The titration curve image represents the titration where the analyte is Blank 1 Question 2[select: , HCl, NaOH, Ammonia, Acetic acid] , and the titrant is Blank 2 Question 2[select: , HCl, NaOH] .

Question

BlackTom AI · Accepted Answer

High initial pH (~13) and a sharp, nearly vertical drop in pH near the midpoint show a strong-base analyte being neutralized by a strong acid, so the analyte is NaOH and the titrant is HCl.

1) Relevant knowledge points and concepts
- Initial pH indicates whether analyte is acidic or basic: pH >> 7 implies a basic analyte (contains OH−).  
- Titration curve shape: strong base titrated with strong acid shows a high starting pH, a steep fall at the equivalence point, and a low final pH when excess strong acid is present.  
- Equivalence-point pH for strong acid/strong base titrations is about 7 (neutral), with a very sharp vertical region. Weak acids or weak bases give buffer regions and equivalence pH shifted away from 7.

2) Step-by-step reasoning
- The graph begins at pH ≈ 13–13.5. That means the solution initially contains a high OH− concentration (basic analyte).  
- As volume of titrant increases, pH slowly declines until a sudden steep decrease around ~10 mL. That steep region is the equivalence region where stoichiometric neutralization occurs.  
- After the equivalence point the curve levels off at a low pH (~1–2), indicating excess strong acid in solution.

3) Intermediate numerical interpretation
- If initial pH ≈ 13, then pOH ≈ 1 and [OH−] ≈ 10−1 M (0.1 M), consistent with a moderately concentrated strong base like NaOH.  
- After the equivalence point the pH ≈ 1 corresponds to [H+] ≈ 10−1 M, consistent with addition of excess strong acid (HCl).

4) Why the correct answer is correct
- Only a strong base analyte combined with a strong acid titrant produces the observed high-starting pH, very steep vertical equivalence region, and very low final pH. That matches NaOH (analyte) titrated with HCl (titrant).

5) Why other options are incorrect
- HCl as analyte with NaOH titrant would start at low pH and show a steep rise, the mirror image of this curve.  
- Ammonia (a weak base) would show a buffer region and an equivalence-point pH > 7 (less steep slope).  
- Acetic acid (a weak acid) titrated with NaOH would start acidic and show an equivalence pH > 7, not the observed profile.

Conclusion: The analyte is NaOH and the titrant is HCl, matching the provided answer.

The titration curve image represents the titration where the analyte is Blank 1 Question 2[select: , HCl, NaOH, Ammonia, Acetic acid] , and the titrant is Blank 2 Question 2[select: , HCl, NaOH] .多重下拉选择题

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