Difference between revisions of "Hydrogen peroxide"
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| − | '''Hydrogen peroxide''' is a mostly clear, blue-ish liquid with similar melting and boiling points to water. It is a powerful and versatile [[Oxidizing agent|oxidizer,]] but can act as a reducing agent in some circumstances. It also acts as a very weak acid (pK<sub>a</sub> 11.6), forming hydrated peroxide salts (such as [[sodium peroxide]] octahydrate) with alkalis in aqueous solution. | + | '''Hydrogen peroxide''' ('''H<sub>2</sub>O<sub>2</sub>''') is a mostly clear, blue-ish liquid with similar melting and boiling points to water. It is a powerful and versatile [[Oxidizing agent|oxidizer,]] but can act as a reducing agent in some circumstances. It also acts as a very weak acid (pK<sub>a</sub> = 11.6), forming hydrated peroxide salts (such as [[sodium peroxide]] octahydrate) with alkalis in aqueous solution. |
==Properties== | ==Properties== | ||
===Chemical=== | ===Chemical=== | ||
| − | Hydrogen peroxide | + | Hydrogen peroxide disproportionates into [[water]] and [[oxygen]] gas. This happens rapidly at high temperatures or when a catalyst, such as [[manganese dioxide]] or [[potassium iodide]], is added and this is often used to produce oxygen gas in a home chemistry setting: |
| − | Hydrogen peroxide | + | : H<sub>2</sub>O<sub>2</sub> → H<sub>2</sub>O + ½ O<sub>2</sub> |
| + | |||
| + | Hydrogen peroxide can be used as an oxidizer, and may enhance the oxidizing capabilities on mixing. For example, mixtures of [[sulfuric acid]] and hydrogen peroxide not only will react faster than the acid alone, but will also react with organic compounds, sometimes explosively. Depending on the ratio of peroxide and sulfuric acid, there are several types: [[piranha solution]] (min H<sub>2</sub>SO<sub>4</sub>:H<sub>2</sub>O<sub>2</sub> ratio 3:1), [[peroxymonosulfuric acid]] (H<sub>2</sub>SO<sub>4</sub>:H<sub>2</sub>O<sub>2</sub> molar ratio of 1:1), [[peroxydisulfuric acid]] (H<sub>2</sub>SO<sub>4</sub>:H<sub>2</sub>O<sub>2</sub> molar ratio of 1:2). | ||
| + | |||
| + | Hydrogen peroxide is dangerous as it can cause explosions when in contact with combustible materials in high concentration. An acid mixture of hydrogen peroxide and [[hydrochloric acid]] behaves like an oxidizing acid, similarly to nitric acid, and reacts with non-reactive metals such as [[copper]]: | ||
| + | |||
| + | : Cu + 2 HCl + H<sub>2</sub>O<sub>2</sub> → CuCl<sub>2</sub> + 2 H<sub>2</sub>O | ||
| + | |||
| + | This acid mixture alone undergoes a number of slow reactions with various products, which include oxygen and chlorine ''in statu nascendi'' and [[hypochlorous acid]], which makes it a powerful oxidizer that can be used as a much safer alternative to concentrated nitric acid for dissolving metals. However, you should never store this "green acid" as it invariably decomposes over time. | ||
| + | |||
| + | Hydrogen peroxide will reduce [[potassium permanganate]] is reduced to Mn<sub>2+</sub>: | ||
| + | |||
| + | : 2 KMnO<sub>4</sub> + 3 H<sub>2</sub>O<sub>2</sub> → 2 MnO<sub>2</sub> + 2 KOH + 2 H<sub>2</sub>O + 3 O<sub>2</sub> | ||
| + | |||
| + | Reaction with hypochlorites, like that with [[sodium hypochlorite]] will also produce oxygen, more specifically singlet oxygen.: | ||
| + | |||
| + | : NaOCl + H<sub>2</sub>O<sub>2</sub> → NaCl + H<sub>2</sub>O + O<sub>2</sub> | ||
| + | |||
| + | This route is a safe way or neutralizing bleach, without producing any unpleasant smells. | ||
| + | |||
| + | Reaction with [[borax]] and [[sodium hydroxide]] leads to [[sodium perborate]]: | ||
| + | |||
| + | : Na<sub>2</sub>B<sub>4</sub>O<sub>7</sub> + 2 NaOH + 4 H<sub>2</sub>O<sub>2</sub> → 2 Na<sub>2</sub>B<sub>2</sub>O<sub>4</sub>(OH)<sub>4</sub> + H<sub>2</sub>O | ||
| + | |||
| + | Reaction with [[ozone]] forms trioxidane. | ||
| + | |||
| + | It converts [[carboxylic acid]]s into peroxy acids | ||
| + | |||
| + | Hydrogen peroxide reacts with [[acetone]] to form the highly dangerous [[acetone peroxide]]. It also forms stable [[adduct]]s with [[urea]] ([[urea peroxide]]), sodium carbonate ([[sodium percarbonate]]) and other compounds. | ||
| + | |||
| + | Hydrogen peroxide will oxidize thioethers to sulfoxides: | ||
| + | |||
| + | : R-S-R' + H<sub>2</sub>O<sub>2</sub> → R-S(=O)-R' + H<sub>2</sub>O | ||
| + | |||
| + | Hydrogen peroxide solution containing ferric ion, is called [[Fenton's reagent]], and can be used to safely neutralize many organic compounds. | ||
===Physical=== | ===Physical=== | ||
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Hydrogen peroxide is available readily as a disinfectant in pharmacies and grocery stores, but may only be obtained easily in low concentrations often as 3% or 6% solutions. | Hydrogen peroxide is available readily as a disinfectant in pharmacies and grocery stores, but may only be obtained easily in low concentrations often as 3% or 6% solutions. | ||
| − | Higher concentration peroxide is sold for animal disinfectants, pool/spa treatments, hair bleaching. Some may contain other chemicals, including stabilizers, so read the label first. | + | Higher concentration peroxide is sold for animal disinfectants, pool/spa treatments, hair bleaching. Some may contain other chemicals, including stabilizers, so read the label first. |
| + | |||
| + | In the EU, the sale of hydrogen peroxide solutions with a concentration higher than 12% is restricted for private individuals. | ||
==Preparation== | ==Preparation== | ||
Hydrogen peroxide can be prepared by reacting concentrated [[sulfuric acid]] and [[barium peroxide]]. | Hydrogen peroxide can be prepared by reacting concentrated [[sulfuric acid]] and [[barium peroxide]]. | ||
| − | :BaO<sub>2</sub> + H<sub>2</sub>SO<sub>4</sub> → H<sub>2</sub>O<sub>2</sub> + BaSO<sub>4</sub> | + | : BaO<sub>2</sub> + H<sub>2</sub>SO<sub>4</sub> → H<sub>2</sub>O<sub>2</sub> + BaSO<sub>4</sub> |
The insoluble [[barium sulfate]] is filtered from the mixture. | The insoluble [[barium sulfate]] is filtered from the mixture. | ||
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While sulfuric acid is more readily available, the ammonium bisulfate process is cheaper and has a higher cell efficiency. The electrolysis is carried out in stoneware tanks with platinum electrodes; conversion of bisulfate to the persulfate takes place at the anode. After hydrolysis of the persulfate (with steam) in an evaporator, the resulting dilute aqueous solution of H<sub>2</sub>O<sub>2</sub> is separated from the bisulfate and further distilled in a stoneware distillation column. The resulting solution is approximately 30 w/o H<sub>2</sub>O<sub>2</sub>. Both the cathode liquor (after purification) and the bisulfate from the evaporator (and separator) are recycled back to the cells. | While sulfuric acid is more readily available, the ammonium bisulfate process is cheaper and has a higher cell efficiency. The electrolysis is carried out in stoneware tanks with platinum electrodes; conversion of bisulfate to the persulfate takes place at the anode. After hydrolysis of the persulfate (with steam) in an evaporator, the resulting dilute aqueous solution of H<sub>2</sub>O<sub>2</sub> is separated from the bisulfate and further distilled in a stoneware distillation column. The resulting solution is approximately 30 w/o H<sub>2</sub>O<sub>2</sub>. Both the cathode liquor (after purification) and the bisulfate from the evaporator (and separator) are recycled back to the cells. | ||
| + | |||
| + | Industrially, hydrogen peroxide is produced via the anthraquinone process (2-ethylanthraquinone gives the best performance, as it has better selectivity), where the anthraquinone can be hydrogenated in the presence of a [[palladium]] catalyst to 9,10-anthrahydroquinone, which, upon oxidation with oxygen, reverts back to anthraquinone releasing hydrogen peroxide. Cody's Lab made a [https://www.youtube.com/watch?v=Mt1itiHT6wU video] on making hydrogen peroxide via this route. | ||
==Projects== | ==Projects== | ||
*Make [[sulfuric acid]] | *Make [[sulfuric acid]] | ||
*Make peroxides | *Make peroxides | ||
| − | *Cleaning silver | + | *Cleaning [[silver]] metal |
*Make [[piranha solution]] | *Make [[piranha solution]] | ||
| − | *[[Fenton's reagent]] | + | *Make [[Fenton's reagent]] |
*Make copper etching solution | *Make copper etching solution | ||
| − | * | + | *Make singlet oxygen |
==Handling== | ==Handling== | ||
===Safety=== | ===Safety=== | ||
| − | As it is an oxidizer, high concentrations of hydrogen peroxide can ignite or detonate combustible or explosive materials. Lower concentrations are much safer, but regardless of concentration, poisonous. | + | As it is an oxidizer, high concentrations of hydrogen peroxide can ignite or detonate combustible or explosive materials. Lower concentrations are much safer, but regardless of concentration, poisonous. Concentrated hydrogen peroxide leaves weak itching or stinging burns and a white discoloration on skin. |
===Storage=== | ===Storage=== | ||
| Line 158: | Line 196: | ||
===Disposal=== | ===Disposal=== | ||
| − | Hydrogen peroxide can be decomposed by adding a catalyst, such as [[manganese dioxide]] or iron oxides (ordinary rust will do). This method however should not be used to neutralize concentrated peroxide as the decomposition will generate lots of heat and can lead to explosion. The explosion that crippled the Kursk submarine for example, occured when the peroxide that leaked from a torpedo entered in contact with some rust. It's recommended to not be poured down the drain, as it will quickly decompose in the sewage and may pose an explosion hazard. Adding a sulfide, such as [[lead(II) sulfide]], will result in [[lead(II) sulfate]] and water. | + | Hydrogen peroxide can be decomposed by adding a catalyst, such as [[manganese dioxide]] or iron oxides (ordinary rust will do). This method however should not be used to neutralize concentrated peroxide (>30%) as the decomposition will generate lots of heat and can lead to explosion, and the peroxide should first be diluted. The explosion that crippled the Kursk submarine for example, occured when the peroxide that leaked from a torpedo entered in contact with some rust. It's recommended to not be poured down the drain, as it will quickly decompose in the sewage and may pose an explosion hazard. Adding a sulfide, such as [[lead(II) sulfide]], will result in [[lead(II) sulfate]] and water. |
==References== | ==References== | ||
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*[http://www.sciencemadness.org/talk/viewthread.php?tid=15881 Hydrogen Peroxide purification] | *[http://www.sciencemadness.org/talk/viewthread.php?tid=15881 Hydrogen Peroxide purification] | ||
*[http://www.sciencemadness.org/talk/viewthread.php?tid=16726 Hydrogen peroxide concentration by freezing I need to make 12% h2o2 from 3%] | *[http://www.sciencemadness.org/talk/viewthread.php?tid=16726 Hydrogen peroxide concentration by freezing I need to make 12% h2o2 from 3%] | ||
| + | *[http://www.sciencemadness.org/talk/viewthread.php?tid=126644 Hydrogen peroxide maximum safe concentration] | ||
| + | *[http://www.sciencemadness.org/talk/viewthread.php?tid=157743 Storage of 35% H2O2] | ||
[[Category:Chemical compounds]] | [[Category:Chemical compounds]] | ||
[[Category:Inorganic compounds]] | [[Category:Inorganic compounds]] | ||
| + | [[Category:Hydrogen compounds]] | ||
| + | [[Category:Oxygen compounds]] | ||
[[Category:Acids]] | [[Category:Acids]] | ||
[[Category:Weak acids]] | [[Category:Weak acids]] | ||
| Line 176: | Line 218: | ||
[[Category:Materials available as food grade]] | [[Category:Materials available as food grade]] | ||
[[Category:Essential reagents]] | [[Category:Essential reagents]] | ||
| + | [[Category:Irritants]] | ||
| + | [[Category:Liquids]] | ||
Latest revision as of 12:58, 23 July 2023
| Names | |
|---|---|
| IUPAC name
Hydrogen peroxide
| |
| Other names
Dioxidane
Oxidanyl Perhydroxic acid | |
| Properties | |
| H2O2 | |
| Molar mass | 34.0147 g/mol |
| Appearance | Very light blue liquid (conc.) Colorless liquid (dil.) |
| Odor | Slightly sharp |
| Density | 1.450 g/cm3 (20 °C, pure) 1.11 g/cm3 (20 °C, 30% aq. solution) |
| Melting point | −0.43 °C (31.23 °F; 272.72 K) |
| Boiling point | 150.2 °C (302.4 °F; 423.3 K) |
| Miscibility | |
| Solubility | Reacts with ketones Soluble in alcohol, ether Insoluble in benzene, chloroform, petroleum ether, toluene |
| Vapor pressure | 5 mmHg (30 °C) |
| Acidity (pKa) | 11.75 |
| Thermochemistry | |
| Std enthalpy of
formation (ΔfH |
−187.80 kJ/mol |
| Hazards | |
| Safety data sheet | Sigma-Aldrich (30%) |
| Flash point | Non-flammable |
| Related compounds | |
| Related compounds
|
Water |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Hydrogen peroxide (H2O2) is a mostly clear, blue-ish liquid with similar melting and boiling points to water. It is a powerful and versatile oxidizer, but can act as a reducing agent in some circumstances. It also acts as a very weak acid (pKa = 11.6), forming hydrated peroxide salts (such as sodium peroxide octahydrate) with alkalis in aqueous solution.
Contents
Properties
Chemical
Hydrogen peroxide disproportionates into water and oxygen gas. This happens rapidly at high temperatures or when a catalyst, such as manganese dioxide or potassium iodide, is added and this is often used to produce oxygen gas in a home chemistry setting:
- H2O2 → H2O + ½ O2
Hydrogen peroxide can be used as an oxidizer, and may enhance the oxidizing capabilities on mixing. For example, mixtures of sulfuric acid and hydrogen peroxide not only will react faster than the acid alone, but will also react with organic compounds, sometimes explosively. Depending on the ratio of peroxide and sulfuric acid, there are several types: piranha solution (min H2SO4:H2O2 ratio 3:1), peroxymonosulfuric acid (H2SO4:H2O2 molar ratio of 1:1), peroxydisulfuric acid (H2SO4:H2O2 molar ratio of 1:2).
Hydrogen peroxide is dangerous as it can cause explosions when in contact with combustible materials in high concentration. An acid mixture of hydrogen peroxide and hydrochloric acid behaves like an oxidizing acid, similarly to nitric acid, and reacts with non-reactive metals such as copper:
- Cu + 2 HCl + H2O2 → CuCl2 + 2 H2O
This acid mixture alone undergoes a number of slow reactions with various products, which include oxygen and chlorine in statu nascendi and hypochlorous acid, which makes it a powerful oxidizer that can be used as a much safer alternative to concentrated nitric acid for dissolving metals. However, you should never store this "green acid" as it invariably decomposes over time.
Hydrogen peroxide will reduce potassium permanganate is reduced to Mn2+:
- 2 KMnO4 + 3 H2O2 → 2 MnO2 + 2 KOH + 2 H2O + 3 O2
Reaction with hypochlorites, like that with sodium hypochlorite will also produce oxygen, more specifically singlet oxygen.:
- NaOCl + H2O2 → NaCl + H2O + O2
This route is a safe way or neutralizing bleach, without producing any unpleasant smells.
Reaction with borax and sodium hydroxide leads to sodium perborate:
- Na2B4O7 + 2 NaOH + 4 H2O2 → 2 Na2B2O4(OH)4 + H2O
Reaction with ozone forms trioxidane.
It converts carboxylic acids into peroxy acids
Hydrogen peroxide reacts with acetone to form the highly dangerous acetone peroxide. It also forms stable adducts with urea (urea peroxide), sodium carbonate (sodium percarbonate) and other compounds.
Hydrogen peroxide will oxidize thioethers to sulfoxides:
- R-S-R' + H2O2 → R-S(=O)-R' + H2O
Hydrogen peroxide solution containing ferric ion, is called Fenton's reagent, and can be used to safely neutralize many organic compounds.
Physical
Hydrogen peroxide is tinted slightly blue in high concentrations. It has boiling and melting points similar to water, but can be concentrated by fractional crystallization. Concentrations of peroxide 30% and above are considered concentrated.
Availability
Hydrogen peroxide is available readily as a disinfectant in pharmacies and grocery stores, but may only be obtained easily in low concentrations often as 3% or 6% solutions.
Higher concentration peroxide is sold for animal disinfectants, pool/spa treatments, hair bleaching. Some may contain other chemicals, including stabilizers, so read the label first.
In the EU, the sale of hydrogen peroxide solutions with a concentration higher than 12% is restricted for private individuals.
Preparation
Hydrogen peroxide can be prepared by reacting concentrated sulfuric acid and barium peroxide.
- BaO2 + H2SO4 → H2O2 + BaSO4
The insoluble barium sulfate is filtered from the mixture.
Due to the availability of low concentrations of peroxide worldwide, concentrated hydrogen peroxide solutions are often prepared by evaporating the water from the peroxide, making sure not to boil the solution (as this will break down the peroxide).
One of the earliest large scale production of hydrogen peroxide involves the electrolysis of a solution of sulfuric acid of 50% concentration, or ammonium bisulfate solution. The resulting hydrogen peroxide solution has a concentration of 30%.
While sulfuric acid is more readily available, the ammonium bisulfate process is cheaper and has a higher cell efficiency. The electrolysis is carried out in stoneware tanks with platinum electrodes; conversion of bisulfate to the persulfate takes place at the anode. After hydrolysis of the persulfate (with steam) in an evaporator, the resulting dilute aqueous solution of H2O2 is separated from the bisulfate and further distilled in a stoneware distillation column. The resulting solution is approximately 30 w/o H2O2. Both the cathode liquor (after purification) and the bisulfate from the evaporator (and separator) are recycled back to the cells.
Industrially, hydrogen peroxide is produced via the anthraquinone process (2-ethylanthraquinone gives the best performance, as it has better selectivity), where the anthraquinone can be hydrogenated in the presence of a palladium catalyst to 9,10-anthrahydroquinone, which, upon oxidation with oxygen, reverts back to anthraquinone releasing hydrogen peroxide. Cody's Lab made a video on making hydrogen peroxide via this route.
Projects
- Make sulfuric acid
- Make peroxides
- Cleaning silver metal
- Make piranha solution
- Make Fenton's reagent
- Make copper etching solution
- Make singlet oxygen
Handling
Safety
As it is an oxidizer, high concentrations of hydrogen peroxide can ignite or detonate combustible or explosive materials. Lower concentrations are much safer, but regardless of concentration, poisonous. Concentrated hydrogen peroxide leaves weak itching or stinging burns and a white discoloration on skin.
Storage
Hydrogen peroxide solutions are best stored in cold dark places, such as a fridge. High concentration peroxides are metastable and will slowly build-up pressure, so it's recommended to open the bottles from time to time, to release the pressure, and store the solutions with ample headroom in the bottles. Phosphoric acid and EDTA are added as stabilizers.
NEVER store hydrogen peroxide near volatile organic compounds, such as acetone, as there is a risk of forming acetone peroxide.
Concentrated solutions of hydrogen peroxide are known to slowly react with glass. This does not harm the glass significantly, but it does harm the peroxide: the reaction yields sodium hydroxide, which can provoke its decomposition. It is preferable to use polyethylene to store such solutions.
Disposal
Hydrogen peroxide can be decomposed by adding a catalyst, such as manganese dioxide or iron oxides (ordinary rust will do). This method however should not be used to neutralize concentrated peroxide (>30%) as the decomposition will generate lots of heat and can lead to explosion, and the peroxide should first be diluted. The explosion that crippled the Kursk submarine for example, occured when the peroxide that leaked from a torpedo entered in contact with some rust. It's recommended to not be poured down the drain, as it will quickly decompose in the sewage and may pose an explosion hazard. Adding a sulfide, such as lead(II) sulfide, will result in lead(II) sulfate and water.
References
Relevant Sciencemadness threads
- Articles containing unverified chemical infoboxes
- Chembox articles without image
- Chemical compounds
- Inorganic compounds
- Hydrogen compounds
- Oxygen compounds
- Acids
- Weak acids
- Oxidizing agents
- Peroxides
- Inorganic peroxides
- Readily available chemicals
- Materials available as food grade
- Essential reagents
- Irritants
- Liquids
