The oxidation state of copper changes when aqueous copper (II) ions react with:

$(I)$ $N a O H (a q)$

$(I I)$ $F e (s)$

$(I I I)$ $K I (a q)$

I, I I, I I I

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I I

only

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I I, I I I

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I

only

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Solution

The correct option is C $I I, I I I$
(I) During the reaction of Copper(II) ions with sodium hydroxide, the oxidation state of copper is unaffected.

$C u S O_{4} + 2 N a O H \to C u (O H)_{2} + N a_{2} S O_{4}$

(II) Iron is more electropositive than copper. Hence, it displaces copper from a copper salt solution.

$C u^{2 +} + F e \to F e^{2 +} + C u$

In this reaction, the oxidation state of copper changes from +2 to 0.

(III) During reaction with KI, the oxidation state of copper changes for +2 to +1.

$2 C u^{2 +} + 4 K I \to C u_{2} I_{2} ↓ + I_{2} + 4 K^{+}$

Hence, the correct option is $C$

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