Noxx
Well-known member
Hello guys !
I have a question about HCl.
Here's the context: in the DBC (Dibutyl Carbitol) patent, they say that the gold bearing solution should be between 0.5-1.75N.
If I remember correctly, one Normal is one Mol/L. ?
If so, how do I know what's the HCl concentration of my solution ?
I dissolved 7.9 grams of gold in 30mL of HCl (30%) and 10mL of nitric acid.
Then I evaporated to remove any nitric remaining.
The only solution I see is to evaporate the solution to a syrupy constancy , add water, then repeat to get rid of the HCl and the nitric acid. Finally, I would add a calculated amount of HCl to the gold chloride solution to reach 1.0N
BTW, I do not own any pH meters so forget about calculating the H+ ions concentration![Stick out tongue :p :p](data:image/gif;base64,R0lGODlhAQABAIAAAAAAAP///yH5BAEAAAAALAAAAAABAAEAAAIBRAA7)
Thanks for any inputs.
I have a question about HCl.
Here's the context: in the DBC (Dibutyl Carbitol) patent, they say that the gold bearing solution should be between 0.5-1.75N.
If I remember correctly, one Normal is one Mol/L. ?
If so, how do I know what's the HCl concentration of my solution ?
I dissolved 7.9 grams of gold in 30mL of HCl (30%) and 10mL of nitric acid.
Then I evaporated to remove any nitric remaining.
The only solution I see is to evaporate the solution to a syrupy constancy , add water, then repeat to get rid of the HCl and the nitric acid. Finally, I would add a calculated amount of HCl to the gold chloride solution to reach 1.0N
BTW, I do not own any pH meters so forget about calculating the H+ ions concentration
Thanks for any inputs.