Hydrogen peroxide

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Hydrogen peroxide
Structural formula of hydrogen peroxide
Ball stick model of the hydrogen peroxide molecule. Top (white): hydrogen, bottom (red): oxygen.
space filling model of the hydrogen peroxide molecule
space filling model of the hydrogen peroxide molecule
IUPAC name
Hydrogen peroxide
Systematic IUPAC name
Other names
Perhydroxic acid
Oxygenated water
3D model (
ECHA InfoCard
100.028.878 Edit this at Wikidata
EC Number
  • 231-765-0
RTECS number
  • MX0900000 (>90% soln.)
    MX0887000 (>30% soln.)
UN number 2015 (>60% soln.)
2014 (20–60% soln.)
2984 (8–20% soln.)
  • InChI=1S/H2O2/c1-2/h1-2H checkY
  • InChI=1/H2O2/c1-2/h1-2H
  • OO
Molar mass 34.014 g·mol−1
Appearance Very light blue liquid
Odor slightly sharp
Density 1.11 g/cm3 (20 °C, 30% (w/w) solution)[1]
1.450 g/cm3 (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 soluble in ether, alcohol
insoluble in petroleum ether
log P -0.43[2]
Vapor pressure 5 mmHg (30 °C)[3]
Acidity (pKa) 11.75
−17.7·10−6 cm3/mol
Viscosity 1.245 cP (20 °C)
2.26 D
1.267 J/(g·K) (gas)
2.619 J/(g·K) (liquid)
Std enthalpy of
−187.80 kJ/mol
A01AB02 (WHO) D08AX01 (WHO), D11AX25 (WHO), S02AA06 (WHO)
GHS labelling:
GHS03: OxidizingGHS05: CorrosiveGHS07: Exclamation mark
H271, H302, H314, H332, H335, H412
P280, P305+P351+P338, P310
NFPA 704 (fire diamond)
Flash point Non-flammable
Lethal dose or concentration (LD, LC):
1518 mg/kg[citation needed]
2000 mg/kg (oral, mouse)[4]
1418 ppm (rat, 4 hr)[4]
227 ppm (mouse)[4]
NIOSH (US health exposure limits):
PEL (Permissible)
TWA 1 ppm (1.4 mg/m3)[3]
REL (Recommended)
TWA 1 ppm (1.4 mg/m3)[3]
(Immediate danger)
75 ppm[3]
Safety data sheet (SDS) ICSC 0164 (>60% soln.)
Related compounds
Related compounds
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
checkY verify (what is checkY☒N ?)

Hydrogen peroxide is a

oxidizer, bleaching agent, and antiseptic, usually as a dilute solution (3%–6% by weight) in water for consumer use, and in higher concentrations for industrial use. Concentrated hydrogen peroxide, or "high-test peroxide", decomposes explosively when heated and has been used both as a monopropellant and an oxidizer in rocketry.[6]

Hydrogen peroxide is a



The boiling point of H2O2 has been extrapolated as being 150.2 °C (302.4 °F), approximately 50 °C (90 °F) 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.[7]

Hydrogen peroxide forms stable adducts with urea (Hydrogen peroxide - urea), sodium carbonate (sodium percarbonate) and other compounds.[8] An acid-base adduct with triphenylphosphine oxide is a useful "carrier" for H2O2 in some reactions.


O−O bond length = 147.4 pm O−H bond length = 95.0 pm
Structure and dimensions of H2O2 in the gas phase
O−O bond length = 145.8 pm O−H bond length = 98.8 pm
Structure and dimensions of H2O2 in the solid (crystalline) phase

Hydrogen peroxide (H2O2) is a nonplanar molecule with (twisted) C2

repulsion between the lone pairs of the adjacent oxygen atoms and dipolar effects between the two O–H bonds. For comparison, the rotational barrier for ethane
is 1040 cm−1 (12.4 kJ/mol).

The approximately 100°

ribonucleic acids and therefore an origin of homochirality in an RNA world.[12]

The molecular structures of gaseous and

tetragonal with the space group D4
or P41212.[14]

Aqueous solutions


eutectic mixture, exhibiting freezing-point depression down as low as -56 °C; pure water has a freezing 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.[15]

  • Phase diagram of H2O2 and water: Area above blue line is liquid. Dotted lines separate solid–liquid phases from solid–solid phases.
  • Density of aqueous solution of H2O2
    H2O2 (
    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
  • Hydrogen peroxide is most commonly available as a solution in water. For consumers, it is usually available from pharmacies at 3 and 6

    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.

    Comparison with analogues

    Hydrogen peroxide has several structural analogues with HmX−XHn bonding arrangements (water also shown for comparison). It has the highest (theoretical) boiling point of this series (X = O, S, N, P). 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. Structurally, the analogues all adopt similar skewed structures, due to repulsion between adjacent lone pairs.

    Properties of H2O2 and its analogues
    Values marked * are extrapolated
    Name Formula Molar mass
    point (°C)
    point (°C)
    Water HOH 18.02 0.00 99.98
    Hydrogen peroxide HOOH 34.01 −0.43 150.2*
    Hydrogen disulfide HSSH 66.15 −89.6 70.7
    Hydrazine H2NNH2 32.05 2 114
    Hydroxylamine NH2OH 33.03 33 58*
    Diphosphane H2PPH2 65.98 −99 63.5*

    Natural occurrence

    Hydrogen peroxide is produced by various biological processes mediated by enzymes.

    Hydrogen peroxide has been detected in surface water, in groundwater, and in the

    orders of magnitude depending in conditions such as season, altitude, daylight and water vapor content. In rural nighttime air it is less than 0.014 μg/m3, and in moderate photochemical smog it is 14 to 42 μg/m3.[17]

    The amount of hydrogen peroxide in biological systems can be assayed using a fluorometric assay.[18]


    Alexander von Humboldt is sometimes said to have been the first to report the first synthetic peroxide, barium peroxide, in 1799 as a by-product of his attempts to decompose air, although this is disputed due to von Humboldt's ambiguous wording.[19] 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 eau oxygénée ("oxygenated water") – subsequently known as hydrogen peroxide.[20][21][22]

    An improved version of Thénard's process used hydrochloric acid, followed by addition of sulfuric acid to precipitate the barium sulfate byproduct. This process was used from the end of the 19th century until the middle of the 20th century.[23]

    The bleaching effect of peroxides and their salts on

    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.[16]

    Early attempts failed to produce neat hydrogen peroxide. Anhydrous hydrogen peroxide was first obtained by vacuum distillation.[24]

    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 H2O2.[25] H2O=O seemed to be just as possible as the modern structure, and as late as in the middle of the 20th century at least half a dozen hypothetical isomeric variants of two main options seemed to be consistent with the available evidence.[26] 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.[27][28]


    Catalytic cycle for the anthraquinone process to produce hydrogen peroxide: an anthraquinone (right) is reduced using hydrogen to produce the corresponding anthrahydroquinone (left). This is oxidized using oxygen to produce hydrogen peroxide and recover anthraquinone.

    In 1994, world production of H2O2 was around 1.9 million tonnes and grew to 2.2 million in 2006,

    USD/kg, equivalent to US$1.50/kg (US$0.68/lb) on a "100% basis"[clarification needed].[30]

    Today, hydrogen peroxide is manufactured almost exclusively by the anthraquinone process, which was originally developed by BASF 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. In the presence of oxygen, the anthrahydroquinone then undergoes autoxidation: the labile hydrogen atoms of the hydroxy groups transfer to the oxygen molecule, to give hydrogen peroxide and regenerating the anthraquinone. Most commercial processes achieve oxidation by bubbling compressed air through a solution of the anthrahydroquinone, with the hydrogen peroxide then extracted from the solution and the anthraquinone recycled back for successive cycles of hydrogenation and oxidation.[30][31]

    The net reaction for the anthraquinone-catalyzed process is :[30]

    H2 + O2 → H2O2

    The economics of the process depend heavily on effective recycling of the extraction solvents, the hydrogenation catalyst and the expensive quinone.

    ISO tank container for hydrogen peroxide transportation
    A tank car designed for transporting hydrogen peroxide by rail

    Historical methods

    Hydrogen peroxide was once prepared industrially by hydrolysis of ammonium persulfate:

    [NH4]2S2O8 + 2 H2O → 2 [NH4]HSO4 + H2O2

    [NH4]2S2O4 was itself obtained by the electrolysis of a solution of ammonium bisulfate ([NH4]HSO4) in sulfuric acid.[32]

    Other routes

    Small amounts are formed by electrolysis, photochemistry, and electric arc, and related methods.[33]

    A commercially viable route for hydrogen peroxide via the reaction of hydrogen with oxygen favours production of water but can be stopped at the peroxide stage.[34][35] One economic obstacle has been that direct processes give a dilute solution uneconomic for transportation. None of these has yet reached a point where it can be used for industrial-scale synthesis.



    Hydrogen peroxide is about 1000x stronger acid than water.[36]

    H2O2 ⇌ H+ + HO2 pK = 11.65


    Hydrogen peroxide disproportionates to form water and oxygen with a

    kJ/kg[37] and a ΔS
    of 70.5 J/(mol·K):

    The rate of decomposition increases with rise in temperature, concentration, and pH. H2O2 is unstable under alkaline conditions. Decomposition is catalysed by various redox-active ions or compounds, including most transition metals and their compounds (e.g. manganese dioxide (MnO2), silver, and platinum).[38]

    Oxidation reactions




    F2 HF 3.0
    O3 O2 2.1
    H2O2 H2O 1.8
    KMnO4 MnO2 1.7
    ClO2 HClO 1.5
    Cl2 Cl 1.4

    Sulfite (SO2−3) is oxidized to sulfate (SO2−4).

    Reduction reactions


    alkaline conditions, hydrogen peroxide is a reductant. When H2O2 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 + H2O2 → O2 + NaCl + H2O
    2 KMnO4 + 3 H2O2 → 2 MnO2 + 2 KOH + 2 H2O + 3 O2

    Although usually a reductant, alkaline hydrogen peroxide converts Mn(II) to the dioxide:

    H2O2 + Mn2+ + 2 OH → MnO2 + 2 H2O

    In a related reaction, potassium permanganate is reduced to Mn2+ by acidic H2O2:[5]

    2 MnO4 + 5 H2O2 + 6 H+ → 2 Mn^+2 + 8 H2O + 5 O2

    The reduction of hydrogen peroxide by sodium hypochlorite yields singlet oxygen.

    Organic reactions

    Hydrogen peroxide is frequently used as an

    thioethers to sulfoxides:[39][40]

    Alkaline hydrogen peroxide is used for

    hydroboration-oxidation. It is also the principal reagent in the Dakin oxidation

    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 (CrO3 and H2SO4) forms a blue peroxide CrO(O2)2.




    The aerobic oxidation of glucose in the presence of the enzyme


    C6H12O7 + O2 → C6H10O7 + H2O2

    Superoxide dismutases (SOD)s are enzymes that promote the disproportionation of superoxide into oxygen and hydrogen peroxide.[43]

    ether phospholipids, which are found in mammalian brains and lungs.[45] They produce hydrogen peroxide in s process catalyzed by flavin adenine dinucleotide (FAD):[46]

    Hydrogen peroxide arises by 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:[47]

    Degradation of hypoxanthine through xanthine to uric acid to form hydrogen peroxide.
    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.[47]


    Catalase, another peroxisomal enzyme, uses this H2O2 to oxidize other substrates, including phenols, formic acid, formaldehyde, and alcohol, by means of a peroxidation reaction:

    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.[48] In addition, when excess H2O2 accumulates in the cell, catalase converts it to H2O through this reaction:

    H2O2 → 0.5 O2 + H2O

    Glutathione peroxidase, a selenoenzyme, also catalyzes the disproportionation of hydrogen peroxide.

    Fenton reaction

    The reaction of

    Fenton reaction, which generates hydroxyl radicals
    , which are of significance in biology:

    Fe(II) + H2O2 → Fe(III)OH + HO·

    The fenton reaction explains the toxicity of hydrogen peroxides because the hydroxyl radicals rapidly and irreversibly oxidize all organic compounds including

    mitochondria.[51][52][53] The compound is a major factor implicated in the free-radical theory of aging, based on its ready conversion into a hydroxyl radical


    Eggs of sea urchin, shortly after fertilization by a sperm, produce hydrogen peroxide. It is then converted to hydroxyl radicals (HO•), which initiate radical polymerization, which surrounds the eggs with a protective layer of polymer.


    exothermic chemical reaction to produce boiling, foul-smelling liquid partially becomes a gas (flash evaporation) and is expelled through an outlet valve with a loud popping sound.[54][55][56]

    As a proposed

    signaling molecule, hydrogen peroxide may regulate of a wide variety of biological processes.[57][58]

    At least one study has also tried to link hydrogen peroxide production to cancer.[59]



    About 60% of the world's production of hydrogen peroxide is used for pulp- and paper-bleaching.[29] The second major industrial application is the manufacture of sodium percarbonate and sodium perborate, which are used as mild bleaches in laundry detergents. A representative conversion is:

    Na2B4O7 + 4 H2O2 + 2 NaOH → 2 Na2B2O4(OH)4 + H2O

    Sodium percarbonate, which is an adduct of

    Tide laundry detergent. When dissolved in water, it releases hydrogen peroxide and sodium carbonate.[23] By themselves these bleaching agents are only effective at wash temperatures of 60 °C (140 °F) or above and so, often are used in conjunction with bleach activators
    , which facilitate cleaning at lower temperatures.

    Hydrogen peroxide has also been used as a flour bleaching agent and a tooth and bone whitening agent.

    Production of organic peroxy compounds

    It is used in the production of various

    phenyl oxalate ester (cyalume), to produce chemiluminescence; this application is most commonly encountered in the form of glow sticks

    Production of inorganic peroxides

    The reaction with borax leads to sodium perborate, a bleach used in laundry detergents:

    Sewage treatment

    Hydrogen peroxide is used in certain waste-water treatment processes to remove organic impurities. In

    halogenated compounds.[63] It can also oxidize sulfur-based compounds present in the waste; which is beneficial as it generally reduces their odour.[64]


    Hydrogen peroxide may be used for the sterilization of various surfaces,

    Gram-negative bacteria; however, the presence of catalase or other peroxidases in these organisms may increase tolerance in the presence of lower concentrations.[70] Lower levels of concentration (3%) will work against most spores; higher concentrations (7 to 30%) and longer contact times will improve sporicidal activity.[69][71]

    Hydrogen peroxide is seen as an environmentally safe alternative to


    Rocket-belt hydrogen-peroxide propulsion system used in a jet pack

    High-concentration H2O2 is referred to as "high-test peroxide" (HTP). It can be used either as a

    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.[74] The RD-107 engines (used from 1957 to present) in the R-7
    series of rockets decompose hydrogen peroxide to power the turbopumps.

    As a bipropellant, H2O2 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 Isp than liquid oxygen, but is dense, storable, non-cryogenic and can be more easily used to drive gas turbines to give high pressures using an efficient closed cycle. It may 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.

    hypergolic combination, and for the low-cost British Black Knight and Black Arrow launchers. Presently, HTP is used on ILR-33 AMBER[75] and Nucleus[76]
    suborbital rockets.

    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 sinking of HMS Sidon and the Russian submarine Kursk.[77] 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.[78][79]

    Household use

    Contact lenses soaking in a 3% hydrogen peroxide-based solution. The case includes a catalytic disc which neutralises the hydrogen peroxide over time.

    Hydrogen peroxide has various domestic uses, primarily as a cleaning and disinfecting agent.

    Hair bleaching

    Diluted H2O2 (between 1.9% and 12%) mixed with

    peroxide blonde".[80]
    Hydrogen peroxide is also used for tooth whitening. It may be found in most whitening toothpastes. Hydrogen peroxide has shown positive results involving teeth lightness and chroma shade parameters.[81] It works by oxidizing colored pigments onto the enamel where the shade of the tooth may become lighter.[further explanation needed] Hydrogen peroxide may be mixed with baking soda and salt to make a homemade toothpaste.[82]

    Removal of blood stains

    Hydrogen peroxide reacts with blood as a bleaching agent, and so if a blood stain is fresh, or not too old, liberal application of hydrogen peroxide, if necessary in more than single application, will bleach the stain fully out. After about two minutes of the application, the blood should be firmly blotted out.[83][84]

    Acne treatment

    Hydrogen peroxide may be used to treat

    acne,[85] although benzoyl peroxide
    is a more common treatment.

    Oral cleaning agent

    The use of dilute hydrogen peroxide as a oral cleansing agent has been reviewed academically to determine its usefulness in treating gingivitis and plaque. Although there is a positive effect when compared with a placebo, it was concluded that chlorhexidine is a much more effective treatment.[86]

    Niche uses

    , as found in a glow stick

    Some horticulturists 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.[87][88]

    For general watering concentrations around 0.1% is in use and this can be increased up to one percent for anti-fungal actions.[89] Tests show that plant foliage can safely tolerate concentrations up to 3%.[90]


    Hydrogen peroxide is used in aquaculture for controlling mortality caused by various microbes. In 2019, the U.S. FDA approved it for control of Saprolegniasis in all coldwater finfish and all fingerling and adult coolwater and warmwater finfish, for control of external columnaris disease in warm-water finfish, and for control of Gyrodactylus spp. in freshwater-reared salmonids.[91] Laboratory tests conducted by fish culturists have demonstrated that common household hydrogen peroxide may 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.

    Removing yellowing from aged plastics

    Hydrogen peroxide may be used in combination with a UV-light source to remove yellowing from white or light grey acrylonitrile butadiene styrene (ABS) plastics to partially or fully restore the original color. In the retrocomputing scene, this process is commonly referred to as retrobright.


    Skin shortly after exposure to 35% H2O2

    Regulations vary, but low concentrations, such as 5%, 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 typically are accompanied by a safety data sheet (SDS). 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 H2O2 will react violently.[92] While concentrations up to 35% produce only "white" oxygen bubbles in the skin (and some biting pain) that disappear with the blood within 30–45 minutes, concentrations of 98% dissolve paper. However concentrations as low as 3% can be dangerous for the eye because of oxygen evolution within the eye.[93]

    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).[94] 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.[95]

    Hydrogen peroxide, either in pure or diluted form, may pose several risks, the main one being that it forms explosive mixtures upon contact with organic compounds.[96] Distillation of hydrogen peroxide at normal pressures is highly dangerous. It is also corrosive, especially when concentrated, but even domestic-strength solutions may cause irritation to the eyes, mucous membranes, and skin.[97] Swallowing hydrogen peroxide solutions is particularly dangerous, as decomposition in the stomach releases large quantities of gas (ten times the volume of a 3% solution), leading to internal bloating. Inhaling over 10% can cause severe pulmonary irritation.[98]

    With a significant vapour pressure (1.2 kPa at 50 °C),

    immediately dangerous to life and health (IDLH) limit is only 75 ppm.[100] 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).[96] Hydrogen peroxide also has been classified by the American Conference of Governmental Industrial Hygienists (ACGIH) as a "known animal carcinogen, with unknown relevance on humans".[101] 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[96] and from the ATSDR.[102]

    Wound healing

    Historically, hydrogen peroxide was used for disinfecting wounds, partly because of its low cost and prompt availability compared to other antiseptics.[103]

    There is conflicting evidence on hydrogen peroxide's effect on wound healing. Some research finds benefit, while other research find delays and healing inhibition.[104] Its use for home treatment of wounds is generally not recommended.[105] 1.5–3% Hydrogen peroxide is used as a disinfectant in dentistry, especially in endodotic treatments together with hypochlorite and chlorhexidin and 1–1.5% is also useful for treatment of inflammation of third molars (wisdom teeth).[106]

    Use in alternative medicine

    Practitioners of

    AIDS, and in particular cancer.[107] There is no evidence of effectiveness and in some cases it has proved fatal.[108][109][110][111]

    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 that also has been proposed as a cause of cancer.[112] Claims that hydrogen peroxide therapy increases 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 is also 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.[108] Ingestion of hydrogen peroxide at concentrations of 35% or higher has been implicated as the cause of numerous gas embolism events resulting in hospitalisation. In these cases, hyperbaric oxygen therapy was used to treat the embolisms.[113]

    Intravenous injection of hydrogen peroxide has been linked to several deaths.[114][110][111] The American Cancer Society states that "there is no scientific evidence that hydrogen peroxide is a safe, effective, or useful cancer treatment."[109] Furthermore, the therapy is not approved by the U.S. FDA.

    Historical incidents

    See also


    1. S2CID 96669623
    2. ^ "Hydrogen peroxide". www.chemsrc.com. Archived from the original on 17 March 2020. Retrieved 3 May 2018.
    3. ^ a b c d NIOSH Pocket Guide to Chemical Hazards. "#0335". National Institute for Occupational Safety and Health (NIOSH).
    4. ^ a b c "Hydrogen peroxide". Immediately Dangerous to Life or Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).
    5. ^ .
    6. from the original on 13 April 2021. Retrieved 24 August 2020.
    7. .
    8. .
    9. (PDF) from the original on 2 December 2017. Retrieved 31 December 2018.
    10. .
    11. (PDF) from the original on 9 April 2014. Retrieved 9 April 2014.
    12. .
    13. .
    14. .
    15. ^ "Hydrogen Peroxide Technical Library" (PDF). Archived from the original (PDF) on 29 December 2009. Retrieved 3 March 2016.
    16. ^ .
    17. ^ Special Report No. 10. Hydrogen Peroxide. OEL Criteria Document. CAS No. 7722-84-1. July 1996.
    18. from the original on 18 March 2020. Retrieved 1 July 2019.
    19. . I checked Humboldt's pertinent publication carefully, but was unable to find an unambiguous proof of this assumption; the description of the starting materials ("Alaun-Erden" or "schwere Erden") were just too unprecise to understand what kind of chemical experiments he performed.
    20. .
    21. ^ Thénard LJ (1818). "Observations sur des nouvelles combinaisons entre l'oxigène et divers acides". Annales de chimie et de physique. 2nd series. 8: 306–312. Archived from the original on 3 September 2016. Retrieved 9 February 2016.
    22. from the original on 30 November 2018. Retrieved 28 November 2018. Hydrogen peroxide was discovered in 1818 by the French chemist Louis-Jacques Thenard, who named it eau oxygénée (oxygenated water).
    23. ^ .
    24. from the original on 13 February 2016. Retrieved 29 June 2014.
    25. ^ Carrara G (1892). "Sul peso molecolare e sul potere rifrangente dell' acqua ossigenata" [On the molecular weight and on the refracting power of hydrogen peroxide]. Atti della Reale Accademia dei Lincei. 1 (2): 19–24. Archived from the original on 4 September 2016.
      Carrara's findings were confirmed by: W. R. Orndorff and John White (1893) "The molecular weight of hydrogen peroxide and of benzoyl peroxide," Archived 4 September 2016 at the Wayback Machine American Chemical Journal, 15 : 347–356.
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