Why is the product of $\ce{Al(OH)3 + NaOH -> Na}$ and not $\ce{NaAlO3H2 + H2O}$? Is this an acid-base reaction?



All reaction sources: Chemiday

As I said in the comment section that aluminium hydroxide is amphoteric i.e. It dissolves in acid, forming $\ce{^3+}$ (hexaaquaaluminium) or its hydrolysis products and dissolves in strong alkaline solutions, forming $\ce{−}$ (tetrahydroxidoaluminate). So, when it is dissolved in base, it forms a sodium aluminohydroxo complex salt. Why? Because as
Pritt mentioned, aluminium has vacant orbital for which free electron can reside there forming a complex salt.

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$$\ce{Al(OH)3 + NaOH(conc.) → Na}$$

$$\ce{Al(OH)3 + 3NaOH → Na3}$$

No worries. There is also an acid-base reaction where the two combines to form a salt and water but this occurs at very high temperature and you won"t find this type of reaction occurring in laboratory. This reaction can only be find in industries.

$$\ce{Al(OH)3 + NaOH -><1000 C> NaAlO2 + 2H2O}$$

If only aluminium was used, there would be evolution of hydrogen gas from a very similar exothermic reaction. Note for simplicity, the species is written $\ce{NaAlO2}$ but it actually contains $\ce{−}$ ion or perhaps the $\ce{−}$ all due to presence of vacant orbital(see sodium aluminate).

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answered Jun 19, 2017 at 5:27

Nilay GhoshNilay Ghosh
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