What is the concentration and % (w/w) of 5.6V `H2O2` solution? (Given molar mass of H2O2 = 34g/mol, density =1g/mL)

Options

A. 0.5,1.70
B. 0.25,1.70
C. 0.5,0.85
D. 0.25,0.85

Answer

To find the concentration and % (w/w) of a 5.6 V H2O2 solution, we can follow these steps:

### Step 1: Understand the Given Information
- Volume strength (V) of H2O2 solution = 5.6 V
- Molar mass of H2O2 = 34 g/mol
- Density of the solution = 1 g/mL

### Step 2: Calculate Molarity from Volume Strength
Volume strength is defined as the volume of oxygen gas (in liters) that can be produced by 1 liter of the solution at standard temperature and pressure (STP).

Using the relationship:
\[ \text{Molarity (M)} = \frac{\text{Volume Strength (V)}}{11.2} \]
Substituting the given volume strength:
\[ M = \frac{5.6}{11.2} = 0.5 \, \text{mol/L} \]

### Step 3: Calculate the Weight of Solute (H2O2)
Using the molarity, we can find the weight of H2O2 in 1 liter of solution:
\[ \text{Weight of solute} = \text{Molarity} \times \text{Molar mass} \times \text{Volume (in L)} \]
\[ \text{Weight of solute} = 0.5 \, \text{mol/L} \times 34 \, \text{g/mol} \times 1 \, \text{L} = 17 \, \text{g} \]

### Step 4: Calculate the Weight of the Solution
Since the density of the solution is given as 1 g/mL, the weight of 1 liter (1000 mL) of the solution is:
\[ \text{Weight of solution} = \text{Density} \times \text{Volume} = 1 \, \text{g/mL} \times 1000 \, \text{mL} = 1000 \, \text{g} \]

### Step 5: Calculate % (w/w) of H2O2
The % (w/w) is calculated using the formula:
\[ \% \text{(w/w)} = \left( \frac{\text{Weight of solute}}{\text{Weight of solution}} \right) \times 100 \]
Substituting the values:
\[ \% \text{(w/w)} = \left( \frac{17 \, \text{g}}{1000 \, \text{g}} \right) \times 100 = 1.7\% \]

### Final Answer
The concentration of the H2O2 solution is **0.5 mol/L** and the % (w/w) is **1.7%**.

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