Question

Consider an amphoteric hydroxide, M ( OH ) 2 ( s ) , where M is a generic metal. M ( OH ) 2 ( s ) − ⇀ ↽ − M 2 + ( aq ) + 2 OH − ( aq ) K s p = 3 × 10 − 16 M ( OH ) 2 ( s ) + 2 OH − ( aq ) − ⇀ ↽ − [ M ( OH ) 4 ] 2 − ( aq ) K f = 0.04 Estimate the solubility of M ( OH ) 2 in a solution buffered at pH = 7.0, 10.0, and 14.0.

Answer 1

The solubility of M(OH)2 in a solution buffered at pH 7.0, 10.0, and 14.0 can be estimated by considering the equilibrium reactions and using the Henderson-Hasselbalch equation. By substituting the concentration of hydroxide ions ([OH-]) into the equilibrium expressions, you can calculate the concentration of metal ions ([M2+]) at each pH.

Step-by-step explanation:

The solubility of M(OH)2 in a solution buffered at pH 7.0, 10.0, and 14.0 can be estimated by considering the equilibrium reactions and using the Henderson-Hasselbalch equation.

At pH 7.0, the concentration of hydroxide ions ([OH-]) is 1 x 10-7 M, and the concentration of metal ions ([M2+]) can be calculated using the Ksp value. At pH 10.0, [OH-] is 1 x 10-4 M, and at pH 14.0, [OH-] is 1 M.

By substituting the concentration of hydroxide ions ([OH-]) into the equilibrium expressions, you can calculate the concentration of metal ions ([M2+]) at each pH.