The amount of HCl needed for complete titration of tri methyl aniline is 50 X 0.125 = (V) X 0.175
V = 35.714 ml
1. Insert values into the Kb expression for acetic acid. The Kb for tri methyl amine is 6.3 x 10-5.
6.3 x 10-5 = [(x) (x)] / 0.125
x = 2.807 x 10-3 M
pOH = 2.5517
pH = 11.4482
2.
1. Calculate moles of acid and base in solution before reaction:
(CH3)3N : 6.25 x 10-3 mol
HCl : (0.0015 L) (0.175 mol/L) = 2.625 x 10-3 mol
2) Determine amounts of base and tri methyl ammonium ion after reaction:
(CH3)3N : 6.25 x 10-3 mol -
2.625 x 10-3 mol = 3.625 x 10-3 mol
(CH3)3NH+ : 2.625 x
10-3 mol
3) Use Henderson-Hasselbalch equation to determine pOH of buffered solution:
pOH = pKb + log (salt/base)
pOH = 4.2 + log (2.625 x 10-3 / 3.625 x 10-3)
pOH = 4.2 + log 0.724
pOH = 4.059
pH = 14 - 4.059 = 9.94
3.
The solution is now completely composed of a salt of a weak base. The pH of this solution will be acidic.
1) Calculate molarity of tri methyl ammonium ions:
6.25 x 10-3 mol / 0.085714 L = 0.0729 M
2) Calculate the Ka of tri methyl ammonium
Kw = KaKb
1.00 x 10-14 = (x) (6.25 x 10-5 )
x = 1.587 x 10-10
3) Calculate pH of the solution:
1.587 x 10-10 = [(x) (x)] / (0.0729-x)
x = 0.34 x 10-5 M
pH = 4.53147
4. After adding 35.714 ml of HCl the amount of tri methyl aniline the total amount is titrated and after that addition of HCl indicates the accumuation of H+ ions in the solution and the resultant solution will be acidic In nature.
The concentration of H+ ions is obtained by using (MacidVacid - MbaseVbase) / (Vacid + Vbase )
[H+] = ((0.175 X 45 ) - (50 X 0.125)) / (50 + 45) = 0.01710
pH = - log[H+] = 1.767
5. Addition of more amount of HCl results in addition of more amount of H+ ions accumulation and a greater increase in pH
[H+] = ((0.175 X 60) - (50 X 0.125)) / (50 + 60) = 0.038636
pH = - log[H+] = 1.413
The data used to draw the graph are volume of the amount of HCl added to tri methyl aniline
Volume of HCl added pH of the resulting solution
intially 0 ml 11.4482
5 ml 10.5884
10 ml 10.210
15 ml 9.94
20 ml 9.695
25 ml 9.432
30 ml 9.0798
35 ml 8.1098
35.714 ml 4.53147
40 ml 2.079
45 ml 1.767
60 ml 1.413
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