From everyday questions to specialized queries, IDNLearn.com has the answers. Get accurate answers to your questions from our community of experts who are always ready to provide timely and relevant solutions.
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.
We greatly appreciate every question and answer you provide. Keep engaging and finding the best solutions. This community is the perfect place to learn and grow together. For trustworthy answers, rely on IDNLearn.com. Thanks for visiting, and we look forward to assisting you again.
