With `Co^(2+)` ions `[Fe(CN)_(6)]^(3-)` gives a ……..ppt of `Co_(3)[Fe(CN)_(6)]`

Options

A. Blue
B. raddish brown
C. chocolate
D. Green

Answer

To solve the question regarding the reaction between \( Co^{2+} \) ions and \( [Fe(CN)_{6}]^{3-} \), we can follow these steps:

### Step 1: Identify the Reactants
The reactants in this reaction are:
- Cobalt ions: \( Co^{2+} \)
- Ferricyanide ions: \( [Fe(CN)_{6}]^{3-} \)

### Step 2: Determine the Reaction
When \( Co^{2+} \) ions react with \( [Fe(CN)_{6}]^{3-} \), they form a complex compound. The expected product is \( Co_3[Fe(CN)_{6}] \).

### Step 3: Write the Balanced Equation
The balanced chemical equation for this reaction can be represented as:
\[ 3 Co^{2+} + 2 [Fe(CN)_{6}]^{3-} \rightarrow Co_3[Fe(CN)_{6}] \]

### Step 4: Identify the Precipitate
The product \( Co_3[Fe(CN)_{6}] \) is a complex that forms a precipitate when these ions react in solution.

### Step 5: Determine the Color of the Precipitate
Based on known chemical properties, the precipitate \( Co_3[Fe(CN)_{6}] \) is characterized by its color. It is known to form a reddish-brown precipitate.

### Final Answer
Thus, the precipitate formed when \( Co^{2+} \) ions react with \( [Fe(CN)_{6}]^{3-} \) is a **reddish-brown precipitate** of \( Co_3[Fe(CN)_{6}] \).

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