Commerical `11.2` volume `H_(2)O_(2)` solution has a molarity of

Options

A. 2M
B. 1 M
C. 3 M
D. 4 M

Explanation

To find the molarity of the commercial 11.2 volume H₂O₂ solution, we can follow these steps:

### Step-by-Step Solution:

1. **Understand the Concept of Volume Strength**:
Volume strength of a solution is defined as the volume of oxygen gas (in liters) that can be liberated by 1 liter of the solution at standard conditions. For hydrogen peroxide (H₂O₂), 1 volume strength corresponds to 1 mole of H₂O₂ producing 1 mole of O₂.

2. **Identify the Given Information**:
We are given that the volume strength of the H₂O₂ solution is 11.2. This means that 1 liter of this solution can liberate 11.2 liters of O₂ gas.

3. **Use the Formula to Relate Volume Strength and Molarity**:
The relationship between volume strength and molarity is given by the formula:
\[ \text{Molarity} = \frac{\text{Volume Strength}}{11.2} \]
Here, the volume strength is in terms of liters of O₂ liberated per liter of solution.

4. **Substitute the Value of Volume Strength**:
Substitute the given volume strength (11.2) into the formula:
\[ \text{Molarity} = \frac{11.2}{11.2} \]

5. **Calculate the Molarity**:
Performing the calculation:
\[ \text{Molarity} = 1 \]

6. **Conclusion**:
Therefore, the molarity of the commercial 11.2 volume H₂O₂ solution is 1 M (1 molar).

### Final Answer:
The molarity of the commercial 11.2 volume H₂O₂ solution is **1 M**.

---