Ionic EquilibriumHard
Question
2.5 mL of 
M weak monoacidic base(Kb = 1 × 10-12 at 25o C) is titrated with 
M HCl in water at 25oC. The concentration of H+ at equivalence point is (Kw = 1 × 10 -14 at 25oC)
M weak monoacidic base(Kb = 1 × 10-12 at 25o C) is titrated with M HCl in water at 25oC. The concentration of H+ at equivalence point is (Kw = 1 × 10 -14 at 25oC)Options
A.3.7 × 10-13 M
B.3.2 × 10-7 M
C.3.2 × 10-2 M
D.2.7 × 10-2 M
Solution
BOH + HCl → BCl + H2O
C
B+ H2O ⇋ BOH + H+
C(1 - h) Ch Ch
Volume of HCl used =
= 7.5ml
Concentration of Salt, C =
= 0.1 M
∴
Solving h = 0.27
[H+] = Ch = 0.1 × 0.27 = 2.7 × 10-2 M
C
B+ H2O ⇋ BOH + H+
C(1 - h) Ch Ch
Volume of HCl used =
= 7.5mlConcentration of Salt, C =
= 0.1 M∴
Solving h = 0.27
[H+] = Ch = 0.1 × 0.27 = 2.7 × 10-2 M
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