1. Lewis-Acid Base Chemistry and Complexation Equilibria
Section 18.3

4. Aqueous Metal Ions

6. Also: CO2 is an acid

7. Complexation Reactions and Equilibria

9. Complex Ion Equilibria
In the presence of excess OH-, the Zn2+(aq) ion forms a hydroxide complex
ion. Calculate the concentration of free Zn2+ ion when mol Zn(NO3)2(s)
is added to 1.00 L of solution in which [OH-] is held constant
(buffered at pH 12.00). Kf(Zn(OH)42- = 4.6 x 1017.

10. Complex Ion Equilibria
In the presence of excess OH-, the Zn2+(aq) ion forms a hydroxide complex
ion. Calculate the concentration of free Zn2+ ion when mol Zn(NO3)2(s)
is added to 1.00 L of solution in which [OH-] is held constant
(buffered at pH 12.00). Kf(Zn(OH)42- = 4.6 x 1017.

11. Solubility of Hydroxide Salts and pH
Calculate the solubility of Fe(OH)2 in solutions below, Ksp = 7.9 x 10-15
pH = 6
pH = 7
pH = 8
pH = 9
pH = 10