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Sodium hypochlorite (NaOCl) in the form of laundry bleach is available in most households. The concentrate is about 5.25 to 6 percent NaOCl, and the pH value is about 12.
I have purchased Calcium hypochlorite (70% available strength in granular form) to disinfect a contaminated water supply, if required. Can any of the above discussion about the disinfecting properties of Sodium hypochlorite be applied to Calcium hypochlorite?
Runninghorses, I plan to do so. First mix up the granulated calcium hypochlorite with the right amount of water for a common household bleach solution, then add water as per directions to further reduce the hypochlorite content and then add the small amount of vinegar to acidify the bleach solution.
It is manufactured using the calcium process and sodium process. Or it can be prepared by the action of slaked lime on chlorine:
Ca(OH)2 + Cl2 → Ca(OCl)2 + H2 [edit]
Properties
It is a yellow white solid which has a strong smell of chlorine. Calcium hypochlorite is not highly soluble in water. For that reason it should preferably be used in soft to middle hard water. There are two types of calcium hypochlorite - a dry form and a hydrated form. The hydrated form is safer to handle.
Calcium hypochlorite reacts with carbon dioxide to form calcium carbonate and release chlorine:
Ca(OCl)2 + CO2 → CaCO3 + Cl2 Calcium hypochlorite reacts with hydrochloric acid to form calcium chloride:
Ca(OCl)2 + 2 HCl → CaCl2 + H2O + Cl2 [edit]
Uses
Calcium hypochlorite is used for the disinfection of drinking water or swimming pool water. For use in outdoor swimming pools, calcium hypochlorite can be used as a sanitiser in combination with a cyanuric acid stabiliser. The stabiliser will reduce the loss of chlorine because of UV radiation.
Calcium hypochlorite is also used for bleaching cotton and linen and used in the manufacture of chloroform.
Retrieved from "http://en.wikipedia.org/wiki/Calcium_hypochlorite" Categories: Antiseptics | Bleaches | Hypochlorites | Calcium compounds
Sodium hypochlorite may be prepared by absorbing chlorine gas in cold sodium hydroxide solution:
2NaOH + Cl2 ⇌ NaCl + NaOCl + H2O Sodium hydroxide and chlorine are commercially produced by the chloralkali process, and there is no need to isolate them to prepare sodium hypochlorite. Hence NaOCl is prepared industrially by the electrolysis of sodium chloride solution without any separation between the anode and the cathode. The solution must be kept below 40 ?C (by cooling coils) to prevent the formation of sodium chlorate.
The commercial solutions always contain significant amounts of sodium chloride (common salt) as the main byproduct, as seen in the equation above.
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Packaging and sale
Household bleach sold for use in laundering clothes is a 3-6% solution of sodium hypochlorite at the time of manufacture. Strength varies from one formulation to another and gradually decreases with long storage.
A 12% solution is widely used in waterworks for the chlorination of water. High-test hypochlorite (HTH) is sold for chlorination of swimming pools and contains approximately 30% sodium hypochlorite. The crystalline salt is also sold for the same use; this salt usually contains less than 50% of sodium hypochlorite. However, the level of "active chlorine" may be much higher.
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Uses
In household bleach form, sodium hypochlorite is used for removal of stains from laundry. It is particularly effective on cotton fiber, which stains easily but bleaches well. 50 to 250 ml per load is usually recommended for a standard-size washer. Hot water increases the activity of the bleach, owing to the thermal decomposition of hypochlorite which ultimately generates environmentally-undesirable chlorate.
A weak solution of 1 % household bleach in warm water is used to sanitize smooth surfaces prior to brewing of beer or wine. Surfaces must be rinsed to avoid imparting flavors to the brew; these chlorinated byproducts of sanitizing surfaces are also harmful.
A 1 in 5 dilution of household bleach with water (1 part bleach to 4 parts water) is effective against many bacteria and some viruses, and is often the disinfectant of choice in cleaning surfaces in hospitals (Primarily in the United States). The solution is corrosive, and needs to be thoroughly removed afterwards, so the bleach disinfection is sometimes followed by an ethanol disinfection.
For shock chlorination of wells or water systems, a 2% solution of household bleach is used. For larger systems, HTH is more practical because lower rates can be used. The alkalinity of the sodium hypochlorite solution also causes the precipitation of minerals such as calcium carbonate, so that the shock chlorination is often accompanied by a clogging effect. The precipitate also preserves bacteria, making this practice somewhat less effective.
Sodium hypochlorite has been used for the disinfection of drinking water, at a concentration equivalent to about 1 liter of household bleach per 4000 liters of water is used. The exact amount required depends on the water chemistry, temperature, contact time, and presence or absence of sediment. In large-scale applications, residual chlorine is measured to titrate the proper dosing rate. For emergency disinfection, the US EPArecommends the use of 2 drops of 5%ac household bleach per quart of water. If the treated water doesn't smell of bleach, 2 more drops are to be added.
The use of chlorine-based disinfectants in domestic water, although widespread, has led to some controversy due to the formation of small quantities of harmful byproducts such as chloroform.
It is also used in dentistry, during root canal treatment, disinfecting the canal and dissolving any remaining pulp tissue. Historically, Henry Drysdale Dakin's solution (0.5%) had been used. Nowadays, 2.5-5.25% solutions are being used.
An alkaline solution (pH 11.0) of sodium hypochlorite is used to treat dilute (< 1 g/L) cyanide wastewater, e.g. rinsewater from an electroplating shop. A well-mixed solution is fully treated when an excess of chlorine is detected. More concentrated cyanide solutions are much more difficult to dispose of.
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Mechanism of action
Like all hypochlorites, sodium hypochlorite is a salt of hypochlorous acid, HClO. Sodium hypochlorite is a colorless, transparent liquid. In water, it partially splits into the sodium cation Na+ and the hypochloriteanion ClO-, while a substantial portion hydrolyses into sodium hydroxide and hypochlorous acid. The oxidizing power of the latter and of the hypochlorite anion cause the bleaching effect. Its negative charge, however, prevents it from diffusing through the cell walls of bacteria and microbes, making it a poor disinfectant. However the hypochlorous acid molecules that exist in equilibrium with the hypochlorite anion, due to their neutral charge and small size, easily diffuse through the cell walls of bacteria. This changes the oxidation-reduction potential (ORP) of the cell, and inactivates the enzyme triosephosphate dehydrogenase. Triosephosphate dehydrogenase (or glyceraldehyde 3-phosphate dehydrogenase/GAPDH) is essential for the digestion of glucose, but is particularly sensitive to oxidizing agents. Its inactivation effectively destroys the micro-organism's ability to function.
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Cautions
Hypochlorite is a strong oxidizer, and the products of the oxidation reactions are corrosive, and can burn skin and cause eye damage, particularly when used in concentrated forms. Hypochlorite must not be mixed with organic materials (e.g. dirt), as the resulting trihalomethanes (also called haloforms) are carcinogenic. The extent of the hazard thus created is a subject of disagreement.
Bleach should never be mixed with other household cleaners, especially not with ones containing acid, since this results in the generation of chlorine gas. It should also never be mixed with anything containing ammonia, since chloramine gas can be gained from this combination. Urine contains ammonia, so bleach should not be used to clean urine spills. Both chlorine gas and chloramine gas are highly toxic. Bleaches also react rather violently with hydrogen peroxide.
It is estimated that there are about 3300 accidents needing hospital treatment caused by sodium hypochlorite solutions each year in British homes (RoSPA, 2002).
[edit]
Jones, F.-L. (1972). "Chlorine poisoning from mixing household cleaners". J. Am. Med. Assoc.222: 1312.
Institut National de Recherche et de S?curit?. (2004). "Eaux et extraits de Javel. Hypochlorite de sodium en solution". Fiche toxicologique n? 157, Paris.
I by ammonia at a 35% solution to mix in with some other chemicals at time to time to boost their efficiency, it is amercing what it can do an amazing are the results if you miss use it, this stuff is not a toy as it can really harm you, and at these %.and is a poison you don’t want to consider inhaling.
Using with below chemicals is not a not minute but second timetable but it gives you some super disinfectants but there is stuff you need to know before you use,
Sulfuric acid is another one of my friends; at 50 % it’s not too dangerous if you know what you doing, a good disinfectant and a super cleaner of surface as long as you remember to neutralize it and sometimes it has to be done in seconds.
The beast is anhydrous hydrochloric acid, this is one I don’t dare to store by the barrel, and the mother will eat your concrete floor at the same time it takes out your lungs at these strengths.
Hydrogen nitrate is something you might think as harsh especially if mixed with some of above but has its place in 1 Litter bottles max as far as im concerned. Not something you need weekly.
Lime bought by us in one tone tanks is cheap and the resale value diluted to 1-5 % is excellent, just mix in a bit of magic and bring the ph to accepted value without harming the wash properties and you have a winner, basically following your countries guidelines you cant make much of it.
On the other hand Virkon S bought in lets say 10 Kg packages is cheap and safe, it gives you a 1000 litters of disinfection solution, the main hazard in poses instead of soluble pills they sell to consumers is possibility of inhaling the dust when pouring it, it is worth using a mask or standing above wind . This is what I recommend to you all who are thinking of foot wash before entering your premises, it is also excellent when used as a spray, you not supposed to use it on your skin but in a emergency situation its quite harmless if you have to use it once or twice (not on the face) and afterward rinse with water.
Washing with everyday soaps using bathroom cleaners and most household cleaners is a ph game.
Ever wonder what is it they use at the new brushless car washes and what would happen to your paint job if the neutralising shower failed to operate, the one that comes right behind before you even notice it? It’s a chemical reaction acid and lime, basic cleaning class one.
And the of course there is the one with a topic skin, also one in our family, never any soaps, all washing done by oils.
Vinegar is something everyone should look up, it’s the most versatile stuff there is, as far as im concerned it is one of the best.
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