Answer
Acid and base used to form this ion, respectively: $HBr$ and $LiOH$,
Complete ionic equation:
$Li^+(aq) + OH^-(aq) + H^+(aq) + Br^-(aq) -- \gt Li^+(aq) + Br^-(aq) + H_2O(l)$
Net ionic equation:
$H^+(aq) + OH^-(aq) -- \gt H_2O(l) $
Work Step by Step
1. Identify the ions of the salt: $(LiBr)$:
$Li^+$ and $Br^-$:
To the cation, add a hydroxide ion: $LiOH$; this is the base.
To the anion, add a hydrogen ion: $HBr$; this is the acid.
2. Now, write the balanced overall equation between then, which is:
$Acid + Base -- \gt Salt + Water$
We already have the salt, so:
$HBr(aq) + LiOH(aq) -- \gt LiBr(aq) + H_2O(l)$
3. Write the complete ionic equation.
- For the completely dissociated/ionized compounds, separate them by their ions:
$Li^+(aq) + OH^-(aq) + H^+(aq) + Br^-(aq) -- \gt Li^+(aq) + Br^-(aq) + H_2O(l)$
* LiOH is a strong base, and $LiBr$ is soluble according to the table 3.1, because it is a compound with the $Li^+$ ion.
* HBr is a strong acid, so it is completely dissociated.
4. Remove the repeated ions:
$H^+(aq) + OH^-(aq) -- \gt H_2O(l) $
This is the net ionic equation.
