AgCl is soluble in (a)____ and `Ag^(o+)` is present in (b)_____.

Answer

To solve the question regarding the solubility of AgCl and the presence of Ag^+ ions, we can break it down into two parts:

### Step 1: Determine the solvent in which AgCl is soluble
1. **Identify the nature of AgCl**: AgCl (silver chloride) is a white precipitate that is generally insoluble in water.
2. **Consider the effect of ammonia**: When AgCl is treated with aqueous ammonia (NH3), it forms a soluble complex. The reaction can be represented as:
\[ \text{AgCl (s)} + 2 \text{NH}_3 \text{(aq)} \rightarrow \text{[Ag(NH}_3\text{)}_2]^+ \text{(aq)} + \text{Cl}^- \text{(aq)} \]
3. **Conclusion for part (a)**: Therefore, AgCl is soluble in **aqueous ammonia (NH3)**.

### Step 2: Identify where Ag^+ ions are present
1. **Understanding the presence of Ag^+ ions**: The soluble complex formed in the previous step contains Ag^+ ions.
2. **Conclusion for part (b)**: Thus, Ag^+ ions are present in **aqueous ammonia (NH3)** as part of the complex ion [Ag(NH3)2]^+.

### Final Answers:
(a) Aqueous ammonia (NH3)
(b) Aqueous ammonia (NH3)

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