Precipitation Reactions Lab Report

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Conclusion: The the precipitation reactions lab eight out of the fourteen occurring reactions were precipitates. A precipitate means that a solid substance was formed or a substance that is not aqueous was formed. The reactions that did not form a precipitate were DNR, which means that they did not react. At station one barium chloride and potassium nitrate did not react but barium chloride and silver nitrate reacted to form barium nitrate and silver chloride. The precipitate at station one was silver chloride. Both reactions at station two did not react. Station three had a reaction occur between sodium carbonate and calcium sulfate forming sodium sulfate and calcium carbonate. The precipitate was calcium carbonate. Station four formed a …show more content…
The solubility rules were used to determine which reactant was aqueous and which one was a solid. The solid is the precipitate formed in the reaction. The formation of the precipitate indicates that a chemical reaction occurred. If no precipitate formed the reaction would be labeled with DNR, which stands for does not react. The solubility rules states which elements are soluble or insoluble, including the exceptions for each rule. For example at station one, barium chloride reacted with silver nitrate yielding to barium nitrate and silver chloride. Barium nitrate is aqueous because all nitrates are soluble. Silver chloride is the precipitate because all chlorides expect silver and a few others are soluble, since silver is an exception silver chloride is insoluble. To determine which reactant out of the chemical reactions the solubility rules provided the guideline necessary to figure out which reactant is the precipitate. The reactions in this equation were all of the same type of chemical reaction. They were double replacement reactions which is the two products are interchanged to formed two new compounds on the reactant side. Intermolecular forces have heavy influence over solubility. Intermolecular forces are between molecules and are weak forces of attraction. There are four intermolecular forces including hydrogen bonding, dipole-dipole forces, dipole-induced dipole forces, and london dispersion forces. Hydrogen bonding is the strongest and occurs when one hydrogen molecule is attracted to another molecule. Next is dipole- dipole forces which occurs between polar molecules. After that is dipole- induced dipole, it is weaker than dipole-dipole because its occurs between a polar and a nonpolar molecule. The weakest intermolecular force is london dispersion forces because it is only temporary

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