Lab Report Worksheet_ What is the Chemical Reaction

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Lab Report Worksheet: What is the Chemical Reaction? Lab Section (or Day-Time): Wednesday 10-11:50 Group Number: 4 Due Date: September 28 Name(s): Daniel C. Musaev, Camryn Kozak, Ammaar Zindani, Fatima Torres-Granados Part 1: Identification of Unknown Solutions 1. Circle the set assigned to your group: RED BLUE YELLOW 2. Complete the table for the theoretical behavior you predicted for the chemical names in the set you were assigned. Chemical Names Given for Your Set Chemical Formulas 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) H 2 O can be a possible product Acidic Basic Neutral Silver nitrate AgNO3 x HCl, NH4OH Lead (ii) nitrate Pb(NO3)2 x HCl, NH4OH Hydrochloric acid HCl x Pb(NO3)2, AgNO3 Ammonium hydroxide NH4OH x AgNO3, Pb(NO3)2 Water H2O x none 3. Identify the following information for each of the unknown solutions after studying each individually: Bottle Letter Label Initial Observations: Color/odor/etc. of substance in bottle Color of Red Litmus After Testing* Color of Blue Litmus After Testing* Acidic, Basic or Neutral? I Clear, does not have a distinct smell Red Red Acidic

E Clear, does not have a distinct smell red blue neutral C Clear, does not have a distinct smell red blue neutral N Clear, does not have a distinct smell red red acidic U Clear, does not have a distinct smell Blue Red Basic *(Litmus Paper (blue and red): pH > 8.3, Red → Blue; pH < 4.5, Blue → Red) 4. Once you have determined which chemical is in which bottle, write the CHEMICAL FORMULA (not the name) next to its solution letter label. Give a short description of how you identified each unknown solution based on your observations BOTH initially and when mixed with another reagent. Chemical Formula Bottle Letter Label Evidence from Lab used to Support this Identification Initially Mixed NH4OH U Basic Formed a precipitate with silver and lead nitrate but formed water with HCl H2O C Neutral Did not form a precipitate with any compound AgNO3 E Neutral Did not form a precipitate with Pb(NO3)2 but did with NH4OH and HCl Pb(NO3)2 N Acidic When mixed with Ag(NO3)2, it did not form a precipitate but it did with HCl and NH4OH HCl I Acidic When mixed with silver and lead nitrate, it formed a precipitate 5. Write balanced molecular, complete ionic and net ionic chemical equations for each set that resulted in a chemical reaction. Include physical states of all reactants and products . * Depending on your set, you will only have 4, 5, or 6 chemical reactions possible. Reagents Combined: AgNO3 + HCl

Molecular AgNO3 (aq) + HCl (aq) -> AgCl (s) + HNO3 (aq) Ionic Ag+ (aq) + NO3- (aq) + H+ (aq) + Cl- (aq) -> AgCl (s) + H+ (aq) + NO3- (aq) Net Ionic Ag + (aq) + Cl- (aq) -> AgCl (s) Reagents Combined: AgNO3 + NH4OH Molecular AgNO3 (aq) + NH4OH (aq) -> AgOH (s) + NH4NO3 (aq) Ionic Ag+ (aq) + NO3- (aq) + NH4+ (aq) + OH- (aq) -> AgOH (s) + NH4+ (aq) + NO3- (aq) Net Ionic Ag+ (aq) + OH- (aq) -> AgOH (s) Reagents Combined: Pb(NO3)2 + HCl Molecular Pb(NO3)2 (aq) + 2HCl (aq) → PbCl2 (s)+ 2HNO3 (aq) Ionic Pb(2+) (aq) + 2(NO3)- (aq) + 2H+ (aq) + 2Cl- (aq) → PbCl2 (s) + 2H+ (aq) +2NO3- (aq) Net Ionic Pb(2+) (aq) + 2Cl- (aq)→ PbCl2 (s) Reagents Combined: Pb(NO3)2 + NH4OH Molecular Pb(NO3)2 (aq) + 2NH4OH (aq) → 2NH4NO3 (aq) + Pb(OH)2 (s) Ionic Pb+ (aq) + 2(NO3)- (aq) + 2NH4+ (aq) + 2OH- (aq) → 2NH4+ (aq) 2NO3- (aq) + Pb(OH)2 (s)

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Net Ionic Pb+ (aq) + 2OH- (aq) → Pb(OH)2 (s) Part 2: Analysis and Identification of Various Reaction Types 6. Summarize the reactions and reaction classes of each of the reactions studied in Part 2 in the following table: R x n #: Questions: Answer: 1 Balanced Molecular Equation: Mg (s) + 2 HCl (aq) -> MgCl2 (aq) + 2H (g) Type of Reaction: Single replacement Description of all indications that the reaction took place: Bubbling of magnesium strip, disintegration of magnesium strip, heat, loss of gas in substance/liquid 2 Balanced Molecular Equation: 3 CuCl2 (aq) + 2 Na3PO4 (aq) -> 6NaCl (s) + Cu3(PO4)2 (aq) Type of Reaction: Double replacement Description of all indications that the reaction took place: A blue precipitate formed at the bottom of the test tube with a clear liquid above it 3 Balanced Molecular Equation: 2H2O2 (aq) —> 2H2+O2 Type of Decomposition

Reaction: Description of all indications that the reaction took place: The mixture of yeast and hydrogen peroxide caused oxygen to form 4 Balanced Molecular Equation: 2Cu (s) + O2 (g) —> 2CuO (s) Type of Reaction: Combustion or Combination Description of all indications that the reaction took place: A change in color occurred in the wire strip from copper to black 5 Balanced Molecular Equation: HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l) Type of Reaction: acid-base Description of all indications that the reaction took place: The indicator had a pH of 3.0, the acid had a pH of 0.0 and the base had a pH of 7.0. The solution changed color when the indicator was added, forming a chalky, white liquid. The litmus paper also showed a reaction in the solution due to the change in pH. 6 Balanced Molecular Equation: 2C3H7OH (l) + 9O2 (g) -> 6H2O (l) + 8CO2 (g) Type of Reaction: combustion Description of all indications that the reaction took place: The isopropanol caught a flame which became smaller and then disappeared as time passed Answer the questions below about the reactions performed in Part 2:

7. For Reaction 1: a) What was the identity of the bubbles formed in the solution? Hydrogen gas b) What is the net ionic equation for Reaction 1? MgH2 c) Name another metal that would react with HCl in a similar way. Lead d) Name another metal that would not react with HCl. Potassium 8. For Reaction 2: a) What are the spectator ions in Reaction 2? Na+ and NO3- are the spectator ions in reaction two. b) Would Na 2 CO 3 aqueous salt combined with copper (II) chloride form a solid precipitate? If so, what would the precipitate be? Show your work. Yes. 2AgNO3 (aq) + Na2CO3 (aq) → 2NaNO3 (aq) + Ag2CO3 (s) Nitrates soluble, carbonate and silver not. Ag2CO3 is the precipitate. c) Would KNO 3 aqueous salt combined with sodium phosphate form a solid precipitate? If so, what would the precipitate be? Show your work. No, the ionic equation shows all ions are soluble and will not combine to form a precipitate. 3KNO3 (aq) + Na3PO4 (aq) → K3PO4 (aq) + 3NaNO3 (aq) 3K+ (aq) + 3NO3- (aq) + 3Na+ (aq) + PO4 3- (aq) → 3K+ + PO4 3- (aq) + 3Na+ (aq) + 3NO3- (aq) d) What technique could you use if you needed to separate the precipitate from the supernatant? Why would you choose this technique? I would use filtration as the liquid would pass through but the solid precipitate would not.

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9. For Reaction 3: a) What is the purpose of yeast in the chemical reaction? How does this relate to why it is not in the balanced chemical reaction? Yeast is the catalyst that causes the chemical reaction to occur. Yeast is not part of the chemical reaction because the identities of the reactants and products are fixed. b) What happens when a glowing splint is inserted into the test tube immediately after the reaction? Why? When a glowing splint is inserted into the test tube immediately after the reaction it reignites the splint because the reaction is producing a lot of Oxygen resulting in the flame to be reignited. 10. For Reaction 4: a) What is reacting with the copper in the presence of the flame? The copper turns black. b) What was the purpose of the flame in this instance? The purpose of the flame is to create a chemical reaction with the copper. 11. For Reaction 5: a) Which is the acid and which is the base for this reaction? The acid is the HCl and the base is the NaOH b) What was the color of the results for the indicator AND pH paper tests for the acid and for the base? Indicator-orange , acid-red , base-green pH Paper Phenolphthalein Indicator Acid Red (0.0) Orange (3.0)

Base Green (7.0) Orange (3.0) c) How was pH paper more useful for this reaction than red & blue litmus paper? It tells you exactly what the pH is instead of telling us whether it is acidic or basic, which we have already determined. d) Are acid base reactions exothermic or endothermic? exothermic e) What is the expected pH of a strong acid/ strong base neutralization reaction? 7.0 f) What is the product of the net ionic reaction for the strong acid /strong base reaction? H(+) +Cl (-) + Na (+) +OH (-) → H20 (l) (-) + Na (+) + Cl (-) 12. For Reaction 6: a) What elements combine to form isopropyl alcohol? Carbon, Hydrogen, and Oxygen. C3H8O b) Name another compound that combines with oxygen to form the same products seen in Reaction 6. Another compound that combines with oxygen to form the same products seen in Reaction 6 is propylene (CH2CHCH3).