معالجة مياه الشرب (استخدام البيروكسيد فى تطهير مياه الشرب)

Peroxides
Oxidants

Chemical oxidation processes use (chemical) oxidants to reduce COD/BOD levels, and to remove both organic and oxidisable inorganic components.
The processes can completely oxidise organic materials to carbon dioxide and water, although it is often not necessary to operate the processes to this level of treatment

Hydrogen peroxide

Hydrogen peroxide is widely used thanks to its properties; it is a safe, effective, powerful and versatile oxidant.
The main applications of H2O2 are oxidation to aid odour control and corrosion control, organic oxidation, metal oxidation and toxicity oxidation.
The most difficult pollutants to oxidize may require H2O2to be activated with catalysts such as iron, copper, manganese or other transition metal compounds.

Hydrogen Peroxide
The hydrogen peroxide is widely used thanks to its very good properties.

Indeed H2O2 is safe, effective, powerful and versatile oxidant.

The table below lists the oxidation Potential scale, hydrogen peroxide is more powerful than chlorine or chlorine dioxide for instance. Furthermore through catalysis, hydrogen peroxide can be converted into hydroxyl radicals which is the second stronger oxidant after fluorine.
There are several advantages in using H2O2:
• Powerful
• Safe
• Versatile
• Selective
• Widely used
The main applications of H2O2 are numerous, such as the odor control, corrosion control, BOD/COD removal, organic oxidation, metal oxidation, toxicity oxidation and disinfection.
Besides hydrogen peroxide can be combinated with different processes to improve the results:
flocculation/precipitation,
Air flotation,
biotreatement,
filtration,
carbon adsorption,
air scrubbers
incineration.
The most difficult pollutant to oxidize may require H2O2 to be activated with catalysts such as iron, copper, manganese or other transition metal compounds.
The most common used solution catalyst is iron, which when is used with H2O2 is called Fenton's reaction.

Hydrogen peroxide
It can also be used for water disinfection.
the characteristics of hydrogen peroxide
Peroxide is a chemical compound that contains the peroxide ion (O22-).

The peroxide ion consists of a single bond between two oxygen atoms: (O-O)2-. It is a strong oxidiser.

Hydrogen peroxide has the chemical formula H2O2 and the following structural formula:
H-O-O-H
The hydrogen peroxide molecule contains one extra oxygen atom, compared to the more stable water molecule.
The bond between the two oxygen atoms, the so-called peroxide bond, is broken while two H-O radicals are formed.
These radicals quickly react with other substances, while new radicals are formed and a chain reaction takes place.
Hydrogen peroxide solutions look like water and can be dissolved in water unrestrainedly.
At high concentrations these solutions give off an irritating, acidic smell.
Hydrogen peroxide is inflammable.
At low temperatures it becomes solid.
The amount of hydrogen peroxide in the solution is expressed in weight percentage.
For water treatment, concentrations of 35 or 50 % hydrogen peroxide are used.
Selectivity
Hydrogen peroxide is used for different applications, because it is very selective.
By changing the reaction conditions (temperature, pH, dose, reaction time and the addition of a catalyser), hydrogen peroxide will attack different pollutions.
Corrosiveness of hydrogen peroxide
The corrosiveness of process water due to hydrogen peroxide depends on the amount of dissolved oxygen that is produced.
Oxygen corrodes iron-containing metals.
The amount of iron and the pH are a greater influence on corrosiveness than the concentration of hydrogen peroxide is.
Destruction of hydrogen peroxide
Hydrogen peroxide can disintegrate during transport.
Oxygen and heat are released. Hydrogen peroxide itself is inflammable, but the oxygen can enhance the inflammation of other substances.
In diluted solutions, the heat is absorbed by water.
In concentrated solutions, the temperature of the solution is increased, accelerating hydrogen peroxide destruction.
The rate of destruction is multiplied with 2,2 for every 10 °C of rise in temperature.
The alkalinity and presence of pollutions also accelerate the destruction of hydrogen peroxide.

For the production of hydrogen peroxide, special catalysers are used to make sure that hydrogen peroxide is not destroyed by pollutants in the water.
hydrogen peroxide production
hydrogen peroxide is a commercial product.
It was first produced in the United Kingdom by burning barium salt (Ba), which produced barium peroxide (BaO2).
Subsequently the barium peroxide was dissolved in water and hydrogen peroxide was produced.
the production of hydrogen peroxide has largely increased.
hydrogen peroxide transporting and storing
Hydrogen peroxide must be transported in polyethylene, stainless steel or aluminium containers.
When hydrogen peroxide comes in contact with flammable substances, such as wood, paper, oil or cotton (cellulose), spontaneous ignition may occur.
When hydrogen peroxide is mixed with organic matter, such as alcohols, acetone and other ketones, aldehydes and glycerol, heavy explosions may occur.

When hydrogen peroxide comes in contact with substances, such as iron, copper, chromium, lead, silver, manganese, sodium, potassium, magnesium, nickel, gold, platinum, metalloids, metal oxides or metal salts, this may result in powerful explosions.
This is why hydrogen peroxide is usually transported in diluted form.
the applications of hydrogen peroxide
The application of hydrogen peroxide was bleaching straw hats, which were fashionable in the beginning of the twentieth century.
hydrogen peroxide was produced through electrolysis.
This method produced pure hydrogen peroxide.
Nowadays, self-oxidation processes are used to produce hydrogen peroxide.
During these processes, hydrogen is the raw material.
Versatility of hydrogen peroxide
Hydrogen peroxide is versatile, it can be used for many applications.
It can be used in all media; air, water, waste water and soils.
It is sometimes used combined with other agents, to enhance and accelerate processes.
Hydrogen peroxide is most commonly used to remove pollutants from waste water and from air.
It contests bacterial growth (for example bio fouling in water systems) and it can enhance bacterial growth (for example bio remediation of polluted soils and ground water) through oxygen addition.
It can also be used to treat pollutions that can be easily oxidized (for example iron and sulphides) and pollutions that are difficult to oxidise (for example dissolved solids, gasoline and pesticides).

Finally, it can be used to bleach paper, textile, teeth and hair or to produce food, minerals, petrochemical substances or washing powder. In pure form, hydrogen peroxide is used as an oxygen provider to drive Russian submarines.
hydrogen peroxide be used as an oxidiser
Hydrogen peroxide is a strong oxidiser.
It is more powerful than chlorine (Cl2), chlorine dioxide (ClO2) and potassium permanganate (KMnO4).
Through catalysis, hydrogen peroxide can be converted into hydroxyradicals (OH).
The oxidation potential of hydrogen peroxide is just below that of ozone.

hydrogen peroxide dosing
Most hydrogen peroxide applications consist of hydrogen peroxide injection into flowing water.
No other chemicals or equipment are required.
This application is used to control biological growth, to add oxygen, to remove chlorine residues and to oxidize sulphides, sulphites, metals and other easily oxidized materials.
The suitability of hydrogen peroxide for these applications is influenced by pH, temperature and reaction time.
Catalytic hydrogen peroxide
Pollutions that are not easily oxidized, require hydrogen peroxide activation by catalysers (iron, manganese or other metalloids).
These catalysers can also be used to enhance hydrogen peroxide reactions, which would otherwise take hours or days.
the advanced oxidation processes
Advanced oxidation processes are a new development in the field of hydrogen peroxide disinfection.
These processes produce reactive oxygen radicals, without the interference of metal catalysers.
Examples are the combination of hydrogen peroxide with ozone (peroxone) or Ultra Violet Light.
The result of these methods is far-reaching oxidation of difficultly degradable substances, without the production of residues or sludge.
These methods are used worldwide for groundwater treatment, for drinking water and process water treatment and for organic matter disinfection and removal from industrial wastewater.
hydrogen peroxide disinfection working
Among other applications, hydrogen peroxide is used as a disinfectant.
It is used to treat inflammation of the gums and to disinfect (drinking) water.
It is also used to combat excessive microbial growth in water systems and cooling towers.
, hydrogen peroxide is used more and more frequently to treat individual water supplies.
It is used to prevent the formation of colors, tastes, corrosion and scaling by pollution degradation (iron, manganese, sulphates) and micro-organism degradation.
Hydrogen peroxide reacts very fast. It will than disintegrate into hydrogen and water, without the formation of byproducts. This increases the amount of oxygen in water.
The disinfection mechanism of hydrogen peroxide is based on the release of free oxygen radicals:
H2O2 → H2O + O2

Pollutions are decomposed by free oxygen radicals, and only water remains.
Free radicals have both oxidising and disinfecting abilities.
Hydrogen peroxide eliminates proteins through oxidation.

Peroxides such as hydrogen peroxide (H2O2), perborate, peroxiphosphate and persulphate, are good disinfectants and oxidisers.
In general these can adequately remove micro-organisms.
However, these peroxides are very unstable.

Perborates are very toxic. Peracetic acid (PAA) is a strong acid. It can be very agressive in its pure form.
Stabilised persulphates can be used to replace chlorine for waste water treatment.
hydrogen peroxide used for drinking water disinfection
hydrogen peroxide was first used for drinking water disinfection in Eastern Europe.
It is known for its high oxidative and biocidal efficiency.
Hydrogen peroxide has not been used often for drinking water disinfection, but it's popularity seems to increase.
It is often used combined with ozone, silver orUV.
hydrogen peroxide used for swimming pool disinfection
The application of peroxides for disinfection and water treatment are limited. Recently, more stable forms have been developed, which can be used for application in swimming pools.

Hydrogen peroxide disinfection requires a high dose.
The main disadvantage is the small disinfecting and oxidising ability of hydrogen peroxide at active concentrations (tens of milligrams per litre), which are required for swimming pool disinfection.
Another problem is the quick decomposition of hydrogen peroxide in water and the presence of oxygen radicals.
Through stabilizer addition, the decomposition of hydrogen peroxide is delayed and the disinfection ability can be maintained.

Compared with chlorine, bromine, ozone and other disinfectants, hydrogen peroxide is not a very powerful disinfectant.
Swimming pools disinfection by hydrogen peroxide is not allowed, unless it is used in combination with other disinfectants (UV, ozone, silver salts or ammonia quart salts).
Hydrogen peroxide improves the disinfection ability of other disinfectants.
hydrogen peroxide used for cooling tower water disinfection
Hydrogen peroxide can be used for cooling tower water disinfection, when it is combined with other disinfectants.
Peracetic acid (CH3COOH, PAA) can also be used for cooling tower water disinfection.
hydrogen peroxide remove chlorine
Hydrogen peroxide can be used for dechlorination, in other words to remove residual chlorine.
Residual chlorine forms corrosive acids when it is oxidised by air or condensates on process systems.

When chlorine reacts with hydrogen peroxide, hydrogen peroxide falls apart into water and oxygen.
Chlorine gas hydrolyses into hypochlorous acid (HOCl), which subsequently ionises into hypochlorite ions (OCl).

Cl2 + HOCl + H+ + Cl
HOCl + H+ + Cl

After tha, hydrogen peroxide reacts with hypochlorite:

OCl- + H2O2 (g) -> Cl- + H2O + O2

The reaction between hydrogen peroxide and hypochlorite takes place very quickly.
Other organic and inorganic substances cannot react with hypochlorite.
the advantages and disadvantages of hydrogen peroxide using
Advantages
Contrary to other chemical substances, hydrogen peroxide does not produce residues or gasses.
Safety depends on the applied concentration, because hydrogen peroxide is completely water soluble.
Disadvantages
Hydrogen peroxide is a powerful oxidizer.
It reacts with a variety of substances.
It is therefore diluted during transport, as a safety measure.
However, for hydrogen peroxide disinfection, high concentrations are required.

Hydrogen peroxide slowly decomposes into water and oxygen.
An elevation of temperature and the presence of pollutions enhance this process.

The concentration of hydrogen peroxide in a solution slowly decreases. This is caused by the following reaction:
2 H2O2 → 2 H2O + O2

This is a redox reaction.
Hydrogen molecules partly function as reductors and partly as oxidizers.
Is hydrogen peroxide efficient?
The efficiency of hydrogen peroxide depends on several factors, such as pH, catalysers, temperature, peroxide concentration and reaction time.
By
Colonel.dr
Bahaa badr
Chemical consultant

المؤكسدات
هى الطرق الكيميائية المؤكسدة لاستخدام مؤكسد كيميائى لتقليل مستويات الاكسجين الحيوى والاكسجين الكيماوى المذابين ولازالة المواد العضوية وغير العضوية المتاكسدة وغير المرغوب فيها وذلك باكسدتها الى ثانى كربون وماء
البيروكسيد
فوق اكسيد الهيدروجين يستخدم بكثرة نظرا لخواصه المتعددة لانه امن/مؤثر/قوى التاثير/مؤكسد قوى
ويستخدم عامة للاكسدة للتخلص من الرائحة والتاكل والمخلفات العضوية والسميات
عندما يكون الملوث قوى نحتاج الى الاستعانة بعامل حفاز قوى لزيادة قوة الاكسدة بالبيروكسيد كاضافة عناصر الحديد او النحاس المنجنيز اليه
خواص البيروكسيد
هو مركب كيميائى يحتوى على ذرتى اكسجين نشطيتين تترتبط برابطة احادية تسمى برابطة البيروكسيد والتى تنكسر عند تكون الراديكال الثنائى(هيدروجين-اكسجين) والذى يتفاعل مع اى عنصر بحواره مكملا تفاعل الاكسدة المطلوب
هو يذوب فى الماء ويعطى رائحة الاحماض وغير قابل للاشتعال وعند درجات الحرارة المنخفضة يتحول للحالة الصلبة
وبناءا على كمية البيروكسيد فى المحلول يعبر عنها بالنسبة المئويه للمحلول
جرعة البيروكسيد المطلوبة لمعالجة المياه=35-50% بناءا على نوعية المياه(الشرب/الصرف الصناعى
يحضر البيروكسيد بحرق املاح الباريوم فينتج بيروكسيد الباريوم الذى يحل فى الماء فينتج البيروكسيد
يعبا وينقل البيروكسيد فى براميل من البولى ايثيلين او الاستانلس استيل او الالومونيوم
فاذا احتك البيروكسيد بالمواد القابلة للاشتعال يحدث حريق لحظى واذا مزج مع المواد العضوية كالالدهيدات والكحوليات والكيتونات او الجليسرول فيحدث انفجار ونفس الشئ يحدث عند الاتحاد المباشر مع المعادن الثقيلة او املاحها
ولذلك دائما ينقل البيروكسيد فى الصورة المخففة التركيز
يستخدم البيروكسيد فى معالجة مياه الشرب ومياه الصرف الصناعى وكذلك الهواء والتربة كمزيل للملوثات بهم وكمزيل للبكتريا والميكروبات وكذلك مزيل قوى للحديد وكبريتيد الهيدروجين والملوثات الصعبة كالجازولين والمبيدات
يعتبر مؤكسد اكثر قوة من الكلورين وثانى اكسيد الكلور وبرمنجنات البوتاسيوم
وفى اثناء وجود عوامل حفازة تزيد درجة اكسدته لتحوله الى هيروكسيل راديكال حيث يعتبر ثانى اقوى مؤكسد بعد الاوزون
يستخدم كمطهر للمياه ومزيل لمسببات اللون/الرائحة/الطعم/التاكل/القشور/الاملاح كالحديد.المنجنيز.الكبريتات/الميكروبات ولانه يتفاعل بسرعة كبيرة محققا اكسدة قوية وفعالة فى زمن قياسى ويزود من كميه الاكسجين الصحية للمياه
مشكلة البيروكسيدات انها غير ثابتة وانواعها سامة وتكون احماض قوية
ومن اهم انواعها البيرسلفات الثابت الذى يستخدم بديلا عن الكلور فى معالجة مياه الصرف الصناعى
لايستخدم البيروكسيد مباشرة فى حمامات السباحة اومياه الشرب النهائية الا مع استخدام الاوزون او املاح الفضة او وحدات الاشعة فوق البنفسجية او املاح الامونيا الرباعية
يستخدم البيروكسيد متحدا مع البير اسيتيك اسيد كمطهر قوى لدورات ابراج التبريد المفتوجة والمغلقة
يستخدم البيروكسيد لازالة رواسب الكلور المستخدم فى التطهير وذلك باكسدة الكلور المترسب الى هيبوكلوريس اسيد والذى يتاين الى هيبوكلوريت ايون ويصبح غير مؤثر على نوعية المياه حيث يحدث التفاعل بسرعة ولاينجح اى من المواد العضوية وغير العضوية فى التفاعل مع الهيبوكلوريت الناتج
عقيد دكتور
بهاء بدر الدين

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