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of chemicals

Learn all about electroplating, its history, applications, lab experiments, and harmful effects of chemicals. Understand how it relates to 'O' Level syllabus and its practical implications. Discover the theory behind electroplating, its uses in jewelry making, rust protection, and more. Conduct your own experiment and delve into the world of electrochemistry. Explore the risks of handling electroplating chemicals and the importance of safety measures.

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of chemicals

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  1. plating of chemicals

  2. Contents • How is it related to syllabus in ‘O’ Levels • History • What is electroplating? • Application • Lab experiment • Harmful effects of electroplating through process and nature of chemicals

  3. ‘O’ Level Syllabus • Under the topic on electrolysis, students should be able to describe the electroplating of metals, e.g. copper plating, and state one use of electroplating

  4. A new era of electrochemistry started when Humphry Davy (1778–1829), a British chemist, built a powerful battery to pass electricity through molten salts. He discovered elements, such as potassium, sodium, calcium and magnesium, by liberating them from their molten compounds. But who actually invented electroplating?

  5. Who was smart enough to have came up with the theory of ELECTROPLATING? • Italian chemist, Luigi Brugnatelli • Invented electroplating in 1805 • Brugnatelli performed electrodeposition of gold using the Voltaic Pile • His work was rebuffed by the dictator Napoleon Bonaparte • He still did write about electroplating in the Belgian Journal of Physics and Chemistry

  6. What is ELECTROPLATING? Electroplating is the deposition of a metallic coating by putting a negative charge on an object and exposing it to a solution containing a metal salt. The positively charged metal ions in the salt solution are attracted to the object and reduced to metallic form upon it.

  7. Putting ELECTROPLATING into APPLICATION • Rust protection • Acid/Alkali protection • Volt increase in conductivity 4. Jewellery making 5. Lead protection

  8. Theory of ELECTROPLATING Anode - connected to the positive terminal of the battery Cathode - connected to the negative terminal of the battery Lemmon battery

  9. When power is switched on: • Copper is oxidized at the anode to Cu2+ by losing 2 electrons • Cu 2+ associates with SO42- in the solution to form CuSO4 • Cu2+ is reduced to metallic Cu at the cathode by gaining 2 electrons • Redox reaction occurs during electroplating.

  10. Why is the object to be plated placed at the cathode? • It is because the cathode is negatively charged by being connected to the negative terminal of the battery. Hence, the Cu2+ ions are attracted to the object at the cathode. Copper (anode) Coin (cathode) Cu2+

  11. Time to conduct a little EXPERIMENT!

  12. PROCEDURES • 200ml of the electrolyte solution is poured into a beaker • Wires with alligator clips are connected to the terminals of the power supply. • The coins are cleaned with a mixture of 3g NaCl and 15ml vinegar, rinsed and dried. • One end of a 10-cm length of copper is tightly wrapped around each coin, leaving 5-6 cm of wire free. • The mass of each coin-copper wire is measured and recorded

  13. 6. The set up is prepared as shown. 7. The electroplating cell is allowed to operated for 60 minutes. 8. The electrode is being removed and dried, being careful not to lose any of the copper plating. 9. The mass of the end product is measured and recorded.

  14. RESULTS 1.6g – 1.4g = 0.2g of copper was coated on the coin.

  15. Conclusion Effective transfer of copper from anode source to a plate covering the cathode. Copper, Nickel, Silver, Gold, Chromium } single metallic elements Brass, Solder } alloys

  16. Is it harmful? As reported in ‘Guidelines For The Safe Use Of Chemicals In Electroplating’, the nature of chemicals used in electroplating processes are toxic and corrosive to the skin. It is important that everyone could potentially come into contact with the chemicals should know and understand the risks involved and the specific handling precautions required for each chemical. In addition, protective equipments and clothings need to be worn.

  17. Hydrochloric acid

  18. Nickel salts chlorides, sulfate

  19. Sulfuric acid

  20. Special THANKS to the following websites • http://www.osh.dol.govt.nz/order/catalogue/pdf/electroplating.pdf • http://sg.images.search.yahoo.com/search/images?ei=UTF-8&p=Trichloroethylene&y=Search&fr2=tab-web&fr=yfp-t-web-s • http://www.enviroliteracy.org/images/page-spec/sulfuric%20acid.gif • http://www3.moe.edu.sg/edsoftware/ir/files/chem-titration-setup/images/hydrochloric_acid_3835.jpg • http://penelopeillustration.com/blog/wp-content/backgrounds.jpg • http://inventors.about.com/od/estartinventions/a/Electroplating.htm • http://www.finishing.com/faqs/howworks.html • http://www.lwkoo.cn/Freepaper/UploadFiles_2179/200809/2008090415142143.jpg • http://savetherobot.files.wordpress.com/2009/01/the-end.jpg • http://www.woodrow.org/teachers/chemistry/institutes/1986/exp30.html • http://www.fotosearch.com.au/clip-art/good.html • http://www.fotosearch.com.au/clip-art/coin.html • www.fotosearch.com.au • www.google.com • www.yahoo.com • www.wikipedia.com • http://www.wondercliparts.com/hugs/graphics/hugs_graphics_04.gif

  21. A big thank you to our fellow teachers for their wisdom, the School for its endless support, the textbook for providing valuable information and any other person that has helped in one way or another.

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