Final answer:
To determine the molarity of a 3.0% m/m H₂O₂ solution with a density of 1.0095 g/mL, calculate the number of moles in 3 g of H₂O₂ and divide by the volume of the solution in liters, resulting in a molarity of approximately 0.89 M.
Step-by-step explanation:
To calculate the molarity of the H₂O₂ solution with a concentration of 3.0% (m/m) and a density of 1.0095 g/mL, you first need to establish the mass of H₂O₂ in 100 g of solution, which is 3 g (since it's 3%).
Then, you can find the volume of that solution by using its density: volume = mass/density. In this case: 100 g / 1.0095 g/mL = 99.06 mL. To get molarity (moles/L), you need the number of moles of H₂O₂ in 3 g.
H₂O₂ has a molar mass of 34.0147 g/mol. So, moles of H₂O₂ = mass/molar mass = 3 g / 34.0147 g/mol = 0.0882 mol. Finally, convert the volume from mL to L (0.09906 L) and calculate the molarity: molarity = moles/volume = 0.0882 mol / 0.09906 L = 0.89 M.