Question

Iodine $\left({\mathrm{I}}_2\right)$ reacts with Concentrated Nitric acid$\left({\mathrm{HNO}}_3\right)$to give:

• A. $\mathrm{HI}$
• B. ${\mathrm{HOIO}}_2$
• C. ${\mathrm{HOIO}}_3$
• D. All Of These

Answer 1

The correct option is B

${\mathrm{HOIO}}_2$

Explanation for the Correct Option:

Option (B):${\mathrm{HOIO}}_2$

• The Iodine reacts with concentrated Nitric acid$\left({\mathrm{HNO}}_3\right)$ it giving Iodic acid $\left({\mathrm{HOIO}}_2\right)\mathrm{or}\left({\mathrm{HIO}}_3\right)$.
• Here, Nitric acid$\left({\mathrm{HNO}}_3\right)$, being the strong oxidizing agent oxidizes Iodine to form Iodic acid $\left({\mathrm{HOIO}}_2\right)\mathrm{or}\left({\mathrm{HIO}}_3\right)$.
• The balanced chemical equation for the above reaction can be given as:
• $\underset{\left(Iodine\right)}{{\mathrm{I}}_2\left(\mathrm{s}\right)}+\underset{\left(\mathrm{Nitric}\mathrm{acid}\right)}{10\mathrm{HN}{\mathrm{O}}_3\left(\mathrm{aq}\right)}\to \underset{\left(\mathrm{Iodic}\mathrm{acid}\right)}{2\mathrm{HOI}{\mathrm{O}}_2\left(\mathrm{aq}\right)}+\underset{\left(\mathrm{Nitrogen}\mathrm{dioxide}\right)}{10\mathrm{N}{\mathrm{O}}_2}+\underset{\left(\mathrm{Water}\right)}{4{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)}$

Explanation for the incorrect Option:

Option (A): $\mathrm{HI}$

• Iodine on reaction with concentrated Nitric acid$\left({\mathrm{HNO}}_3\right)$ doesn't give as the product.
• Hence, the given Option is an incorrect one.

Option (C):${\mathrm{HOIO}}_3$

• When Iodine reacts with concentrated Nitric acid$\left({\mathrm{HNO}}_3\right)$ the reaction does not give ${\mathrm{HOIO}}_3$as the product.
• Hence, this Option given here does not represent the correct concept.

Hence, Iodine $\left({\mathrm{I}}_2\right)$ reacts with Concentrated Nitric acid$\left({\mathrm{HNO}}_3\right)$to give: ${\mathrm{HOIO}}_2$.