Question

Write a balanced net ionic equation for the disproportionation reaction of (a) hypochlorous acid to chlorine gas and chlorous acid in acidic solution. (b) chlorate ion to perchlorate and chlorite ions.

Short answer

Question: Write balanced net ionic equations for the disproportionation reactions. a) Disproportionation reaction of hypochlorous acid to chlorine gas and chlorous acid in acidic solution. b) Disproportionation reaction of the chlorate ion to perchlorate and chlorite ions. Answer: a) 2 HClO(aq) -> Cl2(g) + 2 HClO2(aq) b) 6 ClO3^-(aq) -> 2 ClO4^-(aq) + 4 ClO2^-(aq)

Step-by-step solution

Write the balanced chemical equation

The overall reaction for the disproportionation of hypochlorous acid to chlorine gas and chlorous acid is: 2HClO(aq) -> Cl_2(g) + HClO_2(aq)

Break down the reaction into half-reactions

Split the reaction into two half-reactions involving the loss and gain of electrons: Oxidation half-reaction: HClO -> Cl_2 + e^- Reduction half-reaction: HClO + e^- -> HClO2

Balance the half-reactions

Now we need to balance atoms and charges to obtain balanced half-reactions: Oxidation half-reaction: 2 HClO -> Cl2 + 2 e^- Reduction half-reaction: 2 HClO + 2 e^- -> 2 HClO2

Combine the half-reactions to form the net ionic equation

We can now add the balanced half-reactions to obtain the balanced net ionic equation: 2 HClO -> Cl2 + 2 e^- 2 HClO + 2 e^- -> 2 HClO2 -------------------------------------- 2 HClO -> Cl2 + 2 HClO2 ##(b) Disproportionation of chlorate ion to perchlorate and chlorite ions##

Write the balanced chemical equation

The overall reaction for the disproportionation of the chlorate ion to perchlorate and chlorite ions is: ClO3^-(aq) -> ClO4^-(aq) + ClO2^-(aq)

Break down the reaction into half-reactions

Split the reaction into two half-reactions involving the loss and gain of electrons: Oxidation half-reaction: ClO3^- -> ClO4^- + e^- Reduction half-reaction: ClO3^- + e^- -> ClO2^-

Balance the half-reactions

Now we need to balance atoms and charges to obtain a balanced half-reaction: Oxidation half-reaction: 2 ClO3^- -> 2 ClO4^- + 2 e^- Reduction half-reaction: 4 ClO3^- + 4 e^- -> 4 ClO2^-

Combine the half-reactions to form the net ionic equation

We can now add the balanced half-reactions, making sure we have the same number of electrons on both sides, to obtain the balanced net ionic equation: 2 ClO3^- -> 2 ClO4^- + 2 e^- 4 ClO3^- + 4 e^- -> 4 ClO2^- -------------------------------------- 6 ClO3^- -> 2 ClO4^- + 4 ClO2^-