Question

What will be the pH of a buffer solution containing an acid of pKa7.5, with an acid concentration exactly one fourth of that of the conjugate base

Answer 1

Answer: pH of buffer solution is 8.1

Step-by-step explanation:

The formula for the Henderson–Hasselbalch equation is:

`pH=pK_a+\log([A^-])/([HA])`

`pH` is the concentration of
`[H^+]`

`pK_a` is the acid dissociation constant,

`A^-` and
`HA` are concentrations of the conjugate base and starting acid.

Putting in the values we get:

`pH=7.5+\log(x)/((x)/(4))`

`pH=8.1`

Thus pH of buffer solution is 8.1