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Design an experiment to choose optimum conditions for Electroplating

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Design an experiment to choose optimum conditions for Electroplating Introduction: Electroplating involves the careful control of conditions and of electrolyte. Some of the factors that affect the quality and quantity of the deposit formed in an electroplating cell are observed in this practical. Aim: The aim of this practical is to design and perform an experiment to determine the best and most favourable conditions for electroplating. Diagrams: anode: Cu (s) ------ Cu 2+ (aq) + 2e- (oxidation) cathode: Cu 2+ (aq) +2e- ------ Cu (s) (reduction) Independent variable: concentration of the copper(II) sulfate solution. Dependent variable: volume of the electrolyte solution, time, distance between the electrodes and the current. ...read more.


6. Removed the electrodes from the cell. Dipped them into a beaker with water and then into a solution of acetone. 7. Allowed the acetone to dry for a few seconds and then measured the mass of the electrodes and recorded their results. 9. Modifies the procedure by changing the concentration of the copper sulfate solution. 10. Repeated the process with a lower concentration and recorded the results. Results: 1M 0.5M 0.01M CathodeAnodeCathodeAnodeCathodeAnodeInitial mass(g)6.396.396.706.106.816.02Final mass(g)6.756.116.856.016.825.99Difference (g)+0.36-0.28+0.15-0.10+0.01-0.02 Observation: Anode is being corroded, therefore decrease in mass. Cathode had a shiny coating and had increased in mass. Discussion: There were errors in this practical, which is shown by the results not being identical. ...read more.


The factor that was modified in this practical was the change in concentration, which had effected the mass of the electrodes. The mass change was graphed against the change in concentration of the electrolyte. There are two straight lines of best fit through the points on the graph, which represent, the mass gained at the cathode and the mass lost at the anode. The points on the graph are closely related but are not identical. This shows that an error could have occurred because the mass lost at the anode didn't equal the mass gained at the cathode. Conclusion: When the anode and cathode are absorbed in the electrolyte and an electric current is passed, the anode corrodes and dissolved in the electrolyte and a pure copper metal coating is built up on the cathode. ...read more.

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