a buffer solution contain 0.1 mole per litres of acetic acid and 0.001 moles perlitre of sodium acetate. what will be its pH?(k=1.8×10-5)

The pH of the solution is 2.74.

Explanation:

To calculate the pH of the acidic buffer, the equation for Henderson-Hasselbalch is used:

        .......(1)

The power of the acid dissociation constant is the negative logarithm of the acid dissociation constant. The equation for it is:

       ......(2)

The chemical equation for the reaction of acetic acid and NaOH follows:

Given values:

Putting values in equation 2:

We are given:

= 0.1 M

= 0.001 M

Plugging values in equation 1:

Hence, the pH of the solution is 2.74.

the potential energy of the reactants is 200j.

from the energy diagram, the energy of the product formed is 350j; this means that, this reaction is an endothermic reaction, because it absorbs energy from its environment.

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