Lewis-Acid Base Chemistry and Complexation Equilibria

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Presentation transcript:

Lewis-Acid Base Chemistry and Complexation Equilibria Section 18.3

Aqueous Metal Ions

Also: CO2 is an acid

Complexation Reactions and Equilibria

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 0.010 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.

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 0.010 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.

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