(a, b, c)

The hydration enthalpies of alkaline earth metal ions decrease with increase in ionic size down the group.

Be2+ > Mg2+ > Ca2+ > Sr2+ > Ba2+

The hydration enthalpies of alkaline earth metal ions are larger than those of alkali metal ions, because of their much larger charge to radius ratio, exert a much stronger electrostatic attraction on the oxygen of water molecule surrounding them. Thus, compounds of alkaline earth metals are more extensively hydrated than those of alkali metals, e.g., MgCl2 and CaCl2 exist as MgCl2 .6H2O and CaCl2. 6H2O while NaCl and KCl do not form such hydrates. So all statements are correct