# Question #7507c

##### 1 Answer

The weak acid to conjugate base ratio for your buffer will be **8.70**.

So, you're dealing with a buffer that consists of acetic acid,

Once again, the **Henderson-Hasselbalch equation** will be your tool of choice.

Start by calculating the

Notice that the pH of the buffer is *lower* than the *higher* than that of the weak base, since the solution is *more acidic* than the

This implies that the ratio you're looking for, weak acid to conjugate base, will be *greater than 1*.

So, plug your data into the Henderson - Hasselbalch equation

This is equivalent to

So, the ratio *conjugate base to weak acid* ratio is

This means that the *weak acid to conjugate base* ratio will be

Rounded to three sig figs, the answer will be

The initial prediction turned out to be correct, you do have more weak acid than conjugate base *at that* pH.