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Step-by-Step Solution
Step 1: Understand Volume Strength of Hydrogen Peroxide
The term “volume strength” of hydrogen peroxide indicates the volume of oxygen (in mL) released at NTP (Normal Temperature and Pressure) from 1 mL of the hydrogen peroxide solution. It typically relates to molarity by the relationship:
$\text{Volume strength} = 11.2 \times \text{Molarity}$
Step 2: Calculate Molarity from Volume Strength
Given:
Volume strength of $H_{2}O_{2}$ = 5.6
Relationship: $ \text{Molarity} = \dfrac{\text{Volume strength}}{11.2} $
Substitute the given volume strength:
$$
\text{Molarity} = \dfrac{5.6}{11.2} = 0.5
$$
Step 3: Assume 1 Litre (1000 mL) of This Solution
For ease of calculation, assume the volume of solution is 1 litre. The density of the solution is given as 1 g/mL, which implies:
$$
\text{Mass of 1 litre solution} = 1000 \,\text{mL} \times 1 \,\text{g/mL} = 1000 \,\text{g}
$$
Step 4: Calculate Mass of Solute (Hydrogen Peroxide)
The number of moles of $H_{2}O_{2}$ in 1 litre of 0.5 M solution is:
$$
\text{Moles of }H_{2}O_{2} = 0.5 \,\text{mol}
$$
The molar mass of hydrogen peroxide ($H_{2}O_{2}$) is 34 g/mol. Hence, the mass of $H_{2}O_{2}$ present is:
$$
\text{Mass of }H_{2}O_{2} = 0.5 \,\text{mol} \times 34 \,\text{g/mol} = 17 \,\text{g}
$$
Step 5: Calculate Mass Percentage of Hydrogen Peroxide
Mass percentage % is given by:
$$
\text{Mass \% of }H_{2}O_{2}
= \biggl(\dfrac{\text{Mass of solute}}{\text{Mass of solution}}\biggr) \times 100
$$
Substituting values:
$$
\text{Mass \%}
= \biggl(\dfrac{17 \,\text{g}}{1000 \,\text{g}}\biggr) \times 100
= 1.7\%
$$
Final Answer
The strength of 5.6 volume hydrogen peroxide in terms of mass percentage and molarity is:
1.7% and 0.5 M.
