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HYDROGEN PEROXIDE
CAS NO.: 7722-84-1
EC/LIST NO.: 231-765-0
Hydrogen peroxide is a chemical compound with the formula H2O2.
In its pure form, it is a very pale blue liquid, slightly more viscous than water.
Hydrogen peroxide is used as an 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 as a propellant in rocketry.
Hydrogen peroxide is a reactive oxygen species and the simplest peroxide, a compound having an oxygen–oxygen single bond.
Hydrogen peroxide decomposes slowly when exposed to light, and rapidly in the presence of organic or reactive compounds.
Hydrogen peroxide is typically stored with a stabilizer in a weakly acidic solution in a dark bottle to block light.
Hydrogen peroxide is found in biological systems including the human body.
Enzymes that use or decompose hydrogen peroxide are classified as peroxidases.
Hydrogen peroxide is a mild antiseptic used on the skin to prevent infection of minor cuts, scrapes, and burns.
Hydrogen peroxide may also be used as a mouth rinse to help remove mucus or to relieve minor mouth irritation (e.g., due to canker/cold sores, gingivitis).
Hydrogen peroxide works by releasing oxygen when it is applied to the affected area.
The release of oxygen causes foaming, which helps to remove dead skin and clean the area.
Hydrogen peroxide should not be used to treat deep wounds, animal bites, or serious burns.
Hydrogen peroxide is a colorless liquid at room temperature with a bitter taste.
Small amounts of gaseous hydrogen peroxide occur naturally in the air.
Hydrogen peroxide is unstable, decomposing readily to oxygen and water with release of heat.
Although nonflammable, it is a powerful oxidizing agent that can cause spontaneous combustion when it comes in contact with organic material.
Hydrogen peroxide is found in many households at low concentrations (3-9%) for medicinal applications and as a clothes and hair bleach.
In industry, hydrogen peroxide in higher concentrations is used as a bleach for textiles and paper, as a component of rocket fuels, and for producing foam rubber and organic chemicals.
Hydrogen Peroxide is a peroxide and oxidizing agent with disinfectant, antiviral and anti-bacterial activities.
Upon rinsing and gargling or topical application, hydrogen peroxide exerts its oxidizing activity and produces free radicals which leads to oxidative damage to proteins and membrane lipids.
This may inactivate and destroy pathogens and may prevent spreading of infection.
Hydrogen peroxide, stabilized appears as a crystalline solid at low temperatures.
Has a slightly pungent, irritating odor.
Used in the bleaching and deodorizing of textiles, wood pulp, hair, fur, etc. as a source of organic and inorganic peroxides; pulp and paper industry; plasticizers; rocket fuel; foam rubber; manufacture of glycerol; antichlor; dyeing; electroplating; antiseptic; laboratory reagent; epoxidation; hydroxylation; oxidation and reduction; viscosity control for starch and cellulose derivatives; refining and cleaning metals; bleaching and oxidizing agent in foods; neutralizing agent in wine distillation; seed disinfectant; substitute for chlorine in water and sewage treatment.
Hydrogen peroxide may seem old-fashioned in its dowdy brown bottle — but it’s definitely not a natural home remedy.
Hydrogen peroxide a household chemicalTrusted Source.
True, it differs from water only by the addition of one extra oxygen molecule.
But that extra molecule turns it into a powerful oxidizer.
Hydrogen peroxide the reason hydrogen peroxide is such a versatile cleanser, and it’s also the reason you need to use it cautiously on people and pets.
Hydrogen peroxide breaks down quickly and easily when it comes into contact with air or water, so it’s considered safer than chlorine chemicals.
hydrogen peroxide, (H2O2), a colourless liquid usually produced as aqueous solutions of various strengths, used principally for bleaching cotton and other textiles and wood pulp, in the manufacture of other chemicals, as a rocket propellant, and for cosmetic and medicinal purposes.
Solutions containing more than about 8 percent hydrogen peroxide are corrosive to the skin.
First recognized as a chemical compound in 1818, hydrogen peroxide is the simplest member of the class of peroxides.
Of the several processes of manufacture, the principal ones involve reactions of oxygen from the air with certain organic compounds, especially anthraquinone or isopropyl alcohol.
Major commercial grades are aqueous solutions containing 35, 50, 70, or 90 percent hydrogen peroxide and small amounts of stabilizers (often tin salts and phosphates) to suppress decomposition.
Hydrogen peroxide decomposes into water and oxygen upon heating or in the presence of numerous substances, particularly salts of such metals as iron, copper, manganese, nickel, or chromium.
Hydrogen peroxide combines with many compounds to form crystalline solids useful as mild oxidizing agents; the best-known of these is sodium perborate (NaBO2·H2O2·3H2O or NaBO3·4H2O), used in laundry detergents and chlorine-free bleach products.
With certain organic compounds, hydrogen peroxide reacts to form hydroperoxides or peroxides, several of which are used to initiate polymerization reactions.
In most of its reactions, hydrogen peroxide oxidizes other substances, although it is itself oxidized by a few compounds, such as potassium permanganate.
Pure hydrogen peroxide freezes at −0.43 °C (+31.3 °F) and boils at 150.2 °C (302 °F); it is denser than water and is soluble in it in all proportions.
Hydrogen Peroxide (H₂O₂) is a colorless liquid with a slightly sharp odor.
Hydrogen peroxide can cause irritation to the eyes, nose, skin, and throat.
Workers may be harmed from exposure to hydrogen peroxide.
The level of exposure depends upon the dose, duration, and work being done.
Hydrogen peroxide is used in many industries.
In industry, hydrogen peroxide in higher concentrations is used as a bleach for textiles and paper, as a component of rocket fuels, and for producing foam rubber and organic chemicals.
Hydrogen peroxide also used in medicinal applications and to bleach clothes and hair.
Workers may be exposed to hydrogen peroxide through inhalation or contact with the skin.
Examples of workers who may be exposed to hydrogen peroxide include the following:
Workers in poultry plants that use it in chemical disinfectants
Stylists in beauty salons who use colorant products
Hospitals and healthcare workers
Factory workers in plants that manufacture foam rubber
Hydrogen peroxide, a chemical that appears as a colorless liquid, is used in a wide range of cleaning and personal care products, including hair dyes and bleaches, toothpaste and mouthwashes, bathroom cleaners and laundry stain removers.
Hydrogen peroxide can also be found in over-the-counter (OTC) first aid antiseptics, and it is used as a bleaching agent in some food products.
Hydrogen peroxide has other consumer and industrial uses as well, including water treatment.
Hydrogen peroxide at low concentrations has a variety of medicinal and domestic uses.
At higher concentrations hydrogen peroxide has many commercial and industrial uses.
Hydrogen peroxide and multipurpose solutions both clean and disinfect contact lenses by breaking up and removing trapped debris, protein, and fatty deposits (lipids).
Unlike multipurpose solutions, hydrogen peroxide solutions are preservative-free, which makes them a suitable option for those who are allergic or sensitive to the preservatives found in multipurpose solutions.
They are not risk-free, however, and should be used with appropriate cautions.
Hydrogen Peroxide (H2O2) is a naturally occurring chemical compound composed of a pair of covalently single bonded oxygen atoms each bonded to a hydrogen atom.
Hydrogen peroxide is colorless and is commercially used in both liquid and vaporized form.
Hydrogen peroxide is naturally involved in organism functions, such as mitochondrial respiration, and is naturally found in small amounts in the air.
Since its isolation in the 19th century, hydrogen peroxide has become a common disinfecting and bleaching agent.
For example, hydrogen peroxide is used as a lightening and antimicrobial agent in a variety of foods including milk.
The compound is especially useful in vaporized form for decontaminating materials such as lab stations, pill bottles, or medical rooms, which cannot withstand the high temperatures usually used for sanitation processes.
Because residual levels of hydrogen peroxide (post-decontamination and aeration) can adversely affect drug production, monitoring levels is critical to ensure drug efficacy, safety, and stability,
Picarro has designed and produced a gas concentration analyzer that precisely measures hydrogen peroxide for GMP pharmaceutical manufacturing.
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.
Hydrogen peroxide may be safely distilled at lower temperatures under reduced pressure
Hydrogen peroxide (H2O2) is a nonplanar molecule with (twisted) C2 symmetry; this was first shown by Paul-Antoine Giguère in 1950 using infrared spectroscopy.
Although the O−O bond is a single bond, the molecule has a relatively high rotational barrier of 386 cm−1 (4.62 kJ/mol) for rotation between enantiomers via the trans configuration, and 2460 cm−1 (29.4 kJ/mol) via the cis configuration.
These barriers are proposed to be due to 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° dihedral angle between the two O–H bonds makes the molecule chiral.
Hydrogen peroxide is the smallest and simplest molecule to exhibit enantiomerism.
Hydrogen peroxide has been proposed that the enantiospecific interactions of one rather than the other may have led to amplification of one enantiomeric form of ribonucleic acids and therefore an origin of homochirality in an RNA world.
The molecular structures of gaseous and crystalline H2O2 are significantly different.
This difference is attributed to the effects of hydrogen bonding, which is absent in the gaseous state.
Crystals of H2O2 are tetragonal with the space group D44P4121
In aqueous solutions, hydrogen peroxide differs from the pure substance 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 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).
Hydrogen peroxide 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
Hydrogen peroxide has several structural analogues with Hm−X−X−Hn bonding arrangements (water also shown for comparison).
Hydrogen peroxide has the highest (theoretical) boiling point of this series (X = O, N, S).
Hydrogen peroxide 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.
About 60% of the world's production of hydrogen peroxide is used for pulp- and paper-bleaching.
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 laundry products as OxiClean and Tide laundry detergent.
When dissolved in water, it releases hydrogen peroxide and sodium carbonate, 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
Today, hydrogen peroxide is manufactured almost exclusively by the anthraquinone process, which was originally developed by BASF in 1939.
Hydrogen peroxide 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.
The net reaction for the anthraquinone-catalyzed process is :
H2 + O2 → H2O2
The economics of the process depend heavily on effective recycling of the extraction solvents, the hydrogenation catalyst and the expensive quinone.
Small, but detectable, amounts of hydrogen peroxide can be formed by several methods.
Small amounts are formed by electrolysis of dilute acid around the cathode where hydrogen evolves if oxygen is bubbled around it.
Hydrogen peroxide is also produced by exposing water to ultraviolet rays from a mercury lamp, or an electric arc while confining it in a UV transparent vessel (e.g. quartz).
Hydrogen peroxide is detectable in ice water after burning a hydrogen gas stream aimed towards it and is also detectable on floating ice.
Rapidly cooling humid air blown through an approximately 2,000 °C spark gap results in detectable amounts.
A commercially viable process to produce hydrogen peroxide directly from the environment has been of interest for many years.
Efficient 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 employ finely dispersed metal catalysts similar to those used for hydrogenation of organic substrates.
One economic obstacle has been that direct processes give a dilute solution uneconomic for transportation.
None of these has yet reached a point where they can be used for industrial-scale synthesis.
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 H2O2 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% H2O2 sold for around 0.54 USD/kg, equivalent to US$1.50/kg (US$0.68/lb) on a "100% basis"
Hydrogen peroxide occurs in surface water, groundwater and in the atmosphere.
Hydrogen peroxide 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 billio
Hydrogen peroxide decomposes to form water and oxygen with a ΔHo of –2884.5 kJ/kg[33] and a ΔS of 70.5 J/(mol·K):
2 H2O2 → 2 H2O + O2
The rate of decomposition increases with rise in temperature, concentration, and pH (H2O2 being unstable under alkaline conditions), with cool, dilute, and acidic solutions showing the best stability.
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).
Certain metal ions, such as Fe2+or Ti3+, can cause the decomposition to take a different path, with free radicals such as the hydroxyl radical (HO•) and hydroperoxyl (HOO•) being formed.
Non-metallic catalysts include potassium iodide (KI), which reacts particularly rapidly and forms the basis of the elephant toothpaste demonstration.
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.
Hydrogen peroxide is used in the production of various organic peroxides with dibenzoyl peroxide being a high volume example.
Peroxy acids, such as peracetic acid and meta-chloroperoxybenzoic acid also are produced using hydrogen peroxide.
Hydrogen peroxide has been used for creating organic peroxide-based explosives, such as acetone peroxide.
Hydrogen peroxide is used as an initiator in polymerizations.
Hydrogen peroxide is used in certain waste-water treatment processes to remove organic impurities.
In advanced oxidation processing, the Fenton reaction gives the highly reactive hydroxyl radical (·OH).
This degrades organic compounds, including those that are ordinarily robust, such as aromatic or halogenated compounds.
Hydrogen peroxide can also oxidize sulfur based compounds present in the waste; which is beneficial as it generally reduces their odour.
Hydrogen peroxide may be used for the sterilization of various surfaces, including surgical tools, and may be deployed as a vapour (VHP) for room sterilization.
H2O2 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 may increase tolerance in the presence of lower concentrations.
Lower levels of concentration (3%) will work against most spores; higher concentrations (7 to 30%) and longer contact times will improve 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).
High-concentration H2O2 is referred to as "high-test peroxide" (HTP).
Hydrogen peroxide 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 (1,100 °F), which is expelled through a nozzle, generating thrust.
H2O2 monopropellant produces a maximal specific impulse (Isp) 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, 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. 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 163B), 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 sinking 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
Hydrogen peroxide has various domestic uses, primarily as a cleaning and disinfecting agent.
Hair bleaching Diluted H2O2 (between 1.9% and 12%) mixed with aqueous ammonia has been 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.
Hydrogen peroxide may be found in most whitening toothpastes.
Hydrogen peroxide has shown positive results involving teeth lightness and chroma shade parameters.
Hydrogen peroxide works by oxidizing colored pigments onto the enamel where the shade of the tooth may become lighter.
Hydrogen peroxide may be mixed with baking soda and salt to make a homemade toothpaste.
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.
Hydrogen peroxide may be used to treat acne, although benzoyl peroxide is a more common treatment.
Chemiluminescence of cyalume, as found in a glow stick
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.
Some horticulturalists and users of hydroponics advocate the use of weak hydrogen peroxide solution in watering solutions.
Hydrogen peroxide 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.
For general watering concentrations around 0.1% is in use and this can be increased up to one percent for anti-fungal actions.
Tests show that plant foliage can safely tolerate concentrations up to 3%.
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.
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.
IUPAC NAME :
Acqua Ossigenata 130 V. Stab 35%
dihydrogen dioxide
dihydrogen peroxide
Hidrogen Peroxide
Hidrogén-peroxid 30%-os oldat
hydorgen peroxide
HYDROGEN PEROXIDE
Hydrogen Peroxide
Hydrogen peroxide
hydrogen peroxide
Hydrogen Peroxide
Hydrogen peroxide
hydrogen peroxide
Hydrogen peroxide (H2O2)
Hydrogen peroxide (H2O2)
SYNONYMS:
12325-10-9
231-765-0
30
3170-83-0
7722-84-1
dihydrogen peroxide
Hidrojen peroksit
Hioxyl
HOOH
Hydrogen peroxide
