Explanation
1 M HCl = 100 M HCl and pH = 0. For greater concentration, theoretically pH should further decrease and become negative. However, as concentration increases, dissociation decreases so that [H+] does not increase. Hence pH remains almost zero.
As [NH4Cl] = [NH4OH], p OH= pKb or pKb = pOH =14 - pH = 14 – 9.25 = 4.75
BaCl2 is the limiting reactant.
As their dissociation constants are same and [H+] from CH3COOH =10-4 M Therefore [OH-] from NH4OH = 10-4 M or [H+] = 10-10 M or pH =10.
pH of buffer remains almost constant.
The degree of hydrolysis of a salt of weak acid and weak base does not depend upon concentration.
Smaller the Kb value, weaker is the base.
The equilibrium will shift in the backward direction .
I is basic (pH > 7), II is acidic (pH < 7), III is neutral (pH ≈ 7) IV is strongly basic (pH >>7) i.e. IV >I >III > II.
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