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When two aqueous solutions of soluble ionic compounds mix, the dissociated ions from each solution combine in the resulting mixture. Oppositely charged ions attract each other and may form new ionic products. If one of these products is insoluble, it precipitates from the solution as a solid. This type of reaction is called a precipitation reaction or double displacement reaction.

Solubility rules indicate whether ionic compounds are water-soluble or water-insoluble. By applying these rules, you can identify which ionic products formed from mixed solutions will precipitate. For example, all nitrate salts are soluble, but most silver salts are insoluble exceptions. Using these guidelines, you can predict whether a precipitation reaction will occur before mixing solutions.

A precipitate is an insoluble ionic solid that forms when aqueous solutions of two ionic compounds react. It remains undissolved in the solution and can be visually observed as a solid. The precipitate can be separated from the liquid solution through filtration, which traps the solid particles while allowing the dissolved ions to pass through.

A precipitation reaction is called a double displacement or salt metathesis reaction because the positive and negative ions of two ionic reactants exchange partners. In the reaction between sodium chloride and silver nitrate, sodium cations pair with nitrate anions while silver cations pair with chloride anions, forming two new ionic products through this ion exchange process.

Water-soluble ionic compounds dissolve in water by dissociating into individual ions, which are then surrounded by water molecules to form an aqueous solution. Water-insoluble ionic compounds do not dissolve and remain as undissociated solids in aqueous solutions. When an insoluble compound forms from mixing two solutions, it precipitates out as a visible solid.

The molecular equation for a precipitation reaction shows all reactants and products in their complete chemical form. For example, the equation for sodium chloride reacting with silver nitrate shows aqueous sodium chloride and silver nitrate producing aqueous sodium nitrate and solid silver chloride. This equation represents the overall reaction before considering which ions actually participate in forming the precipitate.

In solution, dissociated ions from soluble ionic compounds are surrounded by water molecules and remain dissolved. When two solutions are mixed, all four ions from both compounds are present in the resulting solution. Oppositely charged ions are attracted to each other, but they remain separated by water molecules until conditions allow them to overcome this attraction and bind together to form an insoluble precipitate.