Answer
The balanced equation for the dissociation of each of these strong electrolytes is:
a. $$LiBr(s) \xrightarrow{H_2O} Li^+(aq) + Br^-(aq) $$
b. $$NaNO_3(s) \xrightarrow{H_2O} Na^{+}(aq) + N{O_3}^-(aq) $$
c. $$CuCl_2(s) \xrightarrow{H_2O} Cu^{2+}(aq) + 2Cl^-(aq) $$
d. $$K_2CO_3(s) \xrightarrow{H_2O} 2 K^{+}(aq) + C{O_3}^{2-}(aq) $$
Work Step by Step
1. Identify the ions in each solute.
a. $Li^+$ and $Br^-$
b. $Na^+$ and $N{O_3}^-$
c. $Cu^{2+}$ and 2 $Cl^{-}$
d. 2 $K^{+}$ and $C{O_3}^{2-}$
2. The dissociation of a strong electrolyte in water follows this pattern:
$$Solute(s) \xrightarrow{H_2O} Ion_1(aq) + Ion_2(aq) ...$$
Use this pattern to write each equation:
a. $$LiBr(s) \xrightarrow{H_2O} Li^+(aq) + Br^-(aq) $$
b. $$NaNO_3(s) \xrightarrow{H_2O} Na^{+}(aq) + N{O_3}^-(aq) $$
c. $$CuCl_2(s) \xrightarrow{H_2O} Cu^{2+}(aq) + 2Cl^-(aq) $$
d. $$K_2CO_3(s) \xrightarrow{H_2O} 2 K^{+}(aq) + C{O_3}^{2-}(aq) $$
