The hydronium ion concentration of an aqueous solution of 0.530 M hydroxylamine (a weak base with...

The hydronium ion concentration of an aqueous solution of 0.530 M hydroxylamine (a weak base with the formula NH₂OH) is ...

[H₃O⁺] = ____M

Expert Solution

kb of hydroxylamine = 1.1*10^-8

NH2OH dissociates as:

NH2OH +H2O     ----->     NH2+   +   OH-
0.53                   0         0
0.53-x                 x         x

Kb = [NH2+][OH-]/[NH2OH]
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 ((1.1*10^-8)*0.53) = 7.635*10^-5

since c is much greater than x, our assumption is correct
so, x = 7.635*10^-5 M

use:
[H3O+] = (1.0*10^-14)/[OH-]
[H3O+] = (1.0*10^-14)/7.635443667528429E-5
[H3O+] = 1.31*10^-10

Answer: 1.31*10^-10 M

queen_honey_blossom answered 2 years ago

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