The strength of 11.2 volume solution of `H_(2)O_(2)` is:
[Given that molar mass of H = 1 g `mol^(-1) and O = 16 g mol^(-1)`]

Options

A. `13.6%`
B. `3.4%`
C. 0.34
D. `1.7%`

Answer

To find the strength of an 11.2 volume solution of hydrogen peroxide (H₂O₂), we can follow these steps:

### Step 1: Understand the Volume Strength
The term "11.2 volume" means that 1 liter of the H₂O₂ solution will produce 11.2 liters of oxygen gas (O₂) at standard temperature and pressure (STP).

### Step 2: Write the Reaction
The decomposition of hydrogen peroxide can be represented by the following reaction:
\[ 2 \text{H}_2\text{O}_2 \rightarrow 2 \text{H}_2\text{O} + \text{O}_2 \]

From this reaction, we can see that 2 moles of H₂O₂ produce 1 mole of O₂.

### Step 3: Calculate Molar Mass of H₂O₂
To find the molar mass of H₂O₂:
- Hydrogen (H) has a molar mass of 1 g/mol.
- Oxygen (O) has a molar mass of 16 g/mol.

Calculating the molar mass of H₂O₂:
\[ \text{Molar mass of H₂O₂} = 2 \times \text{(molar mass of H)} + 2 \times \text{(molar mass of O)} = 2 \times 1 + 2 \times 16 = 2 + 32 = 34 \text{ g/mol} \]

### Step 4: Calculate the Volume of O₂ Produced
Since 1 liter of the H₂O₂ solution produces 11.2 liters of O₂, we can find how many grams of H₂O₂ are needed to produce that volume of O₂.

### Step 5: Relate Volume of O₂ to Grams of H₂O₂
At STP, 1 mole of any gas occupies 22.4 liters. Therefore, to find the number of moles of O₂ produced:
\[ \text{Moles of O₂} = \frac{11.2 \text{ liters}}{22.4 \text{ liters/mole}} = 0.5 \text{ moles} \]

Since 2 moles of H₂O₂ produce 1 mole of O₂, 0.5 moles of O₂ will be produced by:
\[ \text{Moles of H₂O₂} = 2 \times 0.5 = 1 \text{ mole} \]

### Step 6: Calculate Mass of H₂O₂
Now, we can calculate the mass of H₂O₂ in 1 liter of solution:
\[ \text{Mass of H₂O₂} = 1 \text{ mole} \times 34 \text{ g/mol} = 34 \text{ grams} \]

### Step 7: Calculate the Strength of the Solution
The strength (weight/weight percentage) of the solution can be calculated as follows:
\[ \text{Strength} = \left( \frac{\text{mass of H₂O₂}}{\text{mass of solution}} \right) \times 100 \]
Assuming the density of the solution is approximately that of water (1000 g for 1 liter):
\[ \text{Strength} = \left( \frac{34 \text{ g}}{1000 \text{ g}} \right) \times 100 = 3.4\% \]

### Final Answer
The strength of the 11.2 volume solution of H₂O₂ is **3.4%**.

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