Hydrogen peroxide - wikipedia Hydrogen peroxide Hydrogen peroxide Names IUPAC name Hydrogen peroxide Other names Dioxidane Oxidanyl Perhydroxic acid 0 - hydroxyol Dihydrogen dioxide Identifiers CAS Number 7722 - 84 - 1 3D model ( JSmol ) Interactive image ChEBI CHEBI : 16240 ChemSpider 763 ECHA InfoCard 100.028. 878 EC Number 231 - 765 - 0 IUPHAR / BPS 2448 KEGG D00008 PubChem CID 784 RTECS number MX0900000 ( > 90 % soln. ) MX0887000 ( > 30 % soln. ) UNII BBX060AN9V UN number 2015 ( > 60 % soln. ) 2014 ( 20 -- 60 % soln. ) 2984 ( 8 -- 20 % soln. ) InChI InChI = 1S / H2O2 / c1 - 2 / h1 - 2H Key : MHAJPDPJQMAIIY - UHFFFAOYSA - N InChI = 1 / H2O2 / c1 - 2 / h1 - 2H Key : MHAJPDPJQMAIIY - UHFFFAOYAL SMILES OO Properties Chemical formula H O Molar mass 34.0147 g / mol Appearance Very light blue color ; colorless in solution Odor slightly sharp Density 1.11 g / cm ( 20 ° C, 30 % ( w / w ) solution ) 1.450 g / cm ( 20 ° C, pure ) Melting point − 0.43 ° C ( 31.23 ° F ; 272.72 K ) Boiling point 150.2 ° C ( 302.4 ° F ; 423.3 K ) ( decomposes ) Solubility in water Miscible Solubility soluble in ether, alcohol insoluble in petroleum ether Vapor pressure 5 mmHg ( 30 ° C ) Acidity ( pK ) 11.75 Magnetic susceptibility ( χ ) − 17.7 10 cm / mol Refractive index ( n ) 1.4061 Viscosity 1.245 c P ( 20 ° C ) Dipole moment 2.26 D Thermochemistry Specific heat capacity ( C ) 1.267 J / ( g K ) ( gas ) 2.619 J / ( g K ) ( liquid ) Std enthalpy of formation ( Δ H ) − 187.80 kJ / mol Pharmacology ATC code A01AB02 ( WHO ) D08AX01 ( WHO ), S02AA06 ( WHO ) Hazards Safety data sheet ICSC 0164 ( > 60 % soln. ) GHS pictograms GHS signal word danger GHS hazard statements H271, H302, H314, H332, H335, H412 GHS precautionary statements P280, P305 + 351 + 338, P310 NFPA 704 0 OX Flash point Non-flammable Lethal dose or concentration ( LD, LC ) : LD ( median dose ) 1518 mg / kg 2000 mg / kg ( oral, mouse ) LC ( median concentration ) 1418 ppm ( rat, 4 hr ) LC ( lowest published ) 227 ppm ( mouse ) US health exposure limits ( NIOSH ) : PEL ( Permissible ) TWA 1 ppm ( 1.4 mg / m ) REL ( Recommended ) TWA 1 ppm ( 1.4 mg / m ) IDLH ( Immediate danger ) 75 ppm Related compounds Related compounds Water Ozone Hydrazine Hydrogen disulfide Dioxygen difluoride Except where otherwise noted, data are given for materials in their standard state ( at 25 ° C ( 77 ° F ), 100 kPa ). Y verify ( what is ? ) Infobox references Hydrogen peroxide is a chemical compound with the formula H 2O 2. In its pure form, it is a pale blue, clear liquid, slightly more viscous than water. Hydrogen peroxide is the simplest peroxide ( a compound with an oxygen -- oxygen single bond ). It is used as an oxidizer, bleaching agent and antiseptic. Concentrated hydrogen peroxide, or `` high - test peroxide '', is a reactive oxygen species and has been used as a propellant in rocketry. Its chemistry is dominated by the nature of its unstable peroxide bond. Hydrogen peroxide is unstable and slowly decomposes in the presence of base or a catalyst. Because of its instability, hydrogen peroxide is typically stored with a stabilizer in a weakly acidic solution. Hydrogen peroxide is found in biological systems including the human body. Enzymes that use or decompose hydrogen peroxide are classified as peroxidases. Contents 1 Properties 1.1 Aqueous solutions 1.2 Structure 1.3 Comparison with analogues 2 Discovery 3 Manufacture 3.1 Availability 4 Reactions 4.1 Decomposition 4.2 Redox reactions 4.3 Organic reactions 4.4 Precursor to other peroxide compounds 5 Biological function 6 Uses 6.1 Bleaching 6.2 Detergents 6.3 Production of organic compounds 6.4 Disinfectant 6.4. 1 Cosmetic applications 6.4. 2 Use in alternative medicine 6.5 Propellant 6.6 Other uses 7 Safety 7.1 Historical incidents 8 See also 9 References 10 External links Properties The boiling point of H 2O 2 has been extrapolated as being 150.2 ° C, approximately 50 ° C higher than water. In practice, hydrogen peroxide will undergo potentially explosive thermal decomposition if heated to this temperature. It may be safely distilled at lower temperatures under reduced pressure. Aqueous solutions In aqueous solutions hydrogen peroxide differs from the pure material due to the effects of hydrogen bonding between water and hydrogen peroxide molecules. Hydrogen peroxide and water form a eutectic mixture, exhibiting freezing - point depression ; pure water has a melting point of 0 ° C and pure hydrogen peroxide of − 0.43 ° C. The boiling point of the same mixtures is also depressed in relation with the mean of both boiling points ( 125.1 ° C ). It occurs at 114 ° C. This boiling point is 14 ° C greater than that of pure water and 36.2 ° C less than that of pure hydrogen peroxide. Phase diagram of H 2O 2 and water : Area above blue line is liquid. Dotted lines separate solid + liquid phases from solid + solid phases. Density of aqueous solution of H O H O ( w / w ) Density ( g / cm ) Temperature ( ° C ) 3 % 1.0095 15 27 % 1.10 20 35 % 1.13 20 50 % 1.20 20 70 % 1.29 20 75 % 1.33 20 96 % 1.42 20 98 % 1.43 20 100 % 1.45 20 Structure Hydrogen peroxide ( H 2O 2 ) is a nonplanar molecule with ( twisted ) C symmetry. Although the O − O bond is a single bond, the molecule has a relatively high rotational barrier of 2460 cm ( 29.45 kJ / mol ) ; for comparison, the rotational barrier for ethane is 12.5 kJ / mol. The increased barrier is ascribed to repulsion between the lone pairs of the adjacent oxygen atoms and results in hydrogen peroxide displaying atropisomerism. The molecular structures of gaseous and crystalline H 2O 2 are significantly different. This difference is attributed to the effects of hydrogen bonding, which is absent in the gaseous state. Crystals of H 2O 2 are tetragonal with the space group D4 4P4 2. Structure and dimensions of H O in the gas phase Structure and dimensions of H O in the solid ( crystalline ) phase Properties of H O and its analogues Name Formula Molar mass ( g / mol ) T ( ° C ) T ( ° C ) Hydrogen peroxide HOOH 34.01 − 0.43 150.2 * Water HOH 18.02 0.00 99.98 Hydrogen disulfide HSSH 66.15 − 89.6 70.7 Hydrazine H NNH 32.05 114 Hydroxylamine NH OH 33.03 33 58 * Diphosphane H PPH 65.98 − 99 63.5 * Comparison with analogues Hydrogen peroxide has several structural analogues with H − X − X − H bonding arrangements ( water also shown for comparison ). It has the highest ( theoretical ) boiling point of this series ( X = O, N, S ). Its melting point is also fairly high, being comparable to that of hydrazine and water, with only hydroxylamine crystallising significantly more readily, indicative of particularly strong hydrogen bonding. Diphosphane and hydrogen disulfide exhibit only weak hydrogen bonding and have little chemical similarity to hydrogen peroxide. All of these analogues are thermodynamically unstable. Structurally, the analogues all adopt similar skewed structures, due to repulsion between adjacent lone pairs. Discovery Alexander von Humboldt synthesized one of the first synthetic peroxides, barium peroxide, in 1799 as a by - product of his attempts to decompose air. Nineteen years later Louis Jacques Thénard recognized that this compound could be used for the preparation of a previously unknown compound, which he described as oxidized water -- subsequently known as hydrogen peroxide. An improved version of this process used hydrochloric acid, followed by addition of sulfuric acid to precipitate the barium sulfate byproduct. Thénard 's process was used from the end of the 19th century until the middle of the 20th century. Thénard and Joseph Louis Gay - Lussac synthesized sodium peroxide in 1811. The bleaching effect of peroxides and their salts on natural dyes became known around that time, but early attempts of industrial production of peroxides failed, and the first plant producing hydrogen peroxide was built in 1873 in Berlin. The discovery of the synthesis of hydrogen peroxide by electrolysis with sulfuric acid introduced the more efficient electrochemical method. It was first implemented into industry in 1908 in Weißenstein, Carinthia, Austria. The anthraquinone process, which is still used, was developed during the 1930s by the German chemical manufacturer IG Farben in Ludwigshafen. The increased demand and improvements in the synthesis methods resulted in the rise of the annual production of hydrogen peroxide from 35,000 tonnes in 1950, to over 100,000 tonnes in 1960, to 300,000 tonnes by 1970 ; by 1998 it reached 2.7 million tonnes. Pure hydrogen peroxide was long believed to be unstable, as early attempts to separate it from the water, which is present during synthesis, all failed. This instability was due to traces of impurities ( transition - metal salts ), which catalyze the decomposition of the hydrogen peroxide. Pure hydrogen peroxide was first obtained in 1894 -- almost 80 years after its discovery -- by Richard Wolffenstein, who produced it by vacuum distillation. Determination of the molecular structure of hydrogen peroxide proved to be very difficult. In 1892 the Italian physical chemist Giacomo Carrara ( 1864 -- 1925 ) determined its molecular mass by freezing - point depression, which confirmed that its molecular formula is H O. At least half a dozen hypothetical molecular structures seemed to be consistent with the available evidence. In 1934, the English mathematical physicist William Penney and the Scottish physicist Gordon Sutherland proposed a molecular structure for hydrogen peroxide that was very similar to the presently accepted one. Manufacture Previously, hydrogen peroxide was prepared industrially by hydrolysis of the ammonium peroxydisulfate, which was itself obtained by the electrolysis of a solution of ammonium bisulfate ( NH 4HSO 4 ) in sulfuric acid : ( NH 4 ) 2O 8 + 2 H 2O → H 2O 2 + 2 ( NH 4 ) HSO Today, hydrogen peroxide is manufactured almost exclusively by the anthraquinone process, which was formalized in 1936 and patented in 1939. It begins with the reduction of an anthraquinone ( such as 2 - ethylanthraquinone or the 2 - amyl derivative ) to the corresponding anthrahydroquinone, typically by hydrogenation on a palladium catalyst ; the anthrahydroquinone then undergoes autoxidation to regenerate the starting anthraquinone, with hydrogen peroxide as a by - product. Most commercial processes achieve oxidation by bubbling compressed air through a solution of the derivatized anthracene, whereby the oxygen present in the air reacts with the labile hydrogen atoms ( of the hydroxy groups ), giving hydrogen peroxide and regenerating the anthraquinone. Hydrogen peroxide is then extracted, and the anthraquinone derivative is reduced back to the dihydroxy ( anthracene ) compound using hydrogen gas in the presence of a metal catalyst. The cycle then repeats itself. The simplified overall equation for the process is simple : H 2 + O 2 → H 2O The economics of the process depend heavily on effective recycling of the quinone ( which is expensive ) and extraction solvents, and of the hydrogenation catalyst. A process to produce hydrogen peroxide directly from the elements has been of interest for many years. Direct synthesis is difficult to achieve, as the reaction of hydrogen with oxygen thermodynamically favours production of water. Systems for direct synthesis have been developed, most of which are based around finely dispersed metal catalysts. None of these has yet reached a point where they can be used for industrial - scale synthesis. ISO tank container for hydrogen peroxide transportation Availability Hydrogen peroxide is most commonly available as a solution in water. For consumers, it is usually available from pharmacies at 3 and 6 wt % concentrations. The concentrations are sometimes described in terms of the volume of oxygen gas generated ; one milliliter of a 20 - volume solution generates twenty milliliters of oxygen gas when completely decomposed. For laboratory use, 30 wt % solutions are most common. Commercial grades from 70 % to 98 % are also available, but due to the potential of solutions of more than 68 % hydrogen peroxide to be converted entirely to steam and oxygen ( with the temperature of the steam increasing as the concentration increases above 68 % ) these grades are potentially far more hazardous and require special care in dedicated storage areas. Buyers must typically allow inspection by commercial manufacturers. In 1994, world production of H 2O 2 was around 1.9 million tonnes and grew to 2.2 million in 2006, most of which was at a concentration of 70 % or less. In that year bulk 30 % H 2O 2 sold for around 0.54 USD / kg, equivalent to 1.50 USD / kg ( 0.68 USD / lb ) on a `` 100 % basis ''. Hydrogen peroxide occurs in surface water, groundwater and in the atmosphere. It forms upon illumination or natural catalytic action by substances contained in water. Sea water contains 0.5 to 14 μg / L of hydrogen peroxide, freshwater 1 to 30 μg / L and air 0.1 to 1 parts per billion. Reactions Decomposition Hydrogen peroxide is thermodynamically unstable and decomposes to form water and oxygen with a ΔH of − 98.2 kJ / mol and a Δ S of 70.5 J / ( mol K ) : 2 H 2O 2 → 2 H 2O + O The rate of decomposition increases with rising temperature, concentration and pH, with cool, dilute, acidic solutions showing the best stability. Decomposition is catalysed by various compounds, including most transition metals and their compounds ( e.g. manganese dioxide, silver, and platinum ). Certain metal ions, such as Fe 2 + or Ti 3 +, can cause the decomposition to take a different path, with free radicals such as ( HO ) and ( HOO ) being formed. Non-metallic catalysts include potassium iodide, which reacts particularly rapidly and forms the basis of the elephant toothpaste experiment. Hydrogen peroxide can also be decomposed biologically by the enzyme catalase. The decomposition of hydrogen peroxide liberates oxygen and heat ; this can be dangerous, as spilling high - concentration hydrogen peroxide on a flammable substance can cause an immediate fire. Redox reactions Hydrogen peroxide exhibits oxidizing and reducing properties, depending on pH. In acidic solutions, H 2O 2 is one of the most powerful oxidizers known -- stronger than chlorine, chlorine dioxide, and potassium permanganate. Also, through catalysis, H 2O 2 can be converted into hydroxyl radicals ( OH ), which are highly reactive. Oxidant / reduced product Oxidation potential, V fluorine / hydrogen fluoride 3.0 ozone / oxygen hydrogen peroxide / water 1.8 potassium permanganate / manganese dioxide 1.7 chlorine dioxide / HClO 1.5 chlorine / chloride 1.4 In acidic solutions Fe 2 + is oxidized to Fe 3 + ( hydrogen peroxide acting as an oxidizing agent ) : 2 Fe 2 + ( aq ) + H 2O 2 + 2 H + ( aq ) → 2 Fe 3 + ( aq ) + 2 H 2O ( l ) and sulfite ( SO 2 − 3 ) is oxidized to sulfate ( SO 2 − 4 ). However, potassium permanganate is reduced to Mn 2 + by acidic H 2O 2. Under alkaline conditions, however, some of these reactions reverse ; for example, Mn 2 + is oxidized to Mn 4 + ( as MnO 2 ). In basic solution, hydrogen peroxide can reduce a variety of inorganic ions. When it acts as a reducing agent, oxygen gas is also produced. For example, hydrogen peroxide will reduce sodium hypochlorite and potassium permanganate, which is a convenient method for preparing oxygen in the laboratory : NaOCl + H 2O 2 → O 2 + NaCl + H 2O 2 KMnO 4 + 3 H 2O 2 → 2 MnO 2 + 2 KOH + 2 H 2O + 3 O Organic reactions Hydrogen peroxide is frequently used as an oxidizing agent. Illustrative is oxidation of thioethers to sulfoxides : Ph − S − CH 3 + H 2O 2 → Ph − S ( O ) − CH 3 + H 2O Alkaline hydrogen peroxide is used for epoxidation of electron - deficient alkenes such as acrylic acid derivatives, and for the oxidation of alkylboranes to alcohols, the second step of hydroboration - oxidation. It is also the principal reagent in the Dakin oxidation process. Precursor to other peroxide compounds Hydrogen peroxide is a weak acid, forming hydroperoxide or peroxide salts with many metals. It also converts metal oxides into the corresponding peroxides. For example, upon treatment with hydrogen peroxide, chromic acid ( CrO 3 + H 2SO 4 ) forms an unstable blue peroxide CrO ( O 2 ) 2. This kind of reaction is used industrially to produce peroxoanions. For example, reaction with borax leads to sodium perborate, a bleach used in laundry detergents : Na 4O 7 + 4 H 2O 2 + 2 NaOH → 2 Na 2O 4 ( OH ) 4 + H 2O 2O 2 converts carboxylic acids ( RCO H ) into peroxy acids ( RC ( O ) O H ), which are themselves used as oxidizing agents. Hydrogen peroxide reacts with acetone to form acetone peroxide and with ozone to form trioxidane. Hydrogen peroxide forms stable adducts with urea ( hydrogen peroxide - urea ), sodium carbonate ( sodium percarbonate ) and other compounds. An acid - base adduct with triphenylphosphine oxide is a useful `` carrier '' for H 2O 2 in some reactions. The peroxide anion is a stronger nucleophile than hydroxide and displaces hydroxyl from oxyanions e.g. forming perborates and percarbonates. Sodium perborate and sodium percarbonate are important consumer and industrial bleaching agents ; they stabilize hydrogen peroxide and limit side reactions ( e.g. reduction and decomposition note below ). The peroxide anion forms an adduct with urea, hydrogen peroxide -- urea. Hydrogen peroxide is both an oxidizing agent and reducing agent. The oxidation of hydrogen peroxide by sodium hypochlorite yields singlet oxygen. The net reaction of a ferric ion with hydrogen peroxide is a ferrous ion and oxygen. This proceeds via single electron oxidation and hydroxyl radicals. This is used in some organic chemistry oxidations, e.g. in the Fenton 's reagent. Only catalytic quantities of iron ion is needed since peroxide also oxidizes ferrous to ferric ion. The net reaction of hydrogen peroxide and permanganate or manganese dioxide is manganous ion ; however, until the peroxide is spent some manganous ions are reoxidized to make the reaction catalytic. This forms the basis for common monopropellant rockets. Biological function Ascaridole Hydrogen peroxide is formed in human and animals as a short - lived product in biochemical processes and is toxic to cells. The toxicity is due to oxidation of proteins, membrane lipids and DNA by the peroxide ions. The class of biological enzymes called SOD ( superoxide dismutase ) is developed in nearly all living cells as an important antioxidant agent. They promote the disproportionation of superoxide into oxygen and hydrogen peroxide, which is then rapidly decomposed by the enzyme catalase to oxygen and water. 2 O 2 − + 2 H + → SOD H 2 O 2 ⏞ + hydrogen peroxide O 2 ⏞ oxygen ( displaystyle ( ce ( ( 2O2 ^ ( - ) ) + 2H+ - > ( ( ce ( SOD ) ) ) overbrace ( H2O2 ) ^ ( hydrogen peroxide ) + overbrace ( O2 ) ^ ( oxygen ) ) ) ) Formation of hydrogen peroxide by superoxide dismutase ( SOD ) Peroxisomes are organelles found in virtually all eukaryotic cells. They are involved in the catabolism of very long chain fatty acids, branched chain fatty acids, D - amino acids, polyamines, and biosynthesis of plasmalogens, etherphospholipids critical for the normal function of mammalian brains and lungs. Upon oxidation, they produce hydrogen peroxide in the following process : R − CH 2 − CH 2 − CO − SCoA + O 2 → FAD R − CH = CH − CO − SCoA + H 2 O 2 ⏞ hydrogen peroxide ( displaystyle ( ce ( ( R - CH2 - CH2 - CO-SCoA ) + O2 - > ( ( ce ( FAD ) ) ) ( R - CH = CH - CO-SCoA ) + overbrace ( H2O2 ) ^ ( hydrogen peroxide ) ) ) ) FAD = flavin adenine dinucleotide Catalase, another peroxisomal enzyme, uses this H O to oxidize other substrates, including phenols, formic acid, formaldehyde, and alcohol, by means of the peroxidation reaction : H 2 O 2 + R ′ H 2 ⟶ R ′ + 2 H 2 O ( displaystyle ( ce ( ( H2O2 ) + R'H2 - > ( R ' ) + 2H2O ) ) ), thus eliminating the poisonous hydrogen peroxide in the process. This reaction is important in liver and kidney cells, where the peroxisomes neutralize various toxic substances that enter the blood. Some of the ethanol humans drink is oxidized to acetaldehyde in this way. In addition, when excess H O accumulates in the cell, catalase converts it to H O through this reaction : H 2 O 2 ⏞ → CAT hydrogen peroxide 1 2 O 2 + H 2 O ( displaystyle ( ce ( overbrace ( H2O2 ) ^ ( hydrogen peroxide ) - > ( ( ce ( CAT ) ) ) ( 1 / 2O2 ) + H2O ) ) ) Another origin of hydrogen peroxide is the degradation of adenosine monophosphate which yields hypoxanthine. Hypoxanthine is then oxidatively catabolized first to xanthine and then to uric acid, and the reaction is catalyzed by the enzyme xanthine oxidase : Degradation of hypoxanthine to uric acid to form hydrogen peroxide. XO = xanthinoxidase Australian bombardier beetle The degradation of guanosine monophosphate yields xanthine as an intermediate product which is then converted in the same way to uric acid with the formation of hydrogen peroxide. Eggs of sea urchin, shortly after fertilization by a sperm, produce hydrogen peroxide. It is then quickly dissociated to OH radicals. The radicals serve as initiator of radical polymerization, which surrounds the eggs with a protective layer of polymer. The bombardier beetle has a device which allows it to shoot corrosive and foul - smelling bubbles at its enemies. The beetle produces and stores hydroquinone and hydrogen peroxide, in two separate reservoirs in the rear tip of its abdomen. When threatened, the beetle contracts muscles that force the two reactants through valved tubes into a mixing chamber containing water and a mixture of catalytic enzymes. When combined, the reactants undergo a violent exothermic chemical reaction, raising the temperature to near the boiling point of water. The boiling, foul - smelling liquid partially becomes a gas ( flash evaporation ) and is expelled through an outlet valve with a loud popping sound. Hydrogen peroxide is a signaling molecule of plant defense against pathogens. Hydrogen peroxide has roles as a signalling molecule in the regulation of a wide variety of biological processes. The compound is a major factor implicated in the free - radical theory of aging, based on how readily hydrogen peroxide can decompose into a hydroxyl radical and how superoxide radical byproducts of cellular metabolism can react with ambient water to form hydrogen peroxide. These hydroxyl radicals in turn readily react with and damage vital cellular components, especially those of the mitochondria. At least one study has also tried to link hydrogen peroxide production to cancer. These studies have frequently been quoted in fraudulent treatment claims. The amount of hydrogen peroxide in biological systems can be assayed using a fluorimetric assay. Uses Bleaching About 60 % of the world 's production of hydrogen peroxide is used for pulp - and paper - bleaching. Detergents The second major industrial application is the manufacture of sodium percarbonate and sodium perborate, which are used as mild bleaches in laundry detergents. Sodium percarbonate, which is an adduct of sodium carbonate and hydrogen peroxide, is the active ingredient in such products as OxiClean and Tide laundry detergent. When dissolved in water, it releases hydrogen peroxide and sodium carbonate : 2 Na 2 CO 3 ⋅ 3 2 H 2 O 2 ⟶ 2 Na 2 CO 3 + 3 H 2 O 2 ( displaystyle ( ce ( 2Na2CO3. 3 / 2H2O2 - > ( 2Na2CO3 ) + 3 H2O2 ) ) ) Production of organic compounds It is used in the production of various organic peroxides with dibenzoyl peroxide being a high volume example. It is used in polymerisations, as a flour bleaching agent and as a treatment for acne. Peroxy acids, such as peracetic acid and meta - chloroperoxybenzoic acid are also produced using hydrogen peroxide. Hydrogen peroxide has been used for creating organic peroxide - based explosives, such as acetone peroxide. Disinfectant Skin shortly after exposure to 35 % H 2O Hydrogen peroxide is used in certain waste - water treatment processes to remove organic impurities. In advanced oxidation processing, the Fenton reaction gives highly reactive OH. These hydroxyl radicals degrade organic compounds, including those that are ordinarily robust, such as aromatic or halogenated compounds. It can also oxidize sulfur based compounds present in the waste ; which is beneficial as it generally reduces their odour. Hydrogen peroxide can be used for the sterilization of various surfaces, including surgical tools and may be deployed as a vapour ( VHP ) for room sterilization. H O demonstrates broad - spectrum efficacy against viruses, bacteria, yeasts, and bacterial spores. In general, greater activity is seen against Gram - positive than Gram - negative bacteria ; however, the presence of catalase or other peroxidases in these organisms can increase tolerance in the presence of lower concentrations. Higher concentrations of H O ( 10 to 30 % ) and longer contact times are required for sporicidal activity. Hydrogen peroxide is seen as an environmentally safe alternative to chlorine - based bleaches, as it degrades to form oxygen and water and it is generally recognized as safe as an antimicrobial agent by the U.S. Food and Drug Administration ( FDA ). Historically hydrogen peroxide was used for disinfecting wounds, partly because of its low cost and prompt availability compared to other antiseptics. It is now thought to inhibit healing and to induce scarring because it destroys newly formed skin cells. Only a very low concentration of H O can induce healing, and only if not repeatedly applied. Surgical use can lead to gas embolism formation. Despite this it is still used for wound treatment in many developing countries. Dermal exposure to dilute solutions of hydrogen peroxide cause whitening or bleaching of the skin due to microembolism caused by oxygen bubbles in the capillaries. Cosmetic applications Diluted H 2O 2 ( between 1.9 % and 12 % ) mixed with ammonium hydroxide is used to bleach human hair. The chemical 's bleaching property lends its name to the phrase `` peroxide blonde ''. Hydrogen peroxide is also used for tooth whitening. It can be found in most whitening toothpastes. Hydrogen peroxide has shown positive results involving teeth lightness and chroma shade parameters. It works by oxidizing colored pigments onto the enamel where the shade of the tooth can indeed become lighter. Hydrogen peroxide can be mixed with baking soda and salt to make a home - made toothpaste. Hydrogen peroxide may be used to treat acne, although benzoyl peroxide is a more common treatment. Use in alternative medicine Practitioners of alternative medicine have advocated the use of hydrogen peroxide for various conditions, including emphysema, influenza, AIDS and cancer, although there is no evidence of effectiveness and in some cases it may even be fatal. The practice calls for the daily consumption of hydrogen peroxide, either orally or by injection and is, in general, based around two precepts. First, that hydrogen peroxide is naturally produced by the body to combat infection ; and second, that human pathogens ( including cancer : See Warburg hypothesis ) are anaerobic and can not survive in oxygen - rich environments. The ingestion or injection of hydrogen peroxide is therefore believed to kill disease by mimicking the immune response in addition to increasing levels of oxygen within the body. This makes it similar to other oxygen - based therapies, such as ozone therapy and hyperbaric oxygen therapy. Both the effectiveness and safety of hydrogen peroxide therapy is scientifically questionable. Hydrogen peroxide is produced by the immune system but in a carefully controlled manner. Cells called phagocytes engulf pathogens and then use hydrogen peroxide to destroy them. The peroxide is toxic to both the cell and the pathogen and so is kept within a special compartment, called a phagosome. Free hydrogen peroxide will damage any tissue it encounters via oxidative stress ; a process which also has been proposed as a cause of cancer. Claims that hydrogen peroxide therapy increase cellular levels of oxygen have not been supported. The quantities administered would be expected to provide very little additional oxygen compared to that available from normal respiration. It should also be noted that it is difficult to raise the level of oxygen around cancer cells within a tumour, as the blood supply tends to be poor, a situation known as tumor hypoxia. Large oral doses of hydrogen peroxide at a 3 % concentration may cause irritation and blistering to the mouth, throat, and abdomen as well as abdominal pain, vomiting, and diarrhea. Intravenous injection of hydrogen peroxide has been linked to several deaths. The American Cancer Society states that `` there is no scientific evidence that hydrogen peroxide is a safe, effective or useful cancer treatment. '' Furthermore, the therapy is not approved by the U.S. FDA. Propellant For more details on this topic, see High - test peroxide. Rocket - belt hydrogen - peroxide propulsion system used in a jet pack High - concentration H 2O 2 is referred to as `` high - test peroxide '' ( HTP ). It can be used either as a monopropellant ( not mixed with fuel ) or as the oxidizer component of a bipropellant rocket. Use as a monopropellant takes advantage of the decomposition of 70 -- 98 % concentration hydrogen peroxide into steam and oxygen. The propellant is pumped into a reaction chamber, where a catalyst, usually a silver or platinum screen, triggers decomposition, producing steam at over 600 ° C ( 1,112 ° F ), which is expelled through a nozzle, generating thrust. H 2O 2 monopropellant produces a maximal specific impulse ( I ) of 161 s ( 1.6 kN s / kg ). Peroxide was the first major monopropellant adopted for use in rocket applications. Hydrazine eventually replaced hydrogen - peroxide monopropellant thruster applications primarily because of a 25 % increase in the vacuum specific impulse. Hydrazine ( toxic ) and hydrogen peroxide ( less - toxic ( ACGIH TLV 0.01 and 1 ppm respectively ) ) are the only two monopropellants ( other than cold gases ) to have been widely adopted and utilized for propulsion and power applications. The Bell Rocket Belt, reaction - control systems for X-1, X-15, Centaur, Mercury, Little Joe, as well as the turbo - pump gas generators for X-1, X-15, Jupiter, Redstone and Viking used hydrogen peroxide as a monopropellant. As a bipropellant, H 2O 2 is decomposed to burn a fuel as an oxidizer. Specific impulses as high as 350 s ( 3.5 kN s / kg ) can be achieved, depending on the fuel. Peroxide used as an oxidizer gives a somewhat lower I than liquid oxygen, but is dense, storable, noncryogenic and can be more easily used to drive gas turbines to give high pressures using an efficient closed cycle. It can also be used for regenerative cooling of rocket engines. Peroxide was used very successfully as an oxidizer in World War II German rocket motors ( e.g. T - Stoff, containing oxyquinoline stabilizer, for both the Walter HWK 109 - 500 Starthilfe RATO externally podded monopropellant booster system, and for the Walter HWK 109 - 509 rocket motor series used for the Me 163 B ), most often used with C - Stoff in a self - igniting hypergolic combination, and for the low - cost British Black Knight and Black Arrow launchers. In the 1940s and 1950s, the Hellmuth Walter KG - conceived turbine used hydrogen peroxide for use in submarines while submerged ; it was found to be too noisy and require too much maintenance compared to diesel - electric power systems. Some torpedoes used hydrogen peroxide as oxidizer or propellant. Operator error in the use of hydrogen - peroxide torpedoes was named as possible causes for the sinkings of HMS Sidon and the Russian submarine Kursk. SAAB Underwater Systems is manufacturing the Torpedo 2000. This torpedo, used by the Swedish Navy, is powered by a piston engine propelled by HTP as an oxidizer and kerosene as a fuel in a bipropellant system. Other uses Chemiluminescence of cyalume, as found in a glow stick Hydrogen peroxide has various domestic uses, primarily as a cleaning and disinfecting agent. Glow sticks Hydrogen peroxide reacts with certain di - esters, such as phenyl oxalate ester ( cyalume ), to produce chemiluminescence ; this application is most commonly encountered in the form of glow sticks. Horticulture Some horticulturalists and users of hydroponics advocate the use of weak hydrogen peroxide solution in watering solutions. Its spontaneous decomposition releases oxygen that enhances a plant 's root development and helps to treat root rot ( cellular root death due to lack of oxygen ) and a variety of other pests. Fish aeration Laboratory tests conducted by fish culturists in recent years have demonstrated that common household hydrogen peroxide can be used safely to provide oxygen for small fish. The hydrogen peroxide releases oxygen by decomposition when it is exposed to catalysts such as manganese dioxide. Safety Regulations vary, but low concentrations, such as 6 %, are widely available and legal to buy for medical use. Most over-the - counter peroxide solutions are not suitable for ingestion. Higher concentrations may be considered hazardous and are typically accompanied by a Material Safety Data Sheet ( MSDS ). In high concentrations, hydrogen peroxide is an aggressive oxidizer and will corrode many materials, including human skin. In the presence of a reducing agent, high concentrations of H 2O 2 will react violently. High - concentration hydrogen peroxide streams, typically above 40 %, should be considered hazardous due to concentrated hydrogen peroxide 's meeting the definition of a DOT oxidizer according to U.S. regulations, if released into the environment. The EPA Reportable Quantity ( RQ ) for D001 hazardous wastes is 100 pounds ( 45 kg ), or approximately 10 US gallons ( 38 L ), of concentrated hydrogen peroxide. Hydrogen peroxide should be stored in a cool, dry, well - ventilated area and away from any flammable or combustible substances. It should be stored in a container composed of non-reactive materials such as stainless steel or glass ( other materials including some plastics and aluminium alloys may also be suitable ). Because it breaks down quickly when exposed to light, it should be stored in an opaque container, and pharmaceutical formulations typically come in brown bottles that block light. Hydrogen peroxide, either in pure or diluted form, can pose several risks, the main one being that it forms explosive mixtures upon contact with organic compounds. Highly concentrated hydrogen peroxide itself is unstable and can cause a boiling liquid expanding vapour explosion ( BLEVE ) of the remaining liquid. Distillation of hydrogen peroxide at normal pressures is thus highly dangerous. It is also corrosive, especially when concentrated, but even domestic - strength solutions can cause irritation to the eyes, mucous membranes and skin. Swallowing hydrogen peroxide solutions is particularly dangerous, as decomposition in the stomach releases large quantities of gas ( 10 times the volume of a 3 % solution ), leading to internal bloating. Inhaling over 10 % can cause severe pulmonary irritation. With a significant vapour pressure ( 1.2 kPa at 50 ° C ), hydrogen - peroxide vapour is potentially hazardous. According to U.S. NIOSH, the immediately dangerous to life and health ( IDLH ) limit is only 75 ppm. The U.S. Occupational Safety and Health Administration ( OSHA ) has established a permissible exposure limit of 1.0 ppm calculated as an 8 - hour time - weighted average ( 29 CFR 1910.1000, Table Z - 1 ). Hydrogen peroxide has also been classified by the American Conference of Governmental Industrial Hygienists ( ACGIH ) as a `` known animal carcinogen, with unknown relevance on humans ''. For workplaces where there is a risk of exposure to the hazardous concentrations of the vapours, continuous monitors for hydrogen peroxide should be used. Information on the hazards of hydrogen peroxide is available from OSHA and from the ATSDR. Historical incidents On 16 July 1934, in Kummersdorf, Germany, a propellant tank containing an experimental monopropellant mixture consisting of hydrogen peroxide and ethanol exploded during a test, killing three people. During the Second World War, doctors in German concentration camps experimented with the use of hydrogen peroxide injections in the killing of human subjects. Several people received minor injuries after a hydrogen peroxide spill on board a flight between the U.S. cities of Orlando and Memphis on 28 October 1998. The Russian submarine K - 141 Kursk sailed to perform an exercise of firing dummy torpedoes at the Pyotr Velikiy, a Kirov - class battlecruiser. On 12 August 2000, at 11 : 28 local time ( 07 : 28 UTC ), there was an explosion while preparing to fire the torpedoes. The only credible report to date is that this was due to the failure and explosion of one of the Kursk 's hydrogen peroxide - fueled torpedoes. It is believed that HTP, a form of highly concentrated hydrogen peroxide used as propellant for the torpedo, seeped through its container, damaged either by rust or in the loading procedure back on land where an incident involving one of the torpedoes accidentally touching ground went unreported. The vessel was lost with all hands. A similar incident was responsible for the loss of HMS Sidon in 1955. On 15 August 2010, a spill of about 30 US gallons ( 110 L ) of cleaning fluid occurred on the 54th floor of 1515 Broadway, in Times Square, New York City. The spill, which a spokesperson for the New York City fire department said was of hydrogen peroxide, shut down Broadway between West 42nd and West 48th streets as fire engines responded to the hazmat situation. There were no reported injuries. See also FOX reagent, used to measure levels of hydrogen peroxide in biological systems. Hydrogen chalcogenide References Notes Jump up ^ Easton, M.F. ; Mitchell, A.G. ; Wynne - Jones, W.F.K. ( 1952 ). `` The behaviour of mixtures of hydrogen peroxide and water. Part 1. ? Determination of the densities of mixtures of hydrogen peroxide and water ''. Transactions of the Faraday Society. 48 : 796. doi : 10.1039 / TF9524800796. ^ Jump up to : `` NIOSH Pocket Guide to Chemical Hazards # 0335 ''. National Institute for Occupational Safety and Health ( NIOSH ). ^ Jump up to : `` Hydrogen peroxide ''. Immediately Dangerous to Life and Health Concentrations ( IDLH ). National Institute for Occupational Safety and Health ( NIOSH ). Jump up ^ Hill, C.N. ( 2001 ). A Vertical Empire : The History of the UK Rocket launch and Space Programme, 1950 -- 1971. Imperial College Press. ISBN 978 - 1 - 86094 - 268 - 6. Jump up ^ Brauer, Georg, ed. ( 1963 ). Handbook of preparative inorganic chemistry. 1. Translation editing by Reed F. ( 2nd ed. ). New York, N.Y. : Academic Press. p. 140. ISBN 978 - 0 - 12 - 126601 - 1. Jump up ^ `` Hydrogen Peroxide Technical Library '' ( PDF ). Retrieved 3 March 2016. Jump up ^ Hunt, Robert H. ; Leacock, Robert A. ; Peters, C. Wilbur ; Hecht, Karl T. ( 1965 ). `` Internal - Rotation in Hydrogen Peroxide : The Far - Infrared Spectrum and the Determination of the Hindering Potential '' ( PDF ). The Journal of Chemical Physics. 42 ( 6 ) : 1931. Bibcode : 1965JChPh... 42.1931 H. doi : 10.1063 / 1.1696228. Jump up ^ Dougherty, Dennis A. ; Anslyn, Eric V. ( 2005 ). Modern Physical Organic Chemistry. University Science. p. 122. ISBN 1 - 891389 - 31 - 9. Jump up ^ Abrahams, S.C. ; Collin, R.L. ; Lipscomb, W.N. ( 1 January 1951 ). `` The crystal structure of hydrogen peroxide ''. Acta Crystallographica. 4 ( 1 ) : 15 -- 20. doi : 10.1107 / S0365110X51000039. Jump up ^ Gilbert, L.W. ( 1820 ). `` Der tropfbar flüssige Sauerstoff, oder das oxygenierte Wasser ''. Annals of Physics ( in German ). 65 -- 66 : 3. Bibcode : 1820AnP... 64... 1T. doi : 10.1002 / andp. 18200640102. Jump up ^ Thénard, L.J. 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Carrara ( 1892 ) `` Sul peso molecolare e sul potere rifrangente dell ' acqua ossigenata '' ( On the molecular weight and on the refractive power of oxygenated water ( i.e., hydrogen peroxide ) ), Atti della Reale Accademia dei Lincei, series 5, 1 ( 2 ) : 19 -- 24. Carrara 's findings were confirmed by : W.R. Orndorff and John White ( 1893 ) `` The molecular weight of hydrogen peroxide and of benzoyl peroxide, '' American Chemical Journal, 15 : 347 -- 356. Jump up ^ See, for example : In 1882, Kingzett proposed as a structure H O =O. See : Thomas Kingzett, Charles ( 29 September 1882 ). `` On the activity of oxygen and the mode of formation of hydrogen dioxide ''. The Chemical News. 46 ( 1192 ) : 141 -- 142. In his 1922 textbook, Joseph Mellor considered three hypothetical molecular structures for hydrogen peroxide, admitting ( p. 952 ) : ``... the constitution of this compound has not been yet established by unequivocal experiments ''. See : Joseph William Mellor, A Comprehensive Treatise on Inorganic and Theoretical Chemistry, vol. 1 ( London, England : Longmans, Green and Co., 1922 ), p. 952 -- 956. W.C. Schumb, C.N. Satterfield, and R.L. Wentworth ( 1 December 1953 ) `` Report no. 43 : Hydrogen peroxide, Part two '', Office of Naval Research, Contract No. N5ori - 07819 On p. 178, the authors present six hypothetical models for hydrogen peroxide 's molecular structure. On p. 184, the present structure is considered almost certainly correct -- although a small doubt remained. ( Note : The report by Schumb et al. was reprinted as : W.C. Schumb, C.N. Satterfield, and R.L. Wentworth, Hydrogen Peroxide ( New York, New York : Reinhold Publishing Corp. ( American Chemical Society Monograph ), 1955 ). ) Jump up ^ See : Penney, W.G. ; Sutherland, G.B.B.M. ( 1934 ). `` The theory of the structure of hydrogen peroxide and hydrazine ''. Journal of Chemical Physics. 2 ( 8 ) : 492 -- 498. doi : 10.1063 / 1.1749518. 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Farbenindustrie, Germany Jump up ^ Noritaka Mizuno Gabriele Centi, Siglinda Perathoner, Salvatore Abate `` Direct Synthesis of Hydrogen Peroxide : Recent Advances '' in Modern Heterogeneous Oxidation Catalysis : Design, Reactions and Characterization 2009, Wiley - VCH. doi : 10.1002 / 9783527627547. ch8 Jump up ^ Edwards, Jennifer K. ; Solsona, Benjamin ; N, Edwin Ntainjua ; Carley, Albert F. ; Herzing, Andrew A. ; Kiely, Christopher J. ; Hutchings, Graham J. ( 20 February 2009 ). `` Switching Off Hydrogen Peroxide Hydrogenation in the Direct Synthesis Process ''. Science. 323 ( 5917 ) : 1037 -- 1041. Bibcode : 2009Sci... 323.1037 E. doi : 10.1126 / science. 1168980. PMID 19229032. ^ Jump up to : Ronald Hage, Achim Lienke ; Lienke ( 2005 ). `` Applications of Transition - Metal Catalysts to Textile and Wood - Pulp Bleaching ''. Angewandte Chemie International Edition. 45 ( 2 ) : 206 -- 222. doi : 10.1002 / anie. 200500525. PMID 16342123. 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( 2000 ). `` Chapter 27 : Chemical Sporicidal and Sporostatic Agents ''. Disinfection, sterilization, and preservation ( 5th ed. ). Philadelphia : Lea & Febiger. pp. 529 -- 543. ISBN 0 - 683 - 30740 - 1. CS1 maint : Extra text : authors list ( link ) Jump up ^ `` Sec. 184.1366 Hydrogen peroxide ''. U.S. Government Printing Office via GPO Access. 1 April 2001. Archived from the original on 3 July 2007. Retrieved 7 July 2007. Jump up ^ Wilgus TA, Bergdall VK, Dipietro LA, Oberyszyn TM ; Bergdall ; Dipietro ; Oberyszyn ( 2005 ). `` Hydrogen peroxide disrupts scarless fetal wound repair ''. Wound Repair Regen. 13 ( 5 ) : 513 -- 9. doi : 10.1111 / j. 1067 - 1927.2005. 00072. x. PMID 16176460. CS1 maint : Multiple names : authors list ( link ) Jump up ^ Loo, Alvin Eng Kiat ; Wong, Yee Ting ; Ho, Rongjian ; Wasser, Martin ; Du, Tiehua ; Ng, Wee Thong ; Halliwell, Barry ; Sastre, Juan ( 13 November 2012 ). `` Effects of Hydrogen Peroxide on Wound Healing in Mice in Relation to Oxidative Damage ''. PLoS ONE. 7 ( 11 ) : e49215. Bibcode : 2012PLoSO... 749215L. doi : 10.1371 / journal. pone. 0049215. PMC 3496701. PMID 23152875. Jump up ^ Shaw, A ; Cooperman, A ; Fusco, J ( 1967 ). `` Gas embolism produced by hydrogen peroxide ''. N Engl J Med. 277 ( 5 ) : 238 -- 41. doi : 10.1056 / nejm196708032770504. PMID 6029311. Jump up ^ `` Hydrogen peroxide : reminder of risk of gas embolism when used in surgery - GOV.UK ''. www.gov.uk. Jump up ^ Rahman, GA ; Adigun, IA ; Yusuf, IF ; Ofoegbu, CKP ( 28 May 2010 ). `` Wound dressing where there is limitation of choice ''. Nigerian Journal of Surgical Research. 8 ( 3 -- 4 ). doi : 10.4314 / njsr. v8i3 - 4.54882. Jump up ^ Velding, K. ; Klis, S. - A. ; Abass, K.M. ; Tuah, W. ; Stienstra, Y. ; van der Werf, T. ( 9 June 2014 ). `` Wound Care in Buruli Ulcer Disease in Ghana and Benin ''. American Journal of Tropical Medicine and Hygiene. 91 ( 2 ) : 313 -- 318. doi : 10.4269 / ajtmh. 13 - 0255. PMC 4125255. PMID 24914002. Jump up ^ `` Hydrogen peroxide : health effects, incident management and toxicology ''. Retrieved 3 March 2016. Jump up ^ Lane, Nick ( 2003 ). Oxygen : the molecule that made the world ( First issued in paperback, repr. ed. ). Oxford : Oxford University Press. p. 117. ISBN 0 - 19 - 860783 - 0. Jump up ^ Shepherd, Steven. `` Brushing Up on Gum Disease ''. FDA Consumer. Archived from the original on 14 May 2007. Retrieved 7 July 2007. Jump up ^ Capizzi, R. ; Landi, F. ; Milani, M. ; Amerio, P. ( 2004 ). `` Skin tolerability and efficacy of combination therapy with hydrogen peroxide stabilized cream and adapalene gel in comparison with benzoyl peroxide cream and adapalene gel in common acne. A randomized, investigator - masked, controlled trial ''. British Journal of Dermatology. 151 ( 2 ) : 481 -- 484. doi : 10.1111 / j. 1365 - 2133.2004. 06067. x. PMID 15327558. Jump up ^ Douglass, William Campbell ( 1995 ). Hydrogen peroxide : medical miracle. ( Atlanta, GA ) : Second Opinion Pub. ISBN 978 - 1 - 885236 - 07 - 4. ^ Jump up to : Hydrogen Peroxide, 3 %. 3. Hazards Identification Southeast Fisheries Science Center, daughter agency of NOAA. ^ Jump up to : `` Questionable methods of cancer management : hydrogen peroxide and other ' hyperoxygenation ' therapies ''. CA : A Cancer Journal for Clinicians. 43 ( 1 ) : 47 -- 56. 1993. doi : 10.3322 / canjclin. 43.1. 47. PMID 8422605. ^ Jump up to : Cooper, Anderson ( 12 January 2005 ). `` A Prescription for Death ? ''. CBS News. Retrieved 7 July 2007. ^ Jump up to : Mikkelson, Barbara ( 30 April 2006 ). `` Hydrogen Peroxide ''. Snopes.com. Retrieved 7 July 2007. ^ Jump up to : `` Naturopath Sentenced For Injecting Teen With Hydrogen Peroxide -- 7NEWS Denver ''. Thedenverchannel.com. 2006 - 03 - 27. Retrieved 2015 - 02 - 14. Jump up ^ Halliwell, Barry ( 1 January 2007 ). `` Oxidative stress and cancer : have we moved forward ? ''. Biochemical Journal. 401 ( 1 ) : 1 -- 11. doi : 10.1042 / BJ20061131. PMID 17150040. Jump up ^ http://www.hydrogen-peroxide.us/history-US-General-Kinetics/AIAA-2006-5236_hydrogen_peroxide_versus_hydrazine.pdf Jump up ^ http://www.hydrogen-peroxide.us/uses-monoprop-steam-generation/AIAA-1999-2880_The_Use_of_Hydrogen_Peroxide_for_Propulsion_and_Power-pitch.pdf Jump up ^ `` Peroxide Accident -- Walter Web Site ''. Histarmar.com.ar. Retrieved 2015 - 02 - 14. Jump up ^ Scott, Richard ( November 1997 ). `` Homing Instincts ''. Jane 's Navy Steam generated by catalytic decomposition of 80 -- 90 % hydrogen peroxide was used for driving the turbopump turbines of the V - 2 rockets, the X-15 rocketplanes, the early Centaur RL - 10 engines and is still used on Soyuz for that purpose today. International. Jump up ^ Soyuz using hydrogen peroxide propellant ( NASA website ) Jump up ^ `` Ways to use Hydrogen Peroxide in the Garden ''. Using Hydrogen Peroxide. Retrieved 3 March 2016. Jump up ^ Bhattarai SP, Su N, Midmore DJ ; Su ; Midmore ( 2005 ). `` Oxygation Unlocks Yield Potentials of Crops in Oxygen - Limited Soil Environments ''. Advances in Agronomy. Advances in Agronomy. 88 : 313 -- 377. doi : 10.1016 / S0065 - 2113 ( 05 ) 88008 - 3. ISBN 978 - 0 - 12 - 000786 - 8. CS1 maint : Multiple names : authors list ( link ) Jump up ^ `` Material Compatibility with Hydrogen Peroxide ''. Retrieved 3 March 2016. Jump up ^ `` Hydrogen Peroxide Mouthwash is it Safe ? ''. Retrieved 30 October 2013. ^ Jump up to : `` Occupational Safety and Health Guideline for Hydrogen Peroxide ''. Archived from the original on 13 May 2013. Jump up ^ For example, see an MSDS for a 3 % peroxide solution. Jump up ^ H2O2 toxicity and dangers Agency for Toxic Substances and Disease Registry website Jump up ^ CRC Handbook of Chemistry and Physics, 76th Ed, 1995 -- 1996 Jump up ^ `` CDC - Immediately Dangerous to Life or Health Concentrations ( IDLH ) : Chemical Listing and Documentation of Revised IDLH Values - NIOSH Publications and Products ''. Retrieved 3 March 2016. Jump up ^ `` Threshold Limit Values for Chemical Substances and Physical Agents & Biological Exposure Indices, ACGIH '' ( PDF ). Archived from the original ( PDF ) on 2 June 2013. Jump up ^ `` ATSDR - Redirect - MMG : Hydrogen Peroxide ''. Retrieved 3 March 2016. Jump up ^ `` The Nazi Doctors : Medical Killing and the Psychology of Genocide ''. Robert Jay Lifton. Retrieved 1 November 2007. Jump up ^ `` Accident No : DCA - 99 - MZ - 001 '' ( PDF ). U.S National Transportation Safety Board. Retrieved 30 October 2015. Jump up ^ Wheaton, Sarah ( 16 August 2010 ). `` Bleach Spill Shuts Part of Times Square ''. The New York Times. Bibliography J. Drabowicz ; et al. ( 1994 ). G. Capozzi ; et al., eds. The Syntheses of Sulphones, Sulphoxides and Cyclic Sulphides. Chichester UK : John Wiley & Sons. pp. 112 -- 6. ISBN 0 - 471 - 93970 - 6. CS1 maint : Explicit use of et al. ( link ) N.N. Greenwood ; A. Earnshaw ( 1997 ). Chemistry of the Elements ( 2nd ed. ). Oxford UK : Butterworth - Heinemann. A great description of properties & chemistry of H 2O 2. J. March ( 1992 ). Advanced Organic Chemistry ( 4th ed. ). New York : Wiley. p. 723. W.T. Hess ( 1995 ). `` Hydrogen Peroxide ''. Kirk - Othmer Encyclopedia of Chemical Technology. 13 ( 4th ed. ). New York : Wiley. pp. 961 -- 995. External links Hydrogen Peroxide at The Periodic Table of Videos ( University of Nottingham ) Material Safety Data Sheet ATSDR Agency for Toxic Substances and Disease Registry FAQ International Chemical Safety Card 0164 NIOSH Pocket Guide to Chemical Hazards Process flow sheet of Hydrogen Peroxide Production by anthrahydroquinone autoxidation Hydrogen Peroxide Handbook by Rocketdyne Hydrogen compounds H AsO H AsO HAt HSO F HBF HBr HBrO HBrO HBrO HBrO HCl HClO HClO HClO HClO HCN HCNO H CrO / H Cr O H CO H CS HF HFΟ HI HIO HIO HIO HIO HMnO H MoO HNC NaHCO HNCO HNO HNO HNO H N O HNO S H NSO H O H O H O H PO H PO H PO H P O H P O H PtCl H Se H SeO H SeO H SiO H SiF HSCN HNSC H SO H SO H SO H S O H S O H S O H S O CF SO H H Te H TeO H TeO H TiO H Po HCo ( CO ) Antiseptics and disinfectants ( D08 ) Acridine derivatives Ethacridine lactate 9 - Aminoacridine Euflavine Biguanides and amidines Dibrompropamidine Chlorhexidine Propamidine Hexamidine Polihexanide Phenol and derivatives Hexachlorophene Policresulen Phenol Triclosan Triclocarban Chloroxylenol Biphenylol Fenticlor Nitrofuran derivatives Nitrofurazone Iodine products Iodine / octylphenoxypolyglycolether Povidone - 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Silicon dicarbide Silicon naphthalocyanine Sulfur dioxide Thioformyl Thioxoethenylidene Titanium dioxide Tricarbon Water Four atoms Acetylene Ammonia Cyanic acid Cyanoethynyl Cyclopropynylidyne Formaldehyde Fulminic acid HCCN Hydrogen peroxide Hydromagnesium isocyanide Isocyanic acid Isothiocyanic acid Ketenyl Methylene amidogen Methyl radical Propynylidyne Protonated carbon dioxide Protonated hydrogen cyanide Silicon tricarbide Thioformaldehyde Tricarbon monoxide Tricarbon sulfide Thiocyanic acid Five atoms Ammonium ion Butadiynyl Carbodiimide Cyanamide Cyanoacetylene Cyanoformaldehyde Cyanomethyl Cyclopropenylidene Formic acid Isocyanoacetylene Ketene Methane Methoxy radical Methylenimine Propadienylidene Protonated formaldehyde Protonated formaldehyde Silane Silicon - carbide cluster Six atoms Acetonitrile Cyanobutadiynyl radical E-Cyanomethanimine Cyclopropenone Diacetylene Ethylene Formamide HC N Ketenimine Methanethiol Methanol Methyl isocyanide Pentynylidyne Propynal Protonated cyanoacetylene Seven atoms Acetaldehyde Acrylonitrile Vinyl cyanide Cyanodiacetylene Ethylene oxide Hexatriynyl radical Methylacetylene Methylamine Methyl isocyanate Vinyl alcohol Eight atoms Acetic acid Aminoacetonitrile Cyanoallene Ethanimine Glycolaldehyde Heptatrienyl radical Hexapentaenylidene Methylcyanoacetylene Methyl formate Propenal Nine atoms Acetamide Cyanohexatriyne Cyanotriacetylene Dimethyl ether Ethanol Methyldiacetylene Octatetraynyl radical Propene Propionitrile Ten atoms or more Acetone Benzene Buckminsterfullerene ( C fullerene, buckyball ) C fullerene Cyanodecapentayne Cyanopentaacetylene Cyanotetra - acetylene Ethylene glycol Ethyl formate Methyl acetate Methyl - cyano - diacetylene Methyltriacetylene Propanal n - Propyl cyanide Pyrimidine Deuterated molecules Ammonia Ammonium ion Formaldehyde Formyl radical Heavy water Hydrogen cyanide Hydrogen deuteride Hydrogen isocyanide Methylacetylene Trihydrogen cation Unconfirmed Anthracene Dihydroxyacetone Ethyl methyl ether Glycine Graphene H NCO Linear C Naphthalene cation Phosphine Pyrene Silylidine Related Abiogenesis Astrobiology Astrochemistry Atomic and molecular astrophysics Chemical formula Circumstellar envelope Cosmic dust Cosmic ray Cosmochemistry Diffuse interstellar band Earliest known life forms Extraterrestrial life Extraterrestrial liquid water Forbidden mechanism Helium hydride ion Homochirality Intergalactic dust Interplanetary medium Interstellar medium Photodissociation region Iron -- sulfur world theory Kerogen Molecules in stars Nexus for Exoplanet System Science Organic compound Outer space PAH world hypothesis Panspermia Polycyclic aromatic hydrocarbon ( PAH ) RNA world hypothesis Spectroscopy Tholin Book : Chemistry Category : Astrochemistry Category : Molecules Portal : Astrobiology Portal : Astronomy Portal : Chemistry Oxygen compounds AgO Al O AmO Am O As O As O Au O B O BaO BeO Bi O BiO Bi O BrO Br O Br O CO CO C O CaO CaO CdO CeO Ce O Ce O ClO Cl O Cl O Cl O Cl O Cl O CoO Co O Co O CrO Cr O Cr O Cr O CsO Cs O CuO D O Dy O Er O Eu O F O F O F O FeO Fe O Fe O Ga O Ga O GeO GeO H O H O H O HfO HgO Hg O Ho O I O I O I O I O In O InO KO K O La O Li O Li O Lu O MgO Mg O MnO MnO Mn O Mn O MoO MoO Mo O NO NO N O N O N O N O NaO Na O Na O NbO NbO Nd O Chemical formulas TRP channel modulators TRPA Activators 4 - Hydroxynonenal 4 - Oxo - 2 - nonenal 4, 5 - EET 12S - HpETE 15 - Deoxy - Δ - prostaglandin J2 α - Sanshool ( ginger, Sichuan and melegueta peppers ) Acrolein Allicin ( garlic ) Allyl isothiocyanate ( mustard, radish, horseradish, wasabi ) AM404 Bradykinin Cannabichromene ( cannabis ) Cannabidiol ( cannabis ) Cannabigerol ( cannabis ) Cinnamaldehyde ( cinnamon ) CR gas ( dibenzoxazepine ; DBO ) CS gas ( 2 - chlorobenzal malononitrile ) Curcumin ( turmeric ) Dehydroligustilide ( celery ) Diallyl disulfide Dicentrine ( Lindera spp. ) Farnesyl thiosalicylic acid Formalin Gingerols ( ginger ) Hepoxilin A3 Hepoxilin B3 Hydrogen peroxide Icilin Isothiocyanate Ligustilide ( celery, Angelica acutiloba ) Linalool ( Sichuan pepper, thyme ) Methylglyoxal Methyl salicylate ( wintergreen ) N - Methylmaleimide Nicotine ( tobacco ) Oleocanthal ( olive oil ) Paclitaxel ( Pacific yew ) Paracetamol ( acetaminophen ) PF - 4840154 Phenacyl chloride Polygodial ( Dorrigo pepper ) Shogaols ( ginger, Sichuan and melegueta peppers ) Tear gases Tetrahydrocannabinol ( cannabis ) Thiopropanal S - oxide ( onion ) Umbellulone ( Umbellularia californica ) WIN 55,212 - 2 Blockers Dehydroligustilide ( celery ) Nicotine ( tobacco ) Ruthenium red TRPC Activators Adhyperforin ( St John 's wort ) Diacyl glycerol GSK1702934A Hyperforin ( St John 's wort ) Substance P Blockers DCDPC DHEA - S Flufenamic acid GSK417651A GSK2293017A Meclofenamic acid N - ( p - amylcinnamoyl ) anthranilic acid Niflumic acid Pregnenolone sulfate Progesterone Pyr3 Tolfenamic acid TRPM Activators ADP - ribose BCTC Calcium ( intracellular ) Cold Coolact P Cooling Agent 10 CPS - 369 Eucalyptol ( eucalyptus ) Frescolat MGA Frescolat ML Geraniol Hydroxycitronellal Icilin Linalool Menthol ( mint ) PMD 38 Pregnenolone sulfate Rutamarin ( Ruta graveolens ) Steviol glycosides ( e.g., stevioside ) ( Stevia rebaudiana ) Sweet tastants ( e.g., glucose, fructose, sucrose ; indirectly ) Thio - BCTC WS - 3 WS - 12 WS - 23 Blockers Capsazepine Clotrimazole DCDPC Flufenamic acid Meclofenamic acid Mefenamic acid N - ( p - amylcinnamoyl ) anthranilic acid Nicotine ( tobacco ) Niflumic acid Ruthenium red Rutamarin ( Ruta graveolens ) Tolfenamic acid TPPO TRPML Activators MK6 - 83 PI ( 3, 5 ) P SF - 22 TRPP Activators Triptolide ( Tripterygium wilfordii ) Blockers Ruthenium red TRPV Activators 2 - APB 5 ', 6 ' - EET 9 - HODE 9 - oxoODE 12S - HETE 12S - HpETE 13 - HODE 13 - oxoODE 20 - HETE α - Sanshool ( ginger, Sichuan and melegueta peppers ) Allicin ( garlic ) AM404 Anandamide Bisandrographolide ( Andrographis paniculata ) Camphor ( camphor laurel, rosemary, camphorweed, African blue basil, camphor basil ) Cannabidiol ( cannabis ) Cannabidivarin ( cannabis ) Capsaicin ( chili pepper ) Carvacrol ( oregano, thyme, pepperwort, wild bergamot, others ) DHEA Diacyl glycerol Dihydrocapsaicin ( chili pepper ) Estradiol Eugenol ( basil, clove ) Evodiamine ( Euodia ruticarpa ) Gingerols ( ginger ) GSK1016790A Heat Hepoxilin A3 Hepoxilin B3 Homocapsaicin ( chili pepper ) Homodihydrocapsaicin ( chili pepper ) Incensole ( incense ) Lysophosphatidic acid Low pH ( acidic conditions ) Menthol ( mint ) N - Arachidonoyl dopamine N - Oleoyldopamine N - Oleoylethanolamide Nonivamide ( PAVA ) ( PAVA spray ) Nordihydrocapsaicin ( chili pepper ) Paclitaxel ( Pacific yew ) Paracetamol ( acetaminophen ) Phorbol esters ( e.g., 4α - PDD ) Piperine ( black pepper, long pepper ) Polygodial ( Dorrigo pepper ) Probenecid Protons Rutamarin ( Ruta graveolens ) Resiniferatoxin ( RTX ) ( Euphorbia resinifera / pooissonii ) Shogaols ( ginger, Sichuan and melegueta peppers ) Tetrahydrocannabivarin ( cannabis ) Thymol ( thyme, oregano ) Tinyatoxin ( Euphorbia resinifera / pooissonii ) Tramadol Vanillin ( vanilla ) Zucapsaicin Blockers α - Spinasterol ( Vernonia tweediana ) AMG - 517 Asivatrep BCTC Cannabigerol ( cannabis ) Cannabigerolic acid ( cannabis ) Cannabigerovarin ( cannabis ) Cannabinol ( cannabis ) Capsazepine DCDPC DHEA DHEA - S Flufenamic acid GRC - 6211 HC - 067047 Lanthanum Meclofenamic acid N - ( p - amylcinnamoyl ) anthranilic acid NGD - 8243 Niflumic acid Pregnenolone sulfate RN - 1734 RN - 9893 Ruthenium red SB - 705498 Tolfenamic acid See also : Receptor / signaling modulators Ion channel modulators NDL : 00565090 Retrieved from `` https://en.wikipedia.org/w/index.php?title=Hydrogen_peroxide&oldid=818527653 '' Categories : Antiseptics Bleaches Disinfectants 1894 introductions Household chemicals Hydrogen compounds Hydrogen peroxide Light - sensitive chemicals Peroxides Otologicals Oxidizing agents Rocket oxidizers Hair coloring Hidden categories : CS1 German - language sources ( de ) CS1 maint : Multiple names : authors list CS1 maint : Extra text : authors list Use dmy dates from October 2013 ECHA InfoCard ID from Wikidata Chembox having GHS data All articles with unsourced statements Articles with unsourced statements from July 2015 Articles containing unverified chemical infoboxes Articles with unsourced statements from September 2014 CS1 maint : Explicit use of et al. 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Question: where does hydrogen peroxide come from in the body
Answer: nearly all living cells