`Na^(+)` and `Ag^(+)` differ in

Options

A. `Na_(2)CO_(3)` is thermally stable while `Ag_(2)CO_(3)` decomposes into `Ag,CO_(2)` and `O_(2)`
B. `Ag^(+)` forms complexes, `Na^(+)` does not
C. `NaCI` is water soluble, `AgCI` is insoluble
D. All

Answer

To solve the question regarding the differences between \( \text{Na}^+ \) and \( \text{Ag}^+ \), we will analyze the provided options step by step.

### Step 1: Analyze the thermal stability of carbonates
- **Statement**: \( \text{Na}_2\text{CO}_3 \) is thermally stable while \( \text{Ag}_2\text{CO}_3 \) decomposes into \( \text{Ag}_2\text{CO}_2 \) and \( \text{O}_2 \).
- **Explanation**: Sodium carbonate (\( \text{Na}_2\text{CO}_3 \)) is known to be thermally stable and does not decompose easily upon heating. In contrast, silver carbonate (\( \text{Ag}_2\text{CO}_3 \)) is unstable and decomposes when heated to form silver oxide and carbon dioxide. Thus, this statement is correct.

### Step 2: Complex formation
- **Statement**: \( \text{Ag}^+ \) forms complexes while \( \text{Na}^+ \) does not.
- **Explanation**: Silver ions (\( \text{Ag}^+ \)) can form various complexes, such as \( \text{Ag(CN)}_2^- \) (silver cyanide complex). On the other hand, sodium ions (\( \text{Na}^+ \)) do not typically form such complexes. Therefore, this statement is also correct.

### Step 3: Solubility of chlorides
- **Statement**: \( \text{NaCl} \) is water soluble, while \( \text{AgCl} \) is insoluble.
- **Explanation**: Sodium chloride (\( \text{NaCl} \)) is a strong electrolyte and dissolves completely in water, dissociating into \( \text{Na}^+ \) and \( \text{Cl}^- \) ions. Conversely, silver chloride (\( \text{AgCl} \)) is known to be insoluble in water and forms a precipitate when mixed with water. Thus, this statement is also true.

### Conclusion
Since all three statements are correct, the answer to the question is that \( \text{Na}^+ \) and \( \text{Ag}^+ \) differ in all the mentioned aspects.

### Final Answer
The correct option is **all of the above**.

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