This simplifies the above equations to the following: In this case, any spectator ions (those which do not contribute to the reaction) are left out of the formula completely. This reaction can be written emphasizing the dissociated ions in a combined solutionĪg +(aq) + NO 3 -(aq) + K +(aq) + Cl -(aq) → AgCl(solid) + K +(aq) + NO 3 -(aq)Ī final way to represent a precipitate reaction is known as a net ionic reaction. The silver chloride(AgCl) has formed a solid, which is observed as a precipitate. If this energy is not available, and no suitable nucleation surface is available, supersaturation occurs.Īn example of a precipitation reaction: Aqueous silver nitrate (AgNO 3) is added to a solution containing potassium chloride (KCl) and the precipitation of a white solid, silver chloride is observed. The creation of a hypothetical solid particle includes the formation of an interface, which requires some energy based on the relative surface energy of the solid and the solution. Precipitation from a solid solution is also a useful way to strengthen alloys this process is known as solid solution strengthening.Īn important stage of the precipitation process is the onset of nucleation.
This effect is useful in many industrial and scientific applications whereby a chemical reaction may produce a solid that can be collected from the solution by various methods (e.g. Precipitation reactions can be used for making pigments, removing salts from water in water treatment, and for qualitative chemical analysis. 3 Representation using chemical equations.
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