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.

🤓 Based on our data, we think this question is relevant for Professor Plath's class at UCB.

FREE Expert Solution
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


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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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