Assuming a bicarbonate ion concentration [HCO3-]of 1.00 × 10−3 M and avalue of 3.5 × 10−11 for the solubility product of FeCO3, what would youexpect to be the stable iron species at pH 9.5 and pE −8.0, as shown inFigure 3.4? 20Fe3+15.O210+Fe(OH)3pE0-Fe2+-5+H2-10+Fe(OH)2-150 1 2 3 45 67 8 9 10 11 12 13 14pHFIGURE 3.4 Simplified pE-pH diagram for iron in water. The maximum soluble iron concentration is1.00 x 10-5 M.

The equilibrium composition of a redox system involving H+ depends on both the pH and the pE. The…

Assuming a bicarbonate ion concentration [HCO3-]of 1.00 × 10−3 M and a value of 3.5 × 10−11 for the solubility product of FeCO3, what would you expect to be the stable iron species at pH 9.5 and pE −8.0, as shown in Figure 3.4?

Assuming a bicarbonate ion concentration [HCO3-]of 1.00 × 10−3 M and a value of 3.5 × 10−11 for the solubility product of FeCO3, what would you expect to be the stable iron species at pH 9.5 and pE −8.0, as shown in Figure 3.4?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 75QAP: A diprotic acid, H2B(MM=126g/moL), is determined to be a hydrate, H2B xH2O. A 10.00-g sample of this...

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Question

20
Fe3+
15.
O2
10+
Fe(OH)3
pE
0-
Fe2+
-5+
H2
-10+
Fe(OH)2
-15
0 1 2 3 4
5 6
7 8 9 10 11 12 13 14
pH
FIGURE 3.4 Simplified pE-pH diagram for iron in water. The maximum soluble iron concentration is
1.00 x 10-5 M.

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