A 10.0 mL sample of solution requires exactly 25.0 mL of 0.2 N for complete oxidation in an acidic m — Redox Reactions and Volumetric Analysis Chemistry Question

💡 Solution & Explanation

By the Law of Equivalence, milli-equivalents of $H_2O_2$ = milli-equivalents of $KMnO_4$. $N_{H_2O_2} \times 10.0 = 25.0 \times 0.2 \Rightarrow 10 \times N_{H_2O_2} = 5.0 \Rightarrow N_{H_2O_2} = 0.5 N$. The volume strength of an $H_2O_2$ solution is given by $5.6 \times Normality$. Volume strength = $5.6 \times 0.5 = 2.8 V$.