`AgCldarr+2KCN to K[Ag(CN)_(2)]+KCl`

Options

A. For precipitate formation reaction
B. For precipitate dissolution reaction
C. For precipitate exchange reaction
D. For no reaction

Answer

To analyze the reaction \( \text{AgCl} + 2 \text{KCN} \rightarrow \text{K[Ag(CN)}_2] + \text{KCl} \) and determine the type of reaction, we can follow these steps:

### Step 1: Identify the Reactants and Products
The reactants in this reaction are:
- Silver chloride (AgCl), which is a solid precipitate.
- Potassium cyanide (KCN), which is soluble in water.

The products are:
- Potassium dicyanoargentate(I) (K[Ag(CN)₂]), which is a soluble complex.
- Potassium chloride (KCl), which is also soluble in water.

### Step 2: Analyze the Precipitate
In the reactants, AgCl is indicated as a precipitate. This means it is not soluble in the reaction medium (usually water).

### Step 3: Determine the Nature of the Reaction
Since AgCl is a precipitate in the reactants and it is being converted into a soluble complex (K[Ag(CN)₂]) in the products, we can conclude that the precipitate is dissolving in this reaction.

### Step 4: Conclusion
Based on the analysis:
- The reaction involves the dissolution of a precipitate (AgCl) to form a soluble complex (K[Ag(CN)₂]).
- Therefore, this reaction is classified as a **precipitate dissolution reaction**.

### Final Answer
The type of reaction is a **precipitate dissolution reaction**.

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