Question

Which of the following statements are correct for the following unbalanced equation in basic medium?
$I{O}_3^{-}+C{l}^{-}\to I_2+C{l}_2$

• A. This is a disproportionation reaction.
• B. The reaction involves a $10$ electron change.
• C. Iodate is the oxidizing agent and chloride is the reducing agent.
• D. The number of coefficients for NaIO${}_3$ and NaOH in the balanced equation are $2$ and $12$ respectively.

Answer 1

Answer: (B), (C), (D)

The reaction involves a $10$ electron change.
Iodate is the oxidizing agent and chloride is the reducing agent.
The number of coefficients for NaIO${}_3$ and NaOH in the balanced equation are $2$ and $12$ respectively.

The half cell reactions are as follows:

$2C{l}^{-}\to C{l}_2+2e^{-}$ (oxidation)

$2I{O}_3^{-}+6H_{2}O+10e^{-}\to I_2+12O{H}^{-}$ (reduction)

$2I{O}_3^{-}+6H_{2}O+10C{l}^{-}\to 5C{l}_2+I_2+12O{H}^{-}$ (final reaction)

i.e., $2NaI{O}_3+10NaCl+6H_{2}O\to 5C{l}_2+I_2+12NaOH$

Here, iodate is behaving as oxidising agent and chloride is behaving as a reducing agent as they are undergoing reduction and oxidation respectively.