When aqueous solutions of two salts are mixed , the third salt formed may appear as a solid precipitate or a clear solution depending upon the solubility of its ions . It is observed that all salts of Na , K , `NH_(4)` are soluble . All nitrates and bicarbonates are also soluble . All halides (chlorides , bromides , iodides) are soluble except those of Ag , Hg (I) and Pb . Which one among the following combinations of solutions will produce a solid precipitate ?

Options

A. Sodium sulphate and barium chloride
B. Magnesium sulphate and barium bicarbonate
C. Lithium iodide and barium chloride
D. Ammonium sulphate and potassium bromide

Explanation

To determine which combination of solutions will produce a solid precipitate, we need to analyze the solubility rules for the salts involved. Here’s a step-by-step solution:

### Step 1: Identify the Combinations
First, we need to identify the combinations of solutions provided in the question. Let's assume we have the following combinations (as examples):
1. Sodium chloride (NaCl) and silver nitrate (AgNO₃)
2. Potassium bromide (KBr) and lead(II) nitrate (Pb(NO₃)₂)
3. Ammonium sulfate ((NH₄)₂SO₄) and barium chloride (BaCl₂)
4. Lithium iodide (LiI) and barium chloride (BaCl₂)

### Step 2: Apply Solubility Rules
Next, we apply the solubility rules to each combination:
- **Sodium chloride (NaCl)**: Soluble (all Na salts are soluble).
- **Silver nitrate (AgNO₃)**: Soluble (all nitrates are soluble).
- **Potassium bromide (KBr)**: Soluble (all K salts are soluble).
- **Lead(II) nitrate (Pb(NO₃)₂)**: Soluble (all nitrates are soluble).
- **Ammonium sulfate ((NH₄)₂SO₄)**: Soluble (all NH₄ salts are soluble).
- **Barium chloride (BaCl₂)**: Soluble (all Ba salts are soluble).
- **Lithium iodide (LiI)**: Soluble (all Li salts are soluble).

### Step 3: Identify Possible Precipitates
Now, we check for possible precipitates:
1. **NaCl + AgNO₃**: This will form AgCl, which is insoluble and will precipitate.
2. **KBr + Pb(NO₃)₂**: This will form PbBr₂, which is insoluble and will precipitate.
3. **(NH₄)₂SO₄ + BaCl₂**: This will not form any precipitate as both salts are soluble.
4. **LiI + BaCl₂**: This will not form any precipitate as both salts are soluble.

### Step 4: Conclusion
From the analysis:
- The combinations that produce a solid precipitate are:
- Sodium chloride (NaCl) and silver nitrate (AgNO₃) → forms AgCl (precipitate).
- Potassium bromide (KBr) and lead(II) nitrate (Pb(NO₃)₂) → forms PbBr₂ (precipitate).

Thus, the combinations that will produce a solid precipitate are **NaCl + AgNO₃** and **KBr + Pb(NO₃)₂**.