Lab: Chemical Reactions

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1 Lab: Chemical Reactions PRE-LAB: Write the chemical equations (skeleton equations) for the following. Make sure to clearly label what type of product was produced (solid, liquid, gas, or no reaction). 1. barium nitrate reacts with sodium hydroxide 2. barium nitrate reacts with sodium hydrogen carbonate 3. barium nitrate reacts with copper (II) sulfate 4. barium nitrate reacts with potassium iodide 5. barium nitrate reacts with silver nitrate 6. barium nitrate reacts with iron (III) nitrate 7. barium nitrate reacts with hydrochloric acid 8. sodium hydroxide reacts with sodium hydrogen carbonate 9. sodium hydroxide reacts with copper (II) sulfate 10. sodium hydroxide reacts with potassium iodide 11. sodium hydroxide reacts with silver nitrate 12. sodium hydroxide reacts with iron (III) nitrate 13. sodium hydroxide reacts with hydrochloric acid 14. sodium hydrogen carbonate reacts with copper (II) sulfate 1

2 15. sodium hydrogen carbonate reacts with potassium iodide 16. sodium hydrogen carbonate reacts with silver nitrate 17. sodium hydrogen carbonate reacts with iron (III) nitrate 18. sodium hydrogen carbonate reacts with hydrochloric acid 19. copper (II) sulfate reacts with potassium iodide 20. copper (II) sulfate reacts with silver nitrate 21. copper (II) sulfate reacts with iron (III) nitrate 22. copper (II) sulfate reacts with hydrochloric acid 23. potassium iodide reacts with silver nitrate 24. potassium iodide reacts with iron (III) nitrate 25. potassium iodide reacts with hydrochloric acid 26. silver nitrate reacts with iron (III) nitrate 27. silver nitrate reacts with hydrochloric acid 28. iron (III) nitrate reacts with hydrochloric acid 2

3 Objectives: Observe several typical examples of evidence that chemical change is occurring; make generalizations about the combinations of materials that result in the same evidence; practice careful laboratory techniques such as avoiding contamination of reactants, to endure that results observed are repeatable and unambiguous. You will combine the aqueous solutions (one to one) with each other in an organized manner in order to observe their interactions. Problem: What will the various aqueous solutions chemical reactions be when mixed in various combinations? Will some chemical reactions produce precipitate (solid), water (liquid), bubbles (gas) or have no reaction? Hypothesis: Chemicals can undergo chemical changes by creating heat, changing colors, forming bubbles and precipitates. You should have clearly labeled your predictions PRIOR to lab. You must show instructor prior to beginning the lab. Safety Precautions: Safety goggles and lab apron MUST be worn at all times in the Chemistry lab. Silver nitrate will stain skin and clothing. Handle with care. Wash your hands and arms thoroughly after this activity. Hydrochloric acid can be harmful if spilled on you. Be very careful with ALL chemicals! Materials: Aqueous solutions of barium nitrate, sodium hydroxide, sodium hydrogen carbonate, copper (II) sulfate, potassium iodide, silver nitrate, iron (III) nitrate, and hydrochloric acid Chem. well plate Droppers for each solution (as needed) Toothpicks 3

4 Procedure: 1. Make a chart in your lab book to record your data at least one page in your lab book. Allow room to record your observations. A sample chart will be on display on the overhead. You will have to complete the chart including all the chemicals you will use. Notice that some of the boxes in the chart are marked with X, indicating there is no need to mix those particular chemicals. Why do you suppose those particular blocks have an X? (2 pts) 2. Begin mixing with barium nitrate. Add 3 drops of barium nitrate solution to each of 7 wells of the well plate. Add 3 drops of sodium hydroxide solution to the first well. After mixing the two solutions, make notes on your chart of any changes you observe. Don t overlook any color changes, the formation of a precipitate (cloudy solution), the formation of a gas (fizzing or bubbling), or a change in temperature. 3. Using another dropper, continue by adding 3 drops of the sodium hydrogen carbonate to the second well. It is important that you do not allow the top of the dropper of one solution to come in contact with another solution. Your attention to this detail will prevent contamination of the solutions. Continue by adding copper (II) sulfate to the third well, and so on. 4. After mixing the pairs of solutions, make notes on any changes you observe. You have completed the first row of the chart. Begin the second row. Continue by putting 3 drops of sodium hydroxide into each of 7 wells and adding the other solutions. 5. Notice that adding barium nitrate to the sodium hydroxide (in the second row of the chart) produced the same results as adding sodium hydroxide to barium nitrate (in the first row of the chart). If you can explain why this is so, you can shorten the time needed for the investigation by not repeating other mixtures. After completing the entire chart in this fashion and mixing all possible one-to-one combinations of solutions, clean up your lab table and make sure all the chemicals are in the correct location. 4

5 Analysis/Conclusion: 1. Which combination of reactants seems to produce no reaction when mixed together? 2. Which combination of reactants forms a gas? Can you guess which gas is formed? Try to deduce this from the reactants names and chemical formulas. 3. Which combination of reactants produces a color change when mixed together? 4. Which combination of reactants forms precipitates quickly? Slowly? 5. Which combination of reactants forms: a. A yellow precipitate? b. A muddy brown precipitate? c. A white precipitate? d. A blue precipitate? 6. Which combination of reactants produces heat? How could you tell? 7. What evidence indicates that a chemical change is occurring? 5

6 8. Indicate if a chemical change occurred in the following situations or not: a. An acid is dissolved in water and heat is released b. A burning match produces light c. A seed crystal is placed in a supersaturated solution and the extra solute particles join the crystal and come out of the solution d. The glowing filament of a light bulb produces light e. A small piece of metal is placed into an acid and hydrogen is released f. Solutions of sodium hydroxide and copper (II) sulfate are mixed and a blue precipitate appears. 9. Anhydrous copper (II) sulfate (CuSO 4 ) is a white solid. When it is dissolved in water, the solution becomes blue. Is this a chemical change? Give an explanation. 6

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