Ionic EquilibriumHard
Question
In a buffer solution containing equal concentration of B- and HB, the Kb for B-1 is 10-10 . The pH of buffer solution is
Options
A.10
B.7
C.6
D.4
Solution
(i) For basic buffer
pOH = pKb + log
(ii) pH + pOH = 14
Given, Kb = 1 × 10-10, [ salt ] = [ base ]
pOH = - log Kb + log
∴ pOH = - log ( 1 × 10-10) + log1 = 10
pH + pOH = 14
pH = 14 - 10 = 4
pOH = pKb + log
(ii) pH + pOH = 14
Given, Kb = 1 × 10-10, [ salt ] = [ base ]
pOH = - log Kb + log
∴ pOH = - log ( 1 × 10-10) + log1 = 10
pH + pOH = 14
pH = 14 - 10 = 4
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