Search results
Results from the WOW.Com Content Network
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. Thus, the formation of stable hypochlorite bleaches is facilitated by dissolving chlorine gas into basic water solutions, such as sodium hydroxide.
2 which dissociates in water to form hypochlorite. This reaction must be conducted in non-acidic conditions to prevent release of chlorine: 2 Cl − → Cl 2 + 2 e − Cl 2 + H 2 O ⇌ HClO + Cl − + H + Some hypochlorites may also be obtained by a salt metathesis reaction between calcium hypochlorite and various metal sulfates.
At a pH of about 4, such as obtained by the addition of strong acids like hydrochloric acid, the amount of undissociated (nonionized) HOCl is highest. The reaction can be written as: − OCl + H + ⇌ HOCl. Sodium hypochlorite solutions combined with acid evolve chlorine gas, particularly strongly at pH < 2, by the reactions:
Hydrochloric acid is a strong inorganic acid that is used in many industrial processes such as refining metal. The application often determines the required product quality. [25] Hydrogen chloride, not hydrochloric acid, is used more widely in industrial organic chemistry, e.g. for vinyl chloride and dichloroethane. [8]
The reaction of an acid in water solvent is often described as a dissociation + + where HA is a proton acid such as acetic acid, CH 3 COOH. The double arrow means that this is an equilibrium process, with dissociation and recombination occurring at the same time.
Therefore hydrogen is transported away from the anode mostly as hypochlorous acid rather than H +. The hypochlorous acid dissociates in the bulk electrolyte where the pH is high and the hypochlorite ion diffuses back to the anode. More than two thirds of the hypochlorite is consumed by buffering before reaching the anode.
The neutralization reaction can be considered as the difference of the following two acid dissociation reactions HA ⇌ H + + A − K a,A = [A −][H +]/[HA] BH + ⇌ B + H + K a,B = [B][H +]/[BH +] with the dissociation constants K a,A and K a,B of the acids HA and BH +, respectively. Inspection of the reaction quotients shows that K = K a ...
The Pinnick oxidation is an organic reaction by which aldehydes can be oxidized into their corresponding carboxylic acids using sodium chlorite (NaClO 2) under mild acidic conditions. It was originally developed by Lindgren and Nilsson. [ 1 ]