Precipitation (chemistry)

Uses of precipitation reactions

Precipitation reactions can be used for making pigments, removing salts from water in water treatment, and for qualitative chemical analysis.

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. filtration, decanting, centrifugation). Precipitation from a solid solution is also a useful way to strengthen alloys; this process is known as solid solution strengthening.

Mechanism

Precipitation can occur when an insoluble substance is formed in the solution due to a chemical reaction or when the solution has been supersaturated by a compound. The formation of a precipitate is a sign of a chemical change. In most situations, the solid forms ("falls") out of the solute phase, and sinks to the bottom of the solution (though it will float if it is less dense than the solvent, or form a suspension).

The solid may reach the bottom of a container by means of settling, sedimentation, or centrifugation.

An important stage of the precipitation process is the onset of nucleation. 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. If this energy is not available, and no suitable nucleation surface is available, supersaturation occurs.

Representation using chemical equations

An example of a precipitation reaction: Aqueous silver nitrate (AgNO₃) is added to a solution containing potassium chloride (KCl) and the precipitation of a white solid, silver chloride is observed. (Zumdahl, 2005)

AgNO₃ (aq) + KCl (aq) → AgCl (s) + KNO₃ (aq)

The silver chloride(AgCl) has formed a solid, which is observed as a precipitate.

This reaction can be written emphasizing the dissociated ions in a combined solution. This is known as the ionic equation.

Ag⁺ (aq) + NO₃^- (aq) + K⁺ (aq) + Cl^- (aq) → AgCl (s) + K⁺ (aq) + NO₃^- (aq)

A final way to represent a precipitate reaction is known as a net ionic reaction. In this case, any spectator ions (those which do not contribute to the reaction) are left out of the formula completely. This simplifies the above equations to the following:

Ag⁺ (aq) + Cl^- (aq) → AgCl (s)

Cation sensitivity

Precipitate formation is useful in the detection of the type of cation in salt. To do this, an alkali first reacts with the unknown salt to produce a precipitate which is the hydroxide of the unknown salt. To identify the cation, the color of the precipitate and its solubility in excess are noted. Similar processes are often used to separate chemically similar elements, such as the Alkali earth metals.

Digestion

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