can someone please explain acid and base buffers to me like I am 5 years old? I am not understanding this...
When you add a bunch of a weak acid and its conjugate base to a solution (like, say, a bunch of acetic acid and acetate ions, or a bunch of HF and F- ions), the pH will be determined by the ratio acid/conjugate base. AKA, put some stuff in water, pH depends on how much of each.
When you add a small amount of a strong base, the weak acid soaks up the OH-, turning into the conjugate base. But, since there's a bunch of the acid and conjugate base, that little change doesn't affect the ratio acid/conjugate base much, so the pH doesn't change much.
When you add a small amount of a strong acid, the conjugate base soaks up the H+, turning into the weak acid. But, since there's a bunch of the acid and conjugate base, that little change doesn't affect the ratio acid/conjugate base much, so the pH doesn't change much.
Buffers are only effective for small amounts of strong acid or strong base additions. The more weak acid and conjugate base you add in the beginning, the more strong acid or strong base it can neutralize.
Buffers work best when the concentration of the weak acid and the concentration of the conjugate base are about the same. The pH of a buffer when those concentrations are exactly the same equals the pKa (-log of the acid dissociation constant) of the weak acid you're making the buffer out of.
Buffers also work with a weak base/conjugate acid.
To help understand buffers, make sure you understand weak acids and bases, conjugate acid/base pairs, and the common ion effect.
Did this help at all? I wasn't sure how much detail to put in.