Identify the change in the oxidation state of | vedclass

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(B) Step $1$: Assign oxidation states to all atoms. In $H_3AsO_3$, $As$ is $+3$. In $BrO_3^-$, $Br$ is $+5$. In $Br^-$, $Br$ is $-1$. In $H_3AsO_4$, $

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$+5$ to $-1$

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(B) Step $1$: Assign oxidation states to all atoms. In $H_3AsO_3$, $As$ is $+3$. In $BrO_3^-$, $Br$ is $+5$. In $Br^-$, $Br$ is $-1$. In $H_3AsO_4$, $As$ is $+5$.Step $2$: Identify the oxidising agent. The oxidising agent is the species that gets reduced. Here, $Br$ in $BrO_3^-$ changes from $+5$ to $-1$, so $BrO_3^-$ is the oxidising agent.Step $3$: The change in oxidation state of the oxidising agent is from $+5$ to $-1$.

Identify the change in the oxidation state of the oxidising agent in the following redox reaction: $3H_3AsO_3(aq) + BrO_3^-(aq) \rightarrow Br^-(aq) + 3H_3AsO_4(aq)$

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