When 0.22 mole of CH 3 NH 2 (ionization constant, K b = 1 0 − 6 ) is mixed with 0.02 mole HCl and the volume is made up to 1 litre, find the [ H + ] of resulting solution at 2 5 ∘ C .

Question

When 0.22 mole of CH 3 ​ NH 2 ​ (ionization constant, K b ​ = 1 0 − 6 ) is mixed with 0.02 mole HCl and the volume is made up to 1 litre, find the [ H + ] of resulting solution at 2 5 ∘ C .

TestHub · Accepted Answer

CH₃NH₂ + HCl → CH₃NH₃ + Cl⁻

Initial 0.22 0.02 0 0

Final 0.20 0 0.02 0.02

its a basic buffer

$pO H = p K_{b} + lo g (\frac{[ S a lt ]}{[ B a se ]})$

$pO H = 6 + lo g (\frac{0.02}{0.20})$

$pO H = 6 + lo g (0.1)$

$pO H = 6 - 1 = 5$ So $p H = 9$ or $[H^{+}] = 1 0^{- 9} M$

Chemistry - Ionic Equilibrium Question with Solution | TestHub

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