Ionic EquilibriumHard
Question
Equal volumes of following solutions are mixed, in which case the pH of resulting solution will be average value of pH of two solutions.
Options
A.Aqeous HCl of pH = 2, aqueous NaOH of pH = 12
B.Aqeous HCl of pH = 2, aqueous HCl of pH = 4
C.Aqeous NaOH of pH = 12, aqueous NaOH of pH = 10
D.Aqeous CH3COOH of pH = 5, aqueous NH3 of pH = 9. [Ka (CH3COOH) = Kb (NH3)]
Solution
(A) [H+] = 10-2 and [OH-] = 10-2
H+ + OH- → H2O
This leads complete neutralisation
So pH = 7 =
(D) [H+] = 10-5 and [OH-] = 10-5
[H+] + [OH-] H2O
This leads complete neutralisation
so pH = 7 =
H+ + OH- → H2O
This leads complete neutralisation
So pH = 7 =
(D) [H+] = 10-5 and [OH-] = 10-5
[H+] + [OH-] H2O
This leads complete neutralisation
so pH = 7 =
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