Final answer:
The question relates to the Chemistry subject, focusing on writing balanced molecular, complete ionic, and net ionic equations for reactions in an aqueous solution. The complete ionic equation represents all aqueous ions separately, while the net ionic equation includes only the ions that partake in the reaction, excluding spectator ions.
Step-by-step explanation:
The subject of this question is Chemistry, specifically the topic of writing balanced molecular, complete ionic, and net ionic equations for reactions occurring in an aqueous solution. When we write balanced molecular equations, we are representing the chemicals in their formula units as they appear before they are dissolved in water. For instance, NaOH(aq) would simply be written as NaOH in a balanced molecular equation.
However, in a complete ionic equation, we show all of the ions in the solution. For sodium hydroxide, which is a strong base and disassociates completely when aqueous, we would write it as Na+ (aq) + OH¯ (aq) as shown in example 10.1.3. Likewise, Na2CO3 would be represented as 2Na+ (aq) + CO3^2- (aq).
The net ionic equation focuses on the ions that participate in the reaction without including the spectator ions. For a neutralization reaction such as the one between hydrochloric acid (HCl) and NaOH, the net ionic equation would simply be H+ (aq) + OH¯ (aq) → H2O(l), as all other ions (Na+ and Cl¯) are spectator ions and do not participate directly in the reaction.