Final answer:
When LiBr, K₂SO₄, Ca(NO₃)₂, and NaC₂H₃O₂ are combined in water, no precipitate forms as all resulting compounds from potential double-replacement reactions are soluble according to solubility rules.
Step-by-step explanation:
The question revolves around predicting which compound precipitates when specific aqueous solutions are mixed. To determine the precipitate, we look to solubility rules and conduct a double-replacement reaction analysis. In the scenario where LiBr, K₂SO₄, Ca(NO₃)₂, and NaC₂H₃O₂ are combined, no precipitates will form because all the possible products of these reactants are soluble in water according to solubility rules.
For example, if we consider a potential double-replacement reaction between Ca(NO₃)₂ and K₂SO₄, the two possible products would be CaSO₄ and KNO₃. However, since both calcium nitrate and potassium sulfate are soluble, no precipitate forms. In another instance, when alkali metal ions are among the reactants, we can apply the solubility rule that all compounds containing alkali metal ions are soluble, which supports the conclusion that no precipitate will form in this mixture.