Chemical apparatus and process disinfecting – deodorizing – preser – Process disinfecting – preserving – deodorizing – or sterilizing – Using disinfecting or sterilizing substance
Patent
1992-02-28
1994-06-28
Warden, Robert J.
Chemical apparatus and process disinfecting, deodorizing, preser
Process disinfecting, preserving, deodorizing, or sterilizing
Using disinfecting or sterilizing substance
422 7, 134 3, C23F 1100, A01N 3700
Patent
active
053244770
DESCRIPTION:
BRIEF SUMMARY
This invention relates to a process for disinfecting hard surfaces under water-hardness-stabilized and non-corrosive conditions with chlorine dioxide produced in solution by mixing of a solution of sodium chlorite and another acidic component in a generator.
Chlorine dioxide is a disinfectant which has advantages over chlorine, alkali metal or alkaline earth metal hypochlorites, organic chlorine donors and other disinfectants based on active chlorine, above all in the disinfection of bottles, containers, equipment and pipes. Chlorine dioxide forms hardly any trihalomethanes (haloforms) and hardly any relatively high molecular weight organohalogen compounds. In contrast to chlorine, chlorine dioxide does not react with phenols to form chlorophenols which are responsible for the medicated taste in the washing of mineral water and table water bottles. Nor does chlorine dioxide react with amino or ammonium compounds to form chloramines or ammonium chlorides. The effectiveness (redox potential) of chlorine dioxide, which in addition is largely unaffected by pH, is two to three times stronger than that of chlorine. However, this becomes even clearer by comparison with peracids which are also used for disinfection. In addition to greater effectiveness, this results in the use of lower concentrations and, hence, in less wastewater pollution.
In addition to good bactericidal activity, chlorine dioxide also shows good sporicidal, virucidal and algicidal properties. Chlorine dioxide is a powerful disinfectant which affords long-lasting bactericidal and bacteriostatic protection. In addition to its use as a disinfectant, chlorine dioxide--by virtue of its high oxidation potential--is also effective in eliminating unpleasant odors, tastes and colors in the treatment of water. In addition, it reacts with organic bound iron and manganese (for example in huminic and fulvic acids) and degrades carcinogenic substances, such as polycyclic aromatic compounds. In the pretreatment of raw waters or surface waters, chlorine dioxide improves flocculation so that it is preferably used for the disinfection of drinking water. Chlorine dioxide is also used for its disinfecting effect in the food and beverage industry, for example in the disinfection of filling machines, bottle washing machines and pasteurizers, as feed and return water and as washing and rinsing water. In this particular field of application, problems are caused above all by precipitations, particularly of water hardness, which begin in particular at pH values of 10.5 to 11.5 and/or at temperatures above 54.degree. C. However, unwanted precipitation of water ingredients, especially water hardness, also occur at relatively low and relatively high pH values and/or temperatures.
The process used at the present time for the production of chlorine dioxide is based on the chlorine/chlorite process (1) or on the hydrochloric acid/chlorite process (2). The chlorine/chlorite process is preferably used in municipal water treatment (large users) while the hydrochloric acid/chlorite process is used in industry (small and medium users). ##STR1##
In the chlorine/chlorite process (1), a certain excess of chlorine has to be used to obtain a complete reaction in accordance with the reaction equation, with the result that excess chlorine is always present in use. If the chlorine is used in a stoichiometric quantity, the reaction is always incomplete.
In the hydrochloric acid/chlorite process (2), the chlorine dioxide solutions obtained show less contamination, although the maximum theoretical yield, based on chlorite, is limited to 80% by the stoichiometry of the reaction equation. In addition to hydrochloric acid, other acids may also be used.
The three-component process (3) is based on the chlorine/chlorite process (1) and, through the use of additional acid, guarantees a substantially complete chlorite conversion due to the reduction in the pH value.
The disadvantage of the processes industrially used at the present time lies in their corrosive effect because hydrochloric acid is us
REFERENCES:
patent: 4504442 (1985-03-01), Rosenblatt et al.
patent: 4681739 (1987-07-01), Rosenblatt et al.
patent: 4731193 (1988-03-01), Mason et al.
patent: 4747975 (1988-05-01), Ritter
Webster's New Collegiate Dictionary, p. 617.
Falter Wolfgang
Grosse-Boewing Walter
Schroeder Karl-Heinz
Dawson E. Leigh
Henkel Komnmanditgesellschaft auf Aktien
Jaeschke Wayne C.
Millson Jr. Henry E.
Szoke Ernest G.
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