Question

Identify the precipitates (if any) that form when the following solution is mixed. If a precipitate forms, write a i) molecular equation (ME) ii) total ionic equation (TIE) iii) net ionic equation (NIE)a) CaCl2 and Ag2SO4METIENIE

Answer 1

ANSWER

$\begin{gathered} \text{ Molecular equation; CaCl}_{2(aq)}\text{ + Ag}_2SO_{4(aq)}\text{ }\rightarrow\text{ 2AgCl}_{(s)}\text{ + CaSO}_{4(aq)} \\ \text{ Total ionic equation; Ca}^{2+}\text{ + 2Cl}^-\text{ + 2Ag}^+\text{ + SO}_4^{2-}\text{ }\rightarrow\text{ 2AgCl}_{(s)}+\text{ Ca}^{2+}\text{ + SO}_4^{2-} \\ \text{ Net ionic equation; 2Cl}^-\text{ + 2Ag}^+\text{ }\rightarrow\text{ 2AgCl}_{(s)} \end{gathered}$

EXPLANATION

Given that;

The two compounds given are CaCl2 and Ag2SO4

Firstly, write a balance chemical equation between the two compounds

To write a balanced equation, apply the law of conservation of mass

The law of conservation mass states that matter can neither be created nor destroyed but can be transformed from one form to another.

Hence, we have

$\text{ CaCl}_{2(aq)}\text{ + Ag}_2SO_{4(aq)}\text{ }\rightarrow\text{ 2AgCl}_{(s)}\text{ + CaSO}_{4(aq)}$

In an aqueous solution, precipitation is the process of transforming a dissolved substance into an insoluble substance.

Therefore, the precipitate in the above molecular equation is AgCl

Part B

Follow the steps below to write the total ionic equation

Firstly, write the compounds in aqueous inform of ions

$\text{ Ca}^{2+}\text{ + 2Cl}^-\text{ + 2Ag}^+\text{ + SO}_4^{2-}\text{ }\rightarrow\text{ 2AgCl}_{(s)}\text{ + Ca}^{2+}\text{ + SO}_4^{2-}$

Part C

Eliminate the spectator ions to write the net ionic equation.

Recall, spectators ions are ions that appear on both reactant and product sides

$\begin{gathered} \cancel{Ca^{2+}}+\text{ 2Cl}^-\text{ + 2Ag}^++\cancel{SO^{2-}}_4\text{ }\rightarrow\text{ 2AgCl }+\cancel{Ca^{2+}}\text{ }+\cancel{SO^{2-}}_4 \\ \\ \text{ 2Cl}^-\text{ + 2Ag}^+\text{ }\rightarrow\text{ 2AgCl}_{(s)} \end{gathered}$