out? 2. Assuming your buffered solution contains acetic acid, HOAc, and the sodi
ID: 542576 • Letter: O
Question
out? 2. Assuming your buffered solution contains acetic acid, HOAc, and the sodium salt of its conjugate base, NaOAc. Show the net ionic equations that occur when this buffered solution reacts with: (a) added strong acid, H, or (b) added strong base, OH- Biochemists and biologists often use the Henderson-Hasselbalch equation in working with buffers: 3. pH = pKa + log IAT [HA HA + NaOH H2O + Na+ A- When an acid solution is half-neutralized, half of the HA has been converted to A-, and half of it is still in the form of HA. Therefore [HA] [A- What happens to the Henderson-Hasselbalch equation when [HA] equals (A -]? How is it simplified? 89Explanation / Answer
2)
on addition of acid (H+) :
in the buffer on addition of acid the OAc- ion react with H+ forms acid . it is also buffer of the soluton .
H+ + OAc- --------------------------> HOAc
on addition of base OH-
net ionic reaction
HOAc + OH- -----------------------------> OAc- + H2O
3)
pH = pKa + [A- / HA]
if [ A- ] = [ HA ]
pH = pKa + log [A- / A-]
pH = pKa + log (1)
pH = pKa
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