What is the concentration of [Fe3+] in a saturated solution of Fe(OH)3 given that Ksp(Fe(OH)3) = 2.64 x 10^-39?
Solution:
Fe(OH)3--> Fe3+ + 3OH-
Ksp= [Fe3+][OH-]^3
= [x] [3x]^3
=27x^4
2.64 x 10^-39 = 27x^4
(2.64/27) x 10^-39= x^4
I'm stuck here!!! Please explain why the [OH] is raised to the third power in Equilibrium constant AND how the heck do I solve for x when x is raised to the 4th power??
Solution:
Fe(OH)3--> Fe3+ + 3OH-
Ksp= [Fe3+][OH-]^3
= [x] [3x]^3
=27x^4
2.64 x 10^-39 = 27x^4
(2.64/27) x 10^-39= x^4
I'm stuck here!!! Please explain why the [OH] is raised to the third power in Equilibrium constant AND how the heck do I solve for x when x is raised to the 4th power??