0.1 mole of CH3NH2 Kb = 5 × 10-4 is mixed with 0.08 mole of HCl and diluted to one litre. The H+ in solution is
8 × 10-2 M
8 × 10-11 M
1.6 × 10-11 M
8 × 10-5 M
CH3NH2 + HCl → CH3N+H3Cl-
0.1 0.08 0
0.02 0 0.08
[ 0.08mole HCl neutralizes 0.08 mole methylamine. Concentration of base left is (0.1-0.08) = 0.02]
This is basic buffer solution.
OH- = Kb × BaseSalt
=5 × 10-4 × 0.020.08 = 1.25 × 10-4
∴ H+ = 10-14OH- = 10-141.25 × 10-4 = 8 × 10-11 M