Hydrogen peroxide can be preapared by the action of dil. `H_(2)SO_(4)` or `H_(3)PO_(4)` on barium peroxide or by bubbling peroxide . On an industrial scale, it can be prepared by hydrolysis of peroxodisulphuric acid obtained by electrolysis of 50% `H_(2)SO_(4)` or an equimolar mixture of `H_(2)SO_(4)` and ammonium sulphate . The strength of `H_(2)O_(2)` solution can be expressed in a number of ways namely normality , molarity , percentage strength and volume strength . Volume strength refers to the volume of `O_(2)` produced at N.T.P. by decomposition of 1 mL of `H_(2)O_(2)` solution. `H_(2)O_(2)` acts as an oxidising as well as reducing agent both in acidic and basic media.
100 volume hydrogen peroxide solution means

Options

A. 17.86 N
B. 30.36% `H_(2)O_(2)`
C. `8.93 M`
D. all are correct

Explanation

To determine what "100 volume hydrogen peroxide solution" means, we need to understand the relationship between the volume of hydrogen peroxide (H₂O₂) and the volume of oxygen (O₂) produced upon its decomposition.

### Step-by-Step Solution:

1. **Understand the Decomposition Reaction**:
The decomposition of hydrogen peroxide can be represented by the following equation:
\[ 2 \text{H}_2\text{O}_2 \rightarrow 2 \text{H}_2\text{O} + \text{O}_2 \]
This means that 2 moles of H₂O₂ produce 1 mole of O₂.

2. **Volume of Oxygen at STP**:
At Standard Temperature and Pressure (STP), 1 mole of any gas occupies 22.4 liters. Therefore, 1 mole of O₂ will also occupy 22.4 liters.

3. **Calculate Oxygen Produced from H₂O₂**:
From the decomposition reaction, we know:
\[ 2 \text{H}_2\text{O}_2 \text{ produces } 1 \text{ mole of } O_2 \]
Thus, 2 moles of H₂O₂ will produce 22.4 liters of O₂. Therefore, 1 mole of H₂O₂ will produce:
\[ \frac{22.4 \text{ liters}}{2} = 11.2 \text{ liters of } O_2 \]

4. **Understanding 100 Volume**:
A "100 volume" solution of H₂O₂ means that 1 liter of this solution can produce 100 liters of O₂.

5. **Calculating Moles of H₂O₂ Required**:
To find out how many moles of H₂O₂ are needed to produce 100 liters of O₂, we can set up the following proportion:
\[ 1 \text{ mole of } O_2 \text{ produces } 11.2 \text{ liters of } O_2 \]
Therefore, to produce 100 liters of O₂, we need:
\[ \text{Moles of H}_2\text{O}_2 = \frac{100 \text{ liters}}{11.2 \text{ liters/mole}} \approx 8.93 \text{ moles} \]

6. **Concentration of H₂O₂**:
Since 1 liter of the solution produces 100 liters of O₂, the molarity (M) of the H₂O₂ solution is approximately 8.93 M.

7. **Normality Calculation**:
The equivalent weight of H₂O₂ is half its molar mass (34 g/mol), which is 17 g. Therefore, the normality (N) can be calculated as:
\[ \text{Normality} = \frac{\text{Weight (g)}}{\text{Equivalent Weight (g)}} = \frac{8.93 \text{ moles} \times 34 \text{ g/mol}}{1 \text{ L}} \div 17 \text{ g} \approx 17.84 N \]

8. **Percentage Strength**:
The mass of H₂O₂ in 1 liter of the solution is:
\[ 8.93 \text{ moles} \times 34 \text{ g/mol} \approx 303.62 \text{ g} \]
The percentage strength can be calculated as:
\[ \text{Percentage} = \left(\frac{303.62 \text{ g}}{1000 \text{ mL}}\right) \times 100 \approx 30.36\% \]

### Final Answer:
Thus, a "100 volume" hydrogen peroxide solution means that 1 liter of the solution can produce 100 liters of oxygen gas at STP.

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