The solubility product (Ksp) is the equilibrium expression for the dissociation of a substance in a dissolving medium (like water). Ksp for a substance is useful because it provides information about its solubility. Ksp 1 means the substance is soluble, if Ksp is very small, the substances is sparingly soluble. When CaF2 is added to water it dissociates as per the following reaction Al(OH)3(s) → Al3+(aq) + 3OH-(aq)Which of the following is the correct expression for the solubility product of Al(OH)3?

Question

The solubility product (Ksp) is the equilibrium expression for the dissociation of a substance in a dissolving medium (like water). Ksp for a substance is useful because it provides information about its solubility. Ksp > 1 means the substance is soluble, if Ksp is very small, the substances is sparingly soluble. When CaF2 is added to water it dissociates as per the following reaction Al(OH)3(s) →  Al3+(aq) +  3OH-(aq)Which of the following is the correct expression for the solubility product of Al(OH)3?

BlackTom AI · Accepted Answer

The question asks for the correct expression of the solubility product Ksp for Al(OH)3(s) dissociating to Al3+ and OH− in water. 
First, recall the dissolution: Al(OH)3(s) ⇌ Al3+(aq) + 3 OH−(aq). For a sparingly soluble salt, Ksp is the product of the concentrations of the dissolved ions, each raised to the power of its stoichiometric coefficient in the dissolution equation. 
Option a presents [Al^3+][OH−]^3 over 1, which matches the stoichiometry: one Al3+ ion and three OH− ions are produced per formula unit dissolved, so you multiply [Al3+] by ([OH−])^3. This aligns exactly with the definition of Ksp for this salt. 
Option b places [Al^3+][3OH−] in the numerator and divides by [Al(OH)3], which is incorrect because Ksp does not involve the solid activity in the denominator and it should raise OH− to the power of 3, not multiply by 3. 
Option c has [Al^3+][30H−]^3 in the numerator, which is a typographical error (30H− is not a valid species) and also misrepresents the stoichiometry with an extraneous numerical multiplier. 
Option d includes [Al(OH)3] in the denominator and also includes [H2O] in the denominator, which is not part of the Ksp expression; Ksp only involves the dissolved ionic species. 
Option e writes [Al^3+][OH−]^3 but divides by [Al(OH)3], which is incorrect for the same reason as option d; the solid is not in the denominator of Ksp. 
Option f uses [30OH−] (which is not a valid species) and places it incorrectly in the numerator, and similarly ignores the proper product form for Ksp. 
Thus, the only expression that faithfully represents the solubility product for Al(OH)3(s) with the proper stoichiometry is the one that uses [Al^3+] times [OH−]^3 in the numerator, without any solid or water terms in the denominator.

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