Which one of the following alkaline earth met | vedclass

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(D) The solubility of alkaline earth metal sulphates depends on the balance between lattice enthalpy and hydration enthalpy.For a compound to be highl

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$BeSO_4$

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(D) The solubility of alkaline earth metal sulphates depends on the balance between lattice enthalpy and hydration enthalpy.For a compound to be highly soluble,its hydration enthalpy must be greater than its lattice enthalpy.As we move down the group,the size of the metal cation increases,which causes the hydration enthalpy to decrease significantly more than the lattice enthalpy.$Be^{2+}$ is the smallest cation among the alkaline earth metals,resulting in a very high hydration enthalpy that outweighs its lattice enthalpy.Therefore,$BeSO_4$ is highly soluble in water,while the solubility decreases down the group from $BeSO_4$ to $BaSO_4$.

Metal	Uses
$1. \text{Be}$	$c. \text{To prepare windows of X-rays}$
$2. \text{Ca}$	$d. \text{To remove air from vacuumized tubes}$
$3. \text{Mg}$	$a. \text{To prepare Grignard reagent}$

Which one of the following alkaline earth metal sulphates has its hydration enthalpy greater than its lattice enthalpy?

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Metal Uses

$1. \text{Be}$ $c. \text{To prepare windows of X-rays}$

$2. \text{Ca}$ $d. \text{To remove air from vacuumized tubes}$

$3. \text{Mg}$ $a. \text{To prepare Grignard reagent}$

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