# Question #0853f

Jul 20, 2015

You can use it like this:

#### Explanation:

Equation:

$2 A {l}_{\left(s\right)} + 6 H C {l}_{\left(a q\right)} \rightarrow 2 A l C {l}_{3 \left(a q\right)} + 3 {H}_{2 \left(g\right)}$

Aluminium loses it's outer electrons:

$2 A {l}_{\left(s\right)} \rightarrow 2 A {l}_{\left(a q\right)}^{3 +} + 6 e$

These are taken in by the hydrogen ions:

$6 {H}_{\left(a q\right)}^{+} + 6 e \rightarrow 3 {H}_{2 \left(g\right)}$

In this reaction the chloride ions are spectators - they take no part in the reaction.

Jul 20, 2015

If you want to be able to balance the equation using oxidation states, here's how...

#### Explanation:

First you need to work out the oxidation states of each element, notice the ones that have changed, work out how many electrons they have lost/gained. From there find the key number to balance the equation and from then on this trial and error.