Precipitation+Reactions



Precipitates are solids that are formed from ions in an aqueous solution. The input for the precipitate equations deal with compounds that are dissolved into separate ions. These separate ions can join other ions that are present in the aqueous medium potentially creating precipitates. Precipitates are formed based on the solubility rules of each type of compound. When a precipitate is formed, these are removed from the solution in a solid form. The picture below represents what should occur in a precipitation reaction in the equation. Here are some examples of precipitation reactions:

BaCl2(aq) + Na2SO4(aq) -> BaSO4 and NaCl(aq) Due to the solubility rules, Barium Sulfate is not soluble causing it to become a precipitate in the reaction.

AgNO 3 (aq) + KCl (aq) > AgCl (s) + KNO 3 (aq) The solubility rules state that AgCl is insoluble therefore silver chloride is the precipitate in this reaction.

"Precipitation Equations." //An Introduction to Chemistry - Bishop//. N.p., n.d. Web. 30 Sept. 2011. .

http://elearning.flinnsci.com/assets/product_images/1817_2_ALT_375.jpg http://chemwiki.ucdavis.edu/@api/deki/files/4281/=double_replacement.jpg