The Pb 2 ion buffer used inside the electrode for the colored curve in Figure 14 27 was prepared by mixing 1 0 mL of 0 10 M Pb(NO 3 ) 2 with 100 0 mL of 0 050 M Na 2 EDTA At the measured pH of 4 34, 4 1 46 10 8 (Equation 11 4) Show that Pb 2 1 4 10 12 M Figure 14 27 Equation 11 4 150 100 Convention...

There is a large excess of EDTA in the buffer We expect essentially ...

The Pb 2+ ion buffer used inside the electrode for the colored curve in Figure 14-27 was

Question:

The Pb²⁺ ion buffer used inside the electrode for the colored curve in Figure 14-27 was prepared by mixing 1.0 mL of 0.10 M Pb(NO₃)₂ with 100.0 mL of 0.050 M Na₂EDTA. At the measured pH of 4.34,α γ₄- = 1.46 × 10^-8(Equation 11-4). Show that [Pb²⁺] = 1.4 × 10^-12 M.

Figure 14-27

150 100 Conventional 50 filling solution -50 10-12 M Pb2 filling solution -100 -150 -12 -10 -8 -6 -4 -2 log[Pb?