The solubility in water of sulphates down the | vedclass

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(A) The hydration energy decreases from $Be^{2+}$ to $Ba^{2+}$. Since the hydration energy of the smaller $Be^{2+}$ ion is significantly higher than t

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High heat of solvation for smaller ions like $Be^{2+}$

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(A) The hydration energy decreases from $Be^{2+}$ to $Ba^{2+}$. Since the hydration energy of the smaller $Be^{2+}$ ion is significantly higher than the lattice energy of $BeSO_4$,it is highly soluble. As the size of the cation increases down the group,the hydration energy decreases more rapidly than the lattice energy,leading to a decrease in solubility.

The solubility in water of sulphates down the $Group \ 2$ ($Be$ group) is $Be > Mg > Ca > Sr > Ba$. This is due to

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