When an aqueous solution of Barium chloride (BaCl2) reacts with an aqueous solution of silver nitrate (AgNO3), a white precipitate of silver chloride and an aqueous solution of barium nitrate is formed. Write the molecular, complete ionic and net ionic equations for this reaction.

1. Molecular equation

BaCl2(aq) + 2AgNO3(aq) –> 2AgCl(s) + Ba(NO3)2 (aq)

2. Complete Ionic equation

Ba²⁺(aq) + 2Cl¯(aq) + 2Ag⁺(aq) + 2NO3¯ (aq) —> 2AgCl(s) + Ba²⁺(aq) + 2NO3¯(aq)

3. Net ionic equation

Cl¯(aq) + Ag⁺(aq) —> AgCl(s)

Explanation:

1. Molecular equation:

BaCl2(aq) + AgNO3(aq) –> AgCl(s) + Ba(NO3)2 (aq)

The above equation can be balance as follow:

There are 2 atoms of Cl on the left side and 1 atom on the right side. It can be balance by putting 2 in front of AgCl as shown below:

BaCl2(aq) + AgNO3(aq) –> 2AgCl(s) + Ba(NO3)2 (aq)

There are 2 atoms of Ag on the right side and 1 atom on the left side. It can be balance by putting 2 in front of AgNO3 as shown below:

BaCl2(aq) + 2AgNO3(aq) –> 2AgCl(s) + Ba(NO3)2 (aq)

Now, the equation is balanced

2. Complete ionic equation

In solution, BaCl2 and AgNO3 will dissociate as follow:

BaCl2(aq) —> Ba²⁺(aq) + 2Cl¯(aq)

AgNO3(aq) —> Ag⁺(aq) + NO3¯ (aq)

BaCl2(aq) + AgNO3(aq) –>

Ba²⁺(aq) + 2Cl¯(aq) + 2Ag⁺(aq) + 2NO3¯ (aq) —> 2AgCl(s) + Ba²⁺(aq) + 2NO3¯

3. Net ionic equation

Ba²⁺(aq) + 2Cl¯(aq) + 2Ag⁺(aq) + 2NO3¯ (aq) —> 2AgCl(s) + Ba²⁺(aq) + 2NO3¯(aq)

Cancel out the spectator ions i.e ions that appears on both side of the equation in order to get the net ionic equation. This is illustrated below:

2Cl¯(aq) + 2Ag⁺(aq) —> 2AgCl(s)

Cl¯(aq) + Ag⁺(aq) —> AgCl(s)

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