Electrochemical production of perchlorate as an alternative for the valorization of brines

Understanding ozone generation in electrochemical cells at mild pHs

“…Initially, most of these oxidants involved in the decomposition of ozone share the -O-Ogroup and will be denoted in this work simply as peroxo species (named in the mathematical model as 𝑆 3 ), because a full characterization will be pointless as they are known to react fast with ozone once formed and hence, they cannot be properly determined from an analytical perspective. It is important to state that to the best of the authors' knowledge, the decrease observed in the production of ozone is not noticed in previous studies, which focused on the production of peroxosalts [27][28][29]34,35], ferrates [36], total chlorinated oxoanions [37,38] or any other oxidant, and it indicates that ozone electrogeneration is a much more complex process. The kinetics of this process should depend on the concentration of this predator species and also on the concentration of ozone, and can be represented by Eq.…”

A review on the electrochemical production of chlorine dioxide from chlorates and hydrogen peroxide

“…Na2SO4 of 0.05 M and airfeeding flowrate of 2 L min −1 , the average H2O2 generation rate reached 58.9 mg L −1 h −1 cm −2 during 150 min / Effective acetylene black-PTFE cathode with PTFE film/ Solution pH (3)(4)(5)(6)(7)(8)(9)(10)(11), applied current density (5-20 mA cm −2 )/ Two-electrode undivided cell fed with air at 2 L min −1 in Na2SO4 solution of 0.05 M.…”

“…The most important family of oxidants produced with the diamond coating electrodes are the peroxospecies [3], characterized by the presence of the functional group -O-O-and which includes peroxosulfates [4], peroxophosphates [5], peroxocarbonates [6] and peroxoacetates [7]. In addition, these new powerful electrodes can promote the oxidation of chloride, not only to chlorine but also to chlorates and perchlorate [8]. These later species, from the thermodynamic point of view, are very powerful oxidants, although their action is very limited at room temperature because of kinetic considerations and it is only promoted when the temperature is raised, where they may have important uses as explosives.…”

Photocatalytic performance of Ti/MMO/ZnO at degradation of levofloxacin: Effect of pH and chloride anions

“…At basic pH, the ease of forming hydroxyl radicals, in addition to some reactive chlorine species, may have had an antagonistic effect on the degradation of LFX due to the high concentration of these reactive species, which can recombine and finally lead to the dissipation of the oxidation power with the formation of low oxidation capacity species such as oxygen. Thus combination of hydroxyl radicals can lead to the formation of hydrogen peroxide or oxygen and combination of chlorine radicals can lead to the formation of non-desired species such as chlorates or even perchlorates [41].…”