Addition of `HCl` to an aqueous solution of `Pb(NO_(3))_(2)` gives a

Options

A. yellow precipitate
B. brown precipitate
C. white precipitate
D. black precipitate

Explanation

To solve the question regarding the addition of HCl to an aqueous solution of Pb(NO₃)₂, we can follow these steps:

### Step 1: Identify the Reactants
The reactants in this reaction are hydrochloric acid (HCl) and lead(II) nitrate (Pb(NO₃)₂).

### Step 2: Write the Chemical Equation
When HCl is added to Pb(NO₃)₂, a double displacement reaction occurs. The general form of the reaction can be written as:
\[ \text{Pb(NO}_3\text{)}_2 (aq) + 2 \text{HCl} (aq) \rightarrow \text{PbCl}_2 (s) + 2 \text{HNO}_3 (aq) \]

### Step 3: Identify the Products
In this reaction, the products formed are lead(II) chloride (PbCl₂) and nitric acid (HNO₃). Lead(II) chloride is known to be insoluble in water and will precipitate out of the solution.

### Step 4: Determine the State of the Products
Lead(II) chloride (PbCl₂) is a solid precipitate, while nitric acid (HNO₃) remains in aqueous form. Thus, we can denote the states of the products as:
\[ \text{PbCl}_2 (s) \text{ and } 2 \text{HNO}_3 (aq) \]

### Step 5: Color of the Precipitate
Lead(II) chloride (PbCl₂) is known to form a yellow precipitate when formed in this reaction.

### Final Answer
Therefore, the addition of HCl to an aqueous solution of Pb(NO₃)₂ gives a yellow precipitate of PbCl₂.

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