# How does aluminum give aluminate ion in basic solution?

Apr 25, 2017

$\text{Aluminate}$ can be produced by oxidation of $\text{aluminum metal.......}$

#### Explanation:

$A l \left(s\right) + 4 H {O}^{-} \rightarrow A l {\left(O H\right)}_{4}^{-} + 3 {e}^{-}$ $\left(i\right)$

And if aluminum is oxidized, the only species that can be reduced is water to give dihydrogen gas:

${H}_{2} O + {e}^{-} \rightarrow \frac{1}{2} {H}_{2} \left(g\right) + H {O}^{-}$ $\left(i i\right)$

And so we add $\left(i\right) + 3 \times \left(i i\right)$ and gets..........

$A l \left(s\right) + 3 {H}_{2} O \left(l\right) + H {O}^{-} \rightarrow A l {\left(O H\right)}_{4}^{-} + \frac{3}{2} {H}_{2} \left(g\right) \uparrow$

Aluminum is an amphoteric metal. Use of acid would result in a similar oxidation.