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  2. Percent active chlorine - Wikipedia

    en.wikipedia.org/wiki/Percent_active_chlorine

    Liquid bleaches for domestic use fall in 3 categories: for pool-treatment (10% hypochlorite solutions, without surfactants and detergents), for laundry and general purpose cleaning, at 3–5% active chlorine (which are usually recommended to be diluted substantially before use), and in pre-mixed specialty formulations targeted at particular ...

  3. Sodium hypochlorite - Wikipedia

    en.wikipedia.org/wiki/Sodium_hypochlorite

    Household bleach and pool chlorinator solutions are typically stabilized by a significant concentration of lye (caustic soda, NaOH) as part of the manufacturing reaction. This additive will by itself cause caustic irritation or burns due to defatting and saponification of skin oils and destruction of tissue.

  4. Hypochlorite - Wikipedia

    en.wikipedia.org/wiki/Hypochlorite

    Hypochlorite is a sufficiently strong oxidiser to convert Mn(III) to Mn(V) during the Jacobsen epoxidation reaction and to convert Ce 3+ to Ce 4+. [9] This oxidising power is what makes them effective bleaching agents and disinfectants. In organic chemistry, hypochlorites can be used to oxidise primary alcohols to carboxylic acids. [18]

  5. Salt water chlorination - Wikipedia

    en.wikipedia.org/wiki/Salt_water_chlorination

    Salt water chlorination is a process that uses dissolved salt (1000–4000 ppm or 1–4 g/L) for the chlorination of swimming pools and hot tubs.The chlorine generator (also known as salt cell, salt generator, salt chlorinator, or SWG) uses electrolysis in the presence of dissolved salt to produce chlorine gas or its dissolved forms, hypochlorous acid and sodium hypochlorite, which are already ...

  6. Chlorine-releasing compounds - Wikipedia

    en.wikipedia.org/wiki/Chlorine-releasing_compounds

    For example, the label of a household bleach product may specify "5% sodium hypochlorite by weight." That would mean that 1 kilogram of the product contains 0.05 × 1000 g = 50 g of NaClO. A typical oxidation reaction is the conversion of iodide I − to elemental iodine I 2. The relevant reactions are NaClO + 2 H + + 2 I − → NaCl + H 2 O ...

  7. It’s strong enough to eliminate mineral deposits, stains, mold and germs. The post Having Trouble Finding Bleach? Here’s What To Use Instead appeared first on Taste of Home .

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