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Precipitation Reaction

What is Precipitation Reaction?

A precipitation reaction refers to the formation of an insoluble salt when two solutions containing soluble salts are combined. The resulting solution is visibly cloudy due to the formation of small aggregation of the insoluble salt. This insoluble salt that falls out of solution and filtered is known as the precipitate. Precipitation reactions can help determine the presence of various ions in solution, most of which are formed from transition metals. This reaction is a type of a double-replacement reaction [1-7].

General Equation

The general equation of the precipitation chemical reaction is given by:

AB + CD → AD + BC

Precipitation Reaction

Predicting Precipitation Reactions

The fundamental rule used to tell whether a precipitate will form or not is the solubility rule. According to this rule, if an ion is soluble, then it remains in its aqueous ion form. If an ion is insoluble, then it forms a solid with an ion from the other reactant. If all the ions in a reaction are shown to be soluble, then no precipitation reaction occurs. The following table shows the solubility of various compounds. This table can be used to find and identify a precipitate [1,2].

Compounds soluble in water

Exception

All compounds of Li+, Na+, K+, Rb+, Cs+, and NH4+

None

All compounds of NO3 and C2H3O2

None

Compounds of Cl, Br, and I

Ag+, Hg22+, and Pb2+

Compounds of SO42-

Hg22+, Pb2+, Sr2+, and Ba2+

Compounds insoluble in water

Exception

Compounds of CO32− and PO43−

Compounds of Li+, Na+, K+, Rb+, Cs+, and NH4+

Compounds of OH

Compounds of Li+, Na+, K+, Rb+, Cs+, NH4+, Sr2+, and Ba2+

How to Balance Precipitation Reactions

Precipitation reaction can be balanced by ensuring that an equal number of atoms are present on both sides of the equation. Consider the following example:

Iron (III) chloride (FeCl3) and sodium hydroxide (NaOH) react to form sodium chloride (NaCl) and insoluble iron (III) hydroxide (Fe(OH)3).

FeCl3 (aq.) + NaOH (aq.) → NaCl (aq.) + Fe(OH)3 (s/ppt.)

The equation is unbalanced. In order to balance the equation, we look at the Fe, Na, Cl, and OH. We notice that there are three Cl atoms on the left-hand side of the equation and only one on the right. So, we multiply the compound NaCl by 3 and obtain the following:

FeCl3 (aq.) + NaOH (aq.) → 3 NaCl (aq.) + Fe(OH)3 (s/ppt.)

Next, we notice that Na is unbalanced as there are three atoms on the right and only one on the left. So, we multiply NaOH by 3 and obtain:

FeCl3 (aq.) + 3 NaOH (aq.) → 3 NaCl (aq.) + Fe(OH)3 (s/ppt.)

Examples of Precipitation Reaction

Here are some examples of precipitation reactions between salts of metals dissolved in aqueous solution [1-7].

  • Lead nitrate (Pb(NO3)2) and potassium iodide (KI) react to form potassium nitrate (KNO3) and insoluble lead iodide (PbI2).

Pb(NO3)2 (aq.) + 2 KI (aq.) → 2 KNO3 (aq.) + PbI2 (s/ppt.)

  • Barium chloride (BaCl2) reacts with sodium sulfate (Na2SO4) to form sodium chloride (NaCl) and insoluble barium sulfate (BaSO4).

BaCl2 (aq.) + Na2SO4 (aq.) → 2 NaCl (aq.) + BaSO4 (s/ppt.)

  • Mixing solutions of calcium chloride (CaCl2) and sodium carbonate (Na2CO3) forms the precipitated calcium carbonate (CaCO3) along with sodium chloride (NaCl)

CaCl2 (aq.) + Na2CO3 (aq.) → 2 NaCl (aq.) + CaCO3 (s/ppt.)

  • In the chemical reaction between potassium chloride (KCl) and silver nitrate (AgNO3), silver chloride (AgCl) is precipitated out, and potassium nitrate (KNO3) remains in solution.

KCl (aq.) + AgNO3 (aq.) → KNO3 (aq.) + AgCl (s/ppt.)

Precipitation Reaction Examples

Precipitation Reaction Examples in Real Life

Here are some examples of precipitation reaction in everyday life [3,4]:

  • Precipitation in water pipes: Hard water consists of many impurities. Magnesium and calcium oxides are generally found in water pipes as precipitates.
  • Formation of kidney stone: The reaction between calcium ions and oxalic acid that are present in food results in calcium oxalate, which is a type of kidney stone.
  • Formation of the immune complex: Soluble antigens combine with soluble antibodies in the presence of an electrolyte (solution) at a suitable temperature and pH to form an insoluble visible complex in the human body.

Practical Uses of Precipitation Reaction

One of the applications of precipitation reaction is to determine whether a particular element is present in a solution or not. Here are some of its uses [3,4]:

  • Wastewater treatment: A chemical is added to wastewater so that the pollutants and impurities (e.g., lead) precipitate out from the water, which is then sent for further purification.
  • Metallurgy: Oxalic acid is mixed with seawater and brine water to extract calcium and magnesium, both of which form precipitates.

References

  1. Pressbooks.bccampus.ca
  2. Guweb2.gonzaga.edu
  3. Chem.libretexts.org
  4. Cpanhd.sitehost.iu.edu
  5. Bbc.co.uk
  6. Hyperphysics.phy-astr.gsu.edu
  7. Ohsd.netAcsh.org

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