Please help with parts a and b and show work if possible. Thanks!
(a) At any equivalence point sharp change in pH occurs. That is magnitude of d(pH)/dV is highest at the equivalence point.
For the given titration curve this occurs first at V=10.5 ml and then at 21.05 ml, thus first equivalence occurs at V = 10.5 ml of base added and second equivalence point at V= 21.05 ml of base added.
Lets write maleic as H2A for convenience.
Now when we are at halfway to the first equivalence point then [H2A]= [HA-], so Ka1= [HA-]x[H+]/[H2A] gives Ka1 = [H+] and so -logKa1= -log[H+] and hence pKa1 = pH at midway to first equivalence point that is when volume of base added is V=10.5/2 ml= 5.25 ml. Similarly at midway point between first and second equivalence point (when V of base added is 10.5+(21.05-10.5)/2 =15.75 ml), we have pKa2 = pH.
Now we find these two points on the plot as follows:
(b) As found above in the plot we get pKa1 =2.00 and pKa2= 6.19
Now since pKa = -logKa it gives Ka=10-pKa , thus Ka1 = 102.00 = 1.00x102 and Ka2 = 106.19 = 1.55x106.
Comment in case of any doubt.
Please help with parts a and b and show work if possible. Thanks! Using the titration...