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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.
Related Questions: - The aqueous solution of which of the following salt will have the lowest pH
- Which of the following statement concerning lanthanides elements is fals
- What is the mass of the precipitate formed when 50 mL of 16.9% solution of AgNO₃
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- Which one of the following is called a carbylamine
Topics: Equilibrium
(104)
Subject: Chemistry
(2512)
Important MCQs Based on Medical Entrance Examinations To Improve Your NEET Score
- The aqueous solution of which of the following salt will have the lowest pH
- Which of the following statement concerning lanthanides elements is fals
- What is the mass of the precipitate formed when 50 mL of 16.9% solution of AgNO₃
- Which of the following ions can cause coagulation of proteins
- Which one of the following is called a carbylamine
Topics: Equilibrium (104)
Subject: Chemistry (2512)
Important MCQs Based on Medical Entrance Examinations To Improve Your NEET Score
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