The amount of `H_2O_2` present in 1 L of 1.5 N `H_2O_2` solution is

Options

A. 2.5 g
B. 25.5 g
C. 3.0 g
D. 8.0 g

Explanation

To find the amount of hydrogen peroxide (H₂O₂) present in 1 L of a 1.5 N H₂O₂ solution, we can follow these steps:

### Step 1: Understand Normality
Normality (N) is a measure of concentration equivalent to molarity multiplied by the number of equivalents per mole. For H₂O₂, the N factor is 2 because it can donate 2 protons (H⁺ ions).

### Step 2: Calculate Equivalent Weight
The equivalent weight of H₂O₂ can be calculated using the formula:
\[ \text{Equivalent Weight} = \frac{\text{Molar Mass}}{\text{N factor}} \]
The molar mass of H₂O₂ is approximately 34 g/mol. Therefore:
\[ \text{Equivalent Weight} = \frac{34 \text{ g/mol}}{2} = 17 \text{ g/equiv} \]

### Step 3: Calculate Strength
The strength of the solution (in grams per liter) can be calculated using the formula:
\[ \text{Strength} = \text{Normality} \times \text{Equivalent Weight} \]
Substituting the values:
\[ \text{Strength} = 1.5 \text{ N} \times 17 \text{ g/equiv} = 25.5 \text{ g/L} \]

### Step 4: Conclusion
Thus, the amount of H₂O₂ present in 1 L of a 1.5 N H₂O₂ solution is **25.5 grams**.

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