CHLORINE DIOXIDE

Chlorine dioxide is used as a bleach at pulp mills, which make paper and paper products, and in public water-treatment facilities, to make water safe for drinking. 
Chlorine Dioxide has also been used to decontaminate public buildings. 
Chlorine Dioxide is soluble in water and will react rapidly with other compounds. 

CAS Number: 10049-04-4
Molecular Formula: ClO2
Molecular Weight: 67.45
EINECS Number: 233-162-8

Synonyms: CHLORINE DIOXIDE, Alcide, 10049-04-4, Chlorine oxide (ClO2), Chlorine(IV) oxide, Purite, Joyden, Joyden plus, Nobda disinfectant, BlueMAX Pre-Post, Gladiator Super Dry, BlueMAX Premium EU, RefChem:5668, SKIN N CLEAN, VIRUS ZERO-F, ProVtect Hand Sanitizer, Chlorine Dioxide(ClO2), SANI-HEALTH Sanitizer, PURE O2 S, VIRUS KILL SANITIZER, PURE O2-S F, Chlorine dioxide disinfectant, M.C. (Morningcalm) V Zero, DMINE PENTOSE MEDI PLUS, 8061YMS4RM, DTXCID803958, Jiajia Gaseous Air Disinfectant, chlorine dioxide air disinfectant, CHEBI:37750, CHEBI:52357, KO-C100, SFP INC. NVO-2 TOPICAL NAVEL DIP, TBOSEN EMERGENCY STERILIZATION CARD, SFP INC. VO-2 SANITIZING TEAT DIP, Chlorine Dioxide Sustained Release Granules, 233-162-8, Anthium dioxcide, Chlorine Oxide, Chloroperoxyl, Chloryl radical, ClO2, Doxcide 50, DTXSID5023958, chlorosyloxidanyl, Chlorine oxide?, dioxidochlorine(.), dioxido-lambda(5)-chloranyl, (OClO)(.), O2Cl(.), CHEBI:29415, ClO2, chloroperoxyl[qr], Chloryl radical, chlorylradical, chlorylradical[qr], ClO2, dioxydedechlore, Doxcide 50, doxcide50

Chlorine Dioxide is manufactured from the oxidation of chlorite or the reduction of chlorate. 
The latter method is used for large-volume production and is carried out in strongly acidic solution using reducing agents such as NaCl, HCl, sulfur dioxide, and methanol.
Chlorine Dioxide is a yellow to reddish-yellow gas that can decompose rapidly in air. 

Because it is a hazardous gas, chlorine dioxide is always made at the location where it is used. 
When it reacts in water, chlorine dioxide forms chlorite ion, which is also a very reactive chemical. 
Because chlorine dioxide is very reactive, it is able to kill bacteria and microorganisms in water. 

About 5% of large water-treatment facilities (serving more than 100,000 persons) in the United States use chlorine dioxide to treat drinking water. 
An estimated 12 million persons may be exposed in this way to chlorine dioxide and chlorite ions. 
In communities that use chlorine dioxide to treat drinking water, chlorine dioxide and its byproduct, chlorite ions, may be present at low levels in tap water.

Chlorine Dioxide is a chemical compound with the formula ClO2 that exists as yellowish-green gas above 11 °C, a reddish-brown liquid between 11 °C and −59 °C, and as bright orange crystals below −59 °C. 
Chlorine Dioxide is usually handled as an aqueous solution. 
Chlorine Dioxide is commonly used as a bleach. 

More recent developments have extended its applications in food processing and as a disinfectant.
The molecule ClO2 has an odd number of valence electrons, and therefore it is a paramagnetic radical. 
Chlorine Dioxide is an unusual "example of an odd-electron molecule stable toward dimerization" (nitric oxide being another example).

Chlorine dioxide is a yellow-green gas with a sharp, chlorine-like odor and powerful oxidizing properties.
Chlorine Dioxide is composed of one chlorine atom and two oxygen atoms, with the chemical formula ClO₂.
At room temperature, it exists as a gas but can be dissolved in water to form a stable aqueous disinfectant.

It is not the same as chlorine gas (Cl₂), even though both contain chlorine.
Chlorine dioxide disinfects primarily through oxidation, while chlorine acts by chlorination of organic compounds.
This makes chlorine dioxide a more selective and less corrosive sterilizing agent.

Chlorine dioxide is used extensively in drinking water purification, wastewater treatment, and food processing sanitation.
It effectively kills bacteria, viruses, and fungi without forming harmful chlorinated by-products.
Because of its high potency, it can disinfect at very low concentrations.

Industrially, chlorine dioxide is generated on-site because it is unstable when stored under pressure.
It is produced by reducing sodium chlorate or sodium chlorite with acids under controlled conditions.
This freshly generated gas is immediately dissolved in water for use in sanitation systems.

It is also applied in medical sterilization, air disinfection, and surface decontamination.
Many hospitals, food factories, and laboratories use chlorine dioxide as a broad-spectrum biocide.
It has even been tested for neutralizing bioaerosols and viral pathogens in enclosed environments.

In the pulp and paper industry, chlorine dioxide is used as a bleaching agent for wood pulp.
It whitens paper fibers without significantly damaging cellulose, unlike traditional chlorine bleaching.
This property makes it a preferred eco-friendly bleaching chemical.

It can also be found in oil, textile, and electronics industries for oxidation and surface cleaning purposes.
In cooling towers and water systems, it prevents the growth of biofilms and algae.
Its controlled release makes it suitable for continuous microbial protection.

Although a highly effective disinfectant, chlorine dioxide is also toxic and reactive.
At high concentrations, it can irritate the eyes, throat, and lungs or even cause pulmonary edema.
Therefore, it must always be used in ventilated areas with strict concentration control.

When properly managed, chlorine dioxide is one of the most powerful and efficient sanitizing agents available.
It provides high-level disinfection while minimizing environmental impact.
Because of its versatility, it plays a vital role in public health, industry, and environmental protection worldwide.

An orange gas formed by the action of concentrated sulfuric acid on potassium chlorate. 
It is a powerful oxidizing agent and its explosive properties in the presence of a reducing agent were used to make one of the first matches. 
Chlorine Dioxide is widely used in the purification of water and as a bleach in the flour and wood-pulp industry. 

On an industrial scale an aqueous solution of chlorine dioxide is made by passing nitrogen dioxide up a tower packed with a fused mixture of aluminum oxide and clay, down which a solution of sodium chlorate flows.
Because of its high reactivity, chlorine dioxide is best prepared by the reaction of sodium chlorate and moist oxalic acid at90°–100°C, as the product is then dilutedby liberated carbon dioxide.
Commercially the gas is produced by the reaction of sulphuric acid containing chloride ions with sulphur dioxide. 

Chlorine dioxide is widely used as a bleach in flour milling and in wood pulping and also finds applications water purification.
Chlorine dioxide is prepared by passing nitrogen dioxide through sodium chlorate packed in a column: NaClO3 + NO2 → NaNO3 + ClO2
Also, it may be prepared by the reaction of chlorine with sodium chlorite:
2NaClO2 + Cl2 → 2ClO2 + 2NaCl

Alternatively, it may be obtained by the treatment of sodium chlorate or potassium chlorate with sulfur dioxide and sulfuric acid: 2NaClO3 + SO2 + H2SO4 → 2ClO2 + 2 NaHSO4.
Chlorine dioxide was first prepared in 1811 by Sir Humphry Davy.

Melting point: −59 °C
Boiling point: 11 °C
Density: 3.09 g/L
Vapor pressure: 0–22,900 Pa at 20–25 °C
Solubility: Slightly soluble in water
Form: Orange-green gas
Color: Orange-green
Water solubility: Soluble (temperature-dependent)
Exposure limits: TLV–TWA 0.1 ppm (0.3 mg/m³); TLV–STEL 0.3 ppm (ACGIH); IDLH 10 ppm (NIOSH); regulated by ACGIH, MSHA, OSHA, and NIOSH
Dielectric constant: 1.7 (77.0 °C)
Stability: May decompose explosively under shock, friction, or rapid heating; strong oxidizer—reacts violently with combustible or reducing agents, mercury, ammonia, sulfur, and many organics
EPA Primary Drinking Water Standard: MCL: MRDL = 0.81, MCLG: MRDLG = 0.81
LogP: −3.22 to −2.9 (at 20 °C)

Chlorine dioxide is always manufactured on site because of the risk of rapid decomposition. 
In all processes, chlorine dioxide is produced in strong acid solutions from either sodium chlorite or sodium chlorate. 
Small- and medium-scale industrial production of chlorine dioxide utilizes sodium chlorite as the raw material. 

This is typical of water treatment and disinfection applications that require high purity (i.e., chlorine-free) waters. 
Other applications not requiring high purity waters utilize sodium chlorate. 
This is typical of pulp bleaching where large quantities of chlorine dioxide are necessary. 

There are several processes used to generate chlorine dioxide from sodium chlorate. 
In the R2 process, chlorine dioxide is produced from sodium chlorate and sulfuric acid, with sodium chloride as the reducing agent. 
Chlorine dioxide is absorbed from the gas phase in packed towers in cold water, and chlorine leaves the system as a by-product. 

In the Mathieson process, a sulfur dioxide-air mixture is diffused into a solution of sodium chlorate and sulfuric acid. 
Sulfur dioxide is used as the reductant to produce chlorine dioxide with a much lower chlorine content. 
The process also produces sulfuric acid, reducing the overall acid requirement. 

Exit gases from the Mathieson process are passed through a scrubber to remove any unreacted sulfur dioxide. 
The Solvay process uses sodium chlorate and sulfuric acid, with methanol as the reducing agent. 
Products from this process are chlorine dioxide, formic acid, and carbon dioxide. 

In improved Solvay processes, sulfuric acid demand is reduced by crystallizing out the by-products sodium sulfate, sodium sesquisulfate, or sodium bisulfate.
Chlorine dioxide is a flammable, reddish-yellow gas or reddish-brown liquid (below 11℃/52°F) with anirritating odor like chlorine or nitric acid. 
Molecularweight=67.46; Specific gravity (H2O:1)=1.6 (liquid at0℃); Boiling point=11℃; Freezing/Meltingpoint=259℃; Relative vapor density (air=1)=2.3;Vapor pressure=.1 atm at 20℃. Explosive Limits in air:.10%. Hazard Identification (based on NFPA 704 MRating System): Health 3, Flammability 3, Reactivity 3(Shock; Oxidizer). Soluble in water (reactive);solubility=0.3% at 25℃.

The reaction of chlorine with oxygen under conditions of flash photolysis in the presence of ultraviolet light results in trace amounts of chlorine dioxide formation.
Cl2 + 2 O2 →UV
Chlorine Dioxide can decompose violently when separated from diluting substances. 
As a result, preparation methods that involve producing solutions of it without going through a gas-phase stage are often preferred.

In the laboratory, ClO2 can be prepared by oxidation of sodium chlorite with chlorine: NaClO2 + 1⁄2 Cl2 → ClO2 + NaCl
Traditionally, chlorine dioxide for disinfection applications has been made from sodium chlorite or the sodium chlorite–hypochlorite method: 2 NaClO2 + 2 HCl + NaOCl → 2 ClO2 + 3 NaCl + H2O or the sodium chlorite–hydrochloric acid method: 5 NaClO2 + 4 HCl → 5 NaCl + 4 ClO2 + 2 H2O or the chlorite–sulfuric acid method: 4 ClO−2 + 2 H2SO4 → 2 ClO2 + HClO3 + 2 SO2−4 + H2O + HCl

All three methods can produce chlorine dioxide with high chlorite conversion yield. 
Unlike the other processes, the chlorite–sulfuric acid method is completely chlorine-free, although it suffers from the requirement of 25% more chlorite to produce an equivalent amount of chlorine dioxide. 
Alternatively, hydrogen peroxide may be efficiently used in small-scale applications.

Addition of sulfuric acid or any strong acid to chlorate salts produces chlorine dioxide.
Both chlorine dioxide and chlorite react quickly in water and moist body tissues. 
Chlorine Dioxide gas, you might experience irritation in your nose, throat, and lungs. 

Chlorine Dioxide, you might experience irritation in the mouth, esophagus, or stomach. 
Most people will not be exposed to chlorine dioxide or chlorite in amounts large enough to damage other parts of the body, but if you were, you might experience shortness of breath and other respiratory problems because of damage to the substances in blood that carry oxygen throughout the body.
Animal studies have shown effects of chlorine dioxide and chlorite that are similar to those seen in people exposed to very high amounts of these chemicals. 

In addition, exposure to high levels of chlorine dioxide and chlorite in animals both before birth and during early development after birth may cause delays in brain development. 
The levels to which the animals were exposed were much higher than levels that would likely be found in drinking water that has been disinfected with chlorine dioxide.
Chlorine dioxide is a very reactive compound. 

In air, sunlight quickly breaks chlorine dioxide apart into chlorine gas and oxygen. 
In water, chlorine dioxide reacts quickly to form chlorite ions. 
When chlorine dioxide reacts with dissolved organic compounds in water-treatment systems, it forms disinfection by-products, such as chlorite and chlorate ions. 

Like chlorine dioxide, chlorite is very reactive. Since chlorite is an ionic compound, it will exist primarily in water. 
Chlorite ions are mobile in water, and may move into groundwater. 
However, the reaction of chlorite ions with soils and sediments may reduce the concentration of chlorite ions capable of reaching groundwater.

Chlorine Dioxide is a yellow-green gas with an odor similar to chlorine with excellent distribution, penetration and sterilization abilities due to its gaseous nature. 
Although chlorine dioxide has chlorine in its name, its properties are very different, much like carbon dioxide is different than elemental carbon. 
Chlorine dioxide has been recognized as a disinfectant since the early 1900s and has been approved by the US Environmental Protection Agency (EPA) and the US Food and Drug Administration (FDA) for many applications. 

Chlorine Dioxide has been demonstrated effective as a broad spectrum, anti-inflammatory, bactericidal, fungicidal, and virucidal agent, as well as a deodorizer, and also able to inactivate beta-lactams and destroy both pinworms and their eggs.
Chlorine dioxide is a neutral compound—neither an acid nor a base—but it behaves as a powerful oxidizer.

It reacts selectively with sulfur-containing and nitrogen-containing compounds in microorganisms.
This reaction disrupts their metabolic function and destroys their cell walls, leading to rapid disinfection.

It is especially effective in low concentrations, even at parts per million (ppm) levels.
Unlike chlorine, it remains active across a wide pH range (4–10), maintaining consistent disinfecting power.
This stability allows it to work efficiently in both acidic and neutral environments.

In drinking water treatment, chlorine dioxide eliminates bacteria, viruses, and protozoa such as Giardia and Cryptosporidium.
Chlorine Dioxide oxidizes iron and manganese compounds, preventing stains and pipe blockages.
It also removes unpleasant tastes, odors, and sulfides from water supplies.

In the food and beverage industry, chlorine dioxide is used to sanitize processing equipment, tanks, and pipelines.
Chlorine Dioxide disinfects without leaving residues or altering the taste of food products.
It is approved by the U.S. Environmental Protection Agency (EPA) for use in food-contact surfaces.

Chlorine Dioxide is also widely used in agriculture and animal husbandry.
Farmers use chlorine dioxide to disinfect barns, animal drinking water, and hatcheries.
It helps control bacterial and viral infections without harming the animals.

In air treatment systems, chlorine dioxide is used to sterilize ventilation ducts and enclosed spaces.
Its gaseous form can penetrate corners and porous materials, ensuring full-area disinfection.
Chlorine Dioxide is sometimes used in public areas such as airports, hospitals, and offices to control airborne pathogens.

In the medical field, chlorine dioxide is applied as a surface sterilizer and hand sanitizer component.
It destroys infectious microorganisms on surgical instruments and hospital equipment.
Chlorine Dioxide is often used as an alternative to harsh chemicals like glutaraldehyde or formaldehyde.

Because it decomposes into chlorite and chloride ions, chlorine dioxide does not produce toxic residues.
This makes it a preferred option in environmentally regulated industries.
Its breakdown products are less harmful to aquatic life compared to chlorine-based chemicals.

In wastewater treatment, it is used to eliminate odor-causing sulfides and ammonia.
Chlorine Dioxide also oxidizes cyanides and phenols in industrial effluents.
These properties make it an important tool for pollution control and odor management.

Chlorine dioxide is also used in oilfield and pipeline maintenance.
It removes biofilms and prevents the buildup of slime-forming bacteria that corrode metal surfaces.
This extends the life of equipment and ensures smooth fluid flow in pipelines.

In paper and textile bleaching, chlorine dioxide enhances brightness without excessive fiber damage.
Chlorine Dioxide replaces elemental chlorine, which can form harmful dioxins.
Therefore, it contributes to greener and safer industrial bleaching practices.

At high concentrations, chlorine dioxide becomes explosive and unstable.
It can decompose violently when exposed to light, heat, or sparks.
For this reason, it is never stored in pressurized cylinders but produced on-site as needed.

Inhalation of concentrated gas can cause coughing, chest pain, and shortness of breath.
Direct skin or eye contact with solutions can lead to irritation or mild burns.
Prolonged exposure to vapors may damage lung tissue and mucous membranes.

Safe handling of chlorine dioxide requires proper ventilation, gas monitoring, and personal protective equipment.
Workers must use respirators, gloves, and goggles when working near high concentrations.

All storage and generation systems must comply with industrial safety regulations.
Environmentally, chlorine dioxide decomposes into non-persistent products that do not bioaccumulate.

Uses Of Chlorine Dioxide:
Wood-pulp bleaching is the largest use of chlorine dioxide, which is a uniquely selective oxidizer for lignin. 
In general, the trend in the pulp industry has been to eliminate chlorine and hypochochlorite as bleaching agents and replace them with chlorine dioxide. 
Since chlorine dioxide functions via an oxidative reaction rather than a chlorinating reaction, the formation of chlorinated organic compounds is limited. 

Also, unlike other oxidizing agents, chlorine dioxide does not attack cellulose, and thus preserves the mechanical properties of bleached pulp. 
In the final stages of the pulp-bleaching processes, chlorine dioxide is the most frequently used bleaching chemical. 
A unique whiteness can be achieved using chlorine dioxide in kraft pulp, sulfite pulp, and soda pulp processes. 

In the United States, the firststage of the pulp-bleaching process makes use of mixtures of chlorine and chlorine dioxide to reduce the formation of organic chlorine compounds.
In the textile industry, chlorine dioxide is used as a bleaching agent and produces high-quality textile fibers with additional qualities. For example, “shrinkproof” wool owes its qualities to the reaction of chlorine dioxide with the cross-linking sulfur atoms of the wool.

Chlorine dioxide is used for bleaching of wood pulp and for the disinfection (called chlorination) of municipal drinking water,[16][17]: 4–1 treatment of water in oil and gas applications, disinfection in the food industry, microbiological control in cooling towers, and textile bleaching.
As a disinfectant, it is effective even at low concentrations because of its unique qualities.
Chlorine dioxide is used in water disinfection and purification systems.

Chlorine Dioxide destroys bacteria, viruses, and protozoa that cause waterborne diseases.
It is particularly effective against resistant pathogens such as Giardia and Cryptosporidium.
It is added to drinking water treatment plants to oxidize and remove iron, manganese, and sulfides.

These reactions prevent discoloration and unpleasant odors in water supplies.
Chlorine Dioxide also eliminates organic compounds that cause taste and odor problems.

Chlorine dioxide is used in municipal and industrial wastewater treatment.
It neutralizes ammonia, cyanides, phenols, and sulfides, reducing toxicity and odor.
This helps control pollution and improve effluent quality before discharge.

In the food and beverage industry, chlorine dioxide disinfects processing equipment, tanks, and pipelines.
It prevents microbial contamination without leaving harmful chemical residues.
It also sanitizes fruits, vegetables, and meat surfaces to ensure safe food production.

Food producers use chlorine dioxide to rinse and sterilize packaging materials.
It does not affect flavor, color, or texture of food products.
This makes it a preferred disinfectant for ready-to-eat foods and bottled drinks.

Chlorine dioxide is applied in agriculture and animal husbandry.
Farmers use it to sanitize barns, hatcheries, feeding systems, and animal drinking water.
It effectively controls bacterial and viral infections in poultry, cattle, and swine.

In greenhouse and crop protection, it is used to sterilize irrigation water and tools.
It helps prevent the spread of fungal spores, algae, and plant pathogens.
Because it leaves no toxic residue, it can be safely applied around crops.

Chlorine dioxide is used in air disinfection and odor control systems.
Its gaseous form penetrates small areas, killing airborne bacteria, mold, and viruses.
It is commonly used in hospitals, offices, airplanes, and public transportation systems for air purification.

It also disinfects ventilation ducts and HVAC systems.
By eliminating biofilms and fungal growth inside ducts, it improves indoor air quality.
It is especially beneficial for facilities requiring sterile environments.

In the medical field, chlorine dioxide serves as a surface sterilizer and disinfectant.
It is used to decontaminate surgical instruments, hospital floors, and laboratory surfaces.
Because it is less corrosive than chlorine, it can be safely used on stainless steel and plastics.

Medical facilities use chlorine dioxide for infection control and outbreak prevention.
It kills resistant pathogens such as Staphylococcus aureus and Clostridium difficile.
It is also used in hand sanitizers and wound care formulations at controlled concentrations.

In the pulp and paper industry, chlorine dioxide acts as an eco-friendly bleaching agent.
It whitens wood pulp without damaging cellulose fibers.
This allows for high-quality paper production while minimizing environmental pollution.

It replaces traditional chlorine bleaching, which forms toxic chlorinated by-products like dioxins.
As a result, paper mills can comply with stricter environmental regulations.
Its selective oxidation ensures higher brightness and paper strength.

Chlorine dioxide is used in oilfields and pipeline maintenance.
It eliminates biofilms, slime, and microorganisms that corrode pipes and reduce flow.
By preventing bacterial buildup, it extends the lifespan of industrial equipment.

In cooling towers and water systems, chlorine dioxide prevents the growth of algae and Legionella bacteria.
It maintains system efficiency by keeping surfaces clean.
This helps industries avoid health risks like Legionnaires’ disease.

In the textile and electronics sectors, chlorine dioxide is applied as a cleaning and oxidation agent.
It removes organic residues, mold, and dyes from surfaces and fibers.
It is also used for sterilizing semiconductor equipment where contamination control is critical.

Chlorine dioxide is used in environmental sanitation for treating contaminated soil and groundwater.
It breaks down volatile organic compounds (VOCs) and neutralizes pollutants.
This makes it valuable in remediation and decontamination projects.

It is also utilized in emergency response and disaster sanitation.
Authorities use chlorine dioxide to disinfect public water sources and shelters after floods or epidemics.
Its rapid microbial kill rate makes it ideal for crisis hygiene control.

Chlorine dioxide is sometimes used for bleaching of wood pulp in combination with chlorine, but it is used alone in ECF (elemental chlorine-free) bleaching sequences. 
Chlorine Dioxide is used at moderately acidic pH (3.5 to 6). 
The use of chlorine dioxide minimizes the amount of organochlorine compounds produced.

Chlorine Dioxide currently is the most important bleaching method worldwide. 
About 95% of all bleached kraft pulp is made using chlorine dioxide in ECF bleaching sequences.
Chlorine dioxide has been used to bleach flour.

Chlorine dioxide may be used as a fumigant treatment to "sanitize" fruits such as blueberries, raspberries, and strawberries that develop molds and yeast.
Chlorine dioxide may be used to disinfect poultry by spraying or immersing it after slaughtering.
Chlorine dioxide may be used for the disinfection of endoscopes, such as under the trade name Tristel.

Chlorine Dioxide is also available in a trio consisting of a preceding pre-clean with surfactant and a succeeding rinse with deionized water and a low-level antioxidant.
Chlorine dioxide may be used for control of zebra and quagga mussels in water intakes: 4–34 
Chlorine dioxide was shown to be effective in bedbug eradication.

For water purification during camping, disinfecting tablets containing chlorine dioxide are more effective against pathogens than those using household bleach, but typically cost more.
Chlorine dioxide is used as an oxidant for destroying phenols in wastewater streams and for odor control in the air scrubbers of animal byproduct (rendering) plants.
Chlorine Dioxide is also available for use as a deodorant for cars and boats, in chlorine dioxide-generating packages that are activated by water and left in the boat or car overnight.

The water treatment plant at Niagara Falls, New York first used chlorine dioxide for drinking water treatment in 1944 for destroying "taste and odor producing phenolic compounds."
Chlorine dioxide was introduced as a drinking water disinfectant on a large scale in 1956, when Brussels, Belgium, changed from chlorine to chlorine dioxide.
Chlorine Dioxides most common use in water treatment is as a pre-oxidant prior to chlorination of drinking water to destroy natural water impurities that would otherwise produce trihalomethanes upon exposure to free chlorine.

Chlorine Dioxide are suspected carcinogenic disinfection by-products associated with chlorination of naturally occurring organics in raw water.
Chlorine dioxide also produces 70% fewer halomethanes in the presence of natural organic matter compared to when elemental chlorine or bleach is used.
Chlorine dioxide has many applications as an oxidizer or disinfectant.

Chlorine Dioxide can be used for air disinfection[33] and was the principal agent used in the decontamination of buildings in the United States after the 2001 anthrax attacks.
After the disaster of Hurricane Katrina in New Orleans, Louisiana, and the surrounding Gulf Coast, chlorine dioxide was used to eradicate dangerous mold from houses inundated by the flood water.
Bleaching cellulose, paper-pulp, flour, leather, fats and oils, textiles, beeswax; purification of water; taste and odor control of water; cleaning and detanning leather; manufacture of chlorite salts; oxidizing agent; bactericide, antiseptic and deodorizer.

Chlorine dioxide is used for several purposes, including its applications as a bleaching agent to bleach fats, oils, textiles, cellulose, paper pulp, flour, and leather. 
Chlorine Dioxide is also used for purifying water; as an oxidizing agent; as an antiseptic; and in the manufacture of many chlorite salts.
Use large volume of concentrated solution of ferrous salt or bisulfite solution as reducing agent then neutralize and flush to sewer with abundant water.

Chlorine Dioxide is a gas used in bleaching and aging flour. 
Chlorine Dioxide acts on the flour almost instantly, resulting in improved color and dough properties because usage levels are low, the bleaching action is limited.
If this chemical gets into the eyes, remove any contact lenses at once and irrigate immediately for at least15 min, occasionally lifting upper and lower lids.  

If this chemical contacts the skin, remove contaminated clothing and wash immediately with soap and water. 
If this chemical has been inhaled, remove from exposure, begin rescue breathing (using universal precautions, including resuscitation mask) if breathing has stopped and CPR if heart action has stopped. 
Transfer promptly to a medical facility. 
When this chemical has been swallowed, get medical attention. 

Give large quantities of water and in ducevomiting. 
Medical observation is recommended for 24-48 h after breathing overexposure, as pulmonary edema may be delayed. 
As first aid for pulmonary edema, a doctor or authorized paramedic may consider administering a corticosteroid spray.

Storage Of Chlorine Dioxide:
Color Code—Red Stripe: Flammability Hazard:Store separately from all other flammable materials. 
Prior toworking with chlorine dioxide you should be trained on itsproper handling and storage. 
This chemical is a powerful oxidizer, and is shock-, light- and heat-sensitive. 

Chlorine Dioxide is violently explosive in air at concentrations over 10%. 
Keep frozen when not in use. Store in tightly closed containers in a cool, dark, well-ventilated area at temperatures well below 130℃.Gas explosions may occur above 130℃. 
Use only non-sparking tools and equipment, especially when opening and closing containers of this chemical. 

Sources of ignition, such as smoking and open flames, are prohibited where this chemical is used, handled, or stored in a manner that could create potential fire or explosion hazard. 
Use explosion-proof electrical equipment and fittings in storage area. 

Health Hazard Of Chlorine Dioxide:
Chlorine dioxide is highly irritating to the eyes, nose, and throat. 
Inhalation can cause coughing, wheezing, respiratory distress, and congestion in the lungs. 
Its toxicity in humans is moderate to high. 

Its irritant effects in humans can be intense at a con contraption level of 5 ppm in air. 
A concen ration of 19 ppm of the gas inside a bleach tank caused the death of one worker. 

The chronic toxicity signs are mainlydyspnea and asthmatic bronchitis, and in cer tain cases irritation of the gastrointestinaltract. 
Ingestion of the liquid may cause som nolence and respiratory stimulation.

Fire Hazard Of Chlorine Dioxide:
Nonflammable gas; however, it is highly reactive and a strong oxidizing agent. 
Chlo rine dioxide explodes violently upon heating, exposure to sunlight, contact with dust, or when subjected to a spark. 
Detonation occurs at concentrations above 10% in air in the presence of an energy source or catalyst. 

Chlorine Dioxide undergoes violent reactions with organic matter; explosion occurs when the mixture is subjected to shock or a spark. 
Chlorine Dioxide reacts spon taneously with sulfur or phosphorus, caus ing ignition and/or explosion. 

Liquid chlorine dioxide may explode violently when mixed with mercury, caustic potash, caustic soda, or many metal hydrides. 
The gas reacts explo sively with fluorine and with difluoroamine.

Safety Profile Of Chlorine Dioxide:
Moderately toxic by inhalation experimental reproductive effects. 
Mutation data reported an eye irritant a powerful explosive sensitive to spark, impact, sunlight, or heating rapidly to 100℃. 
A powerful oxidzer, concentrations of greater than 10% in air are explosive. 

Explodes on mixing with carbon monoxide, hydrocarbons (e.g., butadiene, ethane, ethylene, methane, propane), fluoramines (e.g., difluoramine, trifluoramine). 
Mixtures with hydrogen explode with sparking or contact with platinum. 
Explodes on contact with mercury, potassium hydroxide, phosphorus pentachloride + chlorine. 

Ignites or explodes on contact with nonmetals (e.g., phosphorus, sulfur, sugar). 
Reacts violently with F2, NHF2, reacts with water or steam to produce toxic and corrosive fumes of HCl. 
When heated to decomposition it emits toxic fumes of Cl-.

In water treatment and purification, chlorine dioxide gas can be toxic if inhaled in high concentrations.
It irritates the eyes, throat, and lungs, leading to coughing and shortness of breath.
Prolonged exposure may cause pulmonary edema or long-term respiratory issues.

Workers handling chlorine dioxide solutions risk skin and eye irritation on contact.
Splashes can result in redness, burning, or chemical dermatitis.
Proper protective equipment — gloves, goggles, and ventilation — is essential during use.

When used in wastewater treatment, chlorine dioxide can react violently with organic matter or reducing agents.
These reactions release heat and toxic gases, increasing the risk of fire or explosion.
Chlorine Dioxide should never be mixed with fuels, ammonia, or concentrated acids outside controlled systems.