# Question #c3e76

May 2, 2017

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

#### Explanation:

$\text{Oxidation:}$

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

$\text{Reduction:}$

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

And thus.............

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

But BASIC solution was specified, and so we simply add $2 \times H {O}^{-}$ to BOTH SIDES of the equation:

$2 C {u}^{2 +} + S {O}_{3}^{2 -} + \cancel{{H}_{2} O} + 2 H {O}^{-} \rightarrow 2 C {u}^{+} + S {O}_{4}^{2 -} + \cancel{2} {H}_{2} O$

To give,.........

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

Which looks balanced to me. Whether it represents an actual redox process is moot.