To prepare a 100 mL solution of 0.1 M hydrogen peroxide (H2O2), one must calculate the number of moles required, which is 0.01 moles. This is derived from the formula: moles = volume (mL) × molarity (M) / 1000. The mass of hydrogen peroxide needed is 0.34 grams, calculated using the molar mass of H2O2, which is 34 g/mol. However, the preparation method may vary depending on the concentration of the commercially available hydrogen peroxide solution.
PREREQUISITESChemistry students, laboratory technicians, and anyone involved in preparing chemical solutions will benefit from this discussion.
Thank you, My teacher gave us the recipe. i just wanted to check the mass number.Borek said:That's a correct mass of hydrogen peroxide, but that's not a recipe.
To be honest I don't see how to answer the question without knowing what you can use to prepare the solution. Commercially hydrogen peroxide is sold in may different form (solutions of different concentrations), not knowing which one will be used it is impossible to give an answer.