`H_(2)O_(2)` is sold as a solution of approximately `5.0gH_(2)O_(2)` per 100 ml of the solution. The molarity of this solution is approximately

Options

A. 0.15M
B. 1.5M
C. 3.0M
D. 3.4M

Explanation

To find the molarity of the hydrogen peroxide (H₂O₂) solution, we will follow these steps:

### Step 1: Determine the mass of H₂O₂ and its molar mass
We know that the mass of H₂O₂ in the solution is given as 5.0 g. The molar mass of H₂O₂ can be calculated as follows:
- Molar mass of H: 1 g/mol (2 hydrogen atoms contribute 2 g/mol)
- Molar mass of O: 16 g/mol (2 oxygen atoms contribute 32 g/mol)

Thus, the molar mass of H₂O₂ = 2 g/mol (from H) + 32 g/mol (from O) = 34 g/mol.

### Step 2: Calculate the number of moles of H₂O₂
Using the formula for moles:
\[ \text{Number of moles} = \frac{\text{mass (g)}}{\text{molar mass (g/mol)}} \]
Substituting the values:
\[ \text{Number of moles of H₂O₂} = \frac{5.0 \, \text{g}}{34 \, \text{g/mol}} \approx 0.147 \, \text{mol} \]

### Step 3: Convert the volume of the solution from mL to L
The volume of the solution is given as 100 mL. To convert this to liters:
\[ \text{Volume in liters} = \frac{100 \, \text{mL}}{1000} = 0.1 \, \text{L} \]

### Step 4: Calculate the molarity of the solution
Molarity (M) is defined as the number of moles of solute per liter of solution:
\[ \text{Molarity (M)} = \frac{\text{Number of moles}}{\text{Volume (L)}} \]
Substituting the values:
\[ \text{Molarity} = \frac{0.147 \, \text{mol}}{0.1 \, \text{L}} = 1.47 \, \text{mol/L} \approx 1.5 \, \text{M} \]

Thus, the molarity of the H₂O₂ solution is approximately **1.5 M**.

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