`K_(4)[Fe(CN)_(6)]+2CuSO_(4)toCu_(2)[Fe(CN)_(6)]darr`

Options

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

Answer

To analyze the given reaction \( K_4[Fe(CN)_6] + 2CuSO_4 \rightarrow Cu_2[Fe(CN)_6] \), we need to determine the type of reaction it represents. Here’s a step-by-step breakdown of the solution:

### Step 1: Identify the Reactants and Products
- **Reactants**: \( K_4[Fe(CN)_6] \) and \( 2CuSO_4 \)
- **Products**: \( Cu_2[Fe(CN)_6] \)

### Step 2: Understand the Reaction Components
- \( K_4[Fe(CN)_6] \) is potassium ferrocyanide.
- \( CuSO_4 \) is copper(II) sulfate.
- \( Cu_2[Fe(CN)_6] \) is copper(II) ferrocyanide.

### Step 3: Analyze the Reaction
- The reaction involves the combination of potassium ferrocyanide and copper(II) sulfate.
- When these reactants combine, they form copper(II) ferrocyanide, which is known to be insoluble in water.

### Step 4: Identify the Type of Reaction
- The presence of a downward arrow (↓) next to \( Cu_2[Fe(CN)_6] \) indicates that this product is a precipitate.
- Since a solid (precipitate) is formed from the reaction of two aqueous solutions, this indicates that the reaction is a **precipitate formation reaction**.

### Conclusion
Thus, the reaction \( K_4[Fe(CN)_6] + 2CuSO_4 \rightarrow Cu_2[Fe(CN)_6] \) is classified as a **precipitate formation reaction**.

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