08+Determinination+of+Concentration+by+Oxidation+Reduction+Titration - Determination of Concentration by OxidationReduction Titration of Hydrogen

08+Determinination+of+Concentration+by+Oxidation+Reduction+Titration

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Adapted from Advanced Chemistry with Vernier & Laboratory Experiments for Advanced Placement Chemistry by Sally Ann Vonderbrink, Ph. D. Determination of Concentration by Oxidation- Reduction Titration of Hydrogen Peroxide One method of determining the concentration of a hydrogen peroxide, H 2 O 2 , solution is by titration with a solution of potassium permanganate, KMnO 4 , of known concentration. A titration, as you recall, is a convenient method of learning more about a solution by reacting it with a second solution of known molar concentration. There are a number of ways to measure the progress of a titration. The method used in this experiment is called a potentiometric titration, in which the electric potential of a reaction is monitored. All acid-base titrations that are measured by a pH probe are potentiometric; thus, this method is not as unusual as it may seem. The reaction is an oxidation-reduction reaction and proceeds as shown below, in net ionic form. 5 H 2 O 2 ( aq ) + 2 MnO 4 ( aq ) + 6 H + ( aq ) 5 O 2 ( g ) + 2 Mn 2+ ( aq ) + 8 H 2 O ( l ) In this experiment, you will use an ORP (Oxidation-Reduction Potential) Sensor to measure the potential of the reaction. Your data will look like an acid-base titration curve. The volume of KMnO 4 titrant used at the equivalence point will be used to determine the concentration of the H 2 O 2 solution. Your sample of H 2 O 2 will come from a bottle of ordinary, over-the-counter hydrogen peroxide purchased at a grocery or a drug store. The concentration of this product is labeled as 3% (by mass). This experiment illustrates the electrical nature of chemical reactions, and offers practice with a process for observing and measuring an oxidation-reduction reaction. OBJECTIVES In this experiment, you will Conduct the potentiometric titration of the reaction between commercially available hydrogen peroxide and potassium permanganate. Measure the potential change of the reaction.
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  • Fall '14
  • STARNES
  • Chemistry, Redox, Potassium permanganate, Sally Ann Vonderbrink, Vernier & Laboratory

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