Can the italicized portion of the problem be explained? I understand up until the 0.015 moles of protonated acetic acid remained and I understand the HH portion of the problem after but I would like some clarity on how this number was concluded.
2. The following question has two parts.
a) What is the final pH of a solution obtained by mixing 250 ml of
0.3 M acetic acid with 300 ml
of 0.2 M KOH? (pKb of acetate = 9.24). (Show your work!)
Moles of acetic acid = 0.25 l X 0.3 M = 0.075
moles
Adding 0.3 l X 0.2 M = 0.06 moles of OH- to this solution will
convert 0.06 moles of acetic
acid to 0.06 moles of acetate, 0.015 moles of protonated acetic acid will remain. pKa = 14 - pKb = 14 - 9.24 = 4.76
pH = pKa + log [CH3CO2-][CH3CO2H]
= 4.76 + log 0.06 moles / 0.55 l 0.015 moles / 0.55 l
= 4.76 + log 0.06 moles0.015 moles
= 5.36
pH = 5.36
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