4.48 lit of ammonia at STP is neutralised using 100 ml of a solution of `H_(2)SO_(4)`, the molarity of acid is

Answer

To solve the problem of finding the molarity of the sulfuric acid (H₂SO₄) solution that neutralizes 4.48 liters of ammonia (NH₃) at STP, we can follow these steps:

### Step 1: Write the balanced chemical equation for the neutralization reaction.
The balanced equation for the reaction between ammonia and sulfuric acid is:
\[ 2 \text{NH}_3 + \text{H}_2\text{SO}_4 \rightarrow \text{(NH}_4)_2\text{SO}_4 \]

### Step 2: Calculate the number of moles of ammonia (NH₃).
At STP (Standard Temperature and Pressure), 1 mole of any gas occupies 22.4 liters. Therefore, we can calculate the number of moles of ammonia using the formula:
\[ \text{Number of moles} = \frac{\text{Volume at STP}}{22.4 \text{ L/mol}} \]
Given that the volume of ammonia is 4.48 liters:
\[ \text{Number of moles of NH}_3 = \frac{4.48 \text{ L}}{22.4 \text{ L/mol}} = 0.2 \text{ moles} \]

### Step 3: Determine the number of moles of sulfuric acid (H₂SO₄) required for neutralization.
From the balanced equation, we see that 2 moles of NH₃ react with 1 mole of H₂SO₄. Therefore, the number of moles of H₂SO₄ needed can be calculated as follows:
\[ \text{Number of moles of H}_2\text{SO}_4 = \frac{0.2 \text{ moles of NH}_3}{2} = 0.1 \text{ moles} \]

### Step 4: Calculate the molarity of the H₂SO₄ solution.
Molarity (M) is defined as the number of moles of solute per liter of solution. Since we have 0.1 moles of H₂SO₄ in 100 mL of solution, we first convert 100 mL to liters:
\[ 100 \text{ mL} = 0.1 \text{ L} \]
Now we can calculate the molarity:
\[ \text{Molarity} = \frac{\text{Number of moles of H}_2\text{SO}_4}{\text{Volume of solution in L}} = \frac{0.1 \text{ moles}}{0.1 \text{ L}} = 1 \text{ M} \]

### Final Answer:
The molarity of the sulfuric acid solution is **1 M**.

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