Sodium chlorate hypochlorite

Oxalic acid Furfuryl alcohol, silver, mercury, sodium chlorate, sodium chlorite, sodium hypochlorite... 

NaClO sodium hypochlorite NaC102 sodium chlorite NaClO sodium chlorate NaClO sodium perchlorate... 

A study of the North American bleaching agent market was completed in June 1988 and includes consumption quantities for the year 1986 (156). Chlorine consumption for 1986 was 1.86 x 10 t. The North American consumption volume of other chlorine-containing bleaching compounds including sodium and calcium hypochlorite, chlorinated isocyanurates, and hydantoins was 286,000 t. The 1986 North American consumption of sodium chlorate was estimated at 5.5 x 10 t. 

Chlora.tes. Sodium chlorate is produced by the electrolysis of sodium chloride at pH 6.5—7.5 in a one-compartment cell. DSA anodes and steel cathodes are generally used in chlorate cells. The electrolysis products, hypochlorous acid, and hypochlorite ions, react chemically to produce chlorate (eq. 

Nitropropane Nitrosyl fluoride Nitrosyl perchlorate Nitrourea Nitrous acid Nitryl chloride Oxalic acid See under Nitromethane chlorosulfonic acid, oleum Haloalkenes, metals, nonmetals Acetones, amines, diethyl ether, metal salts, organic materials Mercury(II) and silver salts Phosphine, phosphorus trichloride, silver nitrate, semicarbazone Ammonia, sulfur trioxide, tin(IV) bromide and iodide Furfuryl alcohol, silver, mercury, sodium chlorate, sodium chlorite, sodium hypochlorite... 

Fig. 14.4 Sodium chlorate concentration in cell-liquor before and after recycling of hypochlorite.

This is the reaction by which sodium chlorate is manufactured commercially. In the present context, however, the formation of chlorates is generally undesirable since they tend to be explosive and toxic. The reaction given by Equation 26.2 is strongly affected by pH and temperature as well as the hypochlorite ion concentration. As the alkali becomes exhausted, and the system is thus over-chlorinated, the rate of chlorate formation is greatly accelerated as the reaction becomes auto-catalysed by hypo-chlorous acid. The acid is formed by... 

The acid, referred to as tetra acid , is prepared as follows In a Friedel-Crafts reaction, acenaphthene 72 is reacted with malonic dinitrile and aluminum chloride. The resulting condensation product 75 is oxidized with sodium chlorate/hy-drochloric acid to form the dichloroacenaphthindandione 76. Oxidation with sodium hypochlorite solution/sodium permanganate affords naphthalene tetracar-boxylic acid 68, mostly existing as the monoanhydride 68a. The dianhydride, on the other hand, evolves only after drying at approx. 150°C. 

Nitric acid. Sulfuric acid, 3,5-DichloranUine Hypochlorites (calciirm/sodium). Glycerin Hydrochloric acid. Aluminum metal Sodium hydroxide. Aluminum metal Sodium chlorate. Fuel oil Aluminum, Sulfur, Starch Sugar, Sodium peroxide... 

Sodium Hypochlorite (see p. 512).—The commercial solution (about 15%) is available. Usual impurities caustic soda, sodium chloride and sodium chlorate. 

Contact of the solid oxidant with organic thiols or sulfides may cause a violent reaction and flash fire [1]. This procedure was recommended formerly for treating spills of sulfur compounds [2,3], but is now withdrawn as potentially hazardous. Use of an aqueous solution of up to 15% concentration, or of 5% sodium hypochlorite solution is recommended [1], Addition of 10 g of oxidant to 5 ml portions of 1-propanethiol or isobutanethiol led to explosions [4]. Application of factorial design techniques to experimental planning gave specific conditions for the safe oxidation of organic sulfides to sulfoxides using calcium hypochlorite or sodium chlorate [5]. 

Chlorine and hypochlorite thus obtained are traditional oxidizing agents of organic pollutants. Chlorine dioxide is another known oxidant for water treatment, which can be generated in divided cells containing sodium chlorite or sodium chlorate. This last compound can also be produced anodically from hypochlorite oxidation ... 

In Eq. (18.1), sodium hypochlorite is produced by feeding chlorine into a 30% aqueous caustic solution in a circulating reactor/cooler system. To avoid sodium chlorate formation, the reaction temperature is kept below 30°C and NaOH concentration is kept below 1 g/liter. Typical reaction temperature is 5 °C132. 

Sodium hypochlorite solution, commonly called bleach, is a light yellowish liquid with a characteristic chlorine-like odor. It is a powerful oxidizing agent, and is used extensively in disinfections and decontamination procedures. It is quite stable at room temperature, but decomposes when heated forming sodium chlorate and salt. It can be easily prepared using a diaphragm cell, or by passing chlorine gas into a cold dilute sodium hydroxide solution. 

Summary Sodium chlorate can be made using an electrochemical process whereby pickling salt is electrolyzed under slightly different conditions then as in the preparation of bleach. During the process, some chlorine gas is evolved at the anode, and sodium hydroxide is liberated at the cathode. As the process proceeds, the chlorine reacts with the sodium hydroxide forming sodium hypochlorite (bleach) this bleach then spontaneous oxidizes under heat to form sodium chlorate and sodium chloride. Some chlorine gas does escape, so use proper ventilation when carrying out this operation. 

Chlor-alkali production — With a 63% production volume of the total world chlorine capacity of about 43.4 million tons (in 1998), the chlor-alkali (or chlorine-caustic) industry is one of the largest electrochemical technologies in the world. Chlorine, Cl2, with its main co-product sodium hydroxide, NaOH, has been produced on industrial scale for more than a century by -> electrolysis of brine, a saturated solution of sodium chloride (-> alkali chloride electrolysis). Today, they are among the top ten chemicals produced in the world. Sodium chlorate (NaC103) and sodium hypochlorite (NaOCl, bleach ) are important side products of the... 

For optimum operation, the cell temperature is maintained at 65-75°C with a pH of 6.9. Current efficiencies of over 90 percent have been reported with a power consumption of 4500-5800 kWhr per metric ton of sodium chlorate produced. Coated titanium metal anodes and steel cathodes are used, and small amounts of dichromate are added to the cell liquor to prevent the cathodic reduction of chlorate and hypochlorite. The cell liquor contains about 50 percent NaC103, which may be used as is, or evaporated to 75 percent... 

Sodium hypochlorite is also manufactured by the electrolysis of sodium-chloride solution without a diaphragm (p. 97), the solution being less concentrated than that prepared by the chlorine process from sodium hydroxide, but free from the excess of alkali characteristic of that prepared by the older method.2 The process is carried out either in the apparatus designed by Kellner,3 or in that of Haas-Oettel,4 sodium chlorate being a by-product (v. infra). It is noteworthy that electrolysis of sodium-chloride solution with an alternating current also produces sodium hypochlorite.5... 

Sodium chlorate, NaC103.—When chlorine is passed into a hot solution of sodium hydroxide, the hypochlorite primarily formed changes into a mixture of chlorate and chloride, both salts crystallizing out ... 

Write formulas for each of the following compounds (a) sodium chloride, (b) sodium chlorate, (c) sodium chlorite, (d) sodium hypochlorite, and (e) sodium perchlorate. 

To reduce production of chlorinated organics during bleaching, the pulp and paper industry has replaced chlorine with chlorine dioxide. Chlorine dioxide or its primary precursor, sodium chlorate, can be produced by the low-tonnage chlorine industry with the same hardware that is used for synthesis of chlorine and hypochlorite. This simple transition from chlorine to chlorine dioxide synthesis may be the reason for the less-than-anticipated usage of hydrogen peroxide in the pulp and paper industry. Increasing use of chlorine dioxide could also lead to its applications in other effluent treatment areas such as industrial wastewater remediation. 

How many faradays of electricity would be required to oxidize 1 mole of sodium chloride in alkaline solution to sodium hypochlorite How many faradays would be required to oxidize 1 mole of sodium chloride to sodium chlorate To sodium perchlorate ... 

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