Question

In basic solution, molecular chlorine, Cl2, reacts with hydroxide ions, OH−, to yield chloride ions, Cl−. and chlorate ions, ClO4−. HINT: This is a disproportionation reaction in which the element chlorine is both oxidized and reduced. Write a balanced equation for this reaction.

Answer 1

$3Cl_{(g)}+6OH^{-} _{(aq)}$ → $5Cl^{-}_{(aq)} + ClO^{-}_{(aq)} + 3H_{2}O_{(l)}$

Explanation:

• We can see that the equation is balanced by putting up the numbers to satisfy their valencies and also the number of atoms on the left side to that of the right side.

• This is a disproportionation reaction because of the simple fact that it is an oxidation-reduction reaction. Both chlorine and hydroxide ions get reduced and oxidised at the same time.

• Industrially, Chlorine reacts with hydroxide in numerous different ways according to the temperature and concentration of the reactants.