Answer:
This is due to smaller cationic size
of the alkaline earth metals (e.g.,\[M{{g}^{2+}}\]) than the alkali metals
(e.g.,\[N{{a}^{+}}\]) present in their salts. As a result, the positive charge
density on the former is more and can attract greater number of\[{{H}_{2}}O\] molecules
compared with latter. Therefore, crystalline salts of alkaline earth metals
contain more water molecules as water of crystallisation as compared to salts
of alkali metals.
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