Complete and balance each of the following molecular...

Complete and balance each of the following molecular equations (in aqueous solution); include phase labels. Then, for each, write the net ionic equation. (a) $\mathrm{NaOH}+\mathrm{HNO}_{3} \longrightarrow$ (b) $\mathrm{HCl}+\mathrm{Ba}(\mathrm{OH})_{2} \longrightarrow$ (c) $\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}+\mathrm{Ca}(\mathrm{OH})_{2} \longrightarrow$ (d) $\mathrm{NH}_{3}+\mathrm{HNO}_{3} \longrightarrow$

Complete and balance each of the following molecular equations (in aqueous solution); include phase labels. Then, for each, write the net ionic equation.
(a) $\mathrm{NaOH}+\mathrm{HNO}_{3} \longrightarrow$
(b) $\mathrm{HCl}+\mathrm{Ba}(\mathrm{OH})_{2} \longrightarrow$
(c) $\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}+\mathrm{Ca}(\mathrm{OH})_{2} \longrightarrow$
(d) $\mathrm{NH}_{3}+\mathrm{HNO}_{3} \longrightarrow$

Key Concepts

Molecular Equations

Molecular equations represent the chemical reaction by showing the reactants and products in their undissociated, complete formula forms along with proper physical state designations (such as (aq) for aqueous, (s) for solid, etc.). They give an overall picture of the reaction before considering ionic dissociation, which is especially useful for reactions in aqueous solutions where many compounds dissociate into ions.

Complete Ionic Equations

Complete ionic equations expand the molecular equation to show all of the strong electrolytes (usually ionic compounds, strong acids, and bases) as they exist in solution, explicitly listing all of the ions present. This form highlights the actual species that can react in solution and lays the groundwork for identifying species that do not change during the reaction.

Net Ionic Equations

Net ionic equations simplify the complete ionic equation by removing the spectator ions—ions that appear on both sides of the equation and do not participate directly in the chemical change. This form focuses only on the species that undergo a chemical transformation, which is particularly useful in acid-base neutralization reactions.

Spectator Ions

Spectator ions are ions present in the solution that do not participate in the chemical reaction. They remain unchanged on both the reactants and products side of the complete ionic equation. Identifying and removing spectator ions simplifies the equation to reflect only the core chemical change taking place.

Balancing Chemical Equations

Balancing chemical equations involves ensuring that the number of atoms of each element, as well as the overall charge, is the same on both the reactants and products sides of the equation. This step is essential for obeying the law of conservation of mass and charge, and it is a prerequisite for writing accurate molecular, complete ionic, and net ionic equations.

Phase Labels

Phase labels (such as (aq) for aqueous, (s) for solid, (l) for liquid, and (g) for gas) are included in chemical equations to specify the physical state of each reactant and product. These labels are important as they often affect how substances interact in a chemical reaction, particularly in aqueous reactions where dissociation into ions is common.

Please give Ace some feedback