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Letter 196 Electroplating for a school science project1 2 3
. Hi, I am an electrical/biomed engineering student at the University of Texas at Austin, and am making a few biomed electrodes for EEG measurement. It has been suggested by my professor that we plate, in some way, a layer of silver chloride on our electrodes due to the favorable half-cell potential of this type of coating (bare copper is poisonous, also). I have seen many posts requesting silver plating advice, but how do I plate chlorine on top of silver? I am planning on using AgNO3 to plate w/ silver. )I will be plating some pins that are already covered in a thin layer of gold.) Ted, I'd buy your book if I had the time (an interesting subject is worth $30 to me), but my project deadline for these bio-electrodes is next week, and by the time the book was shipped to me it'd be too late. I plan on hunting down the AgNO3 and some silver electrodes tomorrow, but if you can give me a quick recipe for plating silver chloride onto gold and/or copper, I'd appreciate it. As far as safety is concerned, I have worked with dangerous chemicals before and assure you I know how to handle them. Thanks in advance, Jeff Triffo
. I am a furniture maker (serious hobbyist). In the course of making many Mission Style lamps and furniture pieces I have used copper as decorative trim. Recently I have incorporated mild steel into my pieces. Is it feasible for me to copper plate small steel pieces in my shop? I tend to err on the side of safety in my endeavors and I definitely am NOT interested in handling cyanide solutions (or any other highly toxic substance for that matter). I there a way for me to accomplish stable copper plating without risk to my health? Many thanks for any guidance. Peter Syvertsen
. I am a secondary school student from the U.K and i am trying to find a picture of an electrolysis experiment using sodium chloride. I was wondering if you could direct me to any links as to where I could find pictures of this experiment. thanking you in advance Katie :) Katie
. Dear Finishing.com I am a sophomore in high school and have been working on a science fair project on fuel cells. For the project I am building a simple methanol cell. The cell uses electrodes made of 5/16" carbon tubes. It was suggested to me by a friend in the physics field that I plate part of the carbon tube with copper so that I can solder a wire to it. I have tried the salt/vinegar and penny method and gotten it to work well on steel nails, but I have had no luck with getting the copper to plate onto the carbon. Do you have any ideas? Scott B.
. To whom it may concern, i am doing electroplating for a science fair project.(i am in grade eight.) I have been looking at your site and have a question. What would be the best metals to use for this experiment and how would i exactly do it? If possible, could you tell me about some other resources i could use? Help would be greatly appreciated. thanks in advance, Zac Greisman
+ How come after electroplating the nickel with copper, the copper in the nickel fades and turns into blue green color. I used vinegar with salt 9 volts battery charger. I put them in separate containers with vinegar using copper as the anode and the nickel as the cathode. Marc Andres
+ I'm not sure I understand you, Marc, but if you don't thoroughly rinse the vinegar off, and dry it, you will still have acid on it that is capable of dissolving copper back into blue-green copper ions.
+ Dear Mr. Mooney, After browsing through your website I stumbled upon an experiment you and another person had found to be quite effective in the electroplating of copper pennies. You used vinegar, sugar, and salt as the electrolytic solution/bath. I've tried and tested your mixture. I changed it a little however....: I used a six volt battery, the sanded down penny as the anode, and the "bright" penny as the cathode. I filled my transparent tank with 1 gallon of warm water. Then I added 1/8 cup of vinegar, salt and sugar. Once placed in the tank, the cathode immediately began to fizz. After ten minutes, and the re-application of the toothbrush cleaning, my "zinc" penney was quite remarkable. I'm not sure of what was being let out at the cathode, though. Can you please tell me what was being released and how this electroplating process took place even without a SALT of zinc serving as the electrolytic solution? How can this work if the electrolytic bath is not composed of ions of the plating metal? Any help you can give me would be much appreciated. (The purpose of my doing this is to show how simple household substances can electroplate dull objects). Thankyou, Danielle Danielle W.
+ Hello Danielle, we're happy to hear that the experiment went well for you. At the anode (the sanded penny) there is a positive charge, i.e., the battery is pulling electrons away. At the cathode (the penny being plated) there is a negative charge, i.e., the battery is supplying electrons. So, what happens at each end of the cell then is reactions that are consistent with this electron activity. At the anode, metallic zinc (Zn0) is available from the sanded penny. Remove two electrons per atom, pulled away by the battery, and you get Zn++ ions of zinc dissolving into the solution. Also available at the anode is water , H+2O- -. Pull electrons away from the oxygen and you get oxygen gas. At the cathode, electrons are added to the Zn++ ions in solution, reducing it to metallic zinc Zn0. Also happening though, is electrons are being added to the water, causing the hydrogen in the H+2O- - to be reduced to H0, hydrogen gas. There is a bit more to it, related to the fact that molecules of gases like hydrogen and oxygen usually contain two atoms rather than one, and that, depending on the pH, water may split into hydrogen gas and hydroxide (OH- )ons rather than hydrogen gas and oxygen gas. But that's the general idea. By the way, I note that some people mix-and-match pieces of experiments, and that's a good learning experience. Because of that I like to discourage people from using table salt (NaCl) in the experiments, suggesting the use of Epson salts MgSO4 instead, because we don't want any possibility of chlorine gas Cl- being released if people get carried away with increasing the voltage, concentration, and acidity.
+ Do you have any information about electricity as a catalyst in chemical reactions please send me any kind of information? Bernadette Angat
+ Mr. Mooney & others, The "silver plating" mentioned in the first inquiry may well have been the mercury replacement reaction that I, too, did as a kid. Mercuric Nitrate solution, kept in a Skippy peanut butter jar, was quite useful for impressing sixth-grade girls with my "magic". Today, however, mercury is limited from common use by the knowledge that it is very toxic (to humans and in the environment). Mercury-containing hazardous wastes are some of the most worrisome by-products concerning industry today. Alas, no more slippery, shiny silver pennies! (I'm glad I learned chemistry when I did and lived to talk about it.) My hat is off to you, Mr. Mooney, for your concern about encouraging learning while advising caution and stimulating independent research. Thank you. John E. Softy
+++++ Why does the copper leave the pennies and deposit on the iron? I need a simplified reason to explain to my 2nd grader. We're doing Immersion copper plating. Aileen Paluck
+++++ Start with an acid, Aileen. It is comprised of 2 kinds of ions paired together, cations and anions. For example, in hydrochloric acid, which is HCl, you have H+ cations and Cl- anions in balance. However, while the Cl is paired by the H, there are things that would balance the Cl better. Copper for one. So copper dissolves into the acid, and the hydrogen bubbles out. But there are things that balance the anions even better than copper. Iron for one. So what happens is the acid dissolves both copper and the iron, but the iron pairs better, so the Cl pairs with the iron, and the copper has no matching anion to keep it in solution, forcing it to fall out of solution and deposit on the iron article. Not a great explantion, but it's hard to explain this kind of chemistry to a second grader.
I am doing a science fair project and I want to electroplate quarters with copper using copper sulphate. what would I need to mix the copper sulphate with to make the solution? and what kind of volt battery would be best to use? Mayra
+++++ Hi, Jenna Mave
+++++ An old book of mine tell a VERY simple method of electroplating targeted towards kids if this is what you are talking about. It says to get 2 long wires (doens't specify) and attachted copper end to penny and nickel and the other to the postitve terminal (penny) and negative terminal (nickel) of a 6 volt battery. it says to wrap wires around pencil and balance over glass jar with water (water used as the electrolyte). it is supposed to go through the water with the electricle curret and copperplate the nickel and be scraped off easily. That the simplest method of electroplating I've come across so far. Michele
+++++ But does it work, Michele? I doubt it because for the copper to get to the nickel, it has to travel there. And it does not travel as a solid in little flakes; rather it must dissolve in the solution as travel as a copper ion. But how are you going to dissolve copper in water? If you think it works, please try it and tell us what you find.
+++++ WELL I'M A FEW MONTHS LATE IN REGARD TO THE ABOVE QUESTION, BUT I ALSO TRIED THAT EXPERIMENT AND NO, IT DIDN'T WORK. I TRIED 4 TIMES AND NOTHING BUT DIRTY (BLUE-GRAY) WATER. MAYBE I DIDN'T ALLOW IT ENOUGH TIME (OVERNIGHT YIELDED NOTHING). ANYWAY I'M SORRY TO SAY OUR FASCINATION WITH PLATING HAS NOT ENDED BECAUSE I AM WORKING ON A SCIENCE PROJECT WHICH IS WHY I'M ON YOUR SITE. Raquel
+++++ No surprise here. Use vinegar instead of water, Raquel, and it will work. Maybe not great, but it will work.
August 1, 2006 A great and somewhat easy "experiment," (should be more of a demo
for for any classroom presentation) is plating copper (Cu) with zinc
(Zn). Jonathan Fields 1 2 3
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