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Ionic Equilibrum question

2010 · Q127
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Ionic Equilibrum question

2010 · Q127

NEETChemistryIonic EquilibrumMCQ+4 / −1
In a buffer solution containing equal concentration of B−-− and HB, the Kb for B−-− is 10−-−10. The pH of buffer solution is
  1. A
    10
  2. B
    7
  3. C
    6
  4. D
    4
View written solutionFree

Correct answer: D

pOH = pKb + log [Salt][Acid]{{\left[ {Salt} \right]} \over {\left[ {Acid} \right]}}[Acid][Salt]​

⇒\Rightarrow⇒ pOH = - log Kb + log [Salt][Acid]{{\left[ {Salt} \right]} \over {\left[ {Acid} \right]}}[Acid][Salt]​

⇒\Rightarrow⇒ pOH = –log10–10 + log 1

[As conc. of HB and B– are same]

⇒\Rightarrow⇒ pOH = 10

⇒\Rightarrow⇒ pH = 14 – pOH = 14 – 10 = 4

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