Disproportionation is a redox reaction in which the same element is both oxidised and reduced. Two examples are the reaction of chlorine with water and the reaction of chlorine and cold, dilute aqueous sodium hydroxide.
Cl2(aq) + H2O(l) → HClO(aq) + HCl(aq)The oxidation state of chlorine is +1 in HClO and -1 in HCl.
Cl2(aq) + 2NaOH(aq) → NaClO(aq) + NaCl(aq) + H2O(l)The oxidation state of chlorine is +1 in NaClO and -1 in NaCl.
Bacteria are killed by adding chlorine to water. The bacteria are killed by chloric (I) acid HClO which acts as a weak bleach. Adding an indicator, the indicator first turns red because of the acid then is bleached by the HClO. NaClO is used as household bleach
Cl2(aq) + H2O(l) → HClO(aq) + HCl(aq)The oxidation state of chlorine is +1 in HClO and -1 in HCl.
Cl2(aq) + 2NaOH(aq) → NaClO(aq) + NaCl(aq) + H2O(l)The oxidation state of chlorine is +1 in NaClO and -1 in NaCl.
Bacteria are killed by adding chlorine to water. The bacteria are killed by chloric (I) acid HClO which acts as a weak bleach. Adding an indicator, the indicator first turns red because of the acid then is bleached by the HClO. NaClO is used as household bleach