how to find the missing data in Table 1? Part 1: Getting Ready1. Obtain 5 pieces of filter paper from your TA.2. Record the exact stock concentrations of the reactants into Table2.3. Obtain one pump (10 mL) of Na2S2O3 in a 50 mL beaker.4. In a 50 mL beaker, obtain (12.5 mL) of 0.2 MKI.5.Obtain one pump (12.5 mL) of 0.1 M H₂O₂ in a 50 mL beaker and add 10drops of 6M HCL.6. Divide the filter paper into quarters.Part 2: Preparation of Solutions1. In a 25.00 mL volumetric flask add one pump (12.5 mL) of 0.1M H₂O2, add10 drops of 6M HCL, and dilute to the mark with RO water.2. In a 25.00 mL volumetric flask add one pump (12.5 mL) of 0.2M KI and diluteto the mark with RO water.Part 3: Run 11. Place your watch glass on top of your white tile.2. Place a piece of filter paper on top of a watch glass. Label the filter paperwith an 'x' to mark the center or target area for your reagents (see Figure 1on next page).3. Add the reagents as shown in Table 1 on the target you marked on the filterpaper. Your medicine dropper should be no more than an inch from thefilter paper.4.Start the timer as soon as you add the first drop H₂O₂.5. Record the time when you see the first sight of brown on the filter paper.Repeat steps 1-5 for this run four more times, cleaning the watch glass andusing a new filter paper for each trial.6. Table 1: Reagents for Runs 1-4Na2S2O3KI0.1M0.005MRun 1Run 21 drop1Run 31 dropRun 4 1 dropdropRun 22 dropsRun 1 210.674.3Run 3Run 4KI0.2MNumerical AnalysisSummary of Numerical ResultsTable 1: Average rates of reaction from experimental dataAverage time (s) [H₂O₂]o (M)[]o (M)3142 drops2 drops2 dropsH₂O₂0.05MPart 4: Runs 2-41. Repeat the steps in Part 3 for runs 2-4. You should have 5 trials per run.821 dropH₂O₂0.1MPart 5: Clean up1. Put your used filter paper into the filter paper waste container in the fumehood.2. All solutions can be disposed of in the inorganic waste (white jug with the CHEM 209 sign).3. Clean your glassware and medicine droppers and return your SET to your TA.drops22 drops1 dropFor the eyedroppersgiven, 1 drop 10 μL[S₂O3² ]0 (M)Be sure to add thereagents in order aslisted from left toright.Average Rate ofReaction (M/s)

To complete the table given for the concentration of H2O2, I- and S2O32- and the average rate of…

Answered: how to find the missing data in Table…

Science

Chemistry

how to find the missing data in Table 1?

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter20: Environmental Chemistry-earth's Environment, Energy, And Sustainability

Section: Chapter Questions

Problem 41PS

See similar textbooks

Similar questions

Quantity Your Data 1. Grams of vinegar sample used for your titration 25.000 g 2. Initial Buret Reading of Sodium Hydroxide solution 10.00 mL 3. Final Buret Reading of Sodium Hydroxide solution 28.00 mL 4. Amount of Sodium Hydroxide Solution used to neutralize the vinegar sample 5. Concentration of NaOH in the NaOH solution 0.050 g/mL 6. Grams of NaOH used to neutralize the vinegar 7. Grams of acetic neutralized by the amount of NaOH 8. Percent acetic acid in the vinegar Hints: For #4, The amount of NaOH used is the difference between the starting buret value and the ending buret value. For #6, Once you calculate the amount of sodium hydroxide used, multiple that value by the concentration of NaOH in the NaOH solution. For #7, Multiply the value obtained in number 6 by the number 1.5. Remember, we learned that every 1 gram of NaOH neutralizes 1.5 grams of acetic acid. For #8, Divide the grams of acetic acid by the grams of vinegar sample and multiply this value by…
to 70 ml of 0.2M Pb solution (NO3) 2 add 30 ml of 0.7 M KIO3 solution. a) Write the equation of the chemical reaction and calculate the number of moles of Pb2 + and IO3- ions before mixing b) count the number of moles of Pb2 + and IO3- ions after mixing, knowing that Ksp of Pb (IO3) 2 = 2.5 × 10-¹³
3I- + OCl- + 2H+ ----> I3- + Cl- + H2: A 25.00 ml sample of liquid bleach was diluted to 1000 ml in a graduated flask. A 25 ml portion of the diluted sample was pipetted into an Erlenmeyer flask and treated with excess KI to oxidize OCl- to Cl- and I3- was produced at the end of the reaction. The released I3 was titrated with 0.09892 M Na2S2O3 and 8.96 ml was spent to reach the turning point besides the starch indicator. What is the percent by weight/volume of NaOCl in the bleach sample? (NaOCl:74.44 g/mol)
Pls do fast and i will rate instantly for sure Solution must be in typed form A 25.0 mL volume of 0.0106 M KIO3 is pipetted into a 250-mL Erlenmeyer flask. The solution is titrated to the stoichiometric point with 16.25 mL of a sodium thiosulfate solution. What is the molar concentration of the sodium thiosulfate solution?
I add 0.1011 g of a primary standard FAS into a volumetric flask and diluted it to the line with water. We then add 2 mL of that solution into another 100 mL volumetric flask and diluted to the line with water. What would be the concentration of the diluted solution in g/mL?
A sample of freshly precipitated and filtered silver chloride weighs 459.0 mg. If 1.00 % of the silver chloride becomes photo decomposed, what is the precipitate’s weigh?
Phosphorus pentachloride reacts with water to form hydrochloric acid and phosphoric acid (below). A solution is created by reacting 4.5 g of PCl5 (MW=208.2 g/mole) with excess H2O. How many moles of NaOH are needed to titrate the resulting solution to completion. PCl5 + 4 H2O ----->5 HCl + H3PO4
You are going to do a precipitate reaction to determine the % purity of the CaBr2 in a very old and crusty bottle labeled “Calcium Bromide.” You carefully measure out 20.000 grams of solid CaBr2 and add water until the total volume of the solution is 750.00 mL. You recently bought a guaranteed 1.0000 M solution of high quality Na3PO4. You measure out 200.00 mL of the 1.0000 M Na3PO4 and add 100.00mL of water to make a dilution. You are going to mix 50.00 mL of your CaBr2 solution with some of your diluted Na3PO4 and filter out the precipitate. Write the molecular equation (it is always implied that you must balance equations and include s,l, g, or aq) Write the net ionic equation (it is always implied that you must balance equations and include s,l, g, or aq) Calculate the molarity of the CaBr2 solution you made if the CaBr2 was 100% pure. (The molar mass of CaBr2 is 199.88 g/mol) Calculate the molarity of the diluted Na3PO4 solution you made In order to ensure that…
You are going to do a precipitate reaction to determine the % purity of the CaBr2 in a very old and crusty bottle labeled “Calcium Bromide.” You carefully measure out 20.000 grams of solid CaBr2 and add water until the total volume of the solution is 750.00 mL. You recently bought a guaranteed 1.0000 M solution of high quality Na3PO4. You measure out 200.00 mL of the 1.0000 M Na3PO4 and add 100.00mL of water to make a dilution. You are going to mix 50.00 mL of your CaBr2 solution with some of your diluted Na3PO4 and filter out the precipitate. a)Calculate the molarity of the diluted Na3PO4 solution you made b)In order to ensure that the reaction is limited by the 50.00 mL of the impure CaBr2 solution, calculate the minimum volume, in mL, of the diluted Na3PO4 solution must you use. To be extra, super sure, that the Na3PO4 is the excess reactant, you add double the minimum volume. What volume do you add? c)What is the theoretical yield of the precipitate in grams? (The molar…
Calculate the maximum mass (in g) of AgCl lost in a chloride analysis as a result of washing the of silver chloride with 130 mL of water at room temperature. (Note: Ksp for silver chloride is 0.000000000160. Pay attention to the sig.fig. in your calculation. Keep three sig.figs. in the answer.)
If 100.0 mL of 0.167 M Na2SO4 is added to 100.0 mL of 0.897 M Pb(NO3)2, How many grams of PbSO4 can be produced? ??2??4(??) + ??(??3)2(??) → 2????3(??) + ????4(?)
Table 4.5 (data)Unmelted sample Melted sampleSolution Color_______________ ____________Result of adding AgNO3 to test solution______________ _____________Result of adding NH4SCN to test solution_____________ _____________Result of adding K4Fe(CN)6 to test solution____________ _____________4.6 (report)Test or observation is a composition change indicated?Solution color _________(Yes or no)Addition of AgNo3 _________(Yes or no)Addition of NH4SCN _________(Yes or no)Addition of K4Fe(CN)6 _________(Yes or no)