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Cu^(2+) ions will be reduced to Cu^(+) i...

`Cu^(2+)` ions will be reduced to `Cu^(+)` ions by the addition of an aqueous solution of:

A

`Kl`

B

`KCl`

C

`KSCN`

D

`KCN`

Text Solution

AI Generated Solution

The correct Answer is:
To solve the question of how `Cu^(2+)` ions can be reduced to `Cu^(+)` ions by the addition of an aqueous solution, we can follow these steps: ### Step-by-Step Solution: 1. **Understanding the Reduction Process**: - The reduction of `Cu^(2+)` to `Cu^(+)` involves a gain of electrons. We need to find a reagent that can provide electrons to facilitate this reduction. 2. **Identifying Possible Reagents**: - The question suggests looking for an aqueous solution that can reduce `Cu^(2+)`. Common reagents that can do this include potassium iodide (KI) and potassium thiocyanate (KSCN). 3. **Reaction with Potassium Iodide (KI)**: - When `Cu^(2+)` reacts with KI, the iodide ions (`I^(-)`) can reduce `Cu^(2+)` to `Cu^(+)`. - The reaction can be represented as: \[ 2Cu^{2+} + 2I^{-} \rightarrow Cu_{2}I_{2} + I_{3}^{-} \] - In this reaction, `Cu^(2+)` is reduced to `Cu^(+)` as it forms a compound with iodide ions. 4. **Reaction with Potassium Thiocyanate (KSCN)**: - Similarly, when `Cu^(2+)` reacts with KSCN, the thiocyanate ions (`SCN^(-)`) can also reduce `Cu^(2+)` to `Cu^(+)`. - The reaction can be represented as: \[ Cu^{2+} + 2SCN^{-} \rightarrow Cu(SCN)_{2} \quad \text{(black precipitate)} \] - This black precipitate can further decompose to form white copper thiocyanate, indicating that `Cu^(2+)` has been reduced to `Cu^(+)`. 5. **Conclusion**: - Both KI and KSCN can reduce `Cu^(2+)` to `Cu^(+)`. Therefore, the correct answers are both options that include KI and KSCN. ### Final Answer: The `Cu^(2+)` ions will be reduced to `Cu^(+)` ions by the addition of an aqueous solution of **KI** or **KSCN**. ---
To solve the question of how `Cu^(2+)` ions can be reduced to `Cu^(+)` ions by the addition of an aqueous solution, we can follow these steps: ### Step-by-Step Solution: 1. **Understanding the Reduction Process**: - The reduction of `Cu^(2+)` to `Cu^(+)` involves a gain of electrons. We need to find a reagent that can provide electrons to facilitate this reduction. 2. **Identifying Possible Reagents**: ...
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