Please help me answer the following problem: I have 30.0 mL of a 0.100 M solutio
ID: 955195 • Letter: P
Question
Please help me answer the following problem: I have 30.0 mL of a 0.100 M solution of a weak acid in a flask, and I am planning to titrate this weak acid (3-nitrophenol) with a 0.300 M solution of NaOH. I need to calculate the following.
A.) Volume at the equivalence point.
B.)The starting pH of nitrophenol-3.
C.) The pH when 1 mL of NaOH has been added.
D.) The pH and 1/2 Ve.
E.) The pH 1 mL before the equivalence point.
F)The pH at the equivalence point.
G) The pH 1 ml after the equivalence point.
H) The pH 10 mL after the equivalence point..
Please add as much detail as you can! Thank you
Explanation / Answer
3-nitrophenol (acid) , pKa value = 8.36
A.) Volume at the equivalence point.
at equivalence point millimoles of acid (phenol compound) = millimoles of base
30 x 0.1 = V x 0.3
V = 10 mL
NaOH volume at the equivalence point = 10 mL
B.)The starting pH of nitrophenol-3.
C = 0.1 M
pKa = 8.36
pH = 1/2 [pKa -logC]
pH = 1/2 (8.36 - log 0.1)
pH = 4.68
C.) The pH when 1 mL of NaOH has been added.
millimoles of acid = 30 x 0.1 = 3
millimoles of NaOH = 1 x 0.3 = 0.3
acid + OH- ----------------------> salt
3 0.3 0 --------------------> initial
2.7 0 0.3 ------------------> after reaction
pH = pKa + log [salt /acid]
pH = 8.36 + log (0.3 /2.7)
pH = 7.41
D.) The pH and 1/2 Ve.
at this point
pH = pka
pH = 8.36
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