Chemical Reactions Lab
Chemical Reactions Lab
Objectives: 1. To examine a variety of reactions including precipitation, acid-base, gas forming, and oxidation-reduction reactions. 2. To identify the products formed in these reactions and summarize the chemical changes in terms of balanced chemical equations and net ionic equations. 3. To identify the species being oxidized and reduced in oxidation-reduction reactions and determine which species is the oxidizing agent and the reducing agent. Chemical equations represent what occurs in a chemical reaction. For example, the equation HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l) describes an acid-base reaction, a type of exchange reaction in which the driving force is the formation of water. In an exchange reaction, the …show more content…
Dispose of the solutions and any precipitates in the waste beakers located in the hoods. Wash your test tubes with soap and water. Rinse with tap water, then deionized water. 5. Add an amount equivalent to the size of a small pea of baking soda (sodium hydrogen carbonate) to a clean test tube. Add 10-20 drops of vinegar. (Vinegar is an aqueous solution of acetic acid, HC2H3O2). Record your observations. 6. IN THE HOOD, add an amount equivalent to the size of a small pea of sodium sulfite, Na2SO3, to a test tube. Add 10-20 drops of 6 M HCl. Record your observations.
7. Put 10 drops of 0.5 M nitric acid and 10 drops of 0.5 M phosphoric acid into separate test tubes. Add 1 drop of phenolphthalein to each test tube. Add drops of dilute (0.5 M) sodium hydroxide solution into each of the test tubes until a permanent color change is observed. (NOTE: Phenolphthalein is an acid-base indicator that is colorless in acidic and neutral solutions, but pink in basic solutions). HINT: When writing your net ionic equations: nitric acid is a strong acid while phosphoric acid is a weak …show more content…
Add a small piece of zinc to a test tube containing 30 drops of 6 M HCl and record what happens. 9. Add a 1 inch piece of copper wire to a test tube containing 30 drops of 6 M HCl and record what happens. (Is copper an active metal or inactive metal with HCl? Look up an activity series of metals online to check). 10. IN THE HOOD, take a 2 inch piece of magnesium ribbon and hold it with a pair of crucible tongs. Light the magnesium metal with a Bunsen burner and record your observations. DO NOT LOOK DIRECTLY AT THE BURNING MAGNESIUM. LABORATORY REPORT Students will write an individual or group laboratory report at the discretion of the professor. Include the following information in your laboratory report, due at the beginning of the laboratory period next week. 1. Title. Title of the experiment, your name, your partner 's name and the date the laboratory was performed. 2. Introduction. This will be your opportunity to practice writing introductions. The introduction to the lab should be about chemical reactions in general (why they are important, examples of specific types of chemical reactions such as combustion, precipitation, redox, etc.), not about how to write and balance an equation. For complete guidelines, go to “Laboratory Reports” on the Chem 1061 website. 3. Experimental Details. A description of the procedure you followed to produce the experimental data and results. Alternatively, you may reference the procedure by citing the URL’s
Objectives: 1. To examine a variety of reactions including precipitation, acid-base, gas forming, and oxidation-reduction reactions. 2. To identify the products formed in these reactions and summarize the chemical changes in terms of balanced chemical equations and net ionic equations. 3. To identify the species being oxidized and reduced in oxidation-reduction reactions and determine which species is the oxidizing agent and the reducing agent. Chemical equations represent what occurs in a chemical reaction. For example, the equation HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l) describes an acid-base reaction, a type of exchange reaction in which the driving force is the formation of water. In an exchange reaction, the …show more content…
Dispose of the solutions and any precipitates in the waste beakers located in the hoods. Wash your test tubes with soap and water. Rinse with tap water, then deionized water. 5. Add an amount equivalent to the size of a small pea of baking soda (sodium hydrogen carbonate) to a clean test tube. Add 10-20 drops of vinegar. (Vinegar is an aqueous solution of acetic acid, HC2H3O2). Record your observations. 6. IN THE HOOD, add an amount equivalent to the size of a small pea of sodium sulfite, Na2SO3, to a test tube. Add 10-20 drops of 6 M HCl. Record your observations.
7. Put 10 drops of 0.5 M nitric acid and 10 drops of 0.5 M phosphoric acid into separate test tubes. Add 1 drop of phenolphthalein to each test tube. Add drops of dilute (0.5 M) sodium hydroxide solution into each of the test tubes until a permanent color change is observed. (NOTE: Phenolphthalein is an acid-base indicator that is colorless in acidic and neutral solutions, but pink in basic solutions). HINT: When writing your net ionic equations: nitric acid is a strong acid while phosphoric acid is a weak …show more content…
Add a small piece of zinc to a test tube containing 30 drops of 6 M HCl and record what happens. 9. Add a 1 inch piece of copper wire to a test tube containing 30 drops of 6 M HCl and record what happens. (Is copper an active metal or inactive metal with HCl? Look up an activity series of metals online to check). 10. IN THE HOOD, take a 2 inch piece of magnesium ribbon and hold it with a pair of crucible tongs. Light the magnesium metal with a Bunsen burner and record your observations. DO NOT LOOK DIRECTLY AT THE BURNING MAGNESIUM. LABORATORY REPORT Students will write an individual or group laboratory report at the discretion of the professor. Include the following information in your laboratory report, due at the beginning of the laboratory period next week. 1. Title. Title of the experiment, your name, your partner 's name and the date the laboratory was performed. 2. Introduction. This will be your opportunity to practice writing introductions. The introduction to the lab should be about chemical reactions in general (why they are important, examples of specific types of chemical reactions such as combustion, precipitation, redox, etc.), not about how to write and balance an equation. For complete guidelines, go to “Laboratory Reports” on the Chem 1061 website. 3. Experimental Details. A description of the procedure you followed to produce the experimental data and results. Alternatively, you may reference the procedure by citing the URL’s