dentify the pair of species that is not a conjugate acio O NH; NH3 O H,PO3; H,PO, O H,SO;; so;- O HBr; Br

Organic Chemistry
8th Edition
ISBN:9781305580350
Author:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. Foote
Publisher:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. Foote
Chapter4: Acids And Bases
Section: Chapter Questions
Problem 4.10P: Complete a net ionic equation for each proton-transfer reaction using curved arrows to show the flow...
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### Quiz: Identifying Conjugate Acid-Base Pairs

#### Question:
Identify the pair of species that is not a conjugate acid-base pair.

#### Options:
- **A.** \( \text{NH}_4^+; \text{NH}_3 \)
- **B.** \( \text{H}_3\text{PO}_3; \text{H}_2\text{PO}_3^- \)
- **C.** \( \text{H}_2\text{SO}_3; \text{SO}_3^{2-} \)
- **D.** \( \text{HBr}; \text{Br}^- \)

#### Explanation:
This question requires knowledge of acid-base chemistry, specifically the concept of conjugate acid-base pairs. Conjugate acid-base pairs differ by one proton (H\(^+\)).

**A.** \( \text{NH}_4^+ \) and \( \text{NH}_3 \): This pair represents a conjugate acid-base pair, where \( \text{NH}_4^+ \) (ammonium ion) is the conjugate acid and \( \text{NH}_3 \) (ammonia) is the conjugate base.

**B.** \( \text{H}_3\text{PO}_3 \) and \( \text{H}_2\text{PO}_3^- \): This pair represents a conjugate acid-base pair, where \( \text{H}_3\text{PO}_3 \) (phosphorous acid) is the conjugate acid and \( \text{H}_2\text{PO}_3^- \) is the conjugate base.

**C.** \( \text{H}_2\text{SO}_3 \) and \( \text{SO}_3^{2-} \): This pair does not represent a conjugate acid-base pair. \( \text{H}_2\text{SO}_3 \) (sulfurous acid) and \( \text{SO}_3^{2-} \) (sulfite ion) do not differ by just one proton.

**D.** \( \text{HBr} \) and \( \text{Br}^- \): This pair represents a conjugate acid-base pair, where \( \text{HBr} \) (hydrobromic
Transcribed Image Text:### Quiz: Identifying Conjugate Acid-Base Pairs #### Question: Identify the pair of species that is not a conjugate acid-base pair. #### Options: - **A.** \( \text{NH}_4^+; \text{NH}_3 \) - **B.** \( \text{H}_3\text{PO}_3; \text{H}_2\text{PO}_3^- \) - **C.** \( \text{H}_2\text{SO}_3; \text{SO}_3^{2-} \) - **D.** \( \text{HBr}; \text{Br}^- \) #### Explanation: This question requires knowledge of acid-base chemistry, specifically the concept of conjugate acid-base pairs. Conjugate acid-base pairs differ by one proton (H\(^+\)). **A.** \( \text{NH}_4^+ \) and \( \text{NH}_3 \): This pair represents a conjugate acid-base pair, where \( \text{NH}_4^+ \) (ammonium ion) is the conjugate acid and \( \text{NH}_3 \) (ammonia) is the conjugate base. **B.** \( \text{H}_3\text{PO}_3 \) and \( \text{H}_2\text{PO}_3^- \): This pair represents a conjugate acid-base pair, where \( \text{H}_3\text{PO}_3 \) (phosphorous acid) is the conjugate acid and \( \text{H}_2\text{PO}_3^- \) is the conjugate base. **C.** \( \text{H}_2\text{SO}_3 \) and \( \text{SO}_3^{2-} \): This pair does not represent a conjugate acid-base pair. \( \text{H}_2\text{SO}_3 \) (sulfurous acid) and \( \text{SO}_3^{2-} \) (sulfite ion) do not differ by just one proton. **D.** \( \text{HBr} \) and \( \text{Br}^- \): This pair represents a conjugate acid-base pair, where \( \text{HBr} \) (hydrobromic
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