Hydrogen Peroxide
WHAT IS HYDROGEN PEROXIDE?
PRODUCTION METHODS, PROPERTIES AND 10 MAIN USES OF THIS SUBSTANCE
Hydrogen peroxide, hydrogen peroxide or hydrogen peroxide, is a chemical compound with the formula H2O2. In its pure form, this compound is a very pale bluish liquid, slightly thicker than water. Hydrogen peroxide is the simplest peroxide (a compound with an oxygen-oxygen single bond). This material is used as an oxidizer, bleach and disinfectant. Concentrated hydrogen oxide is a type of reactive oxygen. Its chemical properties are influenced by the nature of the unstable “peroxide” bond. This substance is unstable and decomposes slowly in the presence of light. Because of its extreme instability, hydrogen oxide is usually stored in dark colored bottles with a stabilizer in a weakly acidic solution. Hydrogen peroxide is also found in biological systems, including the human body. Enzymes that use or decompose hydrogen peroxide are known as “peroxidase”.
A LOOK AT THE HISTORY OF HYDROGEN PEROXIDE
Hydrogen peroxide was isolated for the first time in 1818 by “Louis-Jacques Thenard” from the reaction of barium peroxide with nitric acid. In the optimized version of this process, hydrochloric acid followed by sulfuric acid is used to precipitate the by-product “barium chloride”. The “Tennard” process was used from the end of the 19th century to the middle of the 20th century. More modern methods of producing hydrogen peroxide are discussed below.
H2 + O2 → H2O2
However, the economic efficiency of this process depends on factors such as effective recovery of “quinone” solvents, extraction and hydrogenation catalyst. In the past, inorganic processes were used to produce hydrogen oxide; These reactions included the electrolysis of an aqueous solution of sulfuric acid or acidic ammonium bisulfate (MH4HSO4). In 1994, the world production of hydrogen peroxide was about 1.9 million tons, with a concentration of 70%. Today, in industry, hydrogen oxide is produced almost exclusively by the Anthraquinone process, which was formalized in 1936 and patented in 1939.
PROPERTIES AND APPLICATIONS OF HYDROGEN PEROXIDE
In the following, we will learn about the uses of this material
1- Chemical properties of hydrogen peroxide: H2O2 is one of the strongest known oxidizers; Even stronger than chlorine, chlorine dioxide and potassium permanganate. By catalysis, H2O2, after fluorine, can be converted into hydroxyl radicals (OH°) in the second reaction. The following table shows a comparison between this compound and other strong oxidizers:
| Oxidizer | Oxidation potential (V) |
|---|---|
| Florin | 3.0 |
| Hydroxyl radical | 2.8 |
| Ozone | 2.1 |
| Hydrogen peroxide | 1.8 |
| Potassium permanganate | 1.7 |
| Chlorine dioxide | 1.5 |
| chlorine | 1.5 |
This substance can spontaneously decompose into water and oxygen. It usually acts as an oxidizing agent, but there are many reactions in which it acts as a reducing agent, releasing oxygen as a byproduct. It also readily forms both inorganic and organic peroxides.
2- Hydrogen peroxide decomposition formula: Hydrogen peroxide often spontaneously decomposes into water and oxygen gas in an exothermic reaction:
Energy + 2H2O2 → H2O2 + O2
This reaction is very favorable. The decomposition rate of hydrogen oxide depends on the temperature and concentration of peroxide, as well as pH and the presence of impurities and stabilizers. Hydrogen peroxide is incompatible with many substances that catalysts decompose, including many transition metals and their compounds. Common catalysts include manganese dioxide, potassium permanganate, and silver. Pouring hydrogen oxide with a high concentration on a flammable substance can cause a rapid fire and the release of oxygen due to the decomposition of hydrogen oxide. To prevent the accumulation of oxygen gas, peroxide should be stored in a well-ventilated container. In the presence of specific catalysts, such as Fe2+ or Ti3+, the decomposition of hydrogen oxide may follow another path; Free radicals such as OH (hydroxyl) and OOH are formed. A combination of H2O2 and Fe2+ is known as Fenton’s reagent.
3- Redox reactions – oxidation / reduction in hydrogen peroxide: In aqueous solution, hydrogen oxide can oxidize or reduce (reduce) a variety of inorganic ions. When hydrogen oxide acts as a reducing agent, oxygen gas is also produced. In acidic solution, Fe2+ is oxidized to Fe3+:
(2Fe2+ (aq) + H2O2 +2H + (aq) → 2Fe3 + (aq) + 2H2O (l)
Also, sulfite (SO32-) is oxidized to sulfate (SO42-). In addition, potassium permanganate is reduced to Mn2+ by acidic H2O2. Under alkaline conditions, some of these reactions are reversed. Mn2+ is oxidized to Mn4+.
2Fe3+ + H2O2+2OH− → 2Fe2+ +2H2O + O2
Hydrogen peroxide is often used as an oxidizing agent in organic chemistry. An example of this application is the oxidation of “thioethers” to “sulfoxides”.
4- Formation of peroxide compounds
Hydrogen peroxide is a weak acid and can form hydroperoxide salts or peroxides or derivatives of many metals. For example, hydrogen oxide with aqueous solutions of chromic acid can form an unstable aqueous peroxide. It can also produce “peroxanion” by reacting with anions. For example, reaction with borax results in sodium perborate, a bleaching compound in laundry detergent:
Na2B4O7+ 4H2O2+ 2NaOH → 2Na2B2O4 (OH)4 + H2O
Hydrogen peroxide converts carboxylic acids (R-COOH) to peroxy acids (R-COOOH). hydrogen oxide reacts with acetone and causes the formation of “acetone peroxide” and produces “hydrogen trioxide” in interaction with ozone. The reaction of H2O2 with urea produces “carbamide peroxide” which is used to whiten teeth. hydrogen oxide reacts with ozone and forms trioxidant.
5- Alkaline property of H2O2: Hydrogen peroxide is a much weaker base than water, but it can form additional compounds with strong acidic properties. HF/SbF5 superacid forms unstable compounds containing [H3O2]+ ion.
APPLICATIONS OF HYDROGEN PEROXIDE
1- The use of hydrogen peroxide as a bleach and color carrier
About 60% of hydrogen oxide production in the world is used for paper industry and paper recycling. In these two important industries, this compound has the role of dye or bleaching agent. The second major industrial use of hydrogen oxide is in the production of sodium bicarbonate and sodium sulfate, which are used as mild bleaches in laundry detergents. Sodium bicarbonate is a byproduct of the reaction of sodium carbonate and hydrogen peroxide. When the detergent dissolves in water, hydrogen oxide and sodium carbonate are released. By themselves, these bleaching agents are only effective at wash temperatures of 60°C (140°F) or higher, and are therefore often used in combination with activators; These activators make clothes clean at low temperatures.
2- The use of hydrogen peroxide in the production of organic compounds: Hydrogen oxide is used in the production of organic peroxides. “Dibenzoyl dioxide” is an example that is produced in high volume. Peroxy acids such as peracetic acid and meta-chloroperoxybenzoic acid are also produced using hydrogen oxide. hydrogen oxide is used to produce explosives based on organic peroxides, such as “acetone peroxide”.
3- Using hydrogen peroxide for disinfection: hydrogen oxide is used in some wastewater treatment processes to remove organic impurities. In advanced oxidation process, Fenton reaction produces hydroxyl radical with high reactivity; This reduces organic compounds; Organic compounds, including compounds that are very strong, include aromatic or halogenated compounds. Also, hydrogen oxide can oxidize sulfur-containing compounds in waste or waste. This process is very useful because it generally reduces their unpleasant odor. Hydrogen peroxide may be used to sterilize and disinfect various surfaces, including surgical instruments; On the other hand, it may be used in steam mode to clean and sterilize the operating room. H2O2 shows a strong effect on viruses, bacteria, yeasts and bacterial spores. 3% hydrogen oxide is used to destroy the activity of bacteria and fungi, but higher concentrations, 7% or 30%, require more time to disrupt the activity of microorganisms. hydrogen oxide for disinfection has been introduced as an environmentally safe alternative to chlorine-containing bleaches. This compound breaks down easily and produces oxygen and water. It is generally recognized as safe by the US Food and Drug Administration (FDA) as a safe antimicrobial and antiseptic agent.
4- Removing blood stains with hydrogen peroxide solution: As a bleaching agent, hydrogen oxide reacts with blood stains; Therefore, if a blood stain is fresh or not too old, using hydrogen oxide, if necessary, even more than once, will completely remove the blood stain. Commercial H2O2, as sold in pharmacies as a 2.5% or 3% solution, can be used to remove blood stains from carpets and clothing. If you put a few tablespoons of peroxide on the stain, it will create bubbles in the area of blood. After a few minutes, you can remove the excess liquid with a soft cloth or towel, and this way, the stain will disappear. Care must be taken, however, as hydrogen oxide can loosen fabric fibers or discolor many fabrics.
5- Some home applications: Hydrogen oxide has various household uses, primarily as a cleaning and disinfecting agent. In this section, we mention the most important applications of this important composition in home use. Diluted H2O2 (between 1.9% and 12%) mixed with dissolved ammonia is used for hair bleaching (hair bleaching). The same oxidant that is added to hair color actually contains a different percentage of hydrogen peroxide. Hydrogen peroxide is also used for teeth. This compound may be present in most whitening toothpastes.
6- Application of oxygenated water in agriculture and horticulture
Some gardeners and farmers who use hydroponic growing methods use a very dilute hydrogen oxide solution in their irrigation solutions. The decomposition of this substance causes oxygen to be released by itself. This process increases the growth of plant roots and helps to treat root rot (death of root cells due to lack of oxygen) and fight against various plant pests. Laboratory tests on fish in recent years have shown that ordinary household hydrogen oxide can be used to provide oxygen to small fish. This type of application is also for the same reason as releasing oxygen for the life of aquatic organisms.
7- Industrial applications of hydrogen peroxide Hydrogen oxide is a strong oxidizer that is effective in controlling the odor of sulfide and organic compounds in wastewater collection and treatment systems. This substance is usually applied to the sewage system, where the retention time is less than five hours and at least 30 minutes before the point of release of hydrogen sulfide. Hydrogen oxide breaks down into oxygen and water, adding dissolved oxygen to the treatment plant system, thereby reducing biological oxygen demand (BOD).
8- Hydrogen oxide for corona / uses and benefits: As we mentioned above, this substance is used as an antimicrobial substance and an oxidizing substance. It is also used as an antiseptic to clean wounds. In personal care products, such as colorants and toothpastes, hydrogen oxide acts as an oxidizing agent and provides a lightening/whitening effect. These features show that the importance of hydrogen oxide for Corona has been very prominent in these last few months in 2018 and 2019. Hydrogen oxide is used in the sanitary industry to clean and disinfect surfaces. During the coronavirus pandemic, the US Food and Drug Administration (FDA) approved the use of high-concentration vapor-phase hydrogen oxide to disinfect critical environments. It is also possible to disinfect N95 breathing masks for people who work in hospitals and care centers for corona patients through this combination. This technology allows people to reuse respirators in case of shortage. Hydrogen oxide-based products purchased by consumers for home use are usually 3% hydrogen peroxide. Manufacturer’s instructions should be followed for safe use.
9- Oxygenated water in personal health products: Bacteria, parasites, viruses, toxins and yeast are all agents that hydrogen oxide destroys. This substance oxidizes and neutralizes these living and non-living pathogens. Hospitals and other healthcare systems use hydrogen peroxide to clean and disinfect rooms.
10- Edible hydrogen peroxide in food and beverage industries: Food grade hydrogen oxide is available at 35% purity and is an ideal cleaning and disinfecting agent in this industry. This combination is used in cheese production. This substance is also used to remove the strong smell of some drinks.
SAFETY OF HYDROGEN PEROXIDE
- Even pure or diluted hydrogen oxide can have several dangers. At high concentrations of approximately 70%, hydrogen oxide can produce vapor; Vapors explode at normal atmospheric pressure above 70°C (158°F).
- Distillation of hydrogen oxide at normal pressures is very dangerous and should be avoided.
- Hydrogen oxide vapors can form sensitive explosive substances in contact with hydrocarbons. Hazardous reactions ranging from combustion to explosion have been reported with alcohols, ketones, carboxylic acids (especially acetic acid), amines, and phosphorus.
- If hydrogen oxide is spilled on clothing (or other flammable materials), the water will first gradually evaporate until the concentration is sufficient, then the clothing will spontaneously combust.
- Leather usually contains metal ions from the treatment and catches fire almost immediately upon contact.
- Concentrated hydrogen oxide (>50%) is corrosive and can irritate eyes, mucous membranes, and skin. Swallowing hydrogen oxide solutions is very dangerous. Decomposition of hydrogen oxide in the stomach releases large amounts of gas (10 times the volume of 3% solution), which leads to internal bleeding.
- As a result of inhalation of this compound, severe lung irritation occurs.
- A very important point about the safety of this substance is that for each concentration of 3%, 30%, 50, or higher concentrations, a safety information sheet or MSDS is defined. To learn more about the hazards of working with this chemical, you should obtain the MSDS sheet for the same solution.
STORAGE CONDITIONS FOR HYDROGEN PEROXIDE
Oxygenated water with low concentration can be kept and stored in controlled conditions by following the rules and standards.
- Hydrogen oxide should be stored in a container made of a material that does not react with the chemical. There are countless raw materials available that are used to make tanks and containers based on the concentration of hydrogen oxide and its grade (purity).
- In general, hydrogen oxide is an oxidizer and should be stored away from fuel sources and catalyst sources. Because oxygen is formed during the natural decomposition of peroxide, the resulting pressure increase can cause a glass container to break. Therefore, H2O2 should be stored in plastic containers with full ventilation.
PACKING OF HYDROGEN PEROXIDE
Tanks and containers for packing hydrogen oxide should be made of a compatible material, such as PTFE, polyethylene, stainless steel, or aluminum. Before filling the tanks, the containers must undergo a cleaning process to remove contaminants before entering the peroxide. There are also rules that must be followed for the packaging of this combination. Barrels containing this composition are available in 20 liters, 60 liters or 2.5 liters. Of course, ordering in bulk, shipping by tankers is also possible for this chemical.
TECHNICAL DATA SHEET OF HYDROGEN PEROXIDE
| PROPERTY | REQUIRMENT |
|---|---|
| Color | Colorless |
| CAS | 7722-84-1 |
| Boiling Point | 119°C |
| Melting Point | -56°C |
| Molecular Formula | H2O2 |
| MDL Number | 11333 |
| Synonym | oxydol, perhydrol, superoxol, interox, hydrogen dioxide, inhibine, peroxaan, albone, hioxyl, kastone |
| IUPAC Name | hydrogen peroxide |
| Molecular Weight (g/mol) | 34.014 |
| PubChem CID | 784 |
| ChEBI | CHEBI:16240 |
| Formula Weight | 34.0128g/mol |
| Packaging | HDPE plastic bottle |
| Vapor Pressure | 23 at 30°C |
| pH | 2 |
| Quantity | 1 L |
| Physical Form | Liquid |
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