Lab : Double Replacement Reactions and Solubility Rules

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1 Name Block Lab : Double Replacement Reactions and Solubility Rules Objective To study various double replacement reactions, identifying precipitates and spectator ions. Introduction Combining solutions of soluble ionic compounds often results in a product that precipitates. The insoluble product can be determined by using the rules of solubility shown on Table F of your reference tables. Materials Well plate, dropper bottles containing the following: Sodium chloride, ammonium, silver nitrate, sodium carbonate, potassium iodide, copper sulfate, cobalt chloride, lead nitrate; chemistry reference table. Procedure Take a well plate and clean it completely. Place 1 drop of the following in a well: No. Reactants Reactant 1 Formula Reactant 2 Formula Precipitate Color 1 Sodium chloride and silver nitrate 2 cobalt (II) chloride and silver nitrate 3 sodium carbonate and silver nitrate 4 potassium iodide and silver nitrate 5 lead (II) nitrate and ammonium 6 lead (II) nitrate and sodium chloride 7 lead (II) nitrate and potassium iodide 8 copper (II) sulfate and sodium carbonate 9 copper (II) sulfate and ammonium 10 copper (II) sulfate and lead nitrate 11 cobalt (II) chloride and sodium carbonate 12 cobalt (II) chloride and ammonium

2 Be sure not to mix any of the chemicals accidentally! To avoid this, do not put the dropper directly on the plastic well drop the drop a half an inch above the well plate! Choose a combination of any two solutions that are not combined above. Describe what happens (or doesn t happen) below: There is one other combination that produces a precipitate. Use your reference tables to figure out what it is for extra credit! Results Writing a balanced chemical equation is not that easy. There are a number of simple steps that you must take. The key is figuring out the formulas of the products. 1. Write the oxidation numbers of the elements over the chemical formulas of the reactants. Do the same for the charges on the polyatomic ions use tables E and/or for this. 2. Draw the arrow to the products, and switch partners the metal ion of one compound goes with the non metal ion or polyatomic ion of the other compound. 3. Write the charges on the product side they do not change in double replacement reactions! 4. Using the criss-cross method, determine the chemical formula of the products. Use parenthesis when you have more than one polyatomic ion. Check with the teacher if you re not sure. 5. Balance the equations using coefficients. 6. Determine the identity of the precipitate using Table F. Write a downward arrow or (s) after the chemical formula of the precipitate. Sodium chloride and silver nitrate cobalt chloride and silver nitrate sodium carbonate and silver nitrate

3 potassium iodide and silver nitrate lead nitrate and ammonium lead nitrate and sodium chloride lead nitrate and potassium iodide copper sulfate and sodium carbonate copper sulfate and ammonium copper sulfate and lead nitrate cobalt chloride and sodium carbonate cobalt chloride and ammonium Questions 1. What are some possible sources of error in this experiment?

4 2. One student looked at a precipitate and identified the precipitate as pink. Her lab partner insisted it was white. Sometimes it isn t easy to tell what the color of a precipitate is. Devise a method to find out! 3. Why do some combinations of solutions not produce precipitates?

5 Summary of Results Using Table F, identify the precipitate and give two justifications based on the table. The first one is done for you. No. Precipitate Justification #1 (soluble product) Justification #2 (insoluble product) 1 Silver Chloride Sodium is always soluble (Group 1); Nitrate is always soluble Silver is insoluble with halides

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