A certain weioght of pure `CaCO_(3)` is made to react completely with 200mL of a HCl solution to given 227mL of `CO_(2)` gas at STP. The notmality of the HCl` solution is :

Options

A. `0.05N`
B. `0.1N`
C. `1.0N`
D. `0.2N`

Answer

To find the normality of the HCl solution that reacted with calcium carbonate (CaCO₃) to produce carbon dioxide (CO₂), we can follow these steps:

### Step 1: Write the balanced chemical equation
The reaction between calcium carbonate and hydrochloric acid can be represented as:
\[ \text{CaCO}_3 + 2 \text{HCl} \rightarrow \text{CaCl}_2 + \text{H}_2\text{O} + \text{CO}_2 \]

### Step 2: Calculate the moles of CO₂ produced
At STP (Standard Temperature and Pressure), 1 mole of gas occupies 22.4 liters (or 22400 mL). Given that 227 mL of CO₂ was produced, we can calculate the moles of CO₂:
\[ \text{Moles of CO}_2 = \frac{\text{Volume of CO}_2 \text{ (in mL)}}{22400 \text{ mL/mol}} = \frac{227}{22400} \approx 0.0101 \text{ moles} \]

### Step 3: Determine the moles of HCl required
From the balanced equation, we see that 1 mole of CO₂ is produced from 2 moles of HCl. Therefore, the moles of HCl required can be calculated as:
\[ \text{Moles of HCl} = 2 \times \text{Moles of CO}_2 = 2 \times 0.0101 \approx 0.0202 \text{ moles} \]

### Step 4: Calculate the normality of the HCl solution
Normality (N) is defined as the number of equivalents of solute per liter of solution. For HCl, which is a monoprotic acid (it donates one proton), the number of equivalents is equal to the number of moles.

The volume of the HCl solution used is 200 mL, which is equivalent to 0.200 L. Thus, the normality can be calculated as:
\[ \text{Normality} = \frac{\text{Number of equivalents}}{\text{Volume of solution in L}} = \frac{0.0202 \text{ moles}}{0.200 \text{ L}} = 0.101 \text{ N} \approx 0.1 \text{ N} \]

### Final Answer
The normality of the HCl solution is approximately **0.1 N**.

---