From science to arts, IDNLearn.com has the answers to all your questions. Discover thorough and trustworthy answers from our community of knowledgeable professionals, tailored to meet your specific needs.
Sagot :
To identify the base-conjugate acid pair in the given reaction, it's essential to understand the concept of acid-base conjugation. In a chemical reaction involving acids and bases:
- An acid loses a proton (H⁺) to form its conjugate base.
- A base gains a proton (H⁺) to form its conjugate acid.
Let's analyze the given reaction:
[tex]\[ \text{H}_2\text{PO}_4^- + \text{H}_2\text{O} \rightarrow \text{H}_3\text{O}^+ + \text{HPO}_4^{2-} \][/tex]
From this reaction:
- Di-hydrogen phosphate ([tex]\(\text{H}_2\text{PO}_4^-\)[/tex]) is reacting with water ([tex]\(\text{H}_2\text{O}\)[/tex]).
- The product formed includes hydronium ([tex]\(\text{H}_3\text{O}^+\)[/tex]) and hydrogen phosphate ([tex]\(\text{HPO}_4^{2-}\)[/tex]).
Let's identify what gains or loses a proton:
- [tex]\(\text{H}_2\text{PO}_4^-\)[/tex] loses a proton (H⁺) to form [tex]\(\text{HPO}_4^{2-}\)[/tex]. Therefore, [tex]\(\text{H}_2\text{PO}_4^-\)[/tex] is acting as an acid, and [tex]\(\text{HPO}_4^{2-}\)[/tex] is its conjugate base.
- [tex]\(\text{H}_2\text{O}\)[/tex] gains a proton (H⁺) to form [tex]\(\text{H}_3\text{O}^+\)[/tex]. Thus, [tex]\(\text{H}_2\text{O}\)[/tex] is acting as a base, and [tex]\(\text{H}_3\text{O}^+\)[/tex] is its conjugate acid.
Considering the options provided:
1. [tex]\( \text{H}_2\text{O} \)[/tex] and [tex]\( \text{H}_3\text{O}^+ \)[/tex] form a conjugate base-acid pair.
2. [tex]\( \text{H}_2\text{O} \)[/tex] and [tex]\( \text{H}_2\text{PO}_4^- \)[/tex] do not form a conjugate pair.
3. [tex]\( \text{H}_2\text{PO}_4^- \)[/tex] and [tex]\( \text{HPO}_4^{2-} \)[/tex] form a conjugate acid-base pair.
4. [tex]\( \text{H}_2\text{PO}_4^- \)[/tex] and [tex]\( \text{H}_3\text{O}^+ \)[/tex] do not form a conjugate pair.
The correct pair that forms a base-conjugate acid pair in the given reaction is:
[tex]\[ \text{H}_2\text{PO}_4^- \text{ and } \text{HPO}_4^{2-} \][/tex]
Therefore, the answer is:
[tex]\[ \boxed{3} \][/tex]
- An acid loses a proton (H⁺) to form its conjugate base.
- A base gains a proton (H⁺) to form its conjugate acid.
Let's analyze the given reaction:
[tex]\[ \text{H}_2\text{PO}_4^- + \text{H}_2\text{O} \rightarrow \text{H}_3\text{O}^+ + \text{HPO}_4^{2-} \][/tex]
From this reaction:
- Di-hydrogen phosphate ([tex]\(\text{H}_2\text{PO}_4^-\)[/tex]) is reacting with water ([tex]\(\text{H}_2\text{O}\)[/tex]).
- The product formed includes hydronium ([tex]\(\text{H}_3\text{O}^+\)[/tex]) and hydrogen phosphate ([tex]\(\text{HPO}_4^{2-}\)[/tex]).
Let's identify what gains or loses a proton:
- [tex]\(\text{H}_2\text{PO}_4^-\)[/tex] loses a proton (H⁺) to form [tex]\(\text{HPO}_4^{2-}\)[/tex]. Therefore, [tex]\(\text{H}_2\text{PO}_4^-\)[/tex] is acting as an acid, and [tex]\(\text{HPO}_4^{2-}\)[/tex] is its conjugate base.
- [tex]\(\text{H}_2\text{O}\)[/tex] gains a proton (H⁺) to form [tex]\(\text{H}_3\text{O}^+\)[/tex]. Thus, [tex]\(\text{H}_2\text{O}\)[/tex] is acting as a base, and [tex]\(\text{H}_3\text{O}^+\)[/tex] is its conjugate acid.
Considering the options provided:
1. [tex]\( \text{H}_2\text{O} \)[/tex] and [tex]\( \text{H}_3\text{O}^+ \)[/tex] form a conjugate base-acid pair.
2. [tex]\( \text{H}_2\text{O} \)[/tex] and [tex]\( \text{H}_2\text{PO}_4^- \)[/tex] do not form a conjugate pair.
3. [tex]\( \text{H}_2\text{PO}_4^- \)[/tex] and [tex]\( \text{HPO}_4^{2-} \)[/tex] form a conjugate acid-base pair.
4. [tex]\( \text{H}_2\text{PO}_4^- \)[/tex] and [tex]\( \text{H}_3\text{O}^+ \)[/tex] do not form a conjugate pair.
The correct pair that forms a base-conjugate acid pair in the given reaction is:
[tex]\[ \text{H}_2\text{PO}_4^- \text{ and } \text{HPO}_4^{2-} \][/tex]
Therefore, the answer is:
[tex]\[ \boxed{3} \][/tex]
We appreciate your participation in this forum. Keep exploring, asking questions, and sharing your insights with the community. Together, we can find the best solutions. IDNLearn.com provides the best answers to your questions. Thank you for visiting, and come back soon for more helpful information.