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
Create a free account to view solution
View Solution FreeMore Ionic Equilibrium Questions
From seprate solution of four sodium salt NaW, NaX, NaY and NaZ are having the pH 7, 9, 10 and 11 respectively. When eac...The ratio of dissociation constant of two weak acids HA and HB is 4. At what moar concentration ratio, the two acids wil...The conjugate base of H2PO4- is...Number of H+ ions present in 10 mL of solution of pH = 3 are:...Which shows the maximum rate of alkaline hydrolysis :-...