Write the balanced equation and solubility product expression for the solubility equilibrium of Mn3(PO4)2: i thought the answer was

Mn3(PO4)2 (s) = Mn^2+(aq) + (PO4)2 ^3- (aq) but that's not right. then for the Ksp expression i thought it was [Mn^2+] [PO4]^2

I responded to your post below.

To write the balanced equation for the solubility equilibrium of Mn3(PO4)2, we first need to break apart the compound into its ions, taking into account their charges:

Mn3(PO4)2 (s) → 3 Mn^2+ (aq) + 2 (PO4)^3- (aq)

The balanced equation indicates that when solid Mn3(PO4)2 dissociates in water, it forms three Mn^2+ ions and two (PO4)^3- ions in the aqueous solution.

Now, let's move on to the solubility product expression (Ksp) for Mn3(PO4)2. The solubility product expression relates to the equilibrium expression and is an expression for the equilibrium constant (Ksp) of the dissociation reaction.

Ksp is the product of the concentrations (raised to the power of their stoichiometric coefficients) of the ions involved in the equilibrium. In this case, the expression would be:

Ksp = [Mn^2+]^3 * [(PO4)^3-]^2

The concentration of each ion is raised to the power of its stoichiometric coefficient to account for the balanced equation. In this case, Mn^2+ has a coefficient of 3, and (PO4)^3- has a coefficient of 2.

So, the correct balanced equation for the solubility equilibrium of Mn3(PO4)2 is:

Mn3(PO4)2 (s) → 3 Mn^2+ (aq) + 2 (PO4)^3- (aq)

And the correct solubility product expression (Ksp) for Mn3(PO4)2 is:

Ksp = [Mn^2+]^3 * [(PO4)^3-]^2