Calculate pCu2+ at each of the following points in the titration of 50.00 mL of 0.00100 M Cu2+with 0.00100 M EDTA at pH 11.00 in a solution whose NH3 concentrationis somehow fixed at 0.100 M.∴Log kf Cu2+ = 18.78∴αY4- for EDTA at pH of 11 = 0.81(a) 0 mL(b) 45.00 mL(d) 50.00 mL(e) 55.00 mLI understand this is more than one question but I have to solve for pCu2+ when volume is before, at, and after the equivalence point. I am not sure if I am usingthe right equations so any help would be greatly appreciated.
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