I read that as sodium hydroxide. A little bell went off in my head and I looked it up. And yes, it was what I thought. Considered Mg + 2H2O → Mg(OH)2 + H2? Might not be so good with the flammable gas release, though.
That reaction is harder to get working than it looks, because solid magnesium exposed to the atmosphere very quickly forms a layer of magnesium oxide on the surface, the same way aluminum foil does.
What I was actually referring to is the nontrivial amount of heat released when solid NaOH dissolves.
Oh yes. I figured you meant during solvation. I was offering a slower thermal reaction. And yes, magnesium is difficult to work with. But so is the sudden heat output of the NaOH reaction. I guess I was trying to be silly.
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What I was actually referring to is the nontrivial amount of heat released when solid NaOH dissolves.
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