A 0.0500 M solution of a base is 7.2 % ionized. Calculate thebase ionization con

Question

A 0.0500 M solution of a base is 7.2 % ionized. Calculate thebase ionization constant Kb. Hint: Use the % ionization to calculate the [BH+]and [OH-] formed when the base, B, ionizes. Remember tosubtract the ionized amount from the initial concentration of B, tofind its equilibrium concentration. Show all steps A 0.0500 M solution of a base is 7.2 % ionized. Calculate thebase ionization constant Kb. Hint: Use the % ionization to calculate the [BH+]and [OH-] formed when the base, B, ionizes. Remember tosubtract the ionized amount from the initial concentration of B, tofind its equilibrium concentration. Show all steps

Explanation / Answer

Given Concentration ,c = 0.05 M percentage of ionization = 7.2 %                                       = 7.2 / 100                                       = 0.072                                                                             H 2 O                                          B            ---------->           BH+   +       OH -
Initialconc.                         c                                          0                   0   Equil.conc.                    c ( 1-)                                  c                 c             Dissociation constant Kb =   ( [BH+ ] [OH - ] ) / [ B ]                                                      =   ( c * c ) / c (1-)                                                      = c 2 / (1- )                                                       =2.802 * 10 -4

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