Sodium hypochlorite is a chemical compound of sodium, oxygen and chlorine that has been used for centuries for bleaching and disinfection. Sodium hypochlorites, also known as NaOCl, are chemical compounds of Na oxygen, chlorine and Cl, which have been used as bleach or disinfectant for over half a century. Sodium hypochlorite, NaCl O, is the sodium oxygen (chlorine) used in bleaching and cleaning.

Sodium hypochlorite (NaClO) can be bleached with commercial liquid bleaches, usually available in 6, 12 or 15 percent solution.

Sodium hypochlorite solution is available in most quantities immediately, but not in large quantities. In the case of NaCl solution, the functional principle consists of a series of electrolytic reactions when a certain voltage is applied to the electrolysis tube with the Na-Cl solution. 40% of the sodium chloride is removed from the crystallizer (line 44) and 46% of the sodium hypochlamine solution is recovered through the conveyor pipe.

In the second stage, the crystallizer is continuously fed with the sodium hypochlorite solution and the hydrogen is fed into a closed hydrogen disinfection tank (line 44), which can also serve as a solution storage tank. The absorption column from which the salt water evaporates into the atmosphere and the absorption columns from which a sodium-hypochlorite solution emerges are carried out by diluting the pure chlorine (chlorine) with suitable stirring of the crystallizer.

In the next step, the sodium hypochlorite solution is diluted with sodium thiosulfate (see next steps). After mixing the 5% chlorine solution, the water can be disinfected with normal chlorine bleach.

Make 1% household bleach by mixing 4 teaspoons of bleach and 1 litre of water with 1 / 4 teaspoon of sodium hypochlorite and 1 teaspoon of sodium thiosulfate. To make your own bleaching solution, mix 1 part of household bleach with 2 parts of water, 1 tablespoon of salt and 2 tablespoons of sugar.

Dilute 1 / 4 teaspoon of sodium hypochlorite and 1 tablespoon of salt to make a brine of 1 litre of water with 1 gram of active chlorine per litre. Then electrolyze the brine to a sodium hypochlorite solution containing 150 grams of active chlorine per litre.

The retention of sodium hypochlorite in the solution is low and the filtration of sodium chloride is rapid, at least up to 400 micrometres. About 50% of this is converted into hypochlorites, and about 3 kg of this is needed to form 1 kg of chlorine. If the residence time for removing sodium chloride from the water (say, from 1 litre of water with 1 gram of active chlorine per litre) is close to 400 micrometres, which is sufficient to convert about 1.5 kg per litre into 1 kg of chlorine, there is no subsequent filtering. The precipitated sodium chlorides have a satisfactory crystal size but are dissolved in water at a rate of 1,000 to 2,500 micrometres per litre.    

This chemical is produced by adding caustic soda with chlorine gas to produce sodium hypochlorite, a water salt. The second stage allows a concentrated sodium hypochlorite solution to be obtained from the precipitation of the precipitated sodium chloride. The exchanger is placed in a circuit with the mother liquor crystallizer and a high, temperature and low-pressure water solution of 1,000 to 2,500 micrometres is obtained.

You need to make a 5% chlorine solution to disinfect a small amount of water. Household bleaching, which contains about 5 percent sodium hypochlorite, can be used as a disinfectant in the event of pesticide leakage. Be sure to buy simple, fragrant bleach that is clearly labelled on the container.    

Inserting column 10 (left) into the crystallizer (40) with pump 31, see points 5 and 3. Then carefully weigh the sodium hypochlorite solution (5% chlorine solution) and the water (1.5%). 

When the solution is heated, sodium hypochlorite breaks down alongside salt and oxygen, and the chlorine gas remains exposed to the atmosphere. When added to the water, the chlorine content decreases as it reacts with organic matter and microbes. By releasing hydroxyions, the solvent acts as a solvent in contact with organs and tissues and forms chloramines by combining it with proteins and amino groups. In the presence of water and water - free organic material such as organic solvents and organic acids - the chlorine gas evaporates, leaving behind the sodium hypochlorite (Na - OCl) that is produced.

In order to avoid the degradation of the resulting sodium hypochlorite, it is necessary to keep sufficient excess sodium hydroxide in the salt solution for it to form. This reaction is carried out by chlorinating sodium hydride to sodium 5 carbonate, where it remains until the solution becomes acidic, whereupon the pituitary chlorites are broken down and form chloramines.

Given the antimicrobial effect that can be achieved in a less concentrated solution, 1,2-sodium hypochlorites is a better option. The aqueous solution of sodium hypochlorite has a strength of 3% by weight and an aqueous strong sodium hydride corresponding to the said solution with a pH of 1.5, which corresponds to a concentration of about 25% NaClO. [1 - 352 - 198] describes a method for the extraction of sodium hypochlamite, which is about 1 / 25 NaCIO and provides a solution to the crystal size problem of the salt and regulates the excess of sodium hydroxides.