A) \[Ca{{(OH)}_{2}}\]
B) \[Ba{{(OH)}_{2}}\]
C) \[Be{{(OH)}_{2}}\]
D) \[Mg{{(OH)}_{2}}\]
Correct Answer: C
Solution :
In hydroxides of alkaline earth metals, it is observed that magnitude of hydration energy remains unaltered whereas the value of lattice energy decrease down the group due to increase in size. The overall effect of two factors is \[(\Delta {{H}_{latice}}-\Delta {{H}_{hydration}}=\Delta {{H}_{solution}});\Delta {{H}_{solution}}\] becomes more negative from Be to Ba. Thus solubility increase from top to bottom. \[\underset{\text{almost}\,\text{insoluble}}{\mathop{\text{Be(OH}{{\text{)}}_{\text{2}}}}}\,<Mg{{(OH)}_{2}}<Ca{{(OH)}_{2}}<\underset{\text{Max}\text{.}\,\text{soluble}}{\mathop{\text{Sr(OH}{{\text{)}}_{\text{2}}}}}\,\] \[<Ba{{(OH)}_{2}}\]
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