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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the seeing the electronic configuration we can say that the element is fluorine.

fluorine is the most electronegative element in the periodic table.

but by only seeing the configuration we cannot say about its reactivity because we don't know if its configuration after excitation or by addition of electrons.

but if not then, it is the lightest halogen and exists as a highly toxic pale yellow diatomic gas at standard conditions. as the most electronegative element, it is extremely reactive: almost all other elements, including some noble gases, form compounds with fluorine.