Honors Chemistry Lab notebook 2.19.13 Jane Yang Title: Precipitation Reactions Objective: To predict and perform precipitation reactions in a laboratory setting while utilizing the general rules of solubility. Safety: Barium Chloride and lead (II) nitrate solutions are toxic by ingestion. Silver (I) nitrate solution is toxic, corrosive, lightsensitive, and stains skin and clothing. Avoid all eye and body tissue contact with all solutions. Wear chemical splash goggles and a chemical resistant apron. Materials: 4 drops o.1 m silver (I) nitrate solution, 4 drops 0.1 m aluminum chloride, 4 drops 0.1 m sodium carbonate solution, 4 drops 0.1m Copper (II) sulfate, 4 drops 0.1m lead(II) nitrate solution, 4 drops 0.1m calcium nitrate solution, 4 drops 0.1m potassium phosphate solution. 1 reaction plate, 2 (24 well plates), 8 beryl-type pipets, labeled, and 1 black piece of paper. Procedure: (list format) 1. Our group gathered all the materials (different types of solutions mentioned above.) 2. We used the pipet to drop 4 of each solutions into the well plates. 3.Each person observed precipitations or no color changes. 4. Each person recorded the results on the data paper. Data: table and observations: On data table 1, record the 2 possible products with physical states in each circle along with any colors that form, If any solid precipitates form, use the abbreviation ppt. If no reaction at all occurs, use the abbreviation NR. Make sure to shade in the circles of the empty walls. Data Analysis: (equations) Write the balanced molecular equations, complete ionic, and net ionic equations for the precipitation reactions in the lab.
Conclusion: (paragraph form) Discuss the results of the lab. Explain any unexpected results or errors. My conclusion: Sodium carbonate forms precipitate with nearly all of the other substances we tested. Both potassium phosphate and barium chloride form any precipitate with any of the 6 substances. Calcium chloride only forms precipitations...
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