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We’re being asked to determine the solubility of M(OH)2 in a solution buffered at pH = 7.0, 10.0, and 14.0.
Since the M(OH)2 is an ionic compound, it forms ions when dissociating in water.
The dissociation of M(OH)2 in water is as follows:
The hydroxide ion, OH–, has a charge of –1. M then has a charge of +2:
M(OH)2(s) ⇌ M2+(aq) + 2 OH–(aq)
Since the solution is buffered, we can calculate an initial OH– concentration from the given pH.
Consider an amphoteric hydroxide, M(OH)2(s), where M is a generic metal. Estimate the solubility of M(OH)2 in a solution buffered at pH = 7.0, 10.0, 14.0? The Ksp is 4 x 10-16.
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