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Given that a reaction can be presented in several different forms, we should make a clear distinction between each type of equation. The sulfite ion, [tex]$SO _3{ }^{2-}$[/tex] (aq), is very soluble with respect to most cations, and its fully protonated form, [tex]$H _2 SO _3$[/tex] (aq) (sulfurous acid), is a weak acid. Its singly protonated form, [tex][tex]$HSO _3{ }^{-}$[/tex][/tex], is also a weak acid. The following equations depict several reactions that could occur if sulfurous acid and sodium hydroxide were added to water.

Classify each depicted reaction as being a molecular equation, a complete ionic equation, or a net ionic equation.

Drag the equations to their respective bins.

1. [tex]$Na ^{+} + OH ^{-} + H _2 SO _3 = Na ^{+} + HSO _3{ }^{-} + H _2 O (l)$[/tex]
2. [tex]$NaHSO _3 + H _2 O$[/tex]
3. [tex][tex]$H _2 SO _3 + NaOH$[/tex][/tex]
4. [tex]$HSO _3^{-} (aq) + OH ^{-} (aq) = SO _3^{2-} (aq) + H _2 O (l)$[/tex]
5.
[tex]
\begin{array}{l}
SO _3^{2-} (aq) + H _2 O (l) \rightleftharpoons \\
HSO _3^{-} (aq) + OH ^{-} (aq)
\end{array}
[/tex]



Answer :

GinnyAnswer
To classify the given chemical reactions as molecular equations, complete ionic equations, or net ionic equations, we need to understand what each term means:

1. Molecular Equation: Shows all reactants and products as they are, without breaking them down into ions.
2. Complete Ionic Equation: Shows all the soluble strong electrolytes (compounds) dissociated into their ions.
3. Net Ionic Equation: Focuses only on the species that are actually involved in the chemical change, omitting spectator ions that do not participate in the reaction.

Let's classify each depicted reaction:

### Molecular Equation:
1. Molecular Equation:
[tex]\[ H_2SO_3 + NaOH \rightarrow NaHSO_3 + H_2O \][/tex]

### Complete Ionic Equation:
2. Complete Ionic Equation:
[tex]\[ Na^+ + OH^- + H_2SO_3 \rightarrow Na^+ + HSO_3^- + H_2O \][/tex]

### Net Ionic Equations:
3. Net Ionic Equation 1:
[tex]\[ HSO_3^- (aq) + OH^- (aq) \rightarrow SO_3^{2-} (aq) + H_2O (l) \][/tex]

4. Net Ionic Equation 2:
[tex]\[ \begin{array}{l} SO_3^{2-} (aq) + H_2O (l) \rightleftharpoons \\ HSO_3^- (aq) + OH^- (aq) \end{array} \][/tex]

### Reactions at Equilibrium:
5. Reactions at Equilibrium:
[tex]\[ \begin{aligned} &\text{HSO}_3^- + \text{OH}^- \rightarrow \text{SO}_3^{2-} + \text{H}_2\text{O}, \\ &\text{SO}_3^{2-} + \text{H}_2\text{O} \rightarrow \text{HSO}_3^- + \text{OH}^- \end{aligned} \][/tex]

To summarize, here are the classifications:
- Molecular Equation: [tex]\(H_2SO_3 + NaOH \rightarrow NaHSO_3 + H_2O\)[/tex]
- Complete Ionic Equation: [tex]\(Na^+ + OH^- + H_2SO_3 \rightarrow Na^+ + HSO_3^- + H_2O\)[/tex]
- Net Ionic Equations:
- [tex]\(HSO_3^- (aq) + OH^- (aq) \rightarrow SO_3^{2-} (aq) + H_2O (l)\)[/tex]
- [tex]\(\begin{aligned}[t] &SO_3^{2-} (aq) + H_2O (l) \rightleftharpoons \\ &HSO_3^- (aq) + OH^- (aq) \end{aligned}\)[/tex]

Understanding and identifying the different forms of these equations is crucial in understanding the chemical reactions that occur in solutions.

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