The Ksp for #Fe(OH)_3# = #2.5 x 10^-20#. How would you find the Ksp equation in terms of #Fe^+3# and #OH^-# concentrations?

Answer 1

#K_(sp)=[Fe^(3+)][HO^-]^3#

(i) A chemical equation is required.

#Fe(OH)_3(s) rightleftharpoons Fe^(3+) + 3HO^-#
And (ii) a #K_(sp)# expression:
#K_(sp)=[Fe^(3+)][HO^-]^3#
Given the normal conventions, i.e. if #S# represents solubility etc., then,
#K_(sp)=[S][3S]^3# #=# #27S^4# #=# #2.5xx10^-20#.
#S=""^4sqrt{(2.5xx10^-20)/(27)}#

Of course, the concentration of iron or hydroxide ions may already be artificially elevated.

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Answer 2

The Ksp equation for Fe(OH)3 is: Ksp = [Fe^3+][OH^-]^3

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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