Buffering capacity refers to the effectiveness of commercial antacids the extent to which a buffer solution can counteract the effect of added acid or base the ph of a buffer solution the molecular weight of the substance used as a buffer

 The extent to which a buffer solution can counteract the effect of added acid or base    

Explanation:

A buffer is a solution that is able to resist pH change when a limited amount of acid or base is added. This is because it is can neutralize them and maintain the pH of the solution stable.

The composition of a buffer solution entails a weak base or a weak acid accompanied by its conjugate salt. So a buffer is able to resist changes in its pH due to the addition of an acid or base though consumption of the buffer.

For example, a buffer could be composed of ammonia NH3 (weak base) and  ammonium NH4+ (conjugate acid). If HCl is added to it, the ammona takes the acid's proton to become NH4+. Because that proton is locked up in the ammonium ion, it can not increase the pH of the solution. Them if we add NaOH (a base) to that same buffer, the ammonium ion donates a proton to it to become ammonia. This means, a buffer works by replacing a strong acid or base with a weak one.

Thereby, buffer capacity refers to the quantity of a strong base or strong acid that must be added to one liter of a buffer solution to change it by one pH unit. It means, the buffer capacity measures its efficiency in resisting changes in pH.

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