EXPERIMENT 1 Title: The Potentiometric Titration of Hydrogen Peroxide Objectives: In this experiment, the aim is to conduct the potentiometric titration of the reactionbetween commercially available hydrogen peroxide and potassium permanganate.Furthermore, to measure the potential change of the reaction. Finally, is to determinethe concentration of the hydrogen peroxide solution.INTRODUCTION: Hydrogen peroxide us topical antiseptic commonly used to treat cuts and wounds toprevent infection. However, hydrogen peroxide is relatively unstable anddecomposes to form water and oxygen gas:H2O2(aq) →H2O(l) + O2(g)In daily life, the percentage is probably not exact 3%. One method of determinethe concentration of a hydrogen peroxide, H2O2, which is by titration with asolution of potassium permanganate, KMnO4, of known concentration. The reaction is oxidation-reduction and proceeds as shown below, in net ionicform.5 H2O2(aq) + 2MnO4– (aq) + 6H+ (aq) → 5O2 (g) + 2Mn2+ (aq) + 8H2O (l)In this experiment, an ORP (Oxidation-Reduction Potential) Sensor used tomeasure the potential of the reaction. The ORP sensor is based on StandardHydrogen Electrode (SHE) as a reference. It can detect pH, temperature andpotential of the solution. The data will look like an acid-base titration curve. Thevolume of KMnO4titrant used at the equivalence point will be used to determinethe concentration of the H2O2solution.
Experimental procedure:1.An acidified and diluted hydrogen peroxide, H2O2, is prepared as solution forthe titration a)100mL of 0.3% H2O2from stock solution of 3% H2O2is prepared.b)10mL of the diluted H2O2solution is measured out precisely into a250mL beaker. 25mL of distilled water and 10 mL of 4.5 M sulfuricacid, H2SO4, solution is mixed carefully. CAUTION: H2SO4is astrong acid and should be handled with care.