Calculate percent relative error in hydronium ion concentration by using concentrations instead of activities in calculating pH of a solution of the following species using thermodynamic constants.
a) 0.100 M HOAc, and 0.200 M NaOAc
b) 0.0500 M NH3 and 0.200 M NH4Cl
c) 0.0100 M ClCH2COOH and 0.0600 M ClCH3COONa.
(a)
Henderson-Hasselbalch equation is expressed as
pH = pKa + log { [salt] / [Acid] }
pKa of HOAc = 4.75
pH = 4.75 + log ( 0.200/0.100)
= 4.75 + log 2
= 4.75 + 0.30
= 5.05
pH = 5.05
- log [H+] = 5.05
[H+] = 10-5.05 = 8.9 x 10-6
(b)
Henderson-Hasselbalch equation is expressed as
pOH = pKb + log { [salt] / [Base }
pkb of ammonia = 9.25
pOH = 9.25 + log (0.200 / 0.050)
= 9.25 + log 4
= 9.25 + 0.60
= 9.85
pH + pOH = 14
pH = 14 - pOH
= 14 - 9.85
= 4.15
pH = 4.15
- log [H+] = 4.15
[H+] = 10-4.15 = 7.1 x 10-5
(c)
Henderson-Hasselbalch equation is expressed as
pH = pKa + log { [salt] / [Acid] }
pKa of HOAc = 2.85
pH = 2.85 + log ( 0.060/0.010)
= 2.85 + log 6
= 2.85 + 0.78
= 3.63
pH = 3.63
- log [H+] = 3.63
[H+] = 10-3.63 = 2.3 x 10-4
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