Stoichiometry problem 1. The problem statement, all variables and given/known data 1 g of H2O2 solution containing x % of H2O2 by weight required x ml of KMnO4 for complete oxidation in acid medium. What is the normality of KMnO4 solution? 2. Relevant equations H2O2 + KMnO4 => 2KOH + 2MnO2 + 2O2 3. The attempt at a solution 1 g of H2O2 solution contains x% of H2O2. Molar mass of H2O2 = 34 g, which means in 100 g of solution, 34g of H2O2 are present. In 1 g of solution, 0.34 grams of H2O2 are present. This reacts with 34 ml of KMnO4. I know that 17 g of H2O2 will react with 158.03 g of KMnO4, based on law of fixed proportions. The problem here is only the volume has been given and not the weight. The formula for Normality i.e. 1 mol / 1 L whereby 34 ml or 0.034 L is substituted in the denominator is not correct. I know I am doing something wrong, but can't figure out what it is. Any help is appreciated. The answer is 0.58 N. I am struggling with stoichiometry and I hope that I will be allowed to post thorny (from my point of view) problems in this thread.