Which hydroxide of the II^{nd} A group metals | vedclass

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(B) The hydroxide with the lowest solubility product $(K_{sp})$ is $Be(OH)_2$,which has a $K_{sp}$ value in the $10^{-22}$ range.This is because the $

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$Be(OH)_2$

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(B) The hydroxide with the lowest solubility product $(K_{sp})$ is $Be(OH)_2$,which has a $K_{sp}$ value in the $10^{-22}$ range.This is because the $Be^{2+}$ ion is significantly smaller than the other alkaline earth metal ions,leading to a much stronger lattice energy and a tighter bond with $OH^{-}$ ions,which results in very low solubility.As we move down group $2A$,the size of the metal ions increases,which weakens the lattice energy and the bond between the metal and $OH^{-}$ ions,causing the $K_{sp}$ values to increase.

Which hydroxide of the $II^{nd}$ $A$ group metals has the lowest solubility product $(K_{sp})$ value at $25\,^{\circ}C$?

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Choose the correct answer from options given below.

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