Why Solubilities of Sulphates of Group 2a Elements Decreases down the Group?

Answer

The sulphate ion is large which makes the effect to change the cation size by the lattice energy a small one. And so, the hydration enthalpy decreases down the group as the ion gets bigger.
Q&A Related to "Why Solubilities of Sulphates of Group 2a Elements..."
because down the group the cation becomes gets larger so the hydration energy decreases. so the solubility decreases.
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The proof lies in a consideration of the Ksp values for all these sulfates of the group II metals: BeSO4, soluble. MgSO4, soluble. CaSO4 , 1.9x10E-4. SrSO4, 3.8x10E-7. BaSO4, 1.0x10E
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First you need to understand bonding in metals. Each metal atom loses its outer electrons, which are then free to move between the lattice of positively charged metal ions in the
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as we move down the group solubility of sulphates decrease,for alkaline earth metals because down the group, size of cation increase, thus hydration energy decreases,and thus solubility
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The atomic size of element increases as you look down the first group because the atomic radius of the element increases as we go down the column. The size decreases ...
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