Why are magnesium chloride and calcium chloride more soluble than sodium chloride?

I read that $$\ce{MgCl2}$$ and $$\ce{CaCl2}$$ are more soluble than $$\ce{NaCl}$$ in water. Solubility of $$\ce{MgCl2}$$ is $$\pu{543 g/L}$$ and that of $$\ce{NaCl}$$ is $$\pu{360 g/L}$$ (both at $$20^{\circ} \pu{C}$$).

I think that $$\ce{NaCl}$$ should be more soluble due to its higher ionic nature. $$\ce{Mg^{2+}}$$ and $$\ce{Ca^{2+}}$$ are more polarizing and have more covalent nature and thus should be less soluble.

I want to know the reason for why the opposite is happening.

• How about a few numbers? – Karl May 12 '18 at 8:18
• Who said greater ionic character means greater solubility? – Ivan Neretin May 12 '18 at 10:53
• there should be balance – amish dua May 12 '18 at 12:57
• @Chemist, It is not advised to add questions apart from what was originally intended by the OP. Hence the reject. Your addition of solubility data was carried forward, duly credited, but again lacked the markup. Please make complete edits and try not to add to old questions (you can ask new ones!) – William R. Ebenezer Feb 3 at 15:29
• From my experience by asking new questions it will be immediately marked duplicate without second thought by community members , so I decided to edit this question to make it answerable. – Chemist Feb 4 at 12:27