Commercially 10 volume ${\mathrm{H}}_2{\mathrm{O}}_2$ is a solution  with strength of approximately

 

10 volume ${\mathrm{H}}_2{\mathrm{O}}_2$ indicates the volume strength of hydrogen peroxide and states that 1 L hydrogen peroxide forms 10 L of oxygen gas at STP conditions.

Decomposition of hydrogen peroxide forms water and oxygen gas.

 $2{\mathrm{H}}_2{\mathrm{O}}_2\to 2{\mathrm{H}}_2\mathrm{O}+{\mathrm{O}}_2$

Mass of 2 mole of hydrogen peroxide is 64 g and 2 moles of hydrogen peroxide forms one mole of oxygen gas (or 22.4 L of oxygen gas). Mass of hydrogen peroxide required for the formation of 10 L of oxygen gas is:

$\begin{array}{ccc}22.4 \mathrm{L} \mathrm{of} \mathrm{oxygen} \mathrm{produced} \mathrm{by}& =& 64 \mathrm{g} {\mathrm{H}}_2{\mathrm{O}}_2\\ 10 \mathrm{L} \mathrm{of} \mathrm{oxygen} \mathrm{produced} \mathrm{by}& =& 10 \mathrm{L} \mathrm{of} \mathrm{oxygen} \mathrm{produced} \mathrm{by}\times \frac{64 \mathrm{g} {\mathrm{H}}_2{\mathrm{O}}_2}{22.4 \mathrm{L} \mathrm{of} \mathrm{oxygen} \mathrm{gas} \mathrm{produced} \mathrm{by}}\\ & =& 30 \mathrm{g}/\mathrm{L}\end{array}$

30 g/L is the strength of hydrogen peroxide of 10 volume of H₂O₂ solution.