Question

Consider the following balanced redox reaction:2CrO₂⁻(aq) + 2H₂O(l) + 6ClO⁻(aq) →

Answer 1

The balanced molecular equation , with Na⁺ as the spectator ion .

2NaCrO₂(aq) + 2H₂O(l) + 6NaClO(aq) →2$Na_{2}$CrO₄(aq) + 3Cl₂(g) + 4NaOH(aq)

There are following steps involve in balanced redox reaction in basic medium .

• Divide the reaction into two half reactions .

• Balance the elements other than oxygen and hydrogen .

• Balance the oxygen atom by adding  $H_{2} O$.

• Balance the hydrogen atom by adding  $H^{+}$.
• Add $OH^{-}$ on bath side .
• Combine   $OH^{-}$ and  $H^{+}$ to form form $H_{2} O$.

• Balance the charge by adding $e^{-}$ .

• Add the half reaction and simply .

The species which reduces the other species in the redox reaction is called oxidizing agent . Similarly , the species which oxidize the other species in the redox reaction  is called reducing agent .

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