Answer:
c. [tex]Kc = \frac{[Ag(NH_{3})_2^{+}][Cl^-]}{[NH_3]^2}}[/tex]
d. [tex]Kc = [Ba^{2+}][F^{-}]^2[/tex]
Explanation:
An heterogeneous equilibrium is defined as a system whose reactants, products, or both are in more than one phase.
Also, you must know in an equilibrium constant you don't take solids or pure liquids. Thus:
a. [tex]Kc = \frac{[NH_{4}^+][OH^-]}{[NH_3]}}[/tex]
The reaction must be: NH₃(aq) + H₂O(l) ⇆ NH₄⁺(aq) + OH⁻(aq) All reactants are in the same phase.
b. [tex]Kc = \frac{[H^+][C_2H_3O_{2}^-]}{[HC_2H_3O_2]}}[/tex]
The reaction must be: HC₂H₃O₂(aq) ⇄ H⁺(aq) + C₂H₃O₂⁻(aq) All reactants are in the same phase.
c. [tex]Kc = \frac{[Ag(NH_{3})_2^{+}][Cl^-]}{[NH_3]^2}}[/tex]
The reaction must be: 2NH₃(aq) + AgCl(s) ⇄ Ag(NH₃)₂⁺(aq) + Cl⁻(aq)
Reactants aren´t in the same phase. Heterogeneous equilibrium
d. [tex]Kc = [Ba^{2+}][F^{-}]^2[/tex]
The reaction must be: BaF₂(s) ⇆ Ba²⁺(aq) + 2F⁻(aq)
Reactants aren´t in the same phase. Heterogeneous equilibrium
I hope it helps!
