To identify the acids and bases in the given acid-base reaction, we need to use the Bronsted-Lowry theory of acids and bases. According to this theory:
- An acid is a proton donor.
- A base is a proton acceptor.
Given the reaction:
[tex]\[ H_3C_6H_5O_7 + H_2O \rightleftharpoons H_3O^+ + H_2C_6H_5O_7^- \][/tex]
Let's analyze it step-by-step.
1. Identify the donating and accepting species:
- [tex]\( H_3C_6H_5O_7 \)[/tex]: It donates a proton (H^+) to water, transforming into [tex]\( H_2C_6H_5O_7^- \)[/tex]. Therefore, it acts as an acid.
- [tex]\( H_2O \)[/tex]: It accepts a proton (H^+) from [tex]\( H_3C_6H_5O_7 \)[/tex], transforming into [tex]\( H_3O^+ \)[/tex]. Therefore, it acts as a base.
- [tex]\( H_3O^+ \)[/tex]: It is the hydronium ion, formed after water accepts a proton. In the reverse reaction, it can donate a proton back, so it is recognized as an acid in the reverse reaction context.
- [tex]\( H_2C_6H_5O_7^- \)[/tex]: Formed after [tex]\( H_3C_6H_5O_7 \)[/tex] donates a proton. It can accept a proton in the reverse reaction, so it acts as a base.
2. Label each part of the equation with the correct roles:
- [tex]\( H_3C_6H_5O_7 \)[/tex] is the acid.
- [tex]\( H_2O \)[/tex] is the base.
- [tex]\( H_3O^+ \)[/tex] is the acid.
- [tex]\( H_2C_6H_5O_7^- \)[/tex] is the base.
In summary, here is the identification:
[tex]\[ \underset{\text{(acid)}}{H_3C_6H_5O_7} + \underset{\text{(base)}}{H_2O} \quad \rightleftharpoons \quad \underset{\text{(acid)}}{H_3O^+} + \underset{\text{(base)}}{H_2C_6H_5O_7^-} \][/tex]
