Sodium hypochlorite

Sodium hypochlorite is an <a href="/facts/Alkali/s6NqPGSP">alkaline</a> <a href="/facts/Inorganic_compound/TfFfzxSz">inorganic</a> <a href="/facts/Chemical_compound/37FXqqtv">chemical compound</a> with the <a href="/facts/Chemical_formula/hghUtthl">formula</a> <a href="/facts/Sodium/eYuSPu2V">Na</a><a href="/facts/Oxygen/acyn6o8r">O</a><a href="/facts/Chlorine/y27UwYBM">Cl</a> (also written as NaClO). It is commonly known in a dilute <a href="/facts/Aqueous_solution/eRNr3MH2">aqueous solution</a> as <a href="/facts/Bleach/QPxAysPl">bleach</a> or chlorine bleach. It is the <a href="/facts/Sodium/eYuSPu2V">sodium</a> <a href="/facts/Salt_(chemistry)/lsSKwGpn">salt</a> of <a href="/facts/Hypochlorous_acid/tGrX1C7z">hypochlorous acid</a>, consisting of sodium <a href="/facts/Cations/wrbwhF3z">cations</a> (Na+) and <a href="/facts/Hypochlorite/XMJdjAEM">hypochlorite</a> <a href="/facts/Anions/wrbwhF3z">anions</a> (−OCl, also written as OCl− and ClO−).
The anhydrous <a href="/facts/Chemical_compound/37FXqqtv">compound</a> is unstable and may decompose explosively. It can be crystallized as a <a href="/facts/Hydrate/dev82l69">pentahydrate</a> NaOCl·5H2O, a pale greenish-yellow solid which is not <a href="/facts/Explosive/sUme5Pp8">explosive</a> and is stable if kept refrigerated.
Sodium hypochlorite is most often encountered as a pale greenish-yellow dilute solution referred to as chlorine bleach, which is a <a href="/facts/Household_chemical/E9NyWQy0">household chemical</a> widely used (since the 18th century) as a <a href="/facts/Disinfectant/33fF2QzG">disinfectant</a> and <a href="/facts/Bleaching_agent/QPxAysPl">bleaching agent</a>. In solution, the compound is unstable and easily decomposes, liberating <a href="/facts/Chlorine/y27UwYBM">chlorine</a>, which is the active principle of such products. Sodium hypochlorite is still the most important <a href="/facts/Chlorine-releasing_compounds/0EKvlthM">chlorine-based bleach</a>.
Its corrosive properties, common availability, and reaction products make it a significant safety risk. In particular, <a href="/facts/Mixture/tms8rbmn">mixing</a> liquid bleach with other cleaning products, such as acids found in <a href="/facts/Limescale/1BNaIVAH">limescale</a>-removing products, will release toxic <a href="/facts/Chlorine_gas/y27UwYBM">chlorine gas</a>. A common misconception is that mixing bleach with ammonia also releases chlorine, but in reality they react to produce <a href="/facts/Chloramines/ux5XnB36">chloramines</a> such as <a href="/facts/Nitrogen_trichloride/eC2URITS">nitrogen trichloride</a>. With excess ammonia and <a href="/facts/Sodium_hydroxide/xjtdYtq7">sodium hydroxide</a>, <a href="/facts/Hydrazine/G7P5ITzU">hydrazine</a> may be generated.

Sodium hypochlorite open-in-new

Sodium hypochlorite