What is the relationship between a weak acid and a buffer? give me an example and explain how a weak acid can act as a buffer?

Explanation:

Buffer solutions are solutions capable of maintaining their pH at approximately constant values when small amounts of acid or base are added.

A buffer solution is characterized by simultaneously containing a weak species and its conjugate pair. In other words, it has a weak acid and a salt of the same acid from a strong base or, a base and a salt of this base from a strong acid.

Two examples are:

Given that the buffer solution is a mixture of weak acid with a salt of the same acid from a strong base, the acid will be partially dissociated according to the equation:

HA ⇔

Applying the Law of Mass Action (which establishes the relationship between the masses of reagents and products in a chemical equilibrium at a given temperature) and taking into account the dissociation constant() is obtained the following expression:

Where pKa represents the potential value of the acid acid constant of the weak acid,   is the  common anion concentration, equivalent to salt and  [HA] indicates weak acid concentration  which is part of the buffer solution. Consequently, the above equation can be rewritten as follows:

According to this equation, the pH of a solution  buffer, depends on two factors:

a) The pKa value of the weak acid

b) The proportions between salt and acid concentrations  

In summary, the presence of the conjugate pair causes the weak species to dissociate to a lesser extent and the presence of the weak species causes the conjugate pair to hydrolyze less.

the mass of the cathode increases because ions from the solution get reduced to atoms and become part of the cathode.

explanation:

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