cementing in cold temps.
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Most chemical reactions are more vigorous or move much faster with an elevated temperature with more molecular movement means more the ions will collide better with the metal atoms, and making it easier to transfer electrons in the chemical reaction, besides temperature, a larger clean surface area, mechanical stirring or agitation, and the amount of free acid available will also affect the speed of the reaction...
Thanks Butcher, I was trying to figure out if my cold temp in the northwest or if my lead contamination
was the cause of slow cementation.It's hard to let a solution go not being sure you have done what you can.
When I drop a little salt in a test tube and add my solution from the the drop its only slightly cloudy, but when I dump the rest of tube in the bucket it clouds right up. Is this normal?
was the cause of slow cementation.It's hard to let a solution go not being sure you have done what you can.
When I drop a little salt in a test tube and add my solution from the the drop its only slightly cloudy, but when I dump the rest of tube in the bucket it clouds right up. Is this normal?
It is normal if silver is in a solution as an ionic salt, and NaCl has added it for the solution to turn milky or cloudy as AgCl is formed.
Many metal salts are less soluble cold than when in a warmer solution...
Many metal salts are less soluble cold than when in a warmer solution...
Ok, does that mean there may be ag still un-dropped by the copper or the cold? It gets into the 30's in my shop unless I am in there. Should I try treating it as agcl? I kinda get the feeling that what I am seeing is just trace amounts in my tests.I use a 10,000ml beaker to watch the process, its just so cool to see the different color shades as it works.My solution this time around has always been shades of dark green,I'm guessing the lead,minimal filtering and sun is the cause.Sorry Butcher, but my chemistry skills are max'ed out at making kool-aid
It could be trace amounts, an argentometry titration would solve your riddle.
https://www.canterbury.ac.nz/media/documents/science-outreach/chloride_mohr.pdf
https://en.wikipedia.org/wiki/Argentometry
The nitrate solution should go from a green to a blue copper nitrate solution once saturated with copper, the free nitric is consumed and most of the metals which are less reactive than copper have been reduced from solution.
For many reactions that occur around room temperature, the rate of reaction doubles for about every 10 deg C rise in temperature.
You can get a heating pad or bucket warmers, or build a little warming cabinet with a thermostatically controlled incandescent lamp...
https://www.canterbury.ac.nz/media/documents/science-outreach/chloride_mohr.pdf
https://en.wikipedia.org/wiki/Argentometry
The nitrate solution should go from a green to a blue copper nitrate solution once saturated with copper, the free nitric is consumed and most of the metals which are less reactive than copper have been reduced from solution.
For many reactions that occur around room temperature, the rate of reaction doubles for about every 10 deg C rise in temperature.
You can get a heating pad or bucket warmers, or build a little warming cabinet with a thermostatically controlled incandescent lamp...
arthur kierski
Well-known member
i heat the solution in a large beaker,with copper,as the copper dissolves,one can see the formation of rhodium+gold,silver,palladium,platinum---this way,no base metals are dissolved,because of the electrochemistry series---excellent topic
bigpagoda
Well-known member
do you have a containment vessel for a beaker that large?
