Which equation represents what happens when a small amount of strong base is added to the buffer?

OH- + A- A2- + H2O


OH- + HA A- + H2O


H3O+ + A- HA + H2O


H3O+ + HA H2A+ + H2O

OH- + HA A- + H2O

Kyleigh, Esmeralda, Jameson -- Please stop switching names. Doing so won't get you help any sooner than anyone else.

To follow up on Writeacher's comment, I've looked at your other posts with different screen names and I don't see any effort on your part at all. If you will go back to those posts, tell us what you don't understand about the problem and/or how you think the solution should be approached, someone here will be glad to help you through each of them. The bottom line is that I don't want to spend the next hour answering them in detail when I don't know if I'm helping or not. I may be explaining something you already know

Ok, sure. I added some more info to my previous questions. Please take a look. Thank you for your help!

To determine which equation represents what happens when a small amount of strong base is added to the buffer, we need to understand the behavior of a buffer solution.

A buffer solution is a solution that resists changes in pH when small amounts of acid or base are added. It typically consists of a weak acid (HA) and its conjugate base (A-).

When a small amount of strong base is added to a buffer, it reacts with the weak acid component and forms water along with the conjugate base. The equation representing this reaction is:

OH- + HA A- + H2O

In this equation, OH- represents the strong base and HA represents the weak acid. A- is the conjugate base and H2O is water. The weak acid donates a proton (H+) to the strong base, forming water and the conjugate base.

Therefore, the correct equation that represents what happens when a small amount of strong base is added to the buffer is:

OH- + HA A- + H2O