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Dissolving Brass and Calculating copper content?
As part of a project im going to identify the best method for calculating the copper(II) ion concentration in a solution, and then apply it to a solution of dissolved brass. To dissolve the brass i put it in the minimum quantity of nitric acid needed to fully dissolve it, creatig a solution of copper nitrate and zinc nitrate. I've heard its possible to add zinc to the solution to displace the copper. But it would have to be added to excess, so how would the copper be seperated from the zinc? I thought that acid could be used to get rid of the zinc, and leave the solid copper behind, but that got me wondering why the nitric acid can react with the copper in the first place. Can anyone shine any light on this? Thanks.
Apart from a redox titration what other method could be used to work out the copper content?
The standard approach is to neutralise the solution then add KI (which reacts quantitatively with the Cu2+ ions to produce iodine and CuI) and then titrating the iodine with standard sodium thiosulphate solution. This give consistently accurate results.
Alternatively you could mesure the Cu2+ concentration colorimetrically after producing a suitable transmission v concentration graph using standard solutions of copper(II) nitrate. This, too, gives good results.
After neutralisation adding excess zinc powder will produce solid copper, and the unused zinc can be dissolved out using sulphuric acid which does not react with copper at moderate concentrations. Then filter, wash, dry to constant mass and weigh the copper. It certainly works, but results are less reliable than the other two methods.
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