Answer:
Mixing any cation with any anion will NOT always lead to the formation of an insoluble ionic compound.
Explanation:
Ionic compounds are compounds that have cations and anions.
A polar molecule is one that is neutral, that is, it does not have a net charge. But it has an internal distribution of charges that form a partially positive region and a partially negative region.
Given that "the like dissolves the like" and that water is a polar molecule, it is possible to say that water is good for dissolving ions and polar molecules, but bad for dissolving non-polar molecules.
Water molecules are polar, with positive partial charges on hydrogen, a partial negative charge on oxygen and a general angular structure. Its distribution of charges is due to the greater electronegativity of oxygen with respect to hydrogen, which makes the shared electrons of the O-H bonds more attracted by the O atom than by the H atom.
Precipitation of a poorly soluble ionic compound can occur when two solutions are mixed in which each one contains one of the ions that form said compound.
For example, silver chloride, AgCl is a very insoluble salt. When mixing a solution of silver nitrate, AgNO3, which contains the Ag+ ion, with another solution of sodium chloride containing the Cl– ion, precipitation of AgCl occurs.
But mixing any cation with any anion will not always lead to the formation of an insoluble ionic compound. For example, table salt, which is an ionic compound of the NaCl formula, should be considered. This salt dissociates in water in Na+ and Cl-. The positively charged Na+ ions are surrounded by the negative partial oxygen charges of the water molecules, while the negatively charged ions are surrounded by the hydrogen ends with a positive partial charge. In this way the solubility of the ionic compound is produced.
Finally, mixing any cation with any anion will NOT always lead to the formation of an insoluble ionic compound.
