# Can you represent the oxidation of sulfite ion, SO_3^(2-), to give sulfate ion, SO_4^(2-), accompanied by the reduction of Cu^(2+) to copper metal?

Oct 18, 2016

$S {O}_{3}^{2 -} + C {u}^{2 +} + 2 H {O}^{-} \rightarrow S {O}_{4}^{2 -} + C u \left(s\right) + {H}_{2} O \left(l\right)$

#### Explanation:

When basic conditions are specified, it is normally best to balance the equations in acid, and then modify the final equations.

$\text{Sulfur (IV+)}$ $\rightarrow$ $\text{Sulfur(VI+)} :$

$S {O}_{3}^{2 -} + {H}_{2} O \rightarrow S {O}_{4}^{2 -} + 2 {H}^{+} + 2 {e}^{-}$

For basic conditions, add $2 \times H {O}^{-}$ to EACH side $\left(H {O}^{-} + {H}^{+} \rightarrow {H}_{2} O\right)$:

$S {O}_{3}^{2 -} + 2 H {O}^{-} \rightarrow S {O}_{4}^{2 -} + {H}_{2} O + 2 {e}^{-}$

$\text{Copper (II+)}$ $\rightarrow$ $\text{Copper (0)} :$

$C {u}^{2 +} + 2 {e}^{-} \rightarrow C u$

You have asked another such question recently. Do you follow the method of doing redox equations?