Assignment #4a Group Proposal-Notes

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Arizona State University *

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101A

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Chemistry

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Dec 6, 2023

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What is the Chemical Reaction? Materials within the group (lab bench) kit ● 1 vial each of: o Red Litmus Paper o Blue Litmus Paper o Universal pH Paper ● 6-8 15 mL conical test tubes ● In 125 mL Bottles: o phenolphthalein o 1M HCl o 0.1M Copper (II) chloride o 0.1M Sodium phosphate o 3% H 2 O 2 o label as: 0.1M NaOH o Isopropyl alcohol (C 3 H 7 OH) Materials within TA bin ● 10 extra 15 mL conical test tubes ● 1 large jar of Magnesium strips ● 1 medium jar of baker’s yeast ● 1 medium jar of Cu wire ● 1 bag of wooden splints ● 2-3 boxes of matches ● In 3 separate Bins: o Yellow= E, F, M, I, G Blue= E, M, I, R, G Red= E, N , I , U, C Common Group Glassware Drawers ● Test tube racks ● Various size test tubes ● Watch glasses ● Evaporating dish ● Crucible tongs Drawers in Front of Room Arizona State University School of Molecular Sciences PA

● Disposable plastic pipet BACKGROUND Single Replacement Reaction: A + BC → AC + B To predict whether or not a single-replacement reaction will occur, we refer to the Activity Series for Metals. If a solid metal is “more active” – i.e., higher on the Activity Series – than the metal ion in solution (or hydrogen for acids), the more active metal will displace the less active ion, so a reaction occurs. The more active metal goes into solution while the less active ion either plates out for a metal ion or bubbles out as a gas for hydrogen ion. If the solid metal is less active than the metal ion or hydrogen in the compound, then no reaction occurs. In this type of reaction, a more “active metal” displaces another element in solution. The following examples show a solid metal reacting with a) a metal ion solution, b) H + from an acid solution, or c) H + from water. An example of each is provided below: a) When a solid metal reacts with a metal solution, the solid metal’s ions go into solution while the metal ions originally in solution plate out onto the surface of solid metal, e.g.: Zn (s) + CuSO 4 (aq) → ZnSO 4 (aq) + Cu (s) b) When a solid metal reacts with an acid, the metal replaces hydrogen in the acid to produce hydrogen gas while the metal ion goes into solution with the anion from the acid, e.g.: 2Al (s) + 6HCl (aq) → 3H 2 (g) + 2AlCl 3 (aq) c) When a solid metal reacts with water , the metal replaces hydrogen in the water to produce hydrogen gas while the metal ion goes into solution with hydroxide ion, e.g.: Ca (s) + 2 H 2 O (aq) → H 2 (g) + Ca(OH) 2 (aq) Arizona State University School of Molecular Sciences PA

Double Replacement/Precipitation Reaction: AB + CD → AD + CB These reactions involve the mixing of two aqueous ionic compounds to produce a precipitate , an insoluble ionic compound. The products of a double-replacement/precipitation reaction can be predicted by switching the cations of the two compounds and using the Solubility Rules (below) to determine if the compounds produced are soluble or insoluble. Soluble ionic compounds will dissolve in water, so their physical states are indicated as aqueous, (aq), while insoluble ionic compounds will not dissolve in water, so their physical states are indicated as solid, (s). For a precipitation reaction to occur, at least one of the products must be insoluble; if both products are soluble, then no reaction occurs. The presence of a precipitate is observed in the lab as a cloudy mixture that results when two solutions are mixed. For example, when lead ions, Pb 2+ (aq), and iodide ions, I - (aq), become mixed in solution together, they combine to form PbI 2 (s), an insoluble compound. Pb(NO 3 ) 2 (aq) + 2KI (aq) → 2KNO 3 (aq) + PbI 2 (s) Precipitation reactions may be represented in three different ways, the balanced molecular equation, the total (or complete) ionic equation, and the net ionic equation. From the balanced molecular equation shown above, the complete and net ionic equations can be written as shown below. The complete ionic form of the equation shows SOLUBLE species as their separate ions, being sure to maintain the stoichiometric ratio of the balanced molecular equation. Pb 2+ ( aq ) + 2NO - ( aq ) + 2K + ( aq ) + 2I - ( aq ) → PbI 2 ( s ) + 2K + ( aq ) + 2NO - ( aq ) The net ionic form of the equation omits the spectator ions, or ions not involved in the chemical reaction taking place. The remaining species represent the actual chemical reaction occurring (the net result of the reaction). Pb 2+ ( aq ) + 2I - ( aq ) → PbI 2 ( s ) Double Replacement/Acid-Base Neutralization Reaction: These reactions occur between an acid and a base. In general, acids are compounds that 3 3

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produce hydrogen ions (H + ), also called protons , when dissolved in water. The chemical formulas for acids are most often given with the H’s at the beginning, so acids are usually easy to recognize. A few

common acids are hydrochloric acid, HCl (aq) , nitric acid, HNO 3 (aq) , and sulfuric acid, H 2 SO 4 (aq) . Bases are compounds that produce hydroxide ions ( OH – ) when dissolved in water. A few common bases are sodium hydroxide, NaOH, potassium hydroxide, KOH, calcium hydroxide, Ca(OH) 2 , and barium hydroxide, Ba(OH) 2 . Other types of bases are basic salts that form gases when they combine with acids. Some common basic salts contain carbonates (CO 2- ) and hydrogen carbonates (or bicarbonate, HCO – ). In the presence of an acid, blue litmus paper turns red. In the presence of a base, red litmus paper turns blue. a) When an acid reacts with a base containing the hydroxide ion (OH – ), the product is water and a salt (an ionic compound). e.g.: HCl (aq) + NaOH (aq) → H 2 O (l) + NaCl (aq) Note that the hydrogens from the acid combine with the hydroxide from the base to form water while the salt is formed by combining the cation from the base with the anion from the acid. b) When an acid reacts with a basic salt containing one of the gas forming anions like carbonate (CO –2 ) or hydrogen carbonate ion (HCO – ), the product is water, gas, and a salt. e.g.: HCl (aq) + NaHCO 3 (aq) → H 2 CO 3 (aq) + NaCl (aq) H 2 CO 3 (aq) quickly decomposes to form: HCl (aq) + NaHCO 3 (aq) → H 2 O (l) + CO 2 (g) + NaCl (aq) Note that in this reaction the hydrogens from the acid combine with the hydrogen carbonate from the base to form water and carbon dioxide gas while the salt is formed by combining the cation from the base with the anion from the acid. Decomposition Reaction: AB → A + B In this type of reaction, there is a breaking down of reactant into two or more products. To make this reaction occur, there is often heat, light, or electricity (input of energy). Synthesis or Combination Reaction: A + B → AB In this type of reaction two or more substances (reactants) react to produce one product. Combination reactions are exothermic (heat is released). Combustion Reaction: C x H y O z (l) + O 2 (g) → CO 2 (g) + H 2 O (g) These reactions occur rapidly and produce a flame. Most combustion reactions have O 2 as a reactant in the equation. Hydrocarbons combusted in air react with O 2 to form CO 2 and H 2 O. 3 3 3 3

INVESTIGATION GOALS In this experiment, you will observe examples of basic types of chemical reactions that occur as described below. You will write your observations of the reactions. Based on those observations and the given reactants, you will write complete, balanced chemical equations to effectively communicate the chemistry of the reactions. This investigation is comprised of two parts: Part 1, you will be assigned a set of 5 unknown aqueous solutions that must be identified based on their physical and chemical behavior. Once identified, balanced molecular, total ionic, and net ionic chemical equations will be written for each reaction. Part 2, you will develop a procedure to observe six chemical reactions proposed. Upon observing the results of the reactions, you will classify each reaction type and provide a balanced chemical equation.

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I. OBJECTIVES ● Recognize when a reaction occurs. ● Record initial observation of solutions including pH, color, odor, viscosity, etc. ● Learn how to describe and document the results of mixing solutions. ● Identify 5 unknown solutions based on the results of initial observations and reactivity. ● Provide a brief proposal in you’re here addressing the basic experimental steps to meet these objectives. Once approved, work with your team of investigators to collect and analyze the data. II. PROCEDURE DEVELOPMENT In order to identify each of the 5 unknown solutions, develop a method to react each solution with each of the others for a total of 10 combinations. Document the result of each mixture, use the results to help identify each of the 5 solutions. After identification, write an equation for the reactions that occur. NOTE THAT NOT ALL COMBINATIONS WILL RESULT IN A CHEMICAL REACTION . *For your reference, sample data tables are provided in section IV: DATA COLLECTION & CALCULATIONS You will be provided one of the following sets of chemicals in bottles, each labeled with an unknown letter: YELLOW BIN Bottle Contents BLUE BIN Bottle Contents RED BIN Bottle Contents silver nitrate silver nitrate silver nitrate manganese(II) nitrate barium nitrate lead(II) nitrate barium nitrate hydrochloric acid hydrochloric acid hydrochloric acid sulfuric acid ammonium hydroxide sodium hydroxide sodium hydroxide water *Ba(OH) 2 = According to solubility rules it is predicted to be aqueous, but this isn’t true. It is only partially soluble so a solid precipitate can be seen. Experimental Preparation: Once you have been assigned your set of unknowns, identify the theoretical behavior of each of the contents. This will assist with the chemical analysis you will perform. ● Write the chemical formula for each compound listed for your bin. ● Identify whether you would expect it to be acidic, basic, or neutral. Procedure for Part 1: Identification of UNKNOWN SOLUTIONS

● For each compound, use the solubility rules provided in the introduction to identify any of the other bin contents that would form a precipitate if the two were mixed. ❑ Confirm your proposed theoretical behavior and reactivity with your TA before continuing. Initial Observations: Make initial observations of each individual solution for pH, color, odor, viscosity. ● Consider what glassware you will need to visually inspect small amounts of each solution. ● For pH testing, place a piece of pH paper (~1 inch in length) on a watch glass, moistened with DI water to help stick. Using a disposable pipet, add 1-2 drops of each solution to the pH paper.

Chemical Reactivity: Make chemical reactivity observations by reacting all combinations of two unknown substances in plastic conical test tubes. Record observations including any observations of heat change, formation of insoluble solid/precipitate, solution color changes, gas formation, odor, pH etc. ● What approximate volumes do you plan to use for the reactions? Consider that you only need to have enough to clearly see results and don’t want too much as waste reagents. ● What kind of glassware do you propose to use for these observations based on the volumes you propose above? ● With the help of your TA, use a centrifuge to separate the precipitates. ❑ Confirm your observation results with your TA before continuing. Identification of Unknowns: Use observations to identify the contents of unknown substances in bottles, based on the chemical reactions that occurred. ● Consider how each of your unknowns reacted above and try to match them according to the list provided by your TA. ● Look online for images of possible chemicals and reaction products for each of your substances. Record your findings in here . ❑ Identify the possible chemicals in each bottle. Confirm your results with your TA before continuing. Writing Equations: Recognize various types of chemical reactions occurring, and use solubility rules to write balanced molecular, ionic and net ionic chemical equations for each combination resulting in a chemical reaction. Include physical states of all reactants and products. ● Write balanced molecular, ionic and net ionic chemical equations for each of the combinations resulting in a chemical reaction. Include physical states of all reactants and products. ❑ Confirm with your TA that you have the correct equations for each reaction. III. EXPERIMENTAL CONSIDERATIONS Observations of each reaction are very important! You will need to record your results in detail. ● You will need to be able to identify whether there was evidence of a reaction and properly record results. Remember: Evidence of a reaction occurring can include formation of a solid precipitate, evolution or absorption of heat, change in color, formation of gas, change in pH, etc. ● Use terms like “white solid”, “brown solid”, “clear, colorless solution,” “heat evolved,” “pH changed from to ,” “no change,” “gas bubbles” etc. to describe the reaction results. Specific Waste & Safety: ❑ H2SO4, HCl, NaOH, and NH4OH are highly corrosive. Ba(NO3)2, AgNO3, Mn(NO3)2, and Pb(NO3)2

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are toxic. All chemicals should be disposed in the designated WASTE container in the fume hood. ❑ Please use gloves and paper towels to clean up any spills immediately, disposing of contaminated materials in the trash. Any spills left behind might result in harming skin. ❑ Rinse all solids from spot plate analysis and/or plastic conical test tubes into your waste beaker before washing with soap and water.

IV. DATA COLLECTION & CALCULATIONS For this part of the investigation we recommend that you record the following data and calculations. ● To organize the theoretical chemical behavior for the unknowns in your set: Enter results below: Chemical Names Given for Your Set Chemic a l Formul as Check whether it is expected to be List the formulas of all other compounds in the set that would form a precipitate if mixed with this. (Use Solubility Table/Rules) Acidi c Bas ic Neutr al silver nitrate AgNO 3 Y HCl manganese(II) nitrate Mn(NO 3 ) 2 Y AgNO 3 barium nitrate Ba(NO 3 ) 2 Y HCl hydrochloric acid HCl Y AgNO 3 sodium hydroxide NaOH Y Ba(NO 3 ) 2 ● For Chemical analysis and Observations of the solutions: Enter results below: Bo ttle Le tte r La bel Initial Observations: Color/odor/etc. of substance in bottle Color of Red Litmus After Testin g* Color of Blue Litmus After Testin g* Acidic, Basic or Neutral ? I Colorless, rubberish Red Red Acidic M Colorless, odorless Red Blue Neutr al E Colorless, odorless Red Blue Neutr al G Colorless, Odorless Blue Blue Basic F Colorless, Odorless Red Red Acidic * (Litmus Paper (blue and red): pH > 8.3, Red → Blue; pH < 4.5, Blue → Red ● For recording the reactivity of each combination of the solutions: Remove the following page and fill in the information below to catalog your results: 1. List the letter labels on each of the bottles in your set

2. Indicate which solutions are mixing Ex: A + B 3. Write all observations for the results of mixing of each combination. ● Use terms like “white solid”, “brown solid”, “clear, colorless solution,” “heat evolved,” “pH changed from to ,” “no change,” “gas bubbles” etc. to fill the reaction results. 4. Fill in whether a reaction occurs: Yes or N/R (No Reaction)

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1. Letter Labels on the Bottles 2. What is Mixi ng? 3. Observations upon Mixing 4. Did Rxn Occu r? E F M I G Soluti on Com binati ons x x E + F Still a colorless odorless solution no x x E + M Still a colorless odorless solution no x x E + I A white precipitate is formed yes X X E + G A brown precipitate is formed yes x X F + M Still a colorless odorless solution no x x F + I Still a colorless odorless solution no X x F + G A white precipitate is formed yes x x M + I Still a colorless odorless solution no x x M + G A white precipitate is formed yes x x I + G Heat was released yes ● For the identification of the unknown solutions: Enter results below: Chemical Formula Bo ttle Le tte r La bel Evidence from Lab used to Support this Identification silver nitrate E AgNO 3 + HCl —> AgCl + HNO 3 manganese(II) nitrate F Mg(NO 3 ) 2 + NaOH -> Mg(OH) 2 + NaNO 3 barium nitrate M Ba(NO 3 ) 2 + NaOH -> Ba(OH) 2 + NaNO 3 hydrochloric acid I HCl + AgNO 3 -> HNO 3 + AgCl sodium hydroxide G NaOH + HCl -> NaCl + H 2 O ● Make sure to leave enough space to write the balanced molecular, total ionic, and net ionic equations for all of the reactions that occur *Ba(OH) 2 = According to solubility rules it is predicted to be aqueous, but this isn’t true. It is only partially soluble so a solid precipitate can be seen.

Reagents Combined: AgNO 3 + HCl Molecul ar AgNO 3(aq) + HCl (aq) —> AgCl (s) + HNO 3(aq) Ionic Ag + (aq) + NO 3 - (aq) + H + (aq) + Cl - (aq) -> AgCl (s) + H + (aq) + NO 3 - (aq) Net Ionic Ag + (aq) + Cl - (aq) -> AgCl (s) Reagents Combined: Mg(NO 3 ) 2 + NaOH Molecul ar Mg(NO 3 ) 2(aq) + NaOH (aq) -> Mg(OH) 2(s) + NaNO 3(aq) Ionic Mg 2+ (aq) + NO 3 - (aq) + Na + (aq) + OH - (aq) -> Mg(OH) 2(s) + Na + (aq) + NO 3 - (aq) Net Ionic Mg 2+ (aq) + OH - (aq) -> Mg(OH) 2(s) Reagents Combined: Ba(NO 3 ) 2 (aq) + NaOH (aq) Molecul ar Ba(NO 3 ) 2 (aq) + NaOH (aq) -> Ba(OH) 2 (s) + NaNO 3 (aq) Ionic Ba 2+ (aq) + 2NO 3 - (aq) + Na + (aq) + OH - (aq) -> Ba(OH) 2 (s) + Na + (aq) + NO 3 - (aq) Net Ionic Ba 2+ (aq) + OH - (aq) -> Ba(OH) 2 (s) Reagents Combined: NaOH (aq) + HCl (aq) Molecul ar NaOH (aq) + HCl (aq) -> NaCl (aq) + H 2 O (l) Ionic Na + (aq) + OH - (aq) + H + (aq) + Cl - (aq) -> Na + (aq) + Cl - (aq) + H 2 O (l) Net Ionic no net ionic reaction

I. OBJECTIVES ● Develop procedures to complete the six proposed reactions. ● Properly record experimental observations of each reaction. (initial observations, reaction observations, procedural steps). ● Use reaction observations to objectively analyze the results of the reaction. ● For each of the 6 reactions: Write a balanced molecular equation and include physical states for reactants and products . If the reaction can be simplified further, also write a balanced net ionic equation. ● Use the information provided in the introduction along with your experimental observations and results to identify the reaction class for each of the proposed reactions. ● Provide a brief proposal in you’re here addressing the basic experimental steps to meet these objectives. Once approved, work with your team of investigators to collect and analyze the data. II. PROCEDURE DEVELOPMENT Develop a procedure to meet all of the objectives above for each of the 6 proposed reactions (single- replacement, double-replacement, decomposition, combustion, combination, and acid/base). The six proposed reactions may not contain all information of chemical formulas or specific volumes. Use your knowledge of chemistry to identify the reaction species and propose a procedure for investigating the results of these combinations. PRIOR TO BEGINNING: ALL VOLUMES, PROCEDURES, AND SAFETY CONCERNS IN THE FOLLOWING SECTIONS MUST BE ADDRESSED IN YOUR PROPOSAL AND APPROVED BY YOUR TA. Each proposed reaction should include: ● the proposed amount (and concentration if aqueous) of each reactant, including its chemical formula and physical state. ● a brief or bulleted procedure for combining the reactants (in a p l a s t i c c o n i c a l test tube, beaker, watch glass, introduction of flame, etc.) and any additional procedural steps (centrifuging, filtering, etc.) ● a list or table outlining the data to be collected. Include space for calculations or summaries of results that may be required. *For your reference, sample data tables are provided in section IV: DATA COLLECTION & CALCULATIONS Procedure for Part 2: Analysis and identification of various reaction types

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Reaction #1: magnesium strip and 1M HCl ● IMPORTANT: Use steel wool provided to scrape off oxidation from magnesium strip. Make sure the magnesium strip is completely covered with 1M HCl. ● How long should you allow the reaction to complete? ● What kind of glassware do you propose to use for these observations based on the volumes you expect to use?

Reaction #2: 0.1M copper (II) chloride and 0.1M sodium phosphate ● After combining the solutions, what two phases should exist in your test tube? ● How will you separate the precipitate from the supernatant (remaining aqueous solution) within the test tube? o Develop a procedure to separate the precipitate Reaction #3: 3% hydrogen peroxide with yeast catalyst (*do not include yeast as reactant or product in chemical equation) ● IMPORTANT: Use a 50 mL beaker to allow enough room for the reaction. ● Add 1 mL of yeast solution prepared by your TA. How long should you allow the reaction to continue? ● How will you know when the reaction is complete? ● Where will you place beaker while reaction is occurring? ● What is the purpose of the yeast in the reaction? ● Watch https://youtu.be/-pSstufKCSM ● Develop a procedure to check if oxygen gas was produced using a glowing wooden splint. Reaction #4: introduction of flame to copper metal ● Use candle lighter to light copper metal (while using crucible tongs to hold the metal) ● How long should you allow the reaction to continue? ● How will you know when the reaction is complete? ● Where will you place Cu strip after reaction is complete? ● What is reacting with Cu in the presence of the flame? ● Develop a procedure to check that a chemical reaction occurred. Compare your product with your TA. Reaction #5: 1M HCl and 0.1 M NaOH Reaction #5a&b: Reaction of 1M HCl and 0.1 M NaOH with pH paper ● Consider what procedure can be applied to test each reagent using a strip of pH paper.

● What do the results of the pH paper analysis confirm about the properties of these solutions? ● (A balanced chemical equation is not required for this combination set.) Reaction #5c&d: Reaction of 1M HCl and 0.1 M NaOH with phenolphthalein ● What is the purpose of using phenolphthalein indicator? ● What do the results of the indicator analysis confirm about the properties of these solutions? ● (A balanced chemical equation is not required for this combination set.) Reaction #5e: Combining 1M HCl and 0.1 M NaOH ● Consider how much of each you plan to combine. For complete reaction, should the number of drops be the same or combined in a specific ratio (like 1:2 or 2:3, etc)? ● Carefully consider the physical state of the products when writing the balanced chemical equation for the reaction. ● What do you expect the pH of the products to be? ● Analyze the product using pH paper and phenolphthalein, then decide if the results match your expectation? Reaction #6: Introduction of flame to isopropyl alcohol, C 3 H 7 OH Notify your TA before starting this reaction. 10-12 drops of isopropyl alcohol (C 3 H 7 OH) in an evaporating dish or watch glass towards the back of the lab bench, but away from the plastic clear panel and any papers. Light a match to directly burn the alcohol. ● In order to light a liquid on fire, why would a normal test tube not be appropriate? ● An evaporating dish has the capacity to handle the heat produced by a flame and allow safe introduction of the liquid with the source of the flame. ● In order to keep the fire small, it is more appropriate to use a match as opposed to a long splint. ● Describe a procedure to ignite and completely consume the isopropyl alcohol safely. ● Do not exceed 12 drops of isopropyl alcohol for your proposed volume. ● How will you know the reaction is complete? ● For safety, perform the reaction in the back of the lab bench away from the walls of the hood and clear of any other lab materials or papers. III. EXPERIMENTAL CONSIDERATIONS

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Place test tubes in beakers or on a test tube rack while reacting/studying for results analysis. Copper and Magnesium waste should be placed in solid waste container in the fume hood. Liquids, solution, and precipitate waste can go in the glass bottle waste container in the fume hood. Everything else (paper towels, matches, wooden splints, pH paper, litmus paper, etc,) can go in trash. WARNING: WHEN USING OPEN FLAMES, KEEP PAPERS and OTHER FLAMMABLES DISTANT. Specific Waste & Safety: Copper and Magnesium waste should be placed in solid waste container in the fume hood. Liquids, solution, and precipitate waste can go in the glass bottle waste container in the fume hood. Everything else (paper towels, matches, wooden splints, pH paper, litmus paper, etc,) can go in trash. WARNING: WHEN USING OPEN FLAMES, KEEP PAPERS and OTHER FLAMMABLES DISTANT ❑ HCl and NaOH are highly corrosive. Mg, Cu, CaCl 2 , Na 2 CO 3 , H 2 O 2 are irritants. Phenolphthalein and C 3 H 7 OH are flammable. All chemicals should be disposed in the designated WASTE container in the fume hood. ❑ Please use gloves and paper towels to clean up any spills immediately, disposing of contaminated materials in the trash can. Any spills left behind might result in harming skin. IV. DATA COLLECTION & CALCULATIONS For each reaction, the following information should be recorded in your lab here: a) Approximate amount or volume, the concentration (if applicable), and the physical state of each reactant with initial observations of each reagent before reacting. b) Brief description of procedure and observations of all components upon reaction. c) Write the balanced molecular chemical equation with physical states. If it is possible to simplify to a net ionic equation, write this as well. d) Give the type of reaction and an explanation for how you determined this. A similar table to the one below can be constructed for most of the reactions for this section. Leave plenty of space for your descriptions, observations, balanced equations, and conclusions Rx n # a. Reactant amount, concentration, physical state, and initial observations b. Experimental Procedure and Observations of Reaction Reactant 1 Reactant 2 E x: 5 mL H 2 O Clear / colorless 0.5” filing of Na(s) Soft Silver metal Metal melted into a ball and skipped across solution, catching fire until dissolving completely after 10 minutes of reaction. Solution basic after reaction. c. Balanced Equation(s) with Physical States : Na (s) + H 2 O (l) ? NaOH (aq) + H 2 (g)

d. Type of Reaction: single replacement Final Cleanup and Waste Collection ❑ When you have finished the entire experiment return glassware to your drawer(s). ❑ Place all distilled water used in this investigation down the sink. ❑ Solutions containing dye should go in the designated WASTE container in fume hood. ❑ DO NOT place solids in the original container, dispose of paper towels, litmus paper, wooden splints, metals, etc, in the designated trash. ❑ Clean up your bench area and balance room. Before you Leave: ❑ Confirm your results with your TA and begin worksheet.

Assignment #4a Group Proposal-Notes

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