hypochlorite ion - Carbide chemistry - Synthesis of acetylene Demonstration | The beaker contains HCl and CaC2 pellets and is covered. Sodium hypochlorite (Chlorox) is added to the beaker. | | Observations Flames shoot out from the top of the beaker. Explanation (including important chemical equations) Calcium carbide reacts with water to form acetylene. CaC2 (s) + 2 H2O (l) --> H2C2 (g) + Ca(OH)2 (aq) Chlorine gas is generated when hypochlorite solutions are acidified. This is the opposite of the disproportionation that chlorine gas undergoes under basic conditions, so the reaction has been referred to as a conproportionation. OCl- (aq) + HCl (aq) --> Cl2 (g) + H2O (l) The chlorine gas reacts with the acetylene (as well as many other hydrogenated compounds). This reaction is not what one might first expect, since it is not the product of the addition of the halogen across the carbon-carbon triple bond. The product is formed by the abstraction of hydrogen from the hydrocarbon. H2C2 (g) + Cl2 (g) --> HCl (aq) + HC2Cl (g)

towards disproportionation in acidic solutions than in alkaline solutions: The hypochlorite ions also disproportionate further to produce chloride and chlorate Chlorine is a chemical element; it has symbol Cl and atomic number 17. The second-lightest of the halogens, it appears between fluorine and bromine in the periodic table and its properties are mostly intermediate between them. Chlorine is a yellow-green gas at room temperature. It is an extremely reactive element and a strong oxidising agent: among the elements, it has the highest electron affinit C… The hypochlorite ions also disproportionate further to produce chloride and chlorate (3 ClO− ⇌ 2 Cl− + ClO−3) but this reaction is quite slow at temperatures below 70 °C in spite of the very favourable equilibrium constant of 1027. The chlorate ions may themselves disproportionate to form chloride and perchlorate (4 ClO−3 ⇌ Cl− + 3 ClO−4) but this is still very slow even at 100 °C despite the very favourable equilibrium constant of 1020. The rates of reaction for the chlorine oxyanions increases as the oxidation state of chlorine decreases. The strengths of the chlorine oxyacids increase very quickly as the oxidation state of chlorine increases due to the increasing delocalisation of charge over more and more oxygen atoms in their conjugate bases. Most of the chlorine oxoacids may be produced by exploiting these disproportionation reactions. Hypochlorous acid (HOCl) is highly reactive and quite unstable; its salts are mostly used for their bleaching and sterilising abilities. They are very strong oxidising agents, transferring an oxygen atom to most inorganic species. Chlorous acid (HOClO) is even more unstable and cannot be isolated or concentrated without decomposition: it is known from the decomposition of aqueous chlorine dioxide. However, sodium chlorite is a stable salt and is useful for bleaching and stripping textiles, as an oxidising agent, and as a source of chlorine dioxide. Chloric acid (HOClO2) is a strong acid that is quite stable in cold water up to 30% concentration, but on warming gives chlorine and chlorine dioxide.…