Oxidation – Reduction Reactions

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Introduction: An endless amount of reactions depend on the concept of oxidation and reduction. Life itself is based on the simple concepts of oxidation and reduction. Photosynthesis and the reverse reaction of cellular respiration are considered one of the many redox reactions. The combustion of wood in a fire is another. These processes are essential in every aspect of human life. For this reason it is necessary to understand what is taking place when these reactions happen. An oxidation reduction reaction happens when electrons transfer from one component in a reaction to another. Oxidation refers to a loss of electrons. An element such as oxygen has a negative two charge. When it reacts it takes electrons from the component that is being oxidized. Oxygen in this case can be called an oxidizer. Reduction occurs when a component of a reaction gains electrons. Even though oxygen is the oxidizer, it is being reduced. Therefore the component losing its electrons can be called a reducer. Through looking at these reactions and finding a balanced equation of the elections, a redox reaction equation can be written. This may be useful when trying to find out an unknown molarity of a reactant. This is what we hope to achieve in this experiment. Procedure/Results In this lab using titration, a basic understanding of acid base equilibrium was established. In the lab potassium permanganate (KMnO4), iron chloride (FeCl₂) and phosphoric acid (H3PO4) are used. To get a basic understanding of acid-base reactions in part 1 the group used 10ml of potassium permanganate (KMnO4), iron chloride (FeCl₂), and phosphoric acid (H3PO4) were used. Most acid base reactions need an indicator. In this redox reaction the color was used as an indicator of when equilibrium was reached. A solution of iron chloride (FeCl₂) and phosphoric acid (H3PO4) was

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