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In a buffer solution containing equal concentration of B⁻ and HB, the Kb for B⁻ is 10⁻¹⁰.The pH of buffer solution is
Options
(a) 10
(b) 7
(c) 6
(d) 4
Correct Answer:
4
Explanation:
We know, pOH = pK(b) + log{[B⁻]/[HB]},
Since, [B⁻] = [HB] (given).
Therefore pOH = pK(b) ⇒ pOH = 10,
Therefore pH = 14 – 10 = 4.
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Topics: Equilibrium
(104)
Subject: Chemistry
(2512)
Important MCQs Based on Medical Entrance Examinations To Improve Your NEET Score
- How much quick lime can be obtained from 25g of CaCO₃?
- Two different gases enclosed in different flasks A and B at same temperature and pressure
- If concentration of reactants is increased by ‘x’,then the K becomes
- Which of the following will show a negative deviation from Raoult’s law
- In which of the following conditions a chemical reaction can not occur
Topics: Equilibrium (104)
Subject: Chemistry (2512)
Important MCQs Based on Medical Entrance Examinations To Improve Your NEET Score
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