Is a buffer supposed to keep the pH of a solution at 7?
1 Answer
Sometimes, but usually no.
It just keeps the pH from changing much, and is centered around the pKa of the acid used to make the buffer.
Let's say we made an acetic acid buffer, where the concentration of acetic acid was
Acetic acid is
Using the Henderson-Hasselbalch equation (which you will see often with buffers), we get:
#\mathbf("pH" = "pKa" + log \frac(["A"^(-)])(["HA"]))#
#"pH" = "pKa" + log \frac(["CH"_3"COO"^(-)])(["CH"_3"COOH"])#
#"pH" = 4.76 + log (("1.00 M")/("0.500 M"))#
#"pH" = 4.76 + 0.301029996#
#color(blue)("pH" ~~ 4.79)#
So, with a buffer like this, you should expect the pH to stay generally close to or return to something close to
If it were to become