The mixing od aqueous solution od `Na_(2)SO_(4)` and `BaC1_(2)` results in the formation of

Options

A. white precipitate of sodium chlride and is a combination reaction
B. yellow precipitate of sodium chloride and is a double displacement reaction
C. yellow precipitate of barium sulphate and is a combination reaction
D. white precipitate of barium sulphate and is a double displacemant reaction

Answer

To solve the question regarding the mixing of aqueous solutions of \( \text{Na}_2\text{SO}_4 \) and \( \text{BaCl}_2 \), we can follow these steps:

### Step 1: Identify the Reactants
The reactants in this reaction are:
- Sodium sulfate, \( \text{Na}_2\text{SO}_4 \)
- Barium chloride, \( \text{BaCl}_2 \)

### Step 2: Write the Chemical Equation
When these two compounds are mixed, they undergo a double displacement reaction. The general form of a double displacement reaction can be represented as:
\[ AB + CD \rightarrow AD + CB \]

In our case:
- \( A = \text{Na} \)
- \( B = \text{SO}_4^{2-} \)
- \( C = \text{Ba} \)
- \( D = \text{Cl}^- \)

Thus, the reaction can be written as:
\[ \text{Na}_2\text{SO}_4 + \text{BaCl}_2 \rightarrow \text{BaSO}_4 + 2\text{NaCl} \]

### Step 3: Identify the Products
From the equation, the products formed are:
- Barium sulfate, \( \text{BaSO}_4 \)
- Sodium chloride, \( \text{NaCl} \)

### Step 4: Determine the State of the Products
Barium sulfate, \( \text{BaSO}_4 \), is known to be insoluble in water and forms a white precipitate. Sodium chloride, \( \text{NaCl} \), remains dissolved in the aqueous solution.

### Step 5: Conclusion
The mixing of aqueous solutions of \( \text{Na}_2\text{SO}_4 \) and \( \text{BaCl}_2 \) results in the formation of a white precipitate of barium sulfate and a solution of sodium chloride.

### Final Answer
The final products are:
- White precipitate of \( \text{BaSO}_4 \)
- Aqueous solution of \( \text{NaCl} \)

---