Pb(NO3)2 (aq) + BaCl2 (aq)= PbCl2 (s) + Ba(NO3)2 (aq) Write the balanced net ionic equation for the reaction.

Answer 1

1st: Determine if the reaction provided is already balanced, if not then properly balance it before continuing. We can see here that the reaction is already balanced.

2nd: Write out the ionic equation by breaking up the compounds into separate ions with proper coefficients and charges.

Pb²⁺(aq) + 2NO₃^-(aq) + Ba²⁺(aq) + 2Cl^-(aq) --> PbCl₂(s) + Ba²⁺(aq) + 2NO₃^-(aq)

Now you can cancel out the same ions that appear on both sides of the equation:

2NO₃^- (aq) , Ba²⁺(aq) will be canceled out therefore you are left with....

Pb²⁺(aq) + 2Cl^-(aq) --> PbCl₂(aq)

Which is our net ionic equation (the equation showing us what is actually reacting in the chemical reaction).

Answer 2

Since there are aqueous solutions of Lead (II) Nitrate and barium chloride combined, the state we need to put in the chemical equation is (aq) for each. Solid lead (II) chloride is formed, meaning it is called a precipitate.

First, write the chemical reaction for this situation:

Pb(NO₃)₂(aq) + BaCl₂(aq)  -------> PbCl₂ (s) + Ba(NO₃)₂ (aq)

This equation is balanced as there are the same quantity of atoms in both sides of equation. Therefore, we can write the ionic equation.

Now to write the ionic equation:

In these aqueous species, they typically form ions in solution except when forming a precipitate.

Cl^- is soluble except with certain metals like silver, lead, and mercury.

NO₃^- is always a soluble ion

Equation: Pb²⁺(aq) + 2(NO₃)^-(aq) + Ba²⁺(aq) + 2Cl^-(aq)  -------> PbCl₂ (s) + Ba²⁺(aq) + 2(NO₃)^-(aq)

Net ionic equation means that same ions located in both left and right of chemical equation get cancelled out. The common ions are the Ba²⁺(aq) and 2(NO₃)^-(aq). So cancel like terms and get the net ionic equation:

Pb²⁺(aq) + 2Cl^-(aq)  -------> PbCl₂ (s)