Write balanced net ionic equations for the following reactions in basic solution.
$H_{2} O_{2} (a q) + C l_{2} O_{7} (a q) \to C l O {_{2}}^{-} (a q) + O_{2} (g)$

4 H_{2} O_{2} (a q) + C l_{2} O_{7} (a q) 2 O H^{-} \to 2 C l O {_{2}}^{-} (a q) + 4 O_{2} (g) + 5 H_{2} O

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3 H_{2} O_{2} (a q) + C l_{2} O_{7} (a q) 2 O H^{-} \to 2 C l O {_{2}}^{-} (a q) + 4 O_{2} (g) + 4 H_{2} O

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6 H_{2} O_{2} (a q) + 2 C l_{2} O_{7} (a q) 2 O H^{-} \to 2 C l O {_{2}}^{-} (a q) + 4 O_{2} (g) + 10 H_{2} O

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None of these

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Solution

The correct option is A $4 H_{2} O_{2} (a q) + C l_{2} O_{7} (a q) 2 O H^{-} \to 2 C l O {_{2}}^{-} (a q) + 4 O_{2} (g) + 5 H_{2} O$
The unbalanced chemical equation is,
$H_{2} O_{2} (a q) + C l_{2} O_{7} (a q) \to C l O {_{2}}^{-} (a q) + O_{2} (g)$

Balance $C l$ atoms.
$H_{2} O_{2} (a q) + C l_{2} O_{7} (a q) \to 2 C l O {_{2}}^{-} (a q) + O_{2} (g)$

The oxidation number of $C l$ decreases from $+ 7$ to $+ 3$ . Total decrease in the oxidation number for $2 C l$ atoms is $8$ .

The oxidation number of $O$ atom of hydrogen peroxide increases from $- 1$ to $0$ . Total increase in the oxidation number of $2 O$ atoms of hydrogen peroxide is $2$ .

To balance increase in the oxidation number with decrease in the oxidation number, multiply hydrogen peroxide and oxygen with $4$ .
$4 H_{2} O_{2} (a q) + C l_{2} O_{7} (a q) \to 2 C l O {_{2}}^{-} (a q) + 4 O_{2} (g)$

To balance oxygen atoms, add $3$ water molecules on RHS.
$4 H_{2} O_{2} (a q) + C l_{2} O_{7} (a q) \to 2 C l O {_{2}}^{-} (a q) + 4 O_{2} (g) + 3 H_{2} O (l)$

To balance $H$ atoms, add $2$ protons on RHS.
$4 H_{2} O_{2} (a q) + C l_{2} O_{7} (a q) \to 2 C l O {_{2}}^{-} (a q) + 4 O_{2} (g) + 3 H_{2} O (l) + 2 H^{+} (a q)$

Since the reaction occurs in basic medium, add two hydroxide ions on either side of the equation.
$4 H_{2} O_{2} (a q) + C l_{2} O_{7} (a q) + 2 O H^{-} (a q) \to 2 C l O {_{2}}^{-} (a q) + 4 O_{2} (g) + 3 H_{2} O (l) + 2 H^{+} (a q) + 2 O H^{-} (a q)$

On RHS, two hydrogen ions combine with two hydroxide ions to form two molecules of water.
$4 H_{2} O_{2} (a q) + C l_{2} O_{7} (a q) + 2 O H^{-} (a q) \to 2 C l O {_{2}}^{-} (a q) + 4 O_{2} (g) + 5 H_{2} O (l)$
This is the balanced chemical equation.

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