Chapter 12: Q1 TY (page 269)
At what pH does ?
Short Answer
At pH 10.35 the value of
Chapter 12: Q1 TY (page 269)
At what pH does ?
At pH 10.35 the value of
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Calculate pCu2+ at each of the following points in the titration of 50.00 mL of 0.001 00 M Cu2+ with 0.00100 M EDTA at pH 11.00 in a solution with [NH3] fixed at 1.00 M:
(a) 0 mL(b) 1.00 mL (c) 45.00 mL (d) 50.00 mL (e) 55.00 mL
Spreadsheet equation for formation of the complexes ML and ML2.Consider the titration of metal M (initial concentration = CM, initial volume = VM) with ligand L (concentration = CL, volume added = VL), which can form 1:1 and 2 : 1 complexes:
Let αM be the fraction of metal in the form M, αML be the fraction in the form ML, and be the fraction in the form ML2. Following the derivation in Section 12-5, you could show that these fractions are given by
The concentrations of ML and ML2 are
because is the total concentration of all metal in the solution. The mass balance for ligand is
By substituting expressions for [ML] and [ML2] into the mass balance, show that the master equation for a titration of metal by ligand is
Consider the titration of 25.0 mL of 0.020 0 M MnSO4 with 0.010 0 M EDTA in a solution buffered to pH 8.00. Calculate pMn2+ at the following volumes of added EDTA and sketch the titration curve:
(a) 0 mL (b) 20.0 mL (c) 40.0 mL (d) 49.0 mL (e) 49.9 mL (f) 50.0 mL (g) 50.1 mL(h) 55.0 mL (i) 60.0 mL
Calculate the concentration of H2Y2- at the equivalence point in Exercise 12-C
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