1) HSO4 2- is a weak acid with a Ka=1.20e-2. Calculate the equilibrium concentrations for H+ and SO4 2- given a 0.159 M solution of H2SO4.

2) Determine the percent dissociation of a 2.25 M weak base solution with pH = 11.8

H2SO4 is a strong acid (100% ionized)

H2SO4 + H2O ------> HSO4- + H3O+   

I  0.159 M                      0             0
F   0                             0.159    0.159
         

HSO4- + H2O <------> SO42-  + H3O+
I 0.159                          0              0.159 

Now complete this ICE table
use Ka= [SO42- ][H3O+]/[HSO4- ]
calculate [H3O+] and pH

for the b part Sirisha
you have [H3O+] = 10^-11.8
B + H2O ---. BH+    + OH- (reaction of the weak base with water)
now [OH-] = 10^-2.2
it means 10^-2.2M of the base is dissociated
% = 10^-2.2  x 100% /2.25