Final answer:
Writing net ionic equations involves balancing the molecular equation, then writing the ionic equation, and finally eliminating spectator ions to reveal the net reaction. The net ionic equation for Ag+(aq) + Br-(aq) → AgBr(s) and Ba^2+(aq) + SO4^2-(aq) → BaSO4(s) reflect the actual chemical changes occurring during the reactions.
Step-by-step explanation:
Writing a net ionic equation involves a few steps. First, make sure the molecular equation is balanced, with all formulas correct. Then, write the ionic equation, showing all substances that are aqueous as ions. Next, carry through any coefficients from the balanced molecular equation. Finally, eliminate spectator ions to find the net ionic equation. Here's how you apply these steps to the examples provided:
- For the reaction between K+ (aq), Br- (aq), Ag+ (aq), and C2H3O2- (aq) leading to K+ (aq), C2H3O2- (aq), and AgBr (s), the net ionic equation would be:
Ag+(aq) + Br-(aq) → AgBr(s)
- And for the reaction involving Mg^2+ (aq), SO4^2- (aq), Ba^2+ (aq), and NO3- (aq) leading to Mg^2+ (aq), NO3- (aq), and BaSO4 (s), the net ionic equation would be:
Ba^2+(aq) + SO4^2-(aq) → BaSO4(s)
These show the actual chemistry taking place, emphasizing the precipitate formation and removing ions that do not participate in the reaction (spectator ions).