What is the molar solubility of fe(oh)3 in pure water? (ksp for fe(oh)3 is 4.0 x 10-38.) a. 6.5 x 10-7 m b. 4.5 x 10-10 m c. 4.0 x 10-17 m d. 2.0 x 10-10 m e. 3.4 x 10-13 m?

The molar solubility of Fe(OH)₃ in pure water is 2.0x10⁻¹⁰ M.

Explanation:

First, remember that the molar solubility of a compound is the maximum molar concentration of solute in a specific solvent. In this case, the solute is Fe(OH)₃ and the solvent is water.

- To calculate the molar solubility of a compound, we have to start by writing the dissociation reaction and make sure it is balanced. You can check the attachment for better understanding.

- The molar solubility of each dissociated species is represented by the letter "s" and multiply by its coefficient.

- The molar solubility is calculated from the Ksp of a compound. The Ksp is the Solubility Product Constant, so we have to make the product of molar solubility of each specie:

Kps = [Fe⁺³].[OH⁻]³

It is very important to raise to the power indicated by the coefficient the solubility of each specie when we write it in the Ksp equation.

After a few mathematical steps for clearing the solubility "s" we find that the result is 1.96x10⁻¹⁰ M that it is approximately to 2.0x10⁻¹⁰ M.

Note:

The molar solubility has units of molarity which is represented in chemistry by capital letter M not small letter m. Small letter m represents molality in chemistry. Molarity and molality are differents, be careful.

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