The strength of `H_(2)O_(2)` is expressed in many ways like molarity , normality , % strength and volume strengths But out of all these form of strengths , volume strength has great significance for chemical reactions .
This decomposition of `H_(2)O_(2)` is shown as under
`H_(2)O_(2)(l) to H_(2)O(l) + (1)/(2)O_(2)(g)`
'x' volume strength of `H_(2)O_(2)` means one volume (litre or ml) of `H_(2)O_(2)` releases x volume (litre or ml) of `O_(2)` at NTP .
1 litre `H_(2)O_(2)` release x litre of `O_(2)` at NTP
`=(x)/(22.4)` moles of `O_(2)`
From the equation ,
1 mole of `O_(2)` produces from 2 moles of `H_(2)O_(2)` .
`(x)/(22.4)` moles of `O_(2)` produces from `2xx(x)/(22.4)` moles of `H_(2)O_(2)`
`=(x)/(11.2)` moles of `H_(2)O_(2)`
So, molarity of `H_(2)O_(2)=((x)/(11.2))/(1)=(x)/(11.2)M`
Normality =n-factor `xx` molarity
`=2xx(x)/(11.2)=(x)/(5.6) N`
What volume of `H_(2)O_(2)` solution of "11.2 volume" strength is required to liberate 2240 ml of `O_(2)` at NTP?

Options

A. 300 ml
B. 500 ml
C. 100 ml
D. 200 ml

Answer

To solve the problem, we need to determine the volume of H₂O₂ solution with a volume strength of 11.2 that is required to liberate 2240 ml of O₂ at NTP.

### Step-by-Step Solution:

1. **Understanding Volume Strength**:
- The volume strength of H₂O₂ indicates how many milliliters of O₂ are produced by 1 ml of H₂O₂ solution at NTP.
- Given that the volume strength of H₂O₂ is 11.2, this means that 1 ml of this solution produces 11.2 ml of O₂.

2. **Setting Up the Relationship**:
- We need to find out how many milliliters of H₂O₂ solution are required to produce 2240 ml of O₂.
- From the volume strength, we know that:
\[ 1 \text{ ml of H₂O₂ solution} \rightarrow 11.2 \text{ ml of O₂} \]

3. **Calculating the Required Volume**:
- To find the volume of H₂O₂ solution needed to produce 2240 ml of O₂, we can set up the following proportion:
\[ \text{Volume of H₂O₂ (ml)} = \frac{\text{Volume of O₂ (ml)}}{\text{Volume strength (ml O₂/ml H₂O₂)}} \]
- Substituting the known values:
\[ \text{Volume of H₂O₂} = \frac{2240 \text{ ml}}{11.2 \text{ ml O₂/ml H₂O₂}} \]

4. **Performing the Calculation**:
- Now, we perform the division:
\[ \text{Volume of H₂O₂} = \frac{2240}{11.2} = 200 \text{ ml} \]

5. **Final Answer**:
- Therefore, the volume of H₂O₂ solution required to liberate 2240 ml of O₂ at NTP is **200 ml**.

### Summary:
The volume of H₂O₂ solution with a volume strength of 11.2 required to liberate 2240 ml of O₂ at NTP is **200 ml**.