Which of the gives a white precipitate with a solution of `AgNO_(3)`, a white precipitate with dil `H_(2)SO_(4)` and a green flame test ?

Options

A. Copper chloride
B. Copper nitrate
C. Lead nitrate
D. Barium chloride

Explanation

To solve the question, we need to identify a compound that meets the following criteria:

1. Gives a white precipitate with a solution of AgNO₃.
2. Gives a white precipitate with dilute H₂SO₄.
3. Produces a green flame test.

Let's analyze the options provided: copper chloride, copper nitrate, lead nitrate, and barium chloride.

### Step-by-Step Solution:

**Step 1: White Precipitate with AgNO₃**
- When a solution of AgNO₃ is added to a compound, a white precipitate indicates the formation of silver chloride (AgCl). This means the compound must contain chloride ions (Cl⁻).
- Among the options, copper chloride (CuCl) and barium chloride (BaCl₂) contain chloride ions. Therefore, we can eliminate copper nitrate and lead nitrate as they do not contain chloride ions.

**Step 2: White Precipitate with Dilute H₂SO₄**
- A white precipitate with dilute H₂SO₄ suggests the formation of a sulfate precipitate. The relevant reactions are:
- Copper chloride (CuCl) would react with H₂SO₄ to form copper sulfate (CuSO₄), which is blue in color, not white.
- Barium chloride (BaCl₂) reacts with H₂SO₄ to form barium sulfate (BaSO₄), which is a white precipitate.
- Therefore, barium chloride is the only option that produces a white precipitate with dilute H₂SO₄.

**Step 3: Green Flame Test**
- The flame test for barium ions (Ba²⁺) produces a green flame. This confirms that barium chloride meets the third criterion of the question.
- Copper compounds typically give a blue-green flame, which does not satisfy the requirement for a green flame.

### Conclusion:
Based on the analysis, the compound that gives a white precipitate with AgNO₃, a white precipitate with dilute H₂SO₄, and produces a green flame test is **barium chloride (BaCl₂)**.

### Final Answer:
**Barium Chloride (BaCl₂)**

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