1. Understanding the Information:
* 3.0% hydrogen peroxide: This means that 100 g of the solution contains 3.0 g of H₂O₂.
* Density of 1.0 g/mL: This tells us that 1 mL of the solution weighs 1 g.
2. Calculating the Molarity:
* Molar mass of H₂O₂: 2(1.01 g/mol) + 2(16.00 g/mol) = 34.02 g/mol
* Mass of H₂O₂ in 1 L of solution: Since the density is 1.0 g/mL, 1 L (1000 mL) of solution weighs 1000 g. Therefore, 1 L of solution contains (3.0 g H₂O₂ / 100 g solution) * 1000 g solution = 30 g H₂O₂.
* Moles of H₂O₂ in 1 L of solution: (30 g H₂O₂) / (34.02 g/mol) = 0.882 mol H₂O₂
* Molarity (M): Molarity is defined as moles of solute per liter of solution. Therefore, the molarity of the solution is 0.882 mol/L or 0.882 M.
Therefore, the molarity of a 3.0% hydrogen peroxide aqueous solution is approximately 0.882 M.
