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- Feb 25, 2007
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For starters, the very idea that concentrated nitric is more effective simply isn't the case, at least when digesting silver. Oz said it well. However, my experience in making electrolyte for my silver cell, which was done in one fell swoop, yielded results that are very different from that which may be expected. Note that my comments apply to silver alone---I had more than my share of run-away experiences when processing eye glass frames for gold.
When I made my electrolyte, I used 30 troy ounces of silver crystals from my cell, generally those that were harvested towards the very end of an anode's life, where copper concentration was high. It was my way of proving that my silver was, or was not, pure. At any rate, I'd place the 30 ounces of silver in a 4,000 ml beaker, to which I'd add a liter of concentrated nitric, then a liter of distilled water. It was then placed on heat. I wanted the fastest reaction I could get, for to me, time was money.
Even with applied heat, I never had a problem with a runaway solution. It would foam up to roughly 3 liters in the beaker, then stay steady. I heated the solution to a boil, to insure that I had consumed the free nitric. I always used a trace more silver than was required, which was simply dumped to the silver cell, where it was combined with the next harvest.
Bottom line---silver may be one of the metals that will dissolve with few issues. As I said, I do not recall ever having any problems with silver.
As I've made it known on a regular basis, I am not a chemist. However, consideration should be given to the hydronium ion, which may explain why silver dissolves readily in the presence of water and nitric. There's more going on than creating "space" in the solution.
Harold
When I made my electrolyte, I used 30 troy ounces of silver crystals from my cell, generally those that were harvested towards the very end of an anode's life, where copper concentration was high. It was my way of proving that my silver was, or was not, pure. At any rate, I'd place the 30 ounces of silver in a 4,000 ml beaker, to which I'd add a liter of concentrated nitric, then a liter of distilled water. It was then placed on heat. I wanted the fastest reaction I could get, for to me, time was money.
Even with applied heat, I never had a problem with a runaway solution. It would foam up to roughly 3 liters in the beaker, then stay steady. I heated the solution to a boil, to insure that I had consumed the free nitric. I always used a trace more silver than was required, which was simply dumped to the silver cell, where it was combined with the next harvest.
Bottom line---silver may be one of the metals that will dissolve with few issues. As I said, I do not recall ever having any problems with silver.
As I've made it known on a regular basis, I am not a chemist. However, consideration should be given to the hydronium ion, which may explain why silver dissolves readily in the presence of water and nitric. There's more going on than creating "space" in the solution.
Harold