Peracetat

Peracetat, or peracetate, refers to the salt or conjugate base of peracetic acid. The peracetate ion has the formula CH3COOO−, and common salts include sodium peracetate (NaC2H3O3) and potassium peracetate (KC2H3O3). These salts are encountered in inorganic and organic chemistry as stable, solid forms that can serve as sources of peracetic acid in solution.

Preparation and interconversion: Peracetates are typically obtained by neutralizing peracetic acid with a base, for example CH3COOOH + NaOH → NaC2H3O3 + H2O. In aqueous media, peracetates can release peracetic acid, acting as a reservoir that provides oxidizing power when needed. They can also be prepared by oxidation of acetates under basic conditions in the presence of hydrogen peroxide.

Properties and handling: Peracetates are generally white to off-white crystalline solids with good water solubility. In solution, they can hydrolyze to peracetic acid, a strong oxidizer and antimicrobial agent. As salts, peracetates are usually less volatile and easier to handle than liquid peracetic acid, but they still require appropriate safety precautions due to their oxidizing nature.

Applications: Peracetates are used as sanitizers and disinfectants in food processing, bottling, and medical device cleaning. They serve as oxidants in textile bleaching and certain water-treatment processes. In some applications, they act as a safer, more controllable source of peracetic acid, releasing active oxidant gradually in solution.

Safety: Peracetates are strong oxidizers and can irritate skin and eyes. They decompose to acetic acid and oxygen under certain conditions and should be stored away from heat, organics, and incompatibles. Proper PPE and ventilation are advised.

See also: Peracetic acid, sodium peracetate, potassium peracetate.