A-level Chemistry/OCR (Salters)/Buffer solutions

Calculating the pH of a buffer solution edit

 

Derivation edit

For any equilibrium

 

the equilibrium constant, K, is defined as

 

Therefore, for the dissociation equilibrium of any acid

 

the acid dissociation constant, Ka, is defined as

 

This equation can be rearranged to make [H+(aq)] the subject:

 

Two assumptions are required:

1 Every A ion comes from the salt

Although this is not quite true, it is a close enough that the pH value we get from the final equation is very close to that found experimentally. It allows us to assume that
 

2 Every HA molecule remains undissociated

Again, despite being slightly inaccurate, this assumption creates the following useful equation
 

The equations in assumptions 1 and 2 allow us to replace [A(aq)] with [salt] and [HA(aq)] with [acid] as follows.

The effect of assumption 1 is that

 

becomes

 

The effect of assumption 2 is that

 

becomes

 

By definition,

 

so