dithionate

Dithonate refers to the dianion S2O6^2-, the conjugate base of dithionic acid H2S2O6. It comprises two SO3-like units linked by a single S–S bond, with the two sulfur centers sharing the oxidation state, averaging about +5 for each sulfur. The dithionate ion forms salts with many cations, including common examples such as sodium dithionate Na2S2O6 and potassium dithionate K2S2O6. These salts are typically colorless crystals that dissolve readily in water.

Preparation and occurrence: Dithionates are usually prepared by oxidation of dithionite (S2O4^2-) or by controlled oxidation of sulfite species in aqueous media. They are more stable in neutral to mildly basic solutions and are generally less prone to reduction than dithionite. Upon heating, dithionates decompose to sulfates, and in strongly acidic conditions they can undergo hydrolysis or evolve sulfur- and sulfur-oxide–containing products.

Properties and applications: In solution, dithionate ions are relatively stable and serve as mild oxidizing agents in certain chemical contexts, often participating in redox pairs with dithionite and sulfite under specific conditions. They are primarily encountered in inorganic synthesis and analytical chemistry as reagents or counterions, and they are less common in natural environments than sulfates or sulfites. Safety considerations align with standard handling of inorganic salts: avoid inhalation of powders and store away from heat and strong reducing agents.