A buffer solution contains 0.306 M C6H5NH3Br and 0.418 M C6H5NH2 (aniline). Determine the pH change when 0.124 mol HCl is added to 1.00 L of the buffer.

The pH change of the buffer is 0.30

Explanation:

To calculate the pH of basic buffer, we use the equation given by Henderson Hasselbalch:

       .....(1)

We are given:

= negative logarithm of base dissociation constant of aniline  = 9.13

pOH = ?

Putting values in equation 1, we get:

To calculate pH of the solution, we use the equation:

To calculate the molarity, we use the equation:

Moles hydrochloric acid solution = 0.124 mol

Volume of solution = 1 L

Putting values in above equation, we get:

The chemical reaction for aniline and HCl follows the equation:

Initial:           0.418        0.124           0.306

Final:             0.294          -                0.430

Calculating the pOH by using using equation 1:

= negative logarithm of base dissociation constant of aniline  = 9.13

pOH = ?

Putting values in equation 1, we get:

To calculate pH of the solution, we use the equation:

Calculating the pH change of the solution:

Hence, the pH change of the buffer is 0.30

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