To determine the validity of each statement regarding the reaction:
[tex]\[
CH_3COOH \rightarrow CH_3COO^{-} + H^{+}
\][/tex]
we need to analyze the roles of [tex]\(CH_3COOH\)[/tex] and [tex]\(CH_3COO^{-}\)[/tex] based on different definitions of acids and bases.
1. Statement: [tex]\(CH_3COOH\)[/tex] is a Brønsted-Lowry base.
The Brønsted-Lowry theory defines an acid as a proton (H[tex]\(^+\)[/tex]) donor and a base as a proton acceptor. In the reaction
[tex]\[
CH_3COOH \rightarrow CH_3COO^{-} + H^{+},
\][/tex]
[tex]\(CH_3COOH\)[/tex] is donating a proton (H[tex]\(^+\)[/tex]), hence it acts as a Brønsted-Lowry acid, not a base. Therefore, this statement is False.
2. Statement: [tex]\(CH_3COOH\)[/tex] is a Brønsted-Lowry acid.
As mentioned above, since [tex]\(CH_3COOH\)[/tex] donates a proton (H[tex]\(^+\)[/tex]), it is a Brønsted-Lowry acid. Thus, this statement is True.
3. Statement: [tex]\(CH_3COO^{-}\)[/tex] is an Arrhenius base.
The Arrhenius definition states that an Arrhenius base is a substance that increases the concentration of OH[tex]\(^-\)[/tex] ions in aqueous solution. In this reaction, [tex]\(CH_3COO^{-}\)[/tex] does not directly release OH[tex]\(^-\)[/tex] ions. Thus, this statement is False.
4. Statement: [tex]\(CH_3COO^{-}\)[/tex] is a Lewis base.
According to the Lewis definition, a base is a substance that donates an electron pair. The acetate ion ([tex]\(CH_3COO^{-}\)[/tex]) has lone pairs of electrons that it can donate, qualifying it as a Lewis base. Hence, this statement is True.
So, summarizing the evaluation of the statements:
1. False - [tex]\(CH_3COOH\)[/tex] is not a Brønsted-Lowry base.
2. True - [tex]\(CH_3COOH\)[/tex] is a Brønsted-Lowry acid.
3. False - [tex]\(CH_3COO^{-}\)[/tex] is not an Arrhenius base.
4. True - [tex]\(CH_3COO^{-}\)[/tex] is a Lewis base.
Therefore, the correct answer is:
[tex]\[
(False, True, False, True)
\][/tex]
