Here are the ingredients and steps to properly clean your still. Step 1 — Mix your salt and flour in a small bowl.
Add vinegar until a thick paste forms. Step 2 — Grab a soft cloth and rub the paste all over your still. Allow the paste to dry on the still for about 30 minutes. Step 3 — Rinse the paste off the still in warm water. Your copper still should be much brighter once the paste has been properly washed off. If you are happy with the result then you can simply dry off your still and put it away.
If you desire more shine or want to preserve that glow then you can continue to wax and polish your still. Waxing and polishing copper enhances the natural shine or glow of the metal. The wax also adds a protective coat over the still. This protective coat protects the metal from tarnishing and also forms a layer between oxygen in the air and the copper materials. This prevents the oxidation process and the still will remain deposit free for longer. To treat your still, you need a proper wax or copper cream.
You will also need one of the following polishing tools;. Microfiber cloth — To manually polish your still, apply the polish and start working the wax into the metal until the still shines. Polishing machine — These machines are much quicker and make the polishing process much easier. Only a high density compound would behave that way.
To me, the fact that it oxidises so happily actually shows it has a decent surface area i. After the copper powder was precipitated and filtered, what color was your filtrate? Mine is still bright green. What is this due to? Some copper ascorbate compound? Obviously I just tried this but the ammount of copper powder I got seemed like under a gram.
The ascorbic acid I was using was commercial vitamin C but they were by some hippie brand so I had to filter out some insoluabe particles. The solutions of copper II sulfate and ascorbic acid were combined while hot and were left for the copper powder to precipitate.
I recieved no gas emmited during any stage of the reaction. I am going to try boiling the green filtrate for a while, to see if any more copper will precipitate. Yes it was still green, dark in my case I guess I made sure to use an excess. Copper ascorbate - I'm not sure. It would imply that ascorbic acid is stronger than H2SO4, which surely it is not.
Yet the colour change seems to suggest that. It baffled me too. As to the amount of copper - weigh it. It has a rel. As to gas - it evolved slowly, while I continued to boil it. I can't really say whether this had an effect on the yield. What might help is actually to construct a mechanism of the reaction.
Also, if you continue boiling it down, the colour will go very dark, and a distinct smell is produced - to my nose it smells like decomposing sugars. I have a feeling that only a certain part of the reaction produces the copper powder, and thereafter, whatever you do, you won't get more.
Maybe the product copper, vitamin C's breakdown products inhibiting the reaction. I just don't know. Looks like the subject for a PhD thesis PS good to see someone else is doing some experimenting! Chemoleo, were you using lab grade ascorbic acid or OTC vit C?
After disolving my vit C in water the aqueous layer was yellow so I am assuming some other impurities are in vit C. After filtering the hot dissolved VitC the residue left in the filter paper smelled strongly like citrus and unlike the vitC tablets prior to purification. Hmm, possibly because I was using citrus flavored vitC.
I attempted this reaction again moments ago and I appear to have gotten much more copper powder than before. Last time as I was filtering the citrus impurities out of the Vit C I just had the stem of the funnel leading into the copper sulfate solution. I assume this lead to some cooling of both reactants. However this time I allowed the filtrate from purifing the vit C to go into a mL beaker.
The solutions of copper sulfate and vit C were separatly heated to nearly boiling then mixed quickly and boiled again. I recieved much more copper powder than before. Also, Chemoleo, in your pic of the copper powder, did it look like that upon precipitation and filtering? Or is that pic after you rinsed it with HCl? Mine is much darker after precipitation and filtering. A more exact way for chemoleo's excellent method There's already a method for making nano-sized copper powder with ascorbic acid in the Chemical Abstracts.
The use of PVP is just necessary, if even a finer product is desired. The mol-ratio is the most usefull thing in the following text. Wow, that's actually quite recent! Why does copper precipitate out as a pink solid? Ask Question. Asked 6 years, 5 months ago. Active 6 years, 5 months ago. Viewed 22k times. Improve this question. Naim Sen Naim Sen 1 1 gold badge 2 2 silver badges 6 6 bronze badges. Add a comment.
Active Oldest Votes. Equally good results were obtained from the coal and charcoal, but practically no reduction from the coke at the temperatures used. The significance of these results was not appreciated at the time, as will be explained later. This retort was operated for a couple of weeks with a mixture of 30 parts fine Diamondville coal and 70 parts calcine, with indifferent results. In the meantime it happened that a crucible run was made, in the laboratory, using lumps of coal about thumb size instead of fine coal.
To our surprise, excellent results were obtained, A new line of experiments was started in which calcine was heated and then mixed with coarse coal. The results were poor because of the difficulty of rabbling the coarse coal down into the fine calcine. However, some reduction was obtained. The great disadvantage of the retort method is the low fuel efficiency.
This was especially true when Diamondville coal, 38 per cent, volatile combustible matter, was used. So it was suggested that the coke resulting from the coal must be the reducer and that the hardness and character of the coke must be factors in its efficiency. Diamondville coal assayed in ; volatile combustible matter, It is not a coking coal, in the commercial sense, coke resulting from it being very soft and friable. A charge of coke was ground, mixed with calcine, and reduced in the retort with indifferent success.
The next day the remaining coke, uncrushed, was charged with calcine into the retort. Conditions seemed to be just right this day and an excellent product resulted. The residue was a gray spongy mass mixed with coarse unconsumed coke and had a copper equivalent of 1. It was now decided to preheat coke and calcine under efficient conditions and mix them in an air-tight container.
The retort was shut down and a series of 40 crucible tests made in the laboratory to determine conditions of time, temperature, per cent, of reducer, hardness of coke, possibility of mixing hot, and other details. A double crucible furnace to hold two No. Oil burners were used for heating. The mixer was a sheet-iron shell 2 ft. The mixer was provided with an air-tight cover and three tuyeres, and placed on trunnions so it could be dumped. Coke was burned in the mixer to preheat it, air being supplied through the tuyeres.
When the charge was ready the coke was dumped from the mixer and the tuyeres closed. There was too much cooling in this manipulation and poor results were obtained. Putting the coke in the mixer and heating it by burning a part of it, using air through the tuyeres, was tried.
This failed, due to the difficulty of getting the coke heated to a uniform temperature throughout. However, a copper equivalent of 3. It was then decided to build two small hand-rotated, oil-fired, brick-lined cylinders for preheating, from which the charges could be very quickly drawn into the mixer. This was so promising that a larger furnace of the Bruckner type was made by lining a section of a White Howell furnace, 5 ft.
A 6-in. This gave a furnace 4 ft. The sheet-iron box around the middle of the furnace is stationary and makes a reasonably air-tight space in which the sponge iron can be discharged without excessive oxidation. The discharging door revolves inside the box and the iron falls into a rapid stream of water in a launder below, where it is quenched and washed into a collecting box.
Complete data on this furnace have not been obtained. However, the results obtained so far are satisfactory and no difficulties are apparent which will prevent the development of the process to a commercial basis.
In a commercial plant the calcine would be drawn hot directly from the MacDougall hoppers to the furnace. The oil flame is again started. The discharging door is removed and the charge quenched. We are making sponge iron with a copper equivalent of 1. The coal used amounts to 40 per cent, of the weight of the calcine. It is probable that this percentage. Coke to the extent of 25 per cent, of the weight of the coal is recovered by screening the product discharged from the furnace.
This coke can undoubtedly be used again. The quenching works well, the quenched product averaging 1. The fuel consumption for heating, 20 gal.
We expect to present a paper later giving a full account of this process. When cupric copper in solution is reduced with SO2, in the presence of chlorides, there is a precipitation of cuprous chloride, the amount of.
According to this reaction the equivalent of 1. Actually, from our solutions, 2 to 2. Either pure SO2, gaseous or liquid, or a gas containing 10 per cent. SO2 by volume, can be used for the reduction. A gas containing less than 8 per cent. SO2 by volume does not give satisfactory results. The most satisfactory conditions for the reduction and precipitation of the copper, so far as we have determined them, are saturation of the cold solutions by passing the SO2 gas through at 15 lb.
Three and one-half tons of the 2 per cent. Cu solution carrying 8. NaCl have been precipitated in lb. An average of 80 per cent, of the copper and per cent, of the silver was precipitated, giving a tail solution carrying 0. Cu and 4. H2SO4, the cuprous chloride being soluble in this 8. NaCl solution to the extent of 0. The first experiments were made in a lead-lined iron auto-clave, holding about cc.
The solution was saturated under 10 lb. On a leaching-plant solution carrying 1. Cu a 71 per cent, precipitation was made. The copper solution used in the following experimental work contained: Cu, 2. A lead-lined pressure tank 1 ft. The copper solution from the 2,ton sands-leaching plant will have about this analysis and carry 8.
The solution was saturated under pressure, which was maintained during the heating stage. At first pure SO2 was used. Later 10 per cent.
SO2 gas made from pure SO2 and air was tried. After the details of manipulation were worked out a 90 per cent, precipitation was made with no trouble. Following are the data of one of these runs:. Volume solution, liters………………………………… Cu in head solution…………………………. NaCl in head solution………………………4. Cu in tail solution……………………………0.
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