Fe(OH)3 (s) <—> Fe3+(aq) + 3OH-(aq)
The Ksp expression for this solubility equation is the following:
Ksp =
[Fe3+][OH-]3
Ksp =
[Fe3+][OH-]3
6.3 x 10-38 =
[Fe3+][OH-]3
6.3 x 10-38 = [Fe3+](6.37 x
10-3)3
[Fe3+] = 2.44 x 10-31 M
Fe3+ from iron(iii) hydroxide has a solubility of 2.44 x 10-31 M in a solution of 6.37 x 10-3 M NaOH.
Now we use this information to find the solubility of S2-.
We first write the Ksp expression for the dissolution of Fe2S3 and then substitute the value of [Fe3+] that we calculated in the previous question to determine the solubility of [S2-]
Fe2S3 (s) <—> 2Fe3+(aq) + 3S2-(aq)
Ksp = [Fe3+]2 x [S2-]3
1.4 x 10-88 = (2.44 x 10-31)2 x [S2-]3
[S2-] = 1.33 x 10-9 M
could you please use the ksp values from this list Solid iron(III) hydroxide and solid iron(III)...
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