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Sagot :
Sure, let's classify each species in the reaction as a Brønsted base or a Brønsted acid. The reaction is:
[tex]\[ HSO_3^-(aq) + H_3O^+(aq) \rightleftharpoons H_2SO_3(aq) + H_2O(l) \][/tex]
Understanding how Brønsted-Lowry acids and bases operate:
- A Brønsted-Lowry acid is a species that donates a proton ([tex]\(H^+\)[/tex]).
- A Brønsted-Lowry base is a species that accepts a proton ([tex]\(H^+\)[/tex]).
Now, let's examine each species in the reaction to determine their role:
1. HSO[tex]\(_3^-\)[/tex]:
- In the reaction, [tex]\(\text{HSO}_3^-\)[/tex] combines with [tex]\(H_3O^+\)[/tex].
- To find out if [tex]\(\text{HSO}_3^-\)[/tex] acts as an acid or a base, observe the products:
- [tex]\(\text{HSO}_3^-\)[/tex] gains a proton ([tex]\(H^+\)[/tex]) from [tex]\(H_3O^+\)[/tex] and becomes [tex]\(H_2SO_3\)[/tex].
- Therefore, [tex]\(\text{HSO}_3^-\)[/tex] is accepting a proton and hence is a Brønsted base.
2. H[tex]\(_3O^+\)[/tex]:
- [tex]\(\text{H}_3\text{O}^+\)[/tex] donates a proton ([tex]\(H^+\)[/tex]) to [tex]\(\text{HSO}_3^-\)[/tex].
- When it loses a proton, [tex]\(\text{H}_3\text{O}^+\)[/tex] turns into [tex]\(\text{H}_2\text{O}\)[/tex].
- Thus, [tex]\(\text{H}_3\text{O}^+\)[/tex] is donating a proton and hence is a Brønsted acid.
3. H[tex]\(_2\)[/tex]SO[tex]\(_3\)[/tex]:
- Upon formation, [tex]\(H_2SO_3\)[/tex] could potentially donate a proton if the reaction were to reverse.
- In the context of this single-step depiction, it does not donate a proton directly.
- However, [tex]\(H_2SO_3\)[/tex] can theoretically donate a proton (as it can act as an acid in another context), making it a Brønsted acid.
4. H[tex]\(_2\)[/tex]O:
- By accepting a proton, [tex]\(\text{H}_2\text{O}\)[/tex] can turn into [tex]\(\text{H}_3\text{O}^+\)[/tex], showing it can accept a proton.
- In this reaction, it's the result of [tex]\(\text{H}_3\text{O}^+\)[/tex] losing a proton, indicating its potential to act as a base in future interactions.
- Thus, [tex]\(\text{H}_2\text{O}\)[/tex] is a Brønsted base.
To summarize:
- [tex]\(\text{HSO}_3^-\)[/tex] accepts a proton: Brønsted base.
- [tex]\(\text{H}_3\text{O}^+\)[/tex] donates a proton: Brønsted acid.
- [tex]\(\text{H}_2\text{SO}_3\)[/tex] can donate a proton: Brønsted acid.
- [tex]\(\text{H}_2\text{O}\)[/tex] can accept a proton: Brønsted base.
Hence, the species classifications are:
1. [tex]\(\text{HSO}_3^-\)[/tex] is a Brønsted base.
2. [tex]\(\text{H}_3\text{O}^+\)[/tex] is a Brønsted acid.
3. [tex]\(\text{H}_2\text{SO}_3\)[/tex] is a Brønsted acid.
4. [tex]\(\text{H}_2\text{O}\)[/tex] is a Brønsted base.
[tex]\[ HSO_3^-(aq) + H_3O^+(aq) \rightleftharpoons H_2SO_3(aq) + H_2O(l) \][/tex]
Understanding how Brønsted-Lowry acids and bases operate:
- A Brønsted-Lowry acid is a species that donates a proton ([tex]\(H^+\)[/tex]).
- A Brønsted-Lowry base is a species that accepts a proton ([tex]\(H^+\)[/tex]).
Now, let's examine each species in the reaction to determine their role:
1. HSO[tex]\(_3^-\)[/tex]:
- In the reaction, [tex]\(\text{HSO}_3^-\)[/tex] combines with [tex]\(H_3O^+\)[/tex].
- To find out if [tex]\(\text{HSO}_3^-\)[/tex] acts as an acid or a base, observe the products:
- [tex]\(\text{HSO}_3^-\)[/tex] gains a proton ([tex]\(H^+\)[/tex]) from [tex]\(H_3O^+\)[/tex] and becomes [tex]\(H_2SO_3\)[/tex].
- Therefore, [tex]\(\text{HSO}_3^-\)[/tex] is accepting a proton and hence is a Brønsted base.
2. H[tex]\(_3O^+\)[/tex]:
- [tex]\(\text{H}_3\text{O}^+\)[/tex] donates a proton ([tex]\(H^+\)[/tex]) to [tex]\(\text{HSO}_3^-\)[/tex].
- When it loses a proton, [tex]\(\text{H}_3\text{O}^+\)[/tex] turns into [tex]\(\text{H}_2\text{O}\)[/tex].
- Thus, [tex]\(\text{H}_3\text{O}^+\)[/tex] is donating a proton and hence is a Brønsted acid.
3. H[tex]\(_2\)[/tex]SO[tex]\(_3\)[/tex]:
- Upon formation, [tex]\(H_2SO_3\)[/tex] could potentially donate a proton if the reaction were to reverse.
- In the context of this single-step depiction, it does not donate a proton directly.
- However, [tex]\(H_2SO_3\)[/tex] can theoretically donate a proton (as it can act as an acid in another context), making it a Brønsted acid.
4. H[tex]\(_2\)[/tex]O:
- By accepting a proton, [tex]\(\text{H}_2\text{O}\)[/tex] can turn into [tex]\(\text{H}_3\text{O}^+\)[/tex], showing it can accept a proton.
- In this reaction, it's the result of [tex]\(\text{H}_3\text{O}^+\)[/tex] losing a proton, indicating its potential to act as a base in future interactions.
- Thus, [tex]\(\text{H}_2\text{O}\)[/tex] is a Brønsted base.
To summarize:
- [tex]\(\text{HSO}_3^-\)[/tex] accepts a proton: Brønsted base.
- [tex]\(\text{H}_3\text{O}^+\)[/tex] donates a proton: Brønsted acid.
- [tex]\(\text{H}_2\text{SO}_3\)[/tex] can donate a proton: Brønsted acid.
- [tex]\(\text{H}_2\text{O}\)[/tex] can accept a proton: Brønsted base.
Hence, the species classifications are:
1. [tex]\(\text{HSO}_3^-\)[/tex] is a Brønsted base.
2. [tex]\(\text{H}_3\text{O}^+\)[/tex] is a Brønsted acid.
3. [tex]\(\text{H}_2\text{SO}_3\)[/tex] is a Brønsted acid.
4. [tex]\(\text{H}_2\text{O}\)[/tex] is a Brønsted base.
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