Clorox, oxidant

Chlorine is used to make laundry bleach, such as Clorox, by dissolving chlorine in sodium hydroxide to give a weak solution of sodium hypochlorite. Sodium hypochlorite slowly releases an active form of oxygen, which reacts with many forms of soil and dirt to destroy them by oxidation. Sodium hypochlorite also rapidly destroys bacteria, viruses, and molds. 

Sodium hypochlorite NaOCl is a strong oxidizer used in swimming pools, and when diluted to 5.25%, it is known as the laundry bleach Clorox. 

Synonym Gamma-Chloropropylene Oxide 3-Chloro-1,2-Propylene Oxide Chlorosulfonic Acid Chlorothene Chiorotoluene, Alpha Alpha-Chlorotoluene Omega-Chlorotoluene Chlorotrifluoroethylene Chlorotrimethylsilane Chlorsulfonic Acid Clilorylen Clip Chromic Acid Chromic Anhydride Chromic Oxide Chromium (VI) Dioxychloride Chromium Oxychloride Chromium Trioxide Chromyl Chloride Cianurina Citric Acid Citric Acid, Diammonium Salt Clarified Oil Clorox Cc Ral Coal Tar Oil Cobalt Acetate Cobalt Acetate Tetrahydrate Cobalt (II) Acetate Cobalt Chloride Cobalt (II) Chloride Cobaltous Acetate Cobaltous Chloride Cobaltous Chloride Dihydrate Cobaltous Chloride Hexahydrate Cobaltous Nitrate Cobaltous Nitrate Hexahydrate Cobaltous Sulfate Heptahydrate Cobalt Nitrate Cobalt (II) Nitrate Cobalt Sulfate Compound Name Epichlorohydrin Epichlorohydrin Chlorosulfonic Acid Trichloroethane Benzyl Chloride Benzyl Chloride Benzyl Chloride Trifluorochloroethylene Trimethylchlorosilane Chlorosulfonic Acid Trichloroethylene Cumene Hydroperoxide Chromic Anhydride Chromic Anhydride Chromic Anhydride Chromyl Chloride Chromyl Chloride Chromic Anhydride Chromyl Chloride Mercuric Cyanide Citric Acid Ammonium Citrate Oil Clarified Sodium Hypochlorite Coumaphos Oil Coal Tar Cobalt Acetate Cobalt Acetate Cobalt Acetate Cobalt Chloride Cobalt Chloride Cobalt Acetate Cobalt Chloride Cobalt Chloride Cobalt Chloride Cobalt Nitrate Cobalt Nitrate Cobalt Sulfate Cobalt Nitrate Cobalt Nitrate Cobalt Sulfate... 

Such solutions are marketed as household bleaches and disinfectants (Javex and Clorox, for example) and are used industrially as oxidants. Given the chemical and biological activity of hypochlorite solutions, however, it is necessary to destroy any significant quantities of hypochlorites in wastewater before it is discharged into rivers or lakes. This can be done by reduction with sulfite ion or hydrogen peroxide ... 

Caution. The reaction should be carried out in a well-ventilated hood, because benzenethiol(thiophenol) and carbon monoxide are toxic. The latter is evolved during the reaction. Any excess thiophenol can be destroyed by treatment with a mild oxidant such as chlorine water (5% NaOCl solution, known commercially as Clorox). 

The anode liquid can be evaporated (by simply boiling-off the water), to yield crystals offerrous chloride. Before hand, if you like, add a few drops of your anode liquid to a small sample of Clorox bleach or hydrogen peroxide. Wham What happened It turned black The ferrous chloride was oxidized by the Clorox bleach (or hydrogen peroxide) to ferric chloride. Ferric chloride is commonly used by electricians to etch printed circuit boards ... 

Into a 250-mL Erlenmeyer flask in the hood place 8 mL (0.075 mole) of cyciohexanoi and 4 mL of acetic acid. Introduce a thermometer and slowly add to the flask with swirling 115 mL of a commercial household bleach such as Clorox (usually 5.25% by weight NaOCl, which is 0.75 molar). This can be added from a separatory funnel clamped to a ring stand or from another Erlenmeyer flask. Take care not to come in contact with the reagent. During the addition, keep the temperature in the range of 40-50°C. Have an ice bath available in case the temperature goes above 50°C, but do not allow the temperature to go below 40°C because oxidation will be incomplete. The addition should take about 15-20 min. Swirl the reaction mixture periodically for the next 20 min to complete the reaction. 

Bleaches sold under trade names such as Clorox and Purex are 5% solutions of sodium hypochlorite. The hypochlorite ion is a very strong oxidizing agent in basic solution. It oxidizes many stains to colorless substances. 

Caution. It is recommended that as many of the manipulations as possible be carried out in a hood with a good exhaust. This is particularly important with respect to the volatile mercaptans which can induce allergic reactions in some people any excess mercaptan may be destroyed by the addition of an oxidizing agent such as Clorox. Selenium-containing materials have been noted to have potentially adverse health effects.9... 

Epoxidation. Marmar epoxidized two ,j3-unsaturated ketones, benzalaceto-phenone and fraws-dibenzoylethylene, in yields of >90%, by using ordinary commercial hypochlorite bleach (Clorox) in pyridine solution. 1,4-Naphthoquinone is also epoxidized in 71.5%, yield with sodium hypochlorite in dioxane. In this case addition of pyridine results in further oxidation. 

This experiment is a further illustration of the oxidation of a 2° alcohol to a ketone. The reagent used is sodium hypochlorite solution. This reagent is also used in oxidation reactions described in Experiments [32] and [34A, Bj.The chemistry of the reagent, sodium hypochlorite, is discussed in Experiment [32].This alternative reagent for the oxidation of 9-fluorenone offers a material that is cheap (Clorox, a household bleach), easy to handle, and environmentally safe. 

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