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In particular, this reaction occurs in sodium hypochlorite solutions at high temperatures, forming sodium chlorate and sodium chloride: [25] [26] 3 NaOCl(aq) → 2 NaCl(aq) + NaClO 3 (aq) This reaction is exploited in the industrial production of sodium chlorate. An alternative decomposition of hypochlorite produces oxygen instead: 2 OCl − ...
Hydrogen peroxide (H 2 O 2) can be used as HOCl scavenger whose byproducts do not interfere in the Pinnick oxidation reaction: HOCl + H 2 O 2 → HCl + O 2 + H 2 O. In a weakly acidic condition, fairly concentrated (35%) H 2 O 2 solution undergoes a rapid oxidative reaction with no competitive reduction reaction of HClO 2 to form HOCl. HClO 2 ...
Cl 2 + H 2 O ⇌ HClO + HCl Cl 2 + 4 OH − ⇌ 2 ClO − + 2 H 2 O + 2 e − Cl 2 + 2 e − ⇌ 2 Cl −. When acids are added to aqueous salts of hypochlorous acid (such as sodium hypochlorite in commercial bleach solution), the resultant reaction is driven to the left, and chlorine gas is formed.
The simplified chemical reaction is: NaCl + H 2 O + energy → NaOCl + H 2 [citation needed] That is, energy is added to sodium chloride (table salt) in water, producing sodium hypochlorite and hydrogen gas. Because the reaction takes place in an unpartitioned cell and NaOH is present in the same solution as the Cl 2: 2 NaCl + 2 H 2 O → 2 ...
Non condensible gases and remaining chlorine gas are vented off as part of the pressure control of the liquefaction systems. These gases are routed to a gas scrubber, producing sodium hypochlorite, or used in the production of hydrochloric acid (by combustion with hydrogen) or ethylene dichloride (by reaction with ethylene).
This reaction is accelerated at temperatures above about 60 °C. Other reactions occur, such as the self-ionization of water and the decomposition of hypochlorite at the cathode, the rate of the latter depends on factors such as diffusion and the surface area of the cathode in contact with the electrolyte. [9]
Hypochlorite salts formed by the reaction between chlorine and alkali and alkaline earth metal hydroxides. The reaction is performed at close to room temperature to suppress the formation of chlorates. This process is widely used for the industrial production of sodium hypochlorite (NaClO) and calcium hypochlorite (Ca(ClO) 2).
The most important chlorite is sodium chlorite (NaClO 2), used in the bleaching of textiles, pulp, and paper. However, despite its strongly oxidizing nature, it is often not used directly, being instead used to generate the neutral species chlorine dioxide (ClO 2), normally via a reaction with HCl: 5 NaClO 2 + 4 HCl → 5 NaCl + 4 ClO 2 + 2 H 2 O