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The principal example is tert-butyl hypochlorite, which is a useful chlorinating agent. [3] Most hypochlorite salts are handled as aqueous solutions. Their primary applications are as bleaching, disinfection, and water treatment agents. They are also used in chemistry for chlorination and oxidation reactions.
Chlorine-releasing compounds, also known as chlorine base compounds, is jargon to describe certain chlorine-containing substances that are used as disinfectants and bleaches. They include the following chemicals: sodium hypochlorite (active agent in bleach ), chloramine , halazone , and sodium dichloroisocyanurate . [ 2 ]
Sodium hypochlorite is still the most important chlorine-based bleach. [10] [11] Its corrosive properties, common availability, and reaction products make it a significant safety risk. In particular, mixing liquid bleach with other cleaning products, such as acids found in limescale-removing products, will release chlorine gas.
Pure" samples have 99.2% active chlorine. Given common industrial purity, an active chlorine content of 65-70% is typical. [2] It is the main active ingredient of commercial products called bleaching powder, [a] used for water treatment and as a bleaching agent. [3]
Trichloroisocyanuric acid is an organic compound with the formula (CONCl) 3.It is used as an industrial disinfectant, bleaching agent and a reagent in organic synthesis. [1] [2] [3] This white crystalline powder, which has a strong "chlorine odour," is sometimes sold in tablet or granule form for domestic and industrial use.
Industrial bleaching agents can be sources of concern. For example, the use of elemental chlorine in the bleaching of wood pulp produces organochlorines and persistent organic pollutants, including dioxins. According to an industry group, the use of chlorine dioxide in these processes has reduced the dioxin generation to under-detectable levels ...
Chlorine can result in the bleaching of the dye in the absence of thiosulfate to inhibit the oxidizing chlorine. High levels of bromine can convert phenol red to bromophenol red (dibromophenolsulfonephthalein, whose lowered p K a results in an indicator with a range shifted in the acidic direction – water at pH 6.8 will appear to test at 7.5).
In oxychlorination, hydrogen chloride instead of the more expensive chlorine is used for the same purpose: CH 2 =CH 2 + 2 HCl + 1 ⁄ 2 O 2 → ClCH 2 CH 2 Cl + H 2 O. Secondary and tertiary alcohols react with hydrogen chloride to give the corresponding chlorides. In the laboratory, the related reaction involving zinc chloride in concentrated ...