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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: - Solubility of MX₂ – type electrolytes is 0.5 ˣ 10⁻⁴ mol/L.,
- Standard entropies of X₂, Y₂ and XY₃ are 60, 40 and 50 J K⁻¹ mol⁻¹ respectively.
- The reaction in which phenol differs from alcohol is
- 0.037g of an alcohol, R-OH was added to C₂H₅Mgl and the has evolved measured 11.2cc
- Which of the following will not undergo Hell-Volhard-Zelinsky reaction
Topics: Equilibrium
(104)
Subject: Chemistry
(2512)
Important MCQs Based on Medical Entrance Examinations To Improve Your NEET Score
- Solubility of MX₂ – type electrolytes is 0.5 ˣ 10⁻⁴ mol/L.,
- Standard entropies of X₂, Y₂ and XY₃ are 60, 40 and 50 J K⁻¹ mol⁻¹ respectively.
- The reaction in which phenol differs from alcohol is
- 0.037g of an alcohol, R-OH was added to C₂H₅Mgl and the has evolved measured 11.2cc
- Which of the following will not undergo Hell-Volhard-Zelinsky reaction
Topics: Equilibrium (104)
Subject: Chemistry (2512)
Important MCQs Based on Medical Entrance Examinations To Improve Your NEET Score
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