Consider the titration of 50.0 mL of 1.00 M C5H5N by 0.500 M HCl. For each volume of HCl added, decide which of the components is a major species after the HCl has reacted completely. Kb for C5H5N

The given question is incomplete. The complete question is as follows.

Consider the titration of 50.0 mL of 1.00 M by 0.500 M HCl. For each volume of HCl added, decide which of the components is a major species after the HCl has reacted completely. Kb for = . Calculate the pH at the equivalence point for this titration.

Explanation:

Reaction equation of the given reaction is as follows.

Only is present in the solution before the addition of HCl. Hence, the equation will be as follows.

And, at the equivalence point entire will completely react with the HCl. Hence, the solution contains at the equivalence point. It is acidic with a pH less than 7.

No. of moles of HCl = No. of moles of

                  = 100 ml

Hence, the volume of HCl at the equivalence point is 100 ml.

Also,    

                       =

                       =

Therefore, concentration of the acid is calculated as follows.

              Concentration =

                              =

                              = 0.333 M

Since, is a weak acid. So,

                    =

                    =

Now, we will calculate the pH of the solution at the equivalence point as follows.

      pH =

            = 2.85

Thus, we can conclude that pH at the equivalence point for this titration is 2.85.

thats how its supposed to be