3. Write the equation to calculate percent error. Data Part 1: Length Measurements (all values must include units) A. Length of notebook in cm:

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1 Name: Date: Lab Section Experiment 1: Basic Measurement Techniques REPORT SHEET Pre-lab Study Questions: 1. Objectives of the experiment (in your own words): 2. In our everyday speech, precision and accuracy are used interchangeably. In science, do precision and accuracy mean the same thing? If not, explain the difference. 3. Write the equation to calculate percent error. Data Part 1: Length Measurements (all values must include units) A. Length of notebook in cm: B. Width of notebook in cm: Calculations Part 1 (show your work for full credit): 1. Length of notebook in inches: 2. Width of notebook in inches: 3. Length in mm: 4. Width in mm: Data Part 2: Temperature Measurements (all values must include units) A. Room temperature in C: B. Ice Bath temperature in C: Calculations Part 2 (show your work for full credit): 1. Room temperature in K: 2. Room temperature in F: 3. Ice bath temperature in K: 4. Ice bath temperature in F: 1

2 Data Part 3: Volume Measurements (all values must include units) A. Sketch of graduated cylinder with meniscus in box - : (indicate with an arrow where the volume should be read) B. Volume of H 2 O from small test tube: C. Volume of H 2 O from large test tube: D. Volume of water from 50-mL beaker: E. Volume of water from 50-mL Erlenmeyer Flask: Data Part 4: Mass Measurements (all values must include units) A. Type of balance used: B. Mass of large test tube: C. Mass of 50-mL beaker: D. Mass of 150-mL beaker: Data Part 5: Density determinations (all values must include units) Data for 2-mL sample of unknown liquid: A. Mass of empty 10-mL graduated cylinder: B. Approximate volume of unknown liquid added: C. Actual volume of unknown liquid added (remember sig figs): D. Mass of cylinder plus unknown liquid: E. Mass of liquid alone: Calculate density of 2-mL unknown liquid sample using data from C and E above: (include units) Accepted (textbook) density value for unknown liquid (obtain from instructor): Calculate % error between accepted density and experimental (your) value: % error = Absolute error x 100 Accepted value % error for 2-mL sample: Data for 10-mL sample of unknown liquid: A. Mass of empty 10-mL graduated cylinder: B. Approximate volume of unknown liquid added: C. Actual volume of unknown liquid added (remember sig figs): D. Mass of cylinder plus unknown liquid: E. Mass of liquid alone: Calculate density of 10-mL unknown liquid sample using data from C and E above: (include units) Accepted (textbook) density value for unknown liquid (obtain from instructor): Calculate % error between accepted density and experimental (your) value: % error = Absolute error x 100 Accepted value % error for 10-mL sample: 2

3 Data for the unknown solid A. Unknown number: B. Mass of irregular solid: C. Volume of water in graduated cylinder: D. Volume of water plus object: E. Volume of object alone: Calculate the density of the irregular solid using data from B and E above: Questions: Answer the following questions and turn in with your report. 1. What is the mathematical relationship between ml and cm 3? 2. Which of the following measurements devices do you think would be accurate enough to use for precise measurement of volumes: 50-mL beaker; 50-mL Erlenmeyer flask; 50-mL graduated cylinder. 3. Suppose a student makes an error of 0.1-mL in measuring 1.0-mL of liquid (i.e., he records the value as 1.1-mL when it was actually 1.0-mL). What is the percent error? Show your work. 4. Suppose another student makes an error of 0.1-mL in measuring 10.0-mL of liquid (i.e., she records 9.9-mL when it is actually 10.0-mL). What is the percent error? Show your work. 3

4 5. Based on your answer to questions 3 and 4 above, which of the determinations of density for your unknown liquid would you expect to be more accurate the 2-mL sample or the 10-mL sample? 6. Which of your two values actually was more accurate? 4

5 Name: Date: Lab Section Experiment 2: Molecular Models REPORT SHEET Pre-lab Study Questions: 1. Objectives of the experiment (in your own words): 2. What kinds of electrons form the covalent bonds in molecules? 3. Is a polar molecule symmetrical or asymmetrical? FORMULA OF MOLECULE example: CH 4 LEWIS STRUCTURE H H C H H 3-D SHAPE w/lone pairs MOLECULAR GEOMETRY tetrahedral MOLECULAR POLARITY nonpolar H 2 O H 3 O + C 2 H 6 C 2 H 4 C 2 H 2 CO 2 H 2 O 2 CH 3 Cl 5

6 FORMULA OF MOLECULE LEWIS STRUCTURE 3-D SHAPE w/lone pairs MOLECULAR GEOMETRY MOLECULAR POLARITY CH 2 Cl 2 CHCl 3 CCl 4 H 2 S NH 3 NH 4 + Br 2 N 2 CH 3 OH CH 2 O HCl 6

7 FORMULA OF MOLECULE LEWIS STRUCTURE 3-D SHAPE w/lone pairs MOLECULAR GEOMETRY MOLECULAR POLARITY H 2 CO 3 HCO 3 CO 3 2 SO 2 SO 3 H 2 SO 4 SO 4 2 Questions 1. Explain why the model for each of the following atoms has a specific number of bonds: a. Hydrogen: 1 bond b. Oxygen: 2 bonds c. Nitrogen: 3 bonds d. Carbon: 4 bonds 7

8 2. Discuss the shapes of SO 2 and SO 3. Why is one polar and the other is not? 3. Explain why and ion such as NH 4 +, CO 3 2, and SO 4 2 can be nonpolar, but charged? 4. Explain how molecules of H 3 O + and NH 4 + form from uncharged molecules of H 2 O and NH 3. 8

9 Name: Date: Lab Section Experiment 3: The Gas Burner REPORT SHEET Pre-lab Study Questions: 1. Objectives of the experiment (in your own words): 2. Describe the differences in appearance between a luminous and nonluminous flame. 3. What are the possible products of combustion of natural gas? Observations and Data 1 & 2: Sketch your burner in Box 1 below. Label the base, the barrel, the collar, the air ports and the gas adjustment screw. Box 1 Box 2 Observations and Data 3 & 4: Sketch the non-luminous flame in Box 2 above. Indicate (by drawing a line to) the location of the top of the flame, the tip of the inner blue cone, and the base of the flame. Also, note the comparative temperatures of these locations according to your observations. Time required to turn wire gauze red (include units): Tip of flame tip of inner blue cone flame next to top of barrel 5. What appears on the glass when the flame is dashed across the beaker of cold water? (Hint: check products of combustion in introduction) 6a. What occurs when the crucible is held in the luminous (yellow) flame? 6b. What occurs when the crucible is held in the non-luminous (blue) flame? 9

10 Questions: Refer to the Introduction of the experiment, the Procedures, your instructor s directions, and your observations to answer these questions. 1. Why should you not hold your lighted match over the top of the burner while you turn on the gas? 2. A) Suppose when you lighted your burner, it had a luminous flame. What should you do to get a properly adjusted flame? B) Suppose when you lighted your burner, it had a loud roaring sound. What should you do to correct it? C) Suppose when you lighted your burner, the flame disappeared down into the barrel. How do you obtain a properly adjusted flame? 3. A) What product of combustion is shown to be present by the results of dashing the flame across the cold beaker surface? B) What product of combustion is shown to be present by the results of holding the crucible in the luminous flame? C) Why did the deposit in (B) not appear when you held the crucible in the non-luminous (blue) flame? 10

11 Name: Date: Lab Section Experiment 5: Using qualitative analysis to identify ions REPORT SHEET Pre-lab Study Questions: 1. Objectives of the experiment (in your own words): 2. Which anion in this experiment can give off gas bubbles when tested with HCl? 3. What three cations in this experiment will produce characteristic colors in the flame test? Part 1: Anion observations and Data Procedure Anion Tested Observations for known Observations for unknown Chloride test Cl - Sulfate test SO 4 2- Phosphate test PO 4 3- Carbonate test CO 3 2- Unknown Number Identification of Unknown anion Teacher confirmation initials: Part 2: Cation observations and Data Procedure Cation Tested Observations for known Observations for unknown Flame tests Na + Sr + Ca +2 Oxalate test Ca +2 Ammonium test NH 4+ Unknown Number Identification of Unknown Cation / Teacher confirmation initials: 11

12 Questions (attach extra sheets if you need more space for your answers): 1. For Part 1, write the net ionic equations for any precipitates that formed or gases evolved 2. For Part 2, write the net ionic equations for any precipitations that occurred. 3. Give a simple test that would allow you to distinguish between the following pairs of anions. Tell what you would do and what you should observe for each anion. a. CO 3 2- and SO 4 2- b. Cl - and SO 4 2- c. CO 3 2- and PO Give a simple test that would allow you to distinguish between the following pairs of cations. Tell what you would do and what you should observe for each cation. a. Na + and Ca 2+ b. Ca 2+ and Sr + c. Na + and NH Write the symbol of the cation or anion that give(s) the following reaction: a. Forms a precipitate with AgNO 3 that does not dissolve in HNO 3. b. Forms a gas with HCl. c. Gives a bright, yellow-orange flame test. d. Forms a precipitate with BaCl 2 that does not dissolve in HNO 3. 12

13 Name: Date: Lab Section Experiment 8: Production and Investigation of four gases REPORT SHEET Pre-lab Study Questions: 1. Objectives of the experiment (in your own words): 2. What are the four gases that your will be investigating in this experiment? 3. Which of the gases will your instructor produce as a demonstration? Observations and Data: Part 1 Hydrogen, H 2 A. Reagents used for preparation: B. Color of gas: C. Effect upon lighted splint: Part 2 Carbon Dioxide, CO 2 A. Reagents used for preparation: B. Color of gas: C. Effect upon lighted splint: D. Addition of limewater to carbon dioxide: E. Result of pouring carbon dioxide into limewater: F. Result of blowing into limewater: Part 3 Oxygen, O 2 A. Reagents used for preparation: B. Color of gas: C. Effect upon glowing splint: Part 4 Nitrogen Dioxide, NO 2 A. Reagents used for preparation: B. Color of gas: 13

14 Questions 1. What observation did you make that makes you believe that gases are less dense than water? 2. Is carbon dioxide less dense than air? What evidence do you have for your choice? 3. If you fill a balloon with Helium, He, it rises because He is lighter or less dense than air. What do you think would happen to a balloon filled with CO 2? Hint: consider your answer to question Which of the gases you observed today would be the most helpful in putting out a fire? What evidence do you have to support this choice? 5. Bases on what you learned today, tell how you could distinguish between the following pairs of gases: a. CO 2 and NO 2 b. H 2 and CO 2 c. O 2 and H 2 6. Now suppose you were given a sample of one of the four gases you observed today. a. If the sample gas is colorless, which gas does this eliminate? b. If a portion of the same sample gas is bubbled through limewater and nothing happens, which gas is eliminated? c. If a glowing splint reignites when it is placed in another portion of the same sample gas, what is the identity of the gas? 14

15 Name: Date: Lab Section Experiment 11: Studying Ionic Reactions REPORT SHEET Pre-lab Study Questions: 1. Objectives of the experiment (in your own words): 2. What does an aqueous solution mean? 3. What kind of charge does a cation have? What kind of charge does an anion have? Observations and Data: Provide both possible combinations, check appendix H for solubility. Set I K + / Cl - Na + / NO 3 - K + /CrO 4 2- Na + /CrO 4 2- Ba 2+ / Cl - Ba 2+ / NO 3 - Ba 2+ / Cl - Na + / CrO 4 2- K + / CrO 4 2- Na + / NO 3 - Net ionic equations for set I: Set II Al 3+ /Cl - Ba 2+ - / NO 3 Na + 2- / SO 4 Al / SO 4 Sr 2+ - / NO 3 Ba 2+ / Cl - Ba 2+ - / NO 3 Net ionic equations for set II: Ba 2+ / Cl - Sr 2+ / NO 3 - Al 3+ /SO

16 Set III Na + /NO 3 - Fe 3+ /Cl - Co 2+ / NO 3 - Co 2+ / Cl - Na + / OH - K + / OH - Net ionic equations set III: K + / OH - Na + / OH - Co 2+ / Cl - Co 2+ / NO 3 - Set IV Mg /SO 4 Ni 2+ / Cl - Mg 2+ /Cl - K + 2- / SO 4 Na + / OH - Net ionic equations set IV: Na + / OH - K + / SO 4 2- Mg 2+ /Cl - 16

17 Set V Ag + / NO 3 - K + / CrO 4 2- Al 3+ /SO 4 2- Na + /CrO 4 2- Sr 2+ /NO 3 - Ba 2+ / Cl - Sr 2+ / NO 3 - Na + / CrO 4 2- Al 3+ / SO 4 2- K + / CrO 4 2- Net ionic equations set V: Questions: 1. Make up your own solubility chart by using your observations to fill out the table below. Use the same symbols that are used in Appendix H. Check your results against the solubility table in Appendix H. Cl - CrO 4 2- NO 3 - OH - SO 4 2- Ag + Al 3+ K + Mg 2+ Na + Sr Referring to the table you have just prepared, make generalization about the solubility of compounds containing: a. The nitrate anion b. The sodium cation c. The potassium cation. **** Please attach your scratch work for the ion crosses. Full credit will not be given without showing your work.**** 17

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19 Name: Date: Lab Section Experiment 12: Titrations of Acids and Bases REPORT SHEET Pre-lab Study Questions: 1. Objectives of experiment (in your own words): 2. Show how to calculate the molar mass of oxalic acid dehydrate. 3. Which solution will be used as your standard solution? Part 1 Data, Preparing a Standardized solution: A. Volume of volumetric flask: B. Mass of Oxalic acid dihydrate: Part 1 Calculations (Show your work for full credit): 1. Moles of oxalic acid dehydrate: 2. Molarity of oxalic acid solution: Part 2 Data, Preparing a solution by Dilution: A. Volume of 6 M NaOH used: B. Final volume of diluted solution: Part 2 Calculation: Using the information from A and B above, calculate the approximate concentration of your diluted NaOH solution (Hint: M 1 V 1 = M 2 V 2, show your work for full credit): Part 3 Data, Standardizing a Sodium Hydroxide solution by Titration: Oxalic Acid Trial 1 (ml) Trial 2 (ml) Trial 3 (ml) Initial Volume Reading: Final Volume Reading: Volume Used: Sodium Hydroxide Trial 1 (ml) Trial 2 (ml) Trial 3 (ml) Initial Volume Reading: Final Volume Reading: Volume Used: 19

20 Summary of Calculations for Part 3: (Show your work and attach to this sheet): Trial 1 Trial 2 Trial 3 Mols of oxalic acid: Moles of NaOH: Volume NaOH (L): Molarity of NaOH: 1. Average Molarity of NaOH solution (add all 3 trials, divide by 3): 2. Percentage difference between high and low results: % Diff = {(High value Low value)/ Average} x 100 Part 4 Data, Standardizing an Oxalic Acid Solution by Titration: Oxalic Acid Trial 1 (ml) Trial 2 (ml) Trial 3 (ml) Initial Volume Reading: Final Volume Reading: Volume Used: Sodium Hydroxide Trial 1 (ml) Trial 2 (ml) Trial 3 (ml) Initial Volume Reading: Final Volume Reading: Volume Used: Summary of Calculations for Part 4: (Show all your work and attach to this sheet): Moles NaOH Moles Oxalic Acid: Vol Oxalic Acid (L): Molarity of H 2 C 2 O 4 : Trial 1 Trial 2 Trial 3 1. Average Molarity of Oxalic Acid solution(add all 3 trials, divide by 3): 2. Percentage difference between high and low results: % Diff = {(High value Low value)/ Average} x

21 Questions: 1. Why is the exact amount of water used to prepare the dilute sodium hydroxide solution in Part 2 not critical to know? 2. Suppose some deionized water was left in the buret before it was filled with the oxalic acid solution you were using as a primary standard. When you perform the standardization of sodium hydroxide in Part 3, how would the excess water affect the concentration of sodium hydroxide you calculate? 3. In Parts 3 and 4, why is it not necessary to dry the Erlenmeyer flask you use for titrations? 21

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23 Name: Date: Lab Section Experiment 13: Observing Physical Properties Boiling Point, Solubility and Conductivity REPORT SHEET Pre-lab Study Questions: 1. Objectives of experiment (in your own words): 2. Boiling points, molecular masses and chemical formula of hydrocarbons: (fill in table below) Hydrocarbon Chemical formula molecular mass Boiling Point ( C) (g/mol) Methane Ethane Propane Butane Pentane Hexane Heptane Octane Nonane Decane 3: What trends do you observe in boiling point and molecular mass for the hydrocarbons you checked in the Handbook of Chemistry and Physics? (If you didn t use CRC, please list website(s). Observations and Data Part 1: Boiling Point Determination (all values must contain units) A. Observed boiling point of water: B. Accepted value for the boiling point of water: Observations and Data Part 2: Miscibility Test Tube # Liquid 1 (name) Liquid 2 (name) Miscible or Immiscible? 23

24 Observations and Data Part 3: Solubility of Solids in Liquids. Label each solid as soluble or insoluble in the appropriate solvent. Describe what you see. Liquid sample (3-mL) Iodine I 2 sodium chloride NaCl Sucrose C 12 H 22 O 11 Potassium Nitrate KNO 3 Paraffin wax 1. DI water 2. methanol 3. hexane 4.ethyl acetate Observations and Data Part 4: Electrolytes. For each electrolyte you test, list the name of the material, and tell if the light bulb glows brightly, glow dimly, or not at all. Electrolyte Name Light Bulb? Electrolyte Name Light Bulb? Questions: 1. What generalizations can you make about the nature of solvents that dissolved ionic solids the best? 2. What generalizations can you make about the solids that are electrolytes? 3. The four liquids that you tested may be ranked in order of decreasing polarity as follows: (most polar) water > methanol > ethyl acetate > hexane (least polar) Based on the data you gathered, what generalizations can you make about the relationship between polarity and miscibility? 4. Based on your answer to question 4, which of the four liquids would probably best dissolve a polar solid such as NaCl? 5. Which liquid would best dissolve a nonpolar solid such as paraffin? 24

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63 Formula for a Hydrate Spring 2015 Hyd-1 Handout (MPC) OBJECTIVES The student will be able to: 1. write or identify the definitions of hydrate, hydrated salt, water of hydration, water of crystallization, and anhydrous salt. 2. convert between the name and chemical formula for hydrates. 3. measure the mass of an object accurately to 0.01 g. 4. convert between mass and moles using the molar mass. 5. find the formula for a hydrate from the mass of water released when a measured mass of a hydrate is heated. Introduction Some ionic compounds have water molecules attached to the ions making up the crystalline structure. These compounds are called hydrated salts or hydrates. The water molecules that are loosely attached to these ions are called water of hydration or water of crystallization. Examples of hydrated salts are copper(ii) sulfate pentahydrate (or cupric sulfate 5-hydrate), CuSO 4. 5H2 O, iron(iii) chloride hexahydrate, FeCl 3. 6H2 O, and sodium sulfate decahydrate, Na 2 SO 4. 10H2 O. Many hydrates can be made to lose their water of hydration by heating. CuSO. 4 5H 2 O(s) CuSO 4 (s) + 5 H 2 O(l) The salt without its water of hydration is called an anhydrous salt. In this experiment you will use the hydrated salt of magnesium sulfate, MgSO 4. X H2 O. The goal of the experiment will be to find X. The X value describes the number of water molecules for one magnesium sulfate formula unit. The number of molecules and formula units can be described in moles, so X is the molar ratio of water molecules to formula units of the MgSO 4. X = moles H2 O moles MgSO 4 The hydrate will be weighed and then heated to drive off the water. The anhydrous salt will then be weighed. The difference in mass between the hydrated salt and the anhydrous salt is the mass of water lost. The masses of water and the anhydrous salt can be converted to moles with their molar masses. The ratio of these molar values will yield X.

64 Hyd-2 Spring 2015 Formula of a Hydrate 1. Clean a crucible. Procedure 2. Place the crucible on a triangle supported on a ring stand and heat with a Bunsen burner flame for 5 minutes. 3. Allow the crucible to cool and then weigh. Use crucible tongs to carry crucible. Touching the crucible with your fingers can alter the mass of the crucible. Report your mass to 0.01 g. 4. Add the hydrated magnesium sulfate to the crucible so that the crucible is less than 1/4 full. Weigh the crucible and contents. 5. Return the crucible and contents to the triangle. Heat the sample gently for five minutes. The crucible should be slightly above the flame of the Bunsen burner. 6. Lower the crucible to just above the tip of the inner core of the Bunsen burner flame and heat for ten more minutes. 7. Allow the crucible to cool to room temperature and reweigh. 8. Calculate the original mass of the hydrated salt. 9. Calculate the mass of the anhydrous salt after driving off the water. 10. Calculate the mass of the water released. 11. Calculate the moles of water. 12. Calculate the moles of the anhydrous magnesium sulfate. 13. Find the formula of the salt.

65 Formula for a Hydrate 01/11/15 Hyd-3 Spring 2015 Report Sheet for Formula for a Hydrate Student Date: Section Pre-lab Study Questions: 1. Objective of activity (in your own words): 2. What is a water of hydration or crystallization? 3. How do we indicate that a compound contains waters of hydration? DATA FOR FORMULA OF A HYDRATE Mass of crucible Mass of crucible and hydrated salt Mass of crucible and anhydrous salt after heating Mass of the hydrated salt Mass of the anhydrous salt Mass of the water lost Moles of water Moles of MgSO 4 Formula of the hydrate Show your calculations here.

66 Hyd-4 Spring 2015 Formula of a Hydrate Post-lab Questions: 1. Why was the crucible heated before you took its initial weight? 2. How would incomplete heating affect your calculation of the formula? 3. Would the number of waters in your formula be too high or too low? Why?

67 Activity Series Spring 2015 Single-1 MPC Handout SINGLE DISPLACEMENT REACTIONS: ACTIVITY SERIES OBJECTIVES The student will be able to: 1. write or identify a general description of single displacement reactions. 2. write or identify definitions of activity and activity series. 3. decide the relative activities of metals and hydrogen by doing a series of single exchange reactions. BACKGROUND Single displacement reactions have the following general equations. A + CD AD + C They are often called single exchange or single replacement reactions. In the first four parts of this experiment, you will add a metal to a water solution containing a compound composed of a metal ion and a negative ion. If a reaction takes place the metal that began as a solid will replace the metal ion. The following is an example. Zn(s) + CuSO 4 (aq) ZnSO 4 (aq) + Cu(s) A metal that will replace another metal in the above type of reaction is said to be more active than the metal replaced. Zinc is more active than copper. An activity series lists the relative activities of metal ions and hydrogen. In the next two tests, you will add a metal to a sulfuric acid solution. If a reaction takes place, the metal replaces the hydrogen, and hydrogen gas is released. Mn(s) + H 2 SO 4 (aq) MnSO 4 (aq) + H 2 (g) A metal that will replace hydrogen in this type of reaction is more active than H 2. PROCEDURE 1. Combine the reactant pairs listed on the data sheet. a. Clean a strip of the metal with steel wool. b. Place the metal on a watchglass or in a well of a well plate. c. Add a drop of the other reactant onto the solid metal. 2. Record your observations on the data sheet. Pay special attention to changes of color in the solution, changes of color or texture of the metal, and the evolution of gas. 3. If a reaction takes place, complete the chemical equation for the reaction. All of the metals used form 2+ ions. 4. If there is no obvious reaction, write "no reaction".

68 Single-2 01/11/15 Single Displacement Reactions

69 Single Displacement Reactions Spring 2015 Single-3 Student Name Date: Lab Section: Single Displacement Reactions: Activity Series REPORT SHEET Pre-lab Study Questions: 1. Objectives of this lab activity (in your own words): 2. What is the general format of the equation for a single-displacement reaction? 3. What does is an activity series? DATA & OBSERVATIONS Reactants and Equations (Complete the equations for the combinations that react.) Cu + AgNO 3 Evidence of Reaction Pb + Cu(NO 3 ) 2 Zn + Pb(NO 3 ) 2 Zn + MgSO 4 Cu + H 2 SO 4 Zn + H 2 SO 4 QUESTIONS AND PROBLEMS 1. Complete the following table by writing the symbols of the two elements whose reactivities are being compared in each test: Greater Activity Lesser Activity Rxn 1 Rxn 2 Rxn 3 Rxn 4 Rxn 5 Rxn 6 2. Arrange Pb, Mg and Zn in order of their activities, listing the most active first. (1) (2) (3)

70 Single-4 01/11/15 Single Displacement Reactions 3. Arrange Cu, Ag and Zn in order of their activities, listing the most active first. (1) (2) (3) 4. Arrange Mg, H 2, and Ag, in order of their activities, listing the most active first. (1) (2) (3) 5. Arrange all five of the metals (excluding hydrogen) in an activity series, listing the most active first. (1) (2) (3) (4) (5) 6. From the reactions observed in the six test tubes, explain why the position of hydrogen cannot be fixed exactly with respect to all of the other elements listed in the activity series in Question What additional test(s) would be needed to establish the exact position of hydrogen in the activity series of the elements listed in Question 5? 8. From the evidence developed in this experiment: (a) Would silver react with dilute sulfuric acid? Why or why not? (b) Would magnesium react with dilute sulfuric acid? Why or why not?