The hydronium ion concentration of an aqueous solution of
0.359 M triethanolamine (a weak base with
the formula C6H15O3N) is
...
kb for triethanolamine = 5.8*10^-7
C6H15O3N dissociates as:
C6H15O3N -----> C6H15O3NH+ + OH-
0.359 0 0
0.359-x x x
Kb = [C6H15O3NH+][OH-]/[C6H15O3N]
Kb = x*x/(c-x)
Assuming x can be ignored as compared to c
So, above expression becomes
Kb = x*x/(c)
so, x = sqrt (Kb*c)
x = sqrt ((5.8*10^-7)*0.359) = 4.563*10^-4
since c is much greater than x, our assumption is correct
so, x = 4.563*10^-4 M
use:
[H+] = (1.0*10^-14)/[OH-]
[H+] = (1.0*10^-14)/4.563*10^-4
[H+] = 2.19*10^-11 M
Answer: 2.19*10^-11 M
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