The equilibrium constant expression for the reaction shown below is
Ag3PO4(s) 3 Ag+(aq) + PO43− (aq)

Question

The equilibrium constant expression for the reaction shown below is
Ag3PO4(s)  3 Ag+(aq) + PO43− (aq)

BlackTom AI · Accepted Answer

The question asks for the equilibrium constant expression for the dissolution of a sparingly soluble solid: Ag3PO4(s) ⇌ 3 Ag+(aq) + PO4^3−(aq).
First, recall the general rule: for a heterogeneous equilibrium, the activities of pure solids and liquids are constant and are omitted from the Kc expression. Only the aqueous species appear in the expression.
Next, identify the species that are in aqueous solution at equilibrium: Ag+ and PO4^3−. The solid Ag3PO4 appears as a pure solid, so its activity is taken as 1 and does not appear in the numerator or denominator of Kc.
Then, apply the stoichiometry of the dissolution: for every mole of Ag3PO4 that dissolves, 3 moles of Ag+ and 1 mole of PO4^3− are produced. Therefore, the concentration terms in the Kc expression will be [Ag+]^3 and [PO4^3−].
Putting it together, the equilibrium constant expression is Kc = [Ag+]^3 [PO4^3−].
If you consider other possible forms that might appear in multiple choices, any expression that includes [Ag+]^3 multiplied by [PO4^3−] and excludes the solid Ag3PO4 from the denominator or numerator would be correct. Expressions that place the solid in a denominator or include extra species (like activities of species not present in the equilibrium) would be incorrect.
Be mindful that some erroneous forms might try to raise the solid’s activity to a fractional power or incorrectly balance the exponents, but the correct formulation strictly reflects the stoichiometry of the aqueous ions and omits the solid altogether.
In summary, the correct Kc expression captures three silver ions and one phosphate ion in the product side, giving Kc = [Ag+]^3 [PO4^3−], with Ag3PO4(s) not appearing in the expression.

The equilibrium constant expression for the reaction shown below is Ag3PO4(s) 3 Ag+(aq) + PO43− (aq)

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