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A reaction is catalysed by H+ ion. In presence of HA, rate constant is 2 × 10-3 min-1and in presence of HB rate constant is 1 × 10-3 min-1. HA and HB being strong acids, we may conclude that
  • a)
    HB is stronger acid than HA
  • b)
    HA is stronger acid than HB.
  • c)
    Relative strength HA and HB is 2.
  • d)
    HA is weaker than HB and relative strength is 0.5.
Correct answer is option 'B,C'. Can you explain this answer?
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Most Upvoted Answer
A reaction is catalysed by H+ion. In presence of HA, rate constant is ...

Rate = K[H+][A]
Rate = K’[A]
If K’ has greater value for HA
⇒ [H+] has to be large
⇒ for that acid has be stronger
⇒ [HA] is strongers that HB
Also Relative strength = 2
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A reaction is catalysed by H+ion. In presence of HA, rate constant is ...
Explanation:

1. Introduction:
In this question, we are given that a reaction is catalyzed by H+ ion and the rate constant of the reaction is measured in the presence of two strong acids, HA and HB. We are required to determine the relative strength of HA and HB based on the given rate constants.

2. Rate Constant:
The rate constant of a reaction is a measure of how quickly the reaction proceeds. It is dependent on several factors, including temperature, concentration of reactants, and the presence of catalysts. In this case, the rate constant is given as 2 x 10^-3 min^-1 in the presence of HA and 1 x 10^-3 min^-1 in the presence of HB.

3. Relationship between Rate Constant and Acid Strength:
The rate constant of a reaction can be influenced by the acidity of the medium. Generally, stronger acids have a higher rate constant compared to weaker acids. This is because stronger acids can donate protons more readily, leading to a faster reaction rate.

4. Conclusion:
Based on the given rate constants, we can make the following conclusions:

- HA is stronger acid than HB: Since the rate constant is higher in the presence of HA (2 x 10^-3 min^-1) compared to HB (1 x 10^-3 min^-1), we can conclude that HA is a stronger acid than HB. This is because the reaction proceeds faster in the presence of HA, indicating a higher acidity.

- Relative strength of HA and HB is 2: The rate constant ratio between the two acids is 2:1. This implies that HA is twice as strong as HB. This conclusion is supported by the fact that the reaction rate is twice as fast in the presence of HA compared to HB.

5. Answer:
Therefore, the correct answer is option 'B,C'. HA is a stronger acid than HB, and the relative strength of HA and HB is 2.
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A reaction is catalysed by H+ion. In presence of HA, rate constant is 2 10-3min-1and in presence of HB rate constant is 1 10-3min-1. HA and HB being strong acids, we may conclude thata)HB is stronger acid than HAb)HA is stronger acid than HB.c)Relative strength HA and HB is 2.d)HA is weaker than HB and relative strength is 0.5.Correct answer is option 'B,C'. Can you explain this answer?
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A reaction is catalysed by H+ion. In presence of HA, rate constant is 2 10-3min-1and in presence of HB rate constant is 1 10-3min-1. HA and HB being strong acids, we may conclude thata)HB is stronger acid than HAb)HA is stronger acid than HB.c)Relative strength HA and HB is 2.d)HA is weaker than HB and relative strength is 0.5.Correct answer is option 'B,C'. Can you explain this answer? for JEE 2025 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about A reaction is catalysed by H+ion. In presence of HA, rate constant is 2 10-3min-1and in presence of HB rate constant is 1 10-3min-1. HA and HB being strong acids, we may conclude thata)HB is stronger acid than HAb)HA is stronger acid than HB.c)Relative strength HA and HB is 2.d)HA is weaker than HB and relative strength is 0.5.Correct answer is option 'B,C'. Can you explain this answer? covers all topics & solutions for JEE 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A reaction is catalysed by H+ion. In presence of HA, rate constant is 2 10-3min-1and in presence of HB rate constant is 1 10-3min-1. HA and HB being strong acids, we may conclude thata)HB is stronger acid than HAb)HA is stronger acid than HB.c)Relative strength HA and HB is 2.d)HA is weaker than HB and relative strength is 0.5.Correct answer is option 'B,C'. Can you explain this answer?.
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