Above what Fe? concentration will Fe(OH)a precipitate from a buffer solution that has a pH of 8.32? The Ksp of Fe(OH)2 is 4.8710 Number 1.223x 105 M
Solution
use:
pH = -log [H+]
8.32 = -log [H+]
[H+] = 4.786*10^-9 M
use:
[OH-] = Kw/[H+]
Kw is dissociation constant of water whose value is 1.0*10^-14 at 25 oC
[OH-] = (1.0*10^-14)/[H+]
[OH-] = (1.0*10^-14)/(4.786*10^-9)
[OH-] = 2.089*10^-6 M
At equilibrium:
Fe(OH)2 <----> Fe2+ + 2 OH-
s 2.089*10^-6
Ksp = [Fe2+][OH-]^2
4.87*10^-17=(s)*(2.089*10^-6)^2
4.87*10^-17= (s) * 4.364*10^-12
s = 1.12*10^-5 M
Answer: 1.12*10^-5 M
.
Model Call Girl in Tilak Nagar Delhi reach out to us at 🔝9953056974🔝
Above what Fe- concentration will Fe(OH)a precipitate from a buffer so.docx
1. Above what Fe? concentration will Fe(OH)a precipitate from a buffer solution that has a pH of
8.32? The Ksp of Fe(OH)2 is 4.8710 Number 1.223x 105 M
Solution
use:
pH = -log [H+]
8.32 = -log [H+]
[H+] = 4.786*10^-9 M
use:
[OH-] = Kw/[H+]
Kw is dissociation constant of water whose value is 1.0*10^-14 at 25 oC
[OH-] = (1.0*10^-14)/[H+]
[OH-] = (1.0*10^-14)/(4.786*10^-9)
[OH-] = 2.089*10^-6 M
At equilibrium:
Fe(OH)2 <----> Fe2+ + 2 OH-
s 2.089*10^-6
Ksp = [Fe2+][OH-]^2
4.87*10^-17=(s)*(2.089*10^-6)^2
4.87*10^-17= (s) * 4.364*10^-12
![Above what Fe? concentration will Fe(OH)a precipitate from a buffer solution that has a pH of
8.32? The Ksp of Fe(OH)2 is 4.8710 Number 1.223x 105 M
Solution
use:
pH = -log [H+]
8.32 = -log [H+]
[H+] = 4.786*10^-9 M
use:
[OH-] = Kw/[H+]
Kw is dissociation constant of water whose value is 1.0*10^-14 at 25 oC
[OH-] = (1.0*10^-14)/[H+]
[OH-] = (1.0*10^-14)/(4.786*10^-9)
[OH-] = 2.089*10^-6 M
At equilibrium:
Fe(OH)2 <----> Fe2+ + 2 OH-
s 2.089*10^-6
Ksp = [Fe2+][OH-]^2
4.87*10^-17=(s)*(2.089*10^-6)^2
4.87*10^-17= (s) * 4.364*10^-12](https://image.slidesharecdn.com/abovewhatfe-concentrationwillfeohaprecipitatefromabufferso-230128035313-45cd2f63/85/above-what-fe-concentration-will-feoha-precipitate-from-a-buffer-sodocx-1-320.jpg)
