Answered

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Consider the reaction below.

[tex]\[ Na^{+} + C_2H_3O_2^{-} (aq) + H^{+} + Cl^{-} \longrightarrow Na^{+} + Cl^{-} + HC_2H_3O_2 \][/tex]

Which is the net ionic equation for the reaction?

A. [tex]\( H^{+} + Cl^{-} \longrightarrow HCl \)[/tex]

B. [tex]\( Na^{+} + Cl^{-} \longrightarrow NaCl \)[/tex]

C. [tex]\( Na^{+} + C_2H_3O_2^{-} \longrightarrow NaC_2H_3O_2 \)[/tex]

D. [tex]\( C_2H_3O_2^{-} (aq) + H^{+} \longrightarrow HC_2H_3O_2 \)[/tex]

Sagot :

GinnyAnswer
To identify the net ionic equation for the reaction, we start by examining the given reaction:
[tex]\[ Na^+ + C_2H_3O_2^- (aq) + H^+ + Cl^- \rightarrow Na^+ + Cl^- + HC_2H_3O_2 \][/tex]

In this reaction, we can see the following:

1. Sodium ions ([tex]\( Na^+ \)[/tex]) appear on both sides of the reaction. Therefore, they remain unchanged and do not participate in the chemical reaction. These are spectator ions.
2. Chloride ions ([tex]\( Cl^- \)[/tex]) also appear on both sides of the reaction. Therefore, they are also spectator ions and do not participate in the chemical reaction.

Removing these spectator ions, we obtain the simplified form of the equation:
[tex]\[ C_2H_3O_2^- (aq) + H^+ \rightarrow HC_2H_3O_2 \][/tex]

This represents the net ionic equation for the given reaction.

Among the given choices, the correct net ionic equation is:
[tex]\[ C_2H_3O_2^- (aq) + H^+ \rightarrow HC_2H_3O_2 \][/tex]

Therefore, the correct answer is:
[tex]\[ C_2H_3O_2^- (aq) + H^+ \longrightarrow HC_2H_3O_2 \][/tex]
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