Answer:
c.
![Kc = ([Ag(NH_(3))_2^(+)][Cl^-])/([NH_3]^2)}](https://img.qammunity.org/2021/formulas/chemistry/college/rv84zgbfjwwokjrq1qas4u93he0hyt4mf9.png)
d.
![Kc = [Ba^(2+)][F^(-)]^2](https://img.qammunity.org/2021/formulas/chemistry/college/sc5zvfdw4rsi3wxxedhgkk0ytjd85sscov.png)
Step-by-step 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.
The reaction must be: NH₃(aq) + H₂O(l) ⇆ NH₄⁺(aq) + OH⁻(aq) All reactants are in the same phase.
b.
![Kc = ([H^+][C_2H_3O_(2)^-])/([HC_2H_3O_2])}](https://img.qammunity.org/2021/formulas/chemistry/college/6hchuw5k91m72vij204l7m2ztsmrn84ccj.png)
The reaction must be: HC₂H₃O₂(aq) ⇄ H⁺(aq) + C₂H₃O₂⁻(aq) All reactants are in the same phase.
c.
![Kc = ([Ag(NH_(3))_2^(+)][Cl^-])/([NH_3]^2)}](https://img.qammunity.org/2021/formulas/chemistry/college/rv84zgbfjwwokjrq1qas4u93he0hyt4mf9.png)
The reaction must be: 2NH₃(aq) + AgCl(s) ⇄ Ag(NH₃)₂⁺(aq) + Cl⁻(aq)
Reactants aren´t in the same phase. Heterogeneous equilibrium
d.
![Kc = [Ba^(2+)][F^(-)]^2](https://img.qammunity.org/2021/formulas/chemistry/college/sc5zvfdw4rsi3wxxedhgkk0ytjd85sscov.png)
The reaction must be: BaF₂(s) ⇆ Ba²⁺(aq) + 2F⁻(aq)
Reactants aren´t in the same phase. Heterogeneous equilibrium
I hope it helps!