Though in case of group elements solubility of hydroxide increases down the group due to a much decrease in lattice enthalpy than hydration enthalpy. as we move down the group , the solubility of sulphates of group elements shows a different trend.
Be and Mg sulphates are water soluble.
Ca sulphate sparingly soluble.
Sr and Basulphates insoluble.
Why ? explain
Dear User,
The solubility of sulphates in water decreases on going down the group. This can be attributed to decrease in hydration enthalpy. The magnitude of lattice energy remains constant as the sulphate is so big that the small increase in the size of the cation from Be to Ba does not make any difference. Hence, the solubility of the sulphates decreases as we move down the group. The high solubility of BeSO4 and MgSO4 is due to the high hydration energies due to small size of the cation.
Regards
The solubility of sulphates in water decreases on going down the group. This can be attributed to decrease in hydration enthalpy. The magnitude of lattice energy remains constant as the sulphate is so big that the small increase in the size of the cation from Be to Ba does not make any difference. Hence, the solubility of the sulphates decreases as we move down the group. The high solubility of BeSO4 and MgSO4 is due to the high hydration energies due to small size of the cation.
Regards