Frosty0110idn
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 :

GinnyAnsweridn
To determine the net ionic equation for the given reaction, we need to follow these steps:

1. Write down the full ionic equation:
The given chemical reaction is:
[tex]\[ Na^+ + C_2H_3O_2^-(aq) + H^+ + Cl^- \longrightarrow Na^+ + Cl^- + HC_2H_3O_2 \][/tex]

2. Identify the spectator ions:
Spectator ions are ions that appear on both the reactant and product sides of the equation and do not undergo any chemical change. Here, we identify:
- [tex]\( Na^+ \)[/tex] is present on both sides.
- [tex]\( Cl^- \)[/tex] is present on both sides as well.

3. Remove the spectator ions:
By eliminating [tex]\( Na^+ \)[/tex] and [tex]\( Cl^- \)[/tex] from the equation, we focus on the ions that actually participate in the reaction.

4. Write the net ionic equation:
After removing the spectator ions, we are left with:
[tex]\[ C_2H_3O_2^-(aq) + H^+ \longrightarrow HC_2H_3O_2 \][/tex]

Therefore, the net ionic equation for the reaction is:
[tex]\[ C_2H_3O_2^-(aq) + H^+ \longrightarrow HC_2H_3O_2 \][/tex]

Thus, the correct choice from the given options is:
[tex]\[ C_2H_3O_2^-(aq) + H^+ \longrightarrow HC_2H_3O_2 \][/tex]
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