37. determine whether each compound is soluble or insoluble. if the compound is soluble, list the ions…

Explanation:

Step1: Recall solubility rules

Silver nitrate ($\ce{AgNO3}$) is soluble because all nitrates ($\ce{NO3^{-}}$) are soluble in water. When it dissolves, it dissociates into $\ce{Ag^{+}}$ and $\ce{NO3^{-}}$ ions.

Step2: Analyze lead - acetate

Lead acetate ($\ce{Pb(C2H3O2)2}$) is soluble. Acetates ($\ce{C2H3O2^{-}}$) are generally soluble, and it dissociates into $\ce{Pb^{2 + }}$ and $\ce{C2H3O2^{-}}$ ions.

Step3: Examine potassium nitrate

Potassium nitrate ($\ce{KNO3}$) is soluble. All nitrates are soluble, and it dissociates into $\ce{K^{+}}$ and $\ce{NO3^{-}}$ ions.

Step4: Consider ammonium sulfide

Ammonium sulfide ($\ce{(NH4)2S}$) is soluble. All ammonium - containing compounds ($\ce{NH4^{+}}$) are soluble, and it dissociates into $\ce{NH4^{+}}$ and $\ce{S^{2 - }}$ ions.

Answer:

a. Soluble; $\ce{Ag^{+}}$, $\ce{NO3^{-}}$ b. Soluble; $\ce{Pb^{2 + }}$, $\ce{C2H3O2^{-}}$ c. Soluble; $\ce{K^{+}}$, $\ce{NO3^{-}}$ d. Soluble; $\ce{NH4^{+}}$, $\ce{S^{2 - }}$