Hydrogen Peroxide Essay

The same reaction is catalysed by theenzymecatalase, found in theliver, whose main function in the organic structure is the removal of toxic byproducts ofmetabolismand the reduction ofoxidative stress. The decomposition occurs more rapidly inalkali, soacidis often added as a stabilizer. The liberation of group O and energy in the decomposition has dangerous side-effects. Spilling high concentrations of total heat peroxide on a flammable substance can cause an immediate fire, which is get along fueled by the type O released by the decomposing hydrogen peroxide.High test peroxide, or HTP (also called high-strength peroxide) must be stored in a suitable, vented container to prevent the buildup of oxygen gas, which would otherwise lead to the eventual rupture of the container. In the presence of certain catalysts, such asFe2+orTi3+, the decomposition may take a antithetic path, withfree radicalssuch as HO (hydroxyl) and HOO (hydroperoxyl) being formed. A combination ofH2O2andFe2+is known asFentons reagent.A common concentration for hydrogen peroxide is20-volume, which means that, when 1 volume of hydrogen eroxide is decomposed, it produces 20 volumes of oxygen. A20-volumeconcentration of hydrogen peroxide is equivalent to 1. 667mol/dm3(Molar resolution) or about 6%. Redox reactions In acidic solutions,H2O2is one of the most powerful oxidizers knownstronger thanchlorine,chlorine dioxide, andpotassium permanganate. Also, through catalysis,H2O2can be converted intohydroxyl radicals(OH), which are highly reactive. Oxidant/ cut back product Oxidationpotential, V Fluorine/ henry fluoride 3. 0 Ozone/Oxygen 2. 1 Hydrogen peroxide/Water 1. 8 Potassium permanganate/Manganese dioxide. centiliter dioxide/HClO 1. 5 Chlorine/Chloride 1. 4 In aqueous solutions, hydrogen peroxide can oxidize or reduce a variety of inorganic ions. When it acts as a reducing agent,oxygengas is also produced. InacidicsolutionsFe2+is oxidized toFe3+(hydrogen peroxide acting as an oxidizing agen t), 2Fe2+(aq) +H2O2+ 2H+(aq) 2Fe3+(aq) + 2H2O(l) andsulfite(SO2? 3) is oxidized tosulfate(SO2? 4). However,potassium permanganateis reduced toMn2+by acidicH2O2. Underalkalineconditions, however, some of these reactions reverse for example,Mn2+is oxidized toMn4+(asMnO2).Other examples of hydrogen peroxides action as a reducing agent are reaction withsodium hypochloriteorpotassium permanganate, which is a convenient method for preparingoxygenin the laboratory. NaOCl +H2O2O2+ NaCl +H2O 2KMnO4+ 3H2O2 2MnO2+ 2 KOH + 2H2O+ 3O2 Hydrogen peroxide is frequently used as anoxidizing agentin organic chemistry. One application is for the oxidation ofthioetherstosulfoxides. For example,methyl phenyl sulfidecan be readily oxidized in high yield tomethyl phenyl sulfoxide Ph? S? CH3+H2O2 Ph? S(O)? CH3+H2OAlkaline hydrogen peroxide is used forepoxidationof electron-deficient alkenes such asacrylic acids, and also for oxidation ofalkylboranestoalcohols, the second step ofhydroboration-oxidation. Form ation of peroxide compounds Hydrogen peroxide is a weak acid, and it can formhydroperoxideorperoxidesaltsor derivatives of many metals. For example, on addition to an aqueous solution ofchromic acid(CrO3) or acidic solutions of dichromate salts, it will form an unstable blue peroxide CrO(O2)2. In aqueous solution it rapidly decomposes to form oxygen gas and atomic number 24 salts.It can also produce peroxoanions by reaction withanions for example, reaction withboraxleads tosodium perborate, a bleach used in laundry detergents Na2B4O7+ 4H2O2+ 2 NaOH 2Na2B2O4(OH)4+H2O H2O2convertscarboxylic acids(RCOOH) into peroxy acids (RCOOOH), which are themselves used as oxidizing agents. Hydrogen peroxide reacts withacetoneto formacetone peroxide, and it interacts withozoneto formhydrogen trioxide, also known astrioxidane. Reaction withureaproducescarbamide peroxide, used for whitening teeth.An acid-base adduct withtriphenylphosphine oxideis a useful carrier forH2O2in some reactions. Alkalinit y Hydrogen peroxide can settle down form adducts with very strong acids. ThesuperacidHF/SbF5forms unstable compounds containing theH3O2+ion. Domestic uses * DilutedH2O2(between 3% and 8%) is used to bleach humanhairwhen mixed with ammonium ion hydroxide, hence the phrase peroxide blonde. * It is absorbed byskinupon contact and creates a local skincapillaryembolismthat appears as a temporary whitening of the skin. * It is used to whitenbonesthat are to be put on display. 3%H2O2is effective at treating fresh (red) blood-stains in robes and on other items. It must be applied to clothing before blood stains can be accidentally set with heated irrigate. Cold water and soap are then used to remove the peroxide treatedblood.Some horticulturalists and users ofhydroponicsadvocate the use of weak hydrogen peroxide solution in watering solutions. Its spontaneous decomposition releases oxygen that enhances a plants root development and helps to treatroot rot(cellular root devastation due to lack of oxygen) and a variety of other pests. Laboratory tests conducted by fish culturists in recent years have demonstrated that common sept hydrogen peroxide can be used safely to provide oxygen for small fish. Hydrogen peroxide releases oxygen by decomposition when it is loose tocatalystssuch asmanganese dioxide. * Hydrogen peroxide is a strong oxidizer effective in controlling sulfide and organic-related odors in wastewater entreaty and treatment systems. It is typically applied to a wastewater system where there is a retention time of 30 minutes to 5 hours before hydrogen sulfide is released.