mucous membranes.

Production and handling: Bisulfates are prepared by controlled neutralization of sulfuric acid with bases, or by industrial processes that generate the mono-protonated sulfate species. In practice, sodium bisulfate and other bisulfates are handled as dry, solid materials or as aqueous solutions. They should be stored in a dry, well-ventilated area away from incompatible substances such as strong bases and oxidizers.

Applications: In industry and consumer products, bisulfates serve as acidulants and pH regulators. Sodium bisulfate, for example, is used in pool maintenance, cleaning products, and some food and beverage formulations to impart acidity. They are also employed in descaling processes and certain agricultural contexts as acidity-modifying agents.

Safety considerations: Bisulfates are corrosive and can cause burns on contact. Use appropriate personal protective equipment, avoid inhalation of dust, and store away from incompatible chemicals.

See also: Bisulfite, Sulfate, Sulfuric acid, Sodium bisulfate.