Complete and balance the followig equations in basic solution :
`Hg_2(CN)_2+Ce^(4+)toCO_3^(2-)+NO_3^(ɵ)+Hg(OH)_2+Ce^(3+)`
(a) By considering C in `+4` oxidation state and N in `+5` oxidation state.
(b) By considering C in `+4` oxidation state and N in `+5` oxidation state
(c) By considering Hg in `+2` and C in `+4` oxidation state.
(d) Explain why the same result is obtained regardless of the choice of oxidation state.

Explanation

To solve the problem of balancing the given redox reaction in basic solution, we will follow a systematic approach. The reaction is:

\[ \text{Hg}_2(\text{CN})_2 + \text{Ce}^{4+} \rightarrow \text{CO}_3^{2-} + \text{NO}_3^{-} + \text{Hg(OH)}_2 + \text{Ce}^{3+} \]

### Step 1: Identify Oxidation States
- For **C** in \(\text{Hg}_2(\text{CN})_2\), we consider it to be in the +4 oxidation state.
- For **N**, we consider it to be in the +5 oxidation state.
- For **Hg**, we consider it to be in the +2 oxidation state.
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