Hydrogen Peroxide Essay Example for Free

total heat Peroxide EssayThe same reaction is catalysed by theenzymecatalase, found in theliver, whose main function in the body 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 oxygen and energy in the decomposition has dangerous side-effects. Spilling high concentrations of total heat bleach on a flammable substance can cause an immediate fire, which is further fueled by the oxygen released by the decomposing total heat peroxide. High test peroxide, or HTP (also called high-strength peroxide) bulwarkdiness 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 different path, withfree radicalssuch as HO (hydroxyl) and HOO (hydroperoxyl) being craped. A combin ation ofH2O2andFe2+is known asFentons reagent.A common concentration for total heat 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 solution) 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/Reduced product Oxidationpotential, V Fluorine/Hydrogen fluoride 3. 0 Ozone/Oxygen 2. 1 Hydrogen peroxide/Water 1. 8 Potassium permanganate/Manganese dioxide.Chlorine dioxide/HClO 1. 5 Chlorine/Chloride 1. 4 In sedimentary 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 play acting as an oxidizing agent), 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 purloin 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 at ease method for preparingoxygenin the laboratory. NaOCl +H2O2O2+ NaCl +H2O 2KMnO4+ 3H2O2 2MnO2+ 2 KOH + 2H2O+ 3O2 Hydrogen peroxide is frequently employ 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 flavou r ofhydroboration-oxidation. Formation 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 chromium salts.It can also produce peroxoanions by reaction withanions for example, reaction withboraxleads tosodium perborate, a bleach used in backwash 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. Alkalinity Hydrogen peroxide can still form adducts with very strong acids. ThesuperacidHF/SbF5forms unstable compounds containing theH3O2+ion. Domestic uses * DilutedH2O2(between 3% and 8%) is used to bleach kind-heartedhairwhen mixed withammonium hydroxide, hence the phrase peroxide blonde. * It is absorbed byskinupon contact and creates a local skincapillaryintercalationthat appears as a temporary whitening of the skin. * It is used to whitenbonesthat are to be put on display. 3%H2O2is effective at treating clean-living (red) blood-stains in clothing and on other items. It must be applied to clothing before blood stains can be accidentally set with heat up water. 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 closing due to lack of oxygen) and a variety of other pests. Laboratory tests conducted by fish culturists in recent years have demonstrated that common abode hydrogen peroxide can be used safely to provide oxygen for small fish. Hydrogen peroxide releases oxygen by decomposition when it is opened tocatalystssuch asmanganese dioxide. * Hydrogen peroxide is a strong oxidizer effective in controlling sulfide and organic-related odors in wastewater appeal 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.