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 reaction shown is a solid dissociating: Ag3PO4(s) ⇌ 3 Ag+(aq) + PO4^3−(aq). In equilibrium expressions, pure solids and liquids are not included; their activity is set to 1 and thus do not appear in the Kc expression.
Option 1: Kc = [Ag+]^3 [PO4^3−] / [Ag3PO4]. This option wrongly includes the solid in the denominator. Since solids are omitted from Kc, this form is incorrect.
Option 2: Kc = [Ag+]^3 [PO4^3−]. This is the correct form because it uses the product concentrations raised to their stoichiometric powers (3 for Ag+) and 1 for PO4^3−, and omits the solid entirely as required.
Option 3: Kc = [Ag3PO4] / ([Ag+]^3 [PO4^3−]). This is the reciprocal of the correct expression and incorrectly places the reactant solid in the numerator, so it is incorrect.
Option 4: Kc = 1 / ([Ag+]^3 [PO4^3−]). This form inverts the correct expression and ignores the solid’s exclusion, making it incorrect.

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

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