Aqueous Chemical Reactions

Aqueous Chemical Reactions Introduction Many chemical reactions occur in water and therefore they are considered aqueous chemical reactions. The reagents are typically dissolved or diluted in water and then the reactions are carried out. Three main types of reactions that typically occur as aqueous reactions are single replacement reactions, double replacement/precipitation reactions, and acid-base neutralization reactions. In this lab, these three types of reactions will be carried out and detailed observations will be made to help distinguish them from one another. For more information: Chemistry: Atom’s First by OpenStax section 7.2 – “Classifying Chemical Reactions” Materials: small test tubes test tube rack test tube clamp copper wire 3M HCl 3M NaOH 3M HNO3 3M H2SO4 zinc pieces 1M CuSO4 litmus paper watch glass glass stir rod phenolphthalein 0.1M of the following Ba(NO3)2, Pb(NO3)2, NaNO3, KI, HCl, NaOH saturated Na2CO3. 1M Na2SO4, 1M AgNO3, 1M NaCl well-plate Q-tips DI water bottle Procedure Observations: Record observations for all of the chemical reactions carried out during the lab in your report sheet. These observations should include: • observations of the reactant(s) before the reaction • observations of the reaction mixture during the reaction • observations of the product(s) after the reaction. Your observations of a material should contain the color, clarity and state of matter, plus any useful descriptions of the material (for example, a sample of magnesium might be described as a smooth, shiny, silver, opaque solid). Your observations of the reaction in progress should include anything of potential interest, such as “the color changed from green to blue”, “a pungent odor is present now”, “the test tube is getting warmer” or “bubbles are forming on the surface of the magnesium”. page 1 of 9 Part I – Single Replacement Reactions. 1. Place a piece of copper wire in a test tube with enough 1 M AgNO3 to cover it. CAUTION: AgNO3 will stain skin and clothes! 2. Allow the test tube to stand for 5-10 minutes. 3. Write down observations noting changes in the appearance of both the wire and the solution. 4. Obtain a new, clean test tube and place a small piece of zinc metal in a test tube. 5. Add 2 mL of 3M HCl. CAUTION: 3M HCl(aq) can damage skin and clothing on contact. Rinse any spills on skin immediately with plenty of water for 10 minutes. Neutralize all spills on the lab bench with water or NaHCO3 solution, and rinse your hands thoroughly. 6. Record your observations. 7. Obtain a new, clean test tube and place a small piece of zinc metal in a test tube. 8. Add enough 1M CuSO4 to cover the zinc metal. 9. Record your observations. Part II – Acid-Base Neutralization Reactions 1. Line up three small pieces of red litmus paper and 3 small pieces of blue litmus paper on a watch glass leaving plenty of space between each. 2. Place a drop of 0.1M HCl(aq) on one piece of red and one piece of blue litmus paper using a stirring rod and record your observations. CAUTION! NaOH, HCl, HNO3 and H2SO4 can damage skin, eyes and clothing on contact. Rinse off any spills immediately with plenty of water for 10 minutes. In the event of a spill in the laboratory, notify your instructor immediately. 3. Place a drop of 0.1M NaOH(aq) on new, fresh pieces of blue and red litmus paper and record your observations. 4. Place a drop of deionized water on new, fresh pieces of blue and red pieces of litmus paper and record your observations. 5. Place 10 drops of 3M NaOH in a clean test tube. 6. Now add ten drops of 3M HNO3 to the same test tube holding the NaOH. Feel the outside of the test tube and write down any observations. 7. Write the balanced equation for the reaction of NaOH with HNO3 on your lab report in the observations section for part II. 8. Place 10 drops of 3M NaOH in a new, clean test tube. 9. Add 2 drops of phenolphthalein and stir with a clean stir rod. Record your observations. page 2 of 9 10. Add 3M H2SO4 slowly drop wise to the NaOH in the test tube. Count how many drops it takes to neutralize the NaOH. 11. Record your results. 12. Write the balanced equation for the reaction of NaOH with H2SO4 on your lab report in the observations section for part II. Part III – Double Replacement/Precipitation Reactions 1. Clean the well-plate with warm soapy water and Q-tips. Allow to air dry. 2. Obtain solutions of 1M AgNO3, 1M NaCl, 0.1M Ba(NO3)2, 3M HNO3(aq) and 0.1M Pb(NO3)2. Following the grid outline in your data section of this lab report, drop 3 drops of each solution into the appropriate wells of the well-plate. CAUTION: AgNO3 will stain skin and clothing! Pb containing compounds are toxic and should not be ingested. HCl, HNO3 and NaOH are corrosive and can cause chemical burns and damage clothing. 3. To EACH of these previous well spots in the well-plate, now add 3 drops of the solutions of 0.1M NaNO3, 1M NaCl, 1M Na2SO4, 0.1M NaOH, 0.1M KI, and saturated Na2CO3. Carefully look at the data table to make sure your are placing the solutions in the correct locations. 4. Record observations for each well of the well-plate that the two solutions were mixed. If no reaction occurred write “NR” on your data table. 5. For each of the following combinations, mix 10 drops of each solution in a clean test tube, so any reactions that take place can be observed on a larger scale: • • • 0.1M Ba(NO3)2(aq) and 0.1M NaOH(aq) 3M HNO3(aq) and saturated Na2CO3(aq) 0.1M Pb(NO3)2(aq) and 1M NaCl(aq) 6. Have your lab instructor sign off on your Double Replacement/Precipitation reaction observation table. 7. Write a balanced chemical equation and clearly identify the solid product for any precipitation reactions that you observe. Please refer to the Laboratory Techniques Document on the CHM151LL Course Website for more detailed techniques and images of lab equipment. Clean-Up: Dispose of the contents from all of the test tubes and well-plate in the waste jar in the hood. Rinse everything well with soapy tap water followed by a quick DI water rinse. Clean your benchtop. Put all equipment back exactly where you found it. page 3 of 9 Name: _____________________________ Partners: ________________________ Aqueous Chemical Reactions Lab Report Turn in Pages 4-6 for Your Lab Report Data: Data Table 1: Part I Single-Replacement Reaction Observations Copper Metal AgNO3 solution Before reaction During reaction After reaction Balanced Chemical Reaction: _____________________________________________________ Zinc Metal HCl Solution Before Reaction During Reaction After Reaction Balanced Chemical Reaction: _____________________________________________________ Zinc Metal CuSO4 solution Before reaction During reaction After reaction Balanced Chemical Reaction: _____________________________________________________ page 4 of 9 Data Table 2: Part II Acid-Base Neutralization Reaction Observations Red litmus paper Blue litmus paper Before reaction Reaction with 0.1M HCl Reaction with 0.1M NaOH Reaction with H2O Balanced Chemical Reaction 1: ___HNO3(aq) + ___NaOH(aq) →___________________________ Observations: Balanced Chemical Reaction 2: ___H2SO4(aq) + ___NaOH(aq) →__________________________ Observations: Observed color of NaOH Before Adding Phenolphthalein Observed color of NaOH After Adding Phenolphthalein Number of drops of H2SO4 needed to neutralize the NaOH Data Table 3: Part III Double Replacement/Precipitation Reaction Observation 1M AgNO3 1M NaCl 0.1M Ba(NO3)2 3M HNO3 0.1M Pb(NO3)2 0.1M NaNO3 1M NaCl 1M Na2SO4 0.1M KI 0.1M NaOH saturated Na2CO3 page 5 of 9 Part III Observations of the test tube reactions on a larger scale: 0.1M Ba(NO3)2(aq) 3M HNO3(aq) and 0.1M NaOH(aq) and saturated Na2CO3(aq) 0.1M Pb(NO3)2(aq) and 1M NaCl(aq) For the third reaction, 0.1M Pb(NO3)2(aq) and 1M NaCl(aq), fill in the beaker drawings: + → Part III Double Replacement Reactions: (7 pts) Write out the products for each of the precipitation reactions in Part III that you observed a reaction for. 1. _________________ + _________________ → _________________ + _________________ 2. _________________ + _________________ → _________________ + _________________ 3. _________________ + _________________ → _________________ + _________________ 4. _________________ + _________________ → _________________ + _________________ 5. _________________ + _________________ → _________________ + _________________ 6. _________________ + _________________ → _________________ + _________________ 7. _________________ + _________________ → _________________ + _________________ 8. _________________ + _________________ → _________________ + _________________ 9. _________________ + _________________ → _________________ + _________________ 10. _________________ + _________________ → _________________ + _________________ 11. _________________ + _________________ → _________________ + _________________ 12. _________________ + _________________ → _________________ + _________________ 13. _________________ + _________________ → _________________ + _________________ 14. _________________ + _________________ → _________________ + _________________ page 6 of 9 Conclusion: (5 pts) Summarize the three types of aqueous reactions studied in the lab report and cite examples along with evidence of how you know these types of reactions occur. Make sure you use specific chemical reactions and observations from this lab experiment to demonstrate each type of reaction and how it is recognizable as that type of reaction. page 7 of 9 Post-Lab Questions – These questions will not be graded as part of your lab report grade. You will be responsible for the information in these questions and able to answer these or similar questions on the post-lab quiz at the start of next week’s lab period. Questions will also be similar to your lab report data, observations, calculations, and results. Part II and III Acid-Base Neutralization Reactions and Double Replacement/Precipitation Reactions Refer to your data table for the following selected sets of reactants and fill in the following blanks and beaker drawings. An example NOT from this experiment is presented first. Example: calcium acetate and ammonium sulfate Reaction type: ____precipitation Molecular: Ca(CH3COO)2(aq) + (NH4)2SO4(aq) → CaSO4(s) + 2 NH4CH3COO(aq) Ionic: Ca2+(aq) + 2 CH3COO-(aq) + 2 NH4+(aq) + SO42-(aq) → CaSO4(s) + 2 CH3COO-(aq) + 2 NH4+(aq) Net Ionic: Ca2+(aq) + SO42-(aq) → CaSO4(s) + 1. lead (II) nitrate and potassium iodide → Reaction type: _______________ Molecular: ________________________________________________________________________ Ionic: ____________________________________________________________________________ Net Ionic: ________________________________________________________________________ + → page 8 of 9 2. nitric acid and sodium hydroxide Reaction type: _______________ Molecular: ________________________________________________________________________ Ionic: ____________________________________________________________________________ Net Ionic: ________________________________________________________________________ + → Balancing and Categorizing Chemical Equations: Balance each of the chemical equations given below, and identify each as one of the six types listed below. Single-Replacement reaction (SR) Double-Replacement/Precipitation reaction (DR) Acid-Base Neutralization reaction (N) TYPE _____ NiCl2 (aq) → _____ Ni (s) + _____ AlCl3 (aq) _____ 1. _____ Al (s) + _____ 2. _____ Ba(OH)2 (s) + ____ FeCl3 (aq) → ____ BaCl2 (aq) + ____ Fe(OH)3 (s) _____ 3. _____ H2SO4 (aq) + _____ Mg(OH)2 (s) →_____ H2O (l) + _____ MgSO4 (aq) _____ 4. _____ Na3PO4 (aq) + ____ MgCl2 (aq) → ____ Mg3(PO4)2 (s) + ___ NaCl (aq) _____ 5. _____ H3PO4 (aq) + ____ NaOH (aq) → _____ H2O (l) + ____ Na3PO4 (aq) Discuss two sources of error and how they can be corrected in the future. 1. 2. Now that you have completed the experiment please write a “Purpose” statement that more accurately reflects the function of this lab. page 9 of 9