Buffer capacity is a measure of a buffer solution's resistance to changes in ph as strong acid or base is added. suppose that you have 185 ml of a buffer that is 0.400 m in both acetic acid (ch3cooh) and its conjugate base (ch3coo−) . calculate the maximum volume of 0.180 m hcl that can be added to the buffer before its buffering capacity is lost.

Explanation:

It is given that 185 ml of buffer solution is 0.40 M and .

Now, according to the Handerson equation,

          pH =

It is known that value of acetic acid is 4.76.

        pH =

              =

              = 4.76

If pH of a buffer changes by 1 unit then it means the buffering capacity is lost.

Hence, when HCl is being added it reacts with and gives . So, with increase in the log term gives a negative value. This means that new pH will be less than 4.76.

Therefore, calculate the concentration when pH = 3.6.

                   3.76 = 4.76 +

          = 0.1  ....... (1)

Now, we assume that the moles of acid added or change in moles is x. Therefore, moles of acetic acid and conjugate base present are as follows.

                       No. of moles = Molarity × Volume

                                             = 0.40 × 185 ml

                                             = 74 mmol

Now, we put this value into equation (1) as follows.

                        x = 60.5

This means that moles of acid added is 60.5 mmol.

As it is given that molarity is 0.180 M. Therefore, calculate the volume of acid as follows.

                Volume of acid =

                                          =

                                          = 336.1 ml

Thus, we can conclude that the maximum volume of 0.180 M HCl that can be added to the buffer before its buffering capacity is lost is 336.1 ml.