A solution containing 50 0 mL of 0 100 M EDTA buffered to pH 10 00 was titrated with 50 0 mL of 0 020 0 M Hg(ClO 4 ) 2 in the cell shown in Exercise 14 B S C E 7 titration solution Hg(l) From the cell voltage E 0 027 V, find the formation constant of Hg(EDTA) 2

Question: A solution containing 50.0 mL of 0.100 M EDTA buffered to pH 10.00 was titrated with 50.0 mL of 0.020 0 M Hg(ClO 4 )

A solution containing 50.0 mL of 0.100 M EDTA buffered to pH 10.00 was titrated with 50.0 mL of 0.020 0 M Hg(ClO₄)₂ in the cell shown in Exercise 14-B:

S.C.E. 7 titration solution | Hg(l)

From the cell voltage E = - 0.027 V, find the formation constant of Hg(EDTA)^2-.

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