Consider the use of a solution that is 0.0322 M EDTA in the titration of a 50.00
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Consider the use of a solution that is 0.0322 M EDTA in the titration of a 50.00 mL of a solution that is 0.0129 M in Cu2+. The solution is held at a pH of 10.00 and is buffered in 0.050 M ammonia.
Cu2+ (T = 20 oC, n = 0.1 M)
Log K1=18.80
(a) What is the value of K"f for this solution?
(b) What is the concentration of [CuY2-] at the equivalence point?
(c) What is the free [Cu2+] at the equivalence point (expressed as pCu)?
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