Problem: 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.

FREE Expert Solution
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FREE Expert Solution

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. 

Recall that:


pH + pOH = 14


[OH-] = 10-pOH


83% (142 ratings)
Problem Details

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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