Aq. solution of of `KCl * MgCl_(2) * 6H_(2)O` will give test of

Options

A. `K^(+) and Mg^(2+)` only
B. `K^(+) and Cl^(-)` only
C. `K^(+) ,Mg^(2+) and Cl^(-)`
D. `Mg^(2+) and H_(2)O` only

Answer

To solve the question regarding the aqueous solution of KCl·MgCl₂·6H₂O and the tests it will give, we can follow these steps:

### Step 1: Identify the Components of the Compound
The compound KCl·MgCl₂·6H₂O is a double salt composed of potassium chloride (KCl), magnesium chloride (MgCl₂), and water of crystallization (6H₂O).

### Step 2: Dissociation in Water
When this double salt is dissolved in water, it dissociates into its constituent ions:
- Potassium ions (K⁺)
- Magnesium ions (Mg²⁺)
- Chloride ions (Cl⁻)

The dissociation can be represented as:
\[ \text{KCl} \cdot \text{MgCl}_2 \cdot 6\text{H}_2\text{O} \rightarrow \text{K}^+ + \text{Mg}^{2+} + 2\text{Cl}^- \]

### Step 3: Identify the Tests for Each Ion
1. **Potassium Ion (K⁺)**:
- A flame test can be performed where a sample of the solution is placed in a flame. Potassium ions produce a lilac or light purple color in the flame.

2. **Magnesium Ion (Mg²⁺)**:
- A common test for magnesium ions is the addition of sodium hydroxide (NaOH), which will produce a white precipitate of magnesium hydroxide (Mg(OH)₂).

3. **Chloride Ion (Cl⁻)**:
- The presence of chloride ions can be tested by adding silver nitrate (AgNO₃) to the solution, which will form a white precipitate of silver chloride (AgCl).

### Step 4: Conclusion
Since the solution contains potassium ions, magnesium ions, and chloride ions, it will give tests for all three ions.

### Final Answer:
The aqueous solution of KCl·MgCl₂·6H₂O will give tests for potassium ions (K⁺), magnesium ions (Mg²⁺), and chloride ions (Cl⁻).

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