A sample of iron ore weighing 0.962 g was dissolved in dilute acid solution, and all the Fe(II) was converted to Fe(III) ions. The solution required 32.32 mL of 0.0475M KMnO4 for titration. Fill in the table and calculate the % by mass of iron in the ore. Balance the equation: Fe +2 + MnO4 → Fe+3 + MnO2 Computation Name of analyte Iron ore Mass of analyte 0.2792 g Name of titrant KMnO4 Volume of titrant 23.30 mL Milliequivalents of the titrant 2.260 milliequivalents Mass of the analyte 0.125 g % Fe in analyte 44.81%

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Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.