Question

In the following reaction : $Cr(OH{)}_3+O{H}^{-}+I{O}_3{}^{-}\to Cr{O}_4^{2-}+H_{2}O+I^{-}$:

• A. $I{O}_3{}^{-}$ is oxidising agent
• B. $Cr(OH{)}_3$ is oxidised
• C. $6e^{-}$ are being taken per iodine atom
• D. all of these

Answer 1

The correct option is D all of these

Balanced chemical equation is,

$2Cr(OH{)}_3+I{O}_3^{-}+4O{H}^{-}\to 2Cr{O}_4^{2-}+I^{-}+5H_{2}O$

$I^{5+}+6e^{-}\to I^{-}$(Reduction)

Oxidation state of Cr is changing from +3 to +6,

$2C{r}^{3+}\to 2C{r}^{6+}+6e^{-}$(Oxidation)

Hence $Cr(OH{)}_3$ is oxidized and this implies $I{O}_3^{-}$ is oxidizing agent.