How do solubility rules help us identify which product is the solid?

Question

Caleb Adams · Accepted Answer

I am not quite sure what you are after......

For evaluating solubilities in aqueous solution, the following general guidelines apply: Ammonium and all of the alkali metal salts are soluble. Each and every nitrate and perchlorate is soluble. All halides are soluble EXCEPT for # AgX, Hg_2X_2, PbX_2"#. All sulfates are soluble EXCEPT for #PbSO_4, BaSO_4, HgSO_4#. Every sulfide is insoluble, as are all carbonates and hydroxides. The given rules follow a hierarchy. Alkali metal and ammonium salts tend to be soluble in all circumstances. The one exception to this rule is #K^(+)""^(-)BPh_4# and #NH_4^(+)""^(-)BPh_4#, both of which are as soluble as bricks. #Na^+""^(-)BPh_4#, the which has some aqueous solubility, is sold as #"kalignost"#, i.e. #"potassium recognizer"#.............

Cameron Andrews · Answer

undefined Solubility rules help us identify which product is the solid by determining which combinations of ions will form insoluble compounds, thus precipitating out of solution. By referring to solubility rules, we can predict the formation of a solid product based on the ions present in the reaction and their respective solubilities.