12. A solution contains 1.00 nM Cu at 25 °C. Will adding one of the following sp
ID: 562956 • Letter: 1
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12. A solution contains 1.00 nM Cu at 25 °C. Will adding one of the following species and concentrations react with the 1.00 nM Cu? Basically, will a reaction be spontaneous or not? Make sure you calculate the potential at the non-standard conditions for both Cu+ and the possible interferent and use an energy diagram to help you illustrate your answer. Assume that the half reaction with Cu involves Cu(s) (ignore the half reaction involving Cu' and Cu). Also, assume that for soluble form of the other redox couple in a solution containing a known concentration of a given form of a redox couple the concentration is 1/10,000th of the concentration of the known concentration of the given form of the redox couple. So, if you're given a concentration of Co2+ of 1.00 M, the concentration of Co3+ (which we are then assuming is a contaminant in the starting material) is (1.00 x 10 M)y10000 1.00 x 1010 M Co. And, yes, because you don't know if there is any copper metal, Cu, please assume that there is a Cu metal in the system and therefore the activity of Cu metal is unity If you determine that there is a situation where Cu can be reduced by one of the forms of the other redox couple, consider the total quantity of the two species that are reacting. You don't have to do further alculations to determine new potentials after the species react, but at least note what might happen to Cu' given its low concentration. Here are the possible interferences: (a) 0.0100 M Ru(NH3) (b) 0.0100 M Ru(NHs)% (c) 0.0100 M Fe*Explanation / Answer
Cu+2/cu=o.34v(cathode)
Fe+3/Fe=-0.o4v(anode)
E*cell: E*cathode-E*anode=o.38v
net cell reaction; 3Cu+2/3CU//2Fe/2Fe+3
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