Hydrogen peroxide in aqueous solutions

Hydrogen peroxide in aqueous solution is a weak dibasic aeid the dissociation constant for H2O2 — -1- HO2 is 2.4 x 10 ... 

Hydrogen peroxide in aqueous solution has many uses, because the products from its reaction are either water or oxygen, which are generally innocuous. The chief use is bleaching of textiles, both natural and synthetic, and of wood pulp for paper. Other uses are the oxidation of dyestuffs, in photography and in the production of... 

An example of a reaction that is subject to homogeneous catalysis is the decomposition of hydrogen peroxide in aqueous solution ... 

Enthalpies, Entropies, and Gibb s Energies of Transition Metal Ion Oxidation-Reduction Reactions with Hydrogen Peroxide in Aqueous Solution (T = 298 K) [23]... 

Rate Constants of Transition Metal Ion Reactions with Hydrogen Peroxide in Aqueous Solutions... 

The influence of substituents on the rates of degradation of arylazo reactive dyes based on H acid, caused by the action of hydrogen peroxide in aqueous solution and on cellulose, has been investigated [43]. The results suggested that the oxidative mechanism involves attack of the dissociated form of the o-hydroxyazo grouping by the perhydroxyl radical ion [ OOH]. The mechanism of oxidation of sulphonated amino- and hydroxyarylazo dyes in sodium percarbonate solution at pH 10.6 and various temperatures has also been examined. The initial rate and apparent activation energy of these reactions were determined. The ketohydrazone form of such dyes is more susceptible to attack than the hydroxyazo tautomer [44]. 

As to catalytic reactions in homogeneous media, Moritz Traube found in his studies of the oxidation of hydrogen iodide by hydrogen peroxide in aqueous solution, that the catalyst ferrous sulfate is activated by copper sulfate (5). As to the magnitude of such effects, Price stated in 1898 (6) that the simultaneous action of iron and of copper compounds on the reaction between persulfate and hydrogen iodide causes an unexpected acceleration of the reaction, which is more than twice as great as the acceleration calculated as an additive effect of the two single catalysts. However, effects were also observed of the opposite kind,... 

Peroxynitrite is capable of initiating many of the reactions commonly attributed to hydroxyl radical, particularly under acidic conditions. Halfpenny and Robinson (1952a,b) showed that nitrous acid plus hydrogen peroxide in aqueous solutions at pH 2, which generates peroxynitrous acid, initiated the polymerization of methylmethacrylate (the precurser to Plexiglas) as well as the hydrox-ylation, nitration, and polymerization of benzene. 

Examples have not infrequently been found of reactions which involve the intervention of some impurity in the system, not at first imagined to be playing any part in the chemical change. For example, the rate of decomposition of hydrogen peroxide in aqueous solution is very variable, and Rice and Kilpatrick traced the cause of this behaviour to the fact that the decomposition is mainly determined by the catalytic action of dust particles. As a result, the view has sometimes been held that pure substances are in general very unreactive, and that velocity measurements have no absolute significance, because the reaction mechanism is quite different from what it appears to be, and involves the participation of accidental impurities. Among such impurities water occupies the most prominent position. 

The study of the chemical behavior of concentrated preparations of short-lived isotopes is complicated by the rapid production of hydrogen peroxide in aqueous solutions and the destruction of crystal lattices in solid compounds. These effects are brought about by heavy recoils of high energy alpha particles released in the decay process. 

The oxidation may also be effected by hydrogen peroxide in aqueous solution. 

Luo D, Smith S, Anderson BD. Kinetics and mechanism of the reaction of cysteine and hydrogen peroxide in aqueous solution, J Pharm Sci 2005 94(2) 314—314. 

The reduction of hydrogen peroxide in aqueous solution appears to be analogous to that in CH3CN, with the mechanism represented by the reaction of Eq. (9.70) followed by the reactions of Eqs. (9.71) and (9.72). Thus, the reduction of HOOH yields H2 and HOO- initially, in a one-electron step. The final products are the result of the reaction of HOO- and HOOH, and are analogous to those for the base-induced decomposition of HOOH.43... 

Lucking F, Koser H, Jank M, Ritter A. Iron powder, graphite and activated carbon as catalysts for the oxidation of 4-chlorophenol with hydrogen peroxide in aqueous solution. Water Res 1998 32 2607-2614. 

Amine oxides are the reaction products of tertiary amines and hydrogen peroxide. In aqueous solutions fatty amine oxides exhibit non-ionic or cationic properties depending on pH, and under neutral or alkaline conditions they exist as non-ionised hydrates. 

Sodium percarbonate, Na2C206.—The percarbonate is said4 to be formed by the electrolytic oxidation of the normal carbonate, but it has not been isolated by this method. A substance of the formula 2Na2COs,3H2Oa is obtained by the interaction of 3 molecules of hydrogen peroxide in aqueous solution and 2 molecules of sodium carbonate, the product being subsequently dried in vacuo Other percarbon-ates have been described,8 but their existence is still a subject of debate. 

Fig. 6.5 UV absorbance spectra of hydrogen peroxide in aqueous solution and in the gas phase [redrawn from Bolton and Cater (1994), p. 472, Figure 3].

The hydrogen peroxide in aqueous solution has been known for many years as a polymerization initiator. The dissociation energy801 for the O—O bond is 12.4kJ mol1 and for the O—H 26.4 kJ mol-1. 

P.O. Kvernberg, B. Pedersen (1994). Oxidation of L-ascorbic acid with hydrogen peroxide in aqueous solution. Acta Chem. Scand., 48, 646-651. 

KY Salnis, KP Mishchenko, and El Elis. Thermodynamics for the dissociation fo hydrogen peroxide in aqueous solutions. Zhur. Neorg. Khim. 2 1985-1989, 1957. 

The formation of hydrogen peroxide in aqueous solutions is almost twice as much for Pt(100) than for Pt( 111) and the poly crystalline platinum electrodes. The difference indicates either a more strongly... 

Table 8. Oxygenation of toluene by hydrogen peroxide in aqueous solution at 25 C, catalyzed by iron cyclidenes of various cavity sizes. 

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