In: Chemistry
Calculate pH for a strong acid/strong base titration.
Determine the pH during the titration of 39.8 mL of 0.334 M HI by 0.334 M KOH at the following points:
(a) Before the addition of any KOH-?
(b) After the addition of 19.9 mL of
KOH-?
(c) At the equivalence point-?
(d) After adding 47.8 mL of
KOH-?
a)when 0.0 mL of KOH is added
Given:
M(HI) = 0.334 M
V(HI) = 39.8 mL
M(KOH) = 0.334 M
V(KOH) = 0 mL
mol(HI) = M(HI) * V(HI)
mol(HI) = 0.334 M * 39.8 mL = 13.2932 mmol
mol(KOH) = M(KOH) * V(KOH)
mol(KOH) = 0.334 M * 0 mL = 0 mmol
We have:
mol(HI) = 13.29 mmol
mol(KOH) = 0 mmol
0 mmol of both will react
remaining mol of HI = 13.29 mmol
Total volume = 39.8 mL
[H+]= mol of acid remaining / volume
[H+] = 13.29 mmol/39.8 mL
= 0.334 M
use:
pH = -log [H+]
= -log (0.334)
= 0.4763
Answer: 0.476
b)when 19.9 mL of KOH is added
Given:
M(HI) = 0.334 M
V(HI) = 39.8 mL
M(KOH) = 0.334 M
V(KOH) = 19.9 mL
mol(HI) = M(HI) * V(HI)
mol(HI) = 0.334 M * 39.8 mL = 13.2932 mmol
mol(KOH) = M(KOH) * V(KOH)
mol(KOH) = 0.334 M * 19.9 mL = 6.6466 mmol
We have:
mol(HI) = 13.29 mmol
mol(KOH) = 6.647 mmol
6.647 mmol of both will react
remaining mol of HI = 6.647 mmol
Total volume = 59.7 mL
[H+]= mol of acid remaining / volume
[H+] = 6.647 mmol/59.7 mL
= 0.1113 M
use:
pH = -log [H+]
= -log (0.1113)
= 0.9534
Answer: 0.954
c)
Since this is titration of strong acid and strong base,
the pH will be 7.00 at equivalence point
Answer: 7.00
d)when 47.8 mL of KOH is added
Given:
M(HI) = 0.334 M
V(HI) = 39.8 mL
M(KOH) = 0.334 M
V(KOH) = 47.8 mL
mol(HI) = M(HI) * V(HI)
mol(HI) = 0.334 M * 39.8 mL = 13.2932 mmol
mol(KOH) = M(KOH) * V(KOH)
mol(KOH) = 0.334 M * 47.8 mL = 15.9652 mmol
We have:
mol(HI) = 13.29 mmol
mol(KOH) = 15.97 mmol
13.29 mmol of both will react
remaining mol of KOH = 2.672 mmol
Total volume = 87.6 mL
[OH-]= mol of base remaining / volume
[OH-] = 2.672 mmol/87.6 mL
= 3.05*10^-2 M
use:
pOH = -log [OH-]
= -log (3.05*10^-2)
= 1.5157
use:
PH = 14 - pOH
= 14 - 1.5157
= 12.4843
Answer: 12.48