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.