CHRIS25 - 30-5-2012 at 06:14
Just made a very clean batch of what I believe to be Ferric nitrate solution without impurities and Fe2 ions present. It is a clear deep red colour.
My goal is now to get as close as I can to this: Water @ about 50%. Fe(NO3)3 @ about 40% and most important HNO3 @ or below the 10%.
At the moment I have a solution that is PH 1. I began with 96g of 30% nitric acid (reduced from 126g as per stoichemetry equation, due to the 1.4
density of HNO3) and 6.7 grams very thick Rusted barbed wire. I am left with 65 mils of solution after a heated reaction. The weight of the solution
is 69 grams, I assume that the 4 grams is the actual FE content (69-65), making 17.5 grams of acid and 38.5 grams of water.
Am I shipwrecked here with my reasoning and/or maths?
[Edited on 30-5-2012 by CHRIS25]
Sorry, forgot to just add that I realise that I can alter the ratios of acid to water by simply raising the ph until it hits the 9 or 10 mark, but
that would then dilute the ferric nitrate itself. So I am anticipating that my methodology in my thinking is off target.....hence the original
question
[Edited on 30-5-2012 by CHRIS25]