Chemical Forums
Chemistry Forums for Students => High School Chemistry Forum => Topic started by: tyneoh on September 01, 2012, 07:27:31 AM
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Halogen solution are great oxidising agents right? But when you dissolve halogens(chlorine, bromine) in water, ionic compounds are formed
Cl2+h20 :rarrow: HOCL+HCL.
There aren't any chlorine molecules to act as oxidising agents since only HOCL and HCL present.I am quite confused by this. Thanks in advance :)
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Cl2+h20 :rarrow: HOCL+HCL
More precisely
Cl2 + H2O ::equil:: HOCl + HCl
- this is an equilibrium reaction, so there is always some free chlorine available.
Besides, OCl- is a strong oxidizing agent as well.
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Halogen solution are great oxidising agents right? But when you dissolve halogens(chlorine, bromine) in water, ionic compounds are formed
Cl2+h20 :rarrow: HOCL+HCL.
There aren't any chlorine molecules to act as oxidising agents since only HOCL and HCL present.I am quite confused by this. Thanks in advance :)
the reaction mentioned by you is a disproportionation reaction in which Cl2 is undergoing oxidation and reduction.Cl2 ----> HOCl is oxidation and Cl2---> HCl is reduction.HCl is stable but HOCl has Cl in +1 oxidation state which is very unstable.It has very high tendency to undergo reduction and hence acts like very strong oxidizing agent.