Which of the following shows the relationship between an acid (A) and its conjugate base (B):

Question

BlackTom AI · Accepted Answer

An acid donates a proton (H+); after donation the species left is its conjugate base. This Bronsted–Lowry definition is the key concept.

1. Relevant knowledge points and concepts
- Bronsted–Lowry acid: proton (H+) donor.  
- Conjugate base: the species that remains after the acid has donated a proton.  
- General representation: HA → A− + H+ (here HA is the acid, A− its conjugate base).

2. Step-by-step reasoning
- Replace the general symbols with the problem labels: the acid is A and its conjugate base is B. That means A (acid) donates H+ and becomes B (conjugate base).  
- Writing the reaction consistent with the definition gives A → B + H+. This exactly matches choice d.

3. Intermediate logical steps (mapping)
- Start from HA → A− + H+.  
- Let HA = A and A− = B.  
- Therefore A → B + H+.

4. Why the correct answer is correct
- Answer d explicitly shows A giving up an H+ to form B, which is precisely the acid → conjugate base relationship under Bronsted–Lowry theory.

5. Why the other options are incorrect
- a. B → A + H+: This reverses the relationship (it makes B the acid donating H+ to form A), which contradicts the labels.  
- b. A + B → H+: Implies A and B combine to produce a free proton; that does not represent an acid converting into its conjugate base and has incorrect stoichiometry.  
- c. A + OH− → H+ + B: In reality OH− would accept H+ (forming H2O), so the correct neutralization would be A + OH− → B + H2O, not producing free H+. Thus c is chemically incorrect.

6. Conclusion
The correct representation of an acid A and its conjugate base B is A → B + H+, so the correct answer is d. This matches the provided answer.

Which of the following shows the relationship between an acid (A) and its conjugate base (B):Single choice

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