Why BaO (s) + H2O(l) ---> Ba 2+(aq) + 2 OH - (aq) if Oxygen loves owning all the electrons, why would it bind to hydrogen which competes with Oxygen for electron ownership more so than Barium? Does the reaction happen because water disassociates into a proton and hydroxide and the proton can do cleaving of the barium oxide bond because a proton is even more electronegative than an oxygen or anything neutral?
Alan F Rawle
The example you mention is not a solubility issue - it’s a chemical reaction. You would have similar comments for Na2O, K2O and CaO. The resulting products (hydroxides) have varying solubilities in water.
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