Question

which equation represents the total ionic equation for the reaction of hno₃ and naoh?
○ h⁺ + oh⁻ ⟶ h₂o
○ hno₃ + naoh ⟶ nano₃ + h₂o
○ h⁺ + no₃⁻ + na⁺ + oh⁻ ⟶ na⁺ + no₃⁻ + h₂o
○ h⁺ + no₃⁻ + oh⁻ ⟶ no₃⁻ + h₂o

Explanation:

1. First, recall what a total ionic equation is: it shows all the ions present in the reaction, including spectator ions.

• $\ce{HNO_{3}}$ is a strong acid, so it dissociates completely into $\ce{H^{+}}$ and $\ce{NO^{-}_{3}}$: $\ce{HNO_{3} -> H^{+} + NO^{-}_{3}}$.
• $\ce{NaOH}$ is a strong base, so it dissociates completely into $\ce{Na^{+}}$ and $\ce{OH^{-}}$: $\ce{NaOH -> Na^{+} + OH^{-}}$.
• The products are $\ce{NaNO_{3}}$ (a soluble salt, so it dissociates into $\ce{Na^{+}}$ and $\ce{NO^{-}_{3}}$) and $\ce{H_{2}O}$ (which does not dissociate into ions to a significant extent).

1. Now, write out all the ions from the reactants and the dissociated products:

• Reactants: $\ce{H^{+}}$, $\ce{NO^{-}_{3}}$, $\ce{Na^{+}}$, $\ce{OH^{-}}$.
• Products: $\ce{Na^{+}}$, $\ce{NO^{-}_{3}}$, $\ce{H_{2}O}$.

1. Combine these to form the total ionic equation: $\ce{H^{+} + NO^{-}_{3} + Na^{+} + OH^{-} -> Na^{+} + NO^{-}_{3} + H_{2}O}$.

• Let's analyze the other options:
• The first option ($\ce{H^{+} + OH^{-} -> H_{2}O}$) is the net ionic equation, not the total ionic equation (it omits spectator ions).
• The second option ($\ce{HNO_{3} + NaOH -> NaNO_{3} + H_{2}O}$) is the molecular equation, not the ionic equation.
• The fourth option is incorrect because it misses the $\ce{Na^{+}}$ ion on the reactant side (from $\ce{NaOH}$ dissociation).

Answer:

C. $\ce{H^{+} + NO^{-}_{3} + Na^{+} + OH^{-} -> Na^{+} + NO^{-}_{3} + H_{2}O}$