Fe can displace which of the following ions from their aqueous solutions?
(a) `Na^(+)` (b) `Zn^(2+)` (c) `Cu^(2+)` (d) `Ag^(+)`

Options

A. a & b
B. b & c
C. c & d
D. b,c,d

Answer

To determine which ions can be displaced by iron (Fe) from their aqueous solutions, we can refer to the electrochemical series. The electrochemical series ranks metals and their ions based on their ability to be reduced (gain electrons) or oxidized (lose electrons). A metal can displace another metal ion from solution if it is higher in the electrochemical series.

### Step-by-Step Solution:

1. **Understand the Electrochemical Series**: The electrochemical series lists metals and their ions in order of their standard reduction potentials. Metals that are higher in the series can displace those that are lower.

2. **Identify the Position of Iron (Fe)**: In the electrochemical series, iron (Fe) is positioned between zinc (Zn) and copper (Cu). The relevant part of the series is:
- Ag⁺ + e⁻ → Ag (solid)
- Cu²⁺ + 2e⁻ → Cu (solid)
- Fe²⁺ + 2e⁻ → Fe (solid)
- Zn²⁺ + 2e⁻ → Zn (solid)
- Na⁺ + e⁻ → Na (solid)

3. **Determine the Relative Positions of the Given Ions**:
- **Na⁺**: Lower than Fe
- **Zn²⁺**: Lower than Fe
- **Cu²⁺**: Higher than Fe
- **Ag⁺**: Higher than Fe

4. **Identify Which Ions Can Be Displaced**:
- Since Fe is positioned below Cu²⁺ and Ag⁺ in the electrochemical series, it can displace these ions from their aqueous solutions.
- Therefore, Fe can displace Cu²⁺ and Ag⁺.

5. **Conclusion**: The ions that can be displaced by Fe from their aqueous solutions are Cu²⁺ and Ag⁺. Thus, the correct answer is (c) Cu²⁺ and (d) Ag⁺.

### Final Answer:
Fe can displace Cu²⁺ and Ag⁺ from their aqueous solutions.