There are many other factors that can affect solubility, but these rules are a good first step to determine the outcome of aqueous solution reactions. The solubility rules are a useful guideline to predict whether a compound will dissolve or form a precipitate. This is an example of a double displacement reaction. The finished reaction is:Ģ KCl(aq) + Pb(NO 3) 2(aq) → 2 KNO 3(aq) + PbCl 2(s) Calcium carbonate precipitate is formed as a result: CaCl2 + Na2CO3 -> CaCO3 + NaCl. This means PbCl 2 is insoluble and form a precipitate. Chlorides are soluble in water with the exception of silver, lead and mercury. KNO 3 will remain in solution since all nitrates are soluble in water. The balanced chemical equation for this reaction is: CaCl2 + Na2CO3 CaCO3 (s) + 2 NaCl. KCl(aq) + Pb(NO 3) 2(aq) → KNO 3(?) + PbCl 2(?)Ģ KCl(aq) + Pb(NO 3) 2(aq) → 2 KNO 3(?) + PbCl 2(?) When calcium chloride (CaCl2) and sodium carbonate (Na2CO3) are mixed in an aqueous solution, a precipitation reaction occurs. The products should rearrange the ions to: What would be the expected products and will a precipitate form? The resulting balanced reaction would be:Ģ AgNO 3(aq) + MgBr 2 → 2 AgBr(s) + Mg(NO 3) 2(aq) The other compound Mg(NO 3) 2 will remain in solution because all nitrates, (NO 3) -, are soluble in water. Are the products soluble in water?Īccording to the solubility rules, all silver salts are insoluble in water with the exception of silver nitrate, silver acetate and silver sulfate. The state of the products needs to be determined. The balanced reaction would be:Ģ AgNO 3(aq) + MgBr 2 → 2 AgBr(?) + Mg(NO 3) 2(?) For example, a silver nitrate solution (AgNO 3) is mixed with a solution of magnesium bromide (MgBr 2). The question remains, will AD or CB remain in solution or form a solid precipitate?Ī precipitate will form if the resulting compound is insoluble in water. This reaction is generally a double replacement reaction in the form: When two aqueous solutions are mixed, the ions interact to form products. A simple demonstration of how a precipitate is evidence of a chemical reaction taking place is performed by mixing solutions of calcium chloride and sodium carbonate to form the precipitate calcium carbonate (CaCO 3 ). These solutions are represented in chemical equations in the form: AB(aq) where A is the cation and B is the anion. This guide will show how to use the solubility rules for inorganic compounds to predict whether or not the product will remain in solution or form a precipitate.Īqueous solutions of ionic compounds are comprised of the ions making up the compound dissociated in water. When two aqueous solutions of ionic compounds are mixed together, the resulting reaction may produce a solid precipitate.
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