2.5 mL of 
M weak monoacidic base (K b = 1 × 10 –12 at 25°C) is titrated with 
M HCl in water at 25°C. The concentration of H + at equivalence point is : (K w = 1 × 10 –14 at 25°C)
Text Solution
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BOH + HCl 
BCl + H 2 O (in titration)
B + + H 2 O 
BOH + H +
For titration :
M acid V acid = M base V base (since both are monoacidic and monobasic)
× V = 2.5 × 
V = 3 × 2.5 = 7.5 mL
In resulting solution,
[B + ] = 
= 
= 0.1 M
K h = 
= 
= 10 –2 or K h = 
= 10 –2
(solve quadratic equation to get 'h', as we can't write 1 – h ≈ 1, since h > 0.1)
∴ h = 0.27 & [H + ] = 0.1 × 0.27 = 2.7 × 10 –2 M
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