Answer
The balanced equation for the dissociation of each of these strong electrolytes is:
a. $$KCl(s) \xrightarrow{H_2O} K^+(aq) + Cl^-(aq) $$
b. $$CaCl_2(s) \xrightarrow{H_2O} Ca^{2+}(aq) + 2Cl^-(aq) $$
c. $$K_3PO_4(s) \xrightarrow{H_2O} 3K^+(aq) + P{O_4}^{3-}(aq) $$
d. $$Fe(NO_3)_3(s) \xrightarrow{H_2O} Fe^{3+}(aq) + 3N{O_3}^-(aq) $$
Work Step by Step
1. Identify the ions in each solute.
a. $K^+$ and $Cl^-$
b. $Ca^{2+}$ and 2 $Cl^-$
c. 3 $K^+$ and $P{O_4}^{3-}$
d. $Fe^{3+}$ and 3 $N{O_3}^-$
2. The dissociation of a strong electrolyte follows this pattern:
$$Solute(s) \xrightarrow{H_2O} Ion_1(aq) + Ion_2(aq) ...$$
Use this pattern to write each equation:
a. $$KCl(s) \xrightarrow{H_2O} K^+(aq) + Cl^-(aq) $$
b. $$CaCl_2(s) \xrightarrow{H_2O} Ca^{2+}(aq) + 2Cl^-(aq) $$
c. $$K_3PO_4(s) \xrightarrow{H_2O} 3K^+(aq) + P{O_4}^{3-}(aq) $$
d. $$Fe(NO_3)_3(s) \xrightarrow{H_2O} Fe^{3+}(aq) + 3N{O_3}^-(aq) $$
