In ozonized water

Van der Kooij D, WAM Hijnen (1984) Substrate utilization by an oxalate-consuming Spirillum species in relation to its growth in ozonated water. Appl Environ Microbiol 47 551-559. 

Tsugura H, Watanabe T, Shimazaki H, Sameshima S (1998) Development of a monitor to simultaneously measure dissolved ozone and organic matter in ozonated water. Water Science Technology 37 285-292. 

The mechanism of decomposition of ozone in water has been the subject of numerous studies, starting from the work of Weiss [47], Among more recent studies, the mechanisms of Hoigne et al. [48] and Tomiyashu et al. [49] are the most accepted in ozone water chemistry. The main conclusion that can be drawn is that ozone stability in water is highly dependent on the presence of substances that initiate, promote, and/or inhibit its decomposition. The ozone decomposition mechanism usually assumed is given in Fig. 4 [50]. 

Y. Inoue, T. Sakai, H. Kumagai and Y. Hanaoka, High selective determination of bromate in ozonized water by using ion chromatography with postcolumn derivatization equipped with reagent preparation device. Anal. Chim. Acta, 1997, 346, 299-305. 

Yamanaka, M. Sakai, T. Kumagai, H. Inoue, Y. Specific determination of bromate and iodate in ozonized water by ion chromatography with post column derivatization and inductively-coupled plasma mass spectrometry. J. Chromatogr. 1997, 789, 259-264. 

Very low ionic and organic extractables smooth surfaces inhibit microbial fouling. Operations at 90 = C and in ozonated water (89)... 

As seen the ozone concentrations administered by injection reach 40 mg/1. Upon extracorporeal blood treatment, stimulation and circulatory treatment ozone is employed in concentrations up to 30 mg/1 whereas for colonic insufflations, external gas application in closed system, cleansing of wounds and in ozonized water production it can be used up to 100 mg/1 ... 

Aqueous Phase. In pure water, the decomposition of ozone at 20°C iavolves a complex radical chain mechanism, initiated by OH and propagated by O2 radical ions and HO radicals (25). O3 is a radical ion. 

The two main termination steps for neutral solutions are HO + HO — H2O2 + 2 O3 and HO + HO3 — H2O2 + O3 + O2. An alternative mechanism has been proposed that does not involve HO and HO but has a different initiation step (26). Three ozone molecules are destroyed for each primary event. In the presence of excess HO radical scavengers, ie, bicarbonate, the pseudo-first-order rate constant at 20°C for the initiation step is 175 X. This yields an ozone half-hfe of 66 min at pH 8. In distilled water = 50 mmol/L), the half-hfe is significantly lower, ie, 7 min. 

Sulfur Compounds. Aqueous sulfide and H2S, an odiferous compound in some waters, are oxidized rapidly (initially to sulfite and sulfurous acid) the rate constants ate 3x10 and 3 X 10 , respectively. Thiocyanate is oxidized by ozone to cyanide and sulfate via the intermediate formation of sulfite (47). 

Disinfection. Ozone is a more effective broad-spectmm disinfectant than chlorine-based compounds (105). Ozone is very effective against bacteria because even concentrations as low as 0.01 ppm are toxic to bacteria. Whereas disinfection of bacteria by chlorine involves the diffusion of HOGl through the ceU membrane, disinfection by ozone occurs with the lysing (ie, mpture) of the ceU wall. The disinfection rate depends on the type of organism and is affected by ozone concentration, temperature (106), pH, turbidity, clumping of organisms, oxidizable substances, and the type of contactor employed (107). The presence of oxidizable substances in ordinary water can retard disinfection until the initial ozone demand is satisfied, at which point rapid disinfection is observed. 

Removal of Refractory Organics. Ozone reacts slowly or insignificantly with certain micropoUutants in some source waters such as carbon tetrachloride, trichlorethylene (TCE), and perchlorethylene (PCE), as well as in chlorinated waters, ie, ttihalomethanes, THMs (eg, chloroform and bromoform), and haloacetic acids (HAAs) (eg, trichloroacetic acid). Some removal of these compounds occurs in the ozone contactor as a result of volatilization (115). Air-stripping in a packed column is effective for removing some THMs, but not CHBr. THMs can be adsorbed on granular activated carbon (GAG) but the adsorption efficiency is low. 

Pharmaceutical Industry. In the pharmaceutical industry, sterility of deionized water systems is maintained by using an ozone residual. The ozone residual concentration is maintained at >0.3 ppm ppm in the water recirculation loop. Prior to product compounding, the ozone residual is removed by contact with uvirradiaton for <1 s. Ozone also is used to oxidize pyrogens from distilled water destined for intravenous solutions. 

Electronics Industry. Organic materials on the surface of electronic components are oxidized by immersion in deionized water that contains 0.5—2 ppm ozone residual. In some cases, gaseous ozone is employed to oxidize organic films on the surface of electronic components. In this treatment process, 5—6 wt % ozone, made in an oxygen-fed generator, is required. 

Glaze, W. H., Kang, J. W., and Aieta, M. "Ozone-Hydrogen Peroxide Systems for Control of Organies in Munieipal Water Supplies Proceedings of the Second International Conference in the Role of Ozone on Water and Wastewater Treatment, TekTran International Ltd., Kitchener, Ontario, Canada, pp. 233-244, 1987. 

Disinfection - water completely free of suspended sediment, is treated with a powerful oxidizing agent usually chlorine, chlorine and ammonia (chloramine), or ozone. A residual disinfectant is left in the water to prevent reinfection. Chlorine can form harmful byproducts and has suspected links to stomach cancer and miscarriages. 

Ozone has been used eontinuously for nearly 90 years in municipal water treatment and the disinfeetion of water supplies. This praetiee began in Franee, then extended to Germany, Holland, Switzerland, and other European countries, and in reeent years to Canada. Ozone is a strong oxidizing substance with baetericidal properties similar to those of ehlorine. In test conditions it was shown that the destruetion of baeteria was between 600 and 3,000 times more rapid by ozone than by ehlorine. Further, the baeterieidal aetion of ozone is relatively unaffeeted by ehanges in pH while ehlorine effieaey is strongly dependent on the pH of the water. 

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