LNL7+Ethanol+in+Vodka+Assignment+Sum17_correctedQ9(a)(b)

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Dec 6, 2023

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LNL7 Alcohol Content of Vodka by Dichromate Titration Assignment Introduction Questions: - Refer to the Background and Procedure information to this lab to answer these questions. 1. Why does excess dichromate ion have to be used in the first reaction with ethanol? To ensure the reaction goes to completion. 2. What is the oxidation number of chromium in the reactant and in the product in both reactions? +6, +3 3. What is the full name of the reagent used to consume the excess dichromate in the second reaction? Iron (II) Ammonium Sulfate Hexahydrate 4. What is the full name of the redox indicator used to identify the endpoint in the titration? Sodium Diphenylamine Sulfonate 5. Consider the hypothetical titration where excess B (0.50 mol) is added to reactant A in solution to form product C, and then the excess B is reacted with reagent X to reach the equivalence point: Reaction 1: A + B  C + D Reaction 2: 2X + B  Y + Z If 0.30 mol X is required to reach the equivalence point in Reaction 2, how many moles of A were in the solution prior to Reaction 1? Choose from the following and circle or highlight your choice. A. 0.15 mol A B. 0.35 mol A C. 0.65 mol A D. 0.50 mol A

Experiment 1: Preparing Solutions Show work and include units and the correct number of significant figures on all measurements and calculated results. 6. Calculate the molarity concentration of potassium dichromate, K 2 Cr 2 O 7 , in the first volumetric flask. This is also the concentration of dichromate ion. 0.136M K 2 Cr 2 O 7 7. Calculate the molarity concentration of Fe(NH 4 ) 2 (SO 4 ) 2 · 6H 2 O in the second two volumetric flasks. This is also the concentration of Fe 2+ ion. 0.102M Fe(NH 4 ) 2 (SO 4 ) 2 · 6H 2 O Experiment 2: Titrating the Vodka Sample 8. For the Course Titration , what volume of iron(II) solution was required to change the color of the solution? Report as the volume range as indicated in the procedure. 13.99-14.29mL

9. For the Fine Titrations, record and calculate the following for your best two trials. Be sure to indicate which of your two trials these were in the first line of the table. Be sure to include units and the correct number of significant figures on all measurements and calculated results. Trial Number: 1 2 (a) Volume of dichromate ion solution added to the Erlenmeyer flask (mL) in Part 1 Part 2 : 5.0mL 5.0mL (b) Moles of dichromate ion in the solution added to the Erlenmeyer flask (Part 1 Part 2 ): 0.00068mol 0.00068mol (c) Initial volume of iron(II) solution in burrette (mL): 50.00mL 50.00mL (d) Final volume of iron(II) solution in burrette (mL): 35.86mL 35.88mL (e) Volume of iron(II) solution delivered from the burette (mL): 14.14mL 14.12mL (f) Moles of iron(II) ion delivered from the burette: 0.001442mol 0.001440mol (g) Moles of excess dichromate ion reacted with the iron(II) ions. (Remember to use the correct mole ratio that’s given by the balanced equation.) 0.00024mol 0.00024mol (h) Moles of dichromate ion that originally oxidized the ethanol in the vodka. (Subtract moles of excess dichromate ions that reacted with the iron(II) ions from the original moles of dichromate ion present before any reaction.) 0.00044mol 0.00044mol (i) Moles of ethanol in the 5.00 mL dilute-vodka sample. (Remember to use the correct mole ratio of C 2 H 5 OH to Cr 2 O 7 -2 that’s given by the balanced equation.) 0.00066mol 0.00066mol (j) Average moles of ethanol in the 5.00 mL diluted-vodka sample. Average your two best trials. 0.00066mol

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10. Show your work for all calculations done for results shown in your first column of the table in #9. Be sure to include units and the correct number of significant figures on all measurements and calculated results. (a) Not a calculation. Leave Blank (b) 0.135 mol L ∗ 0.0050 L = 0.00068 mol (c) Not a calculation. Leave Blank (d) Not a calculation. Leave Blank (e) 50.00 mL − 35.86 mL = 14.14 mL (f) 0.102 mol L ∗ 0.01414 L = 0.001442 mol (g) 0.102 mol L ∗ 0.01414 L 6 = 0.00024 mol (h) 0.00068 mol − 0.00024 mol = 0.00044 mol (i) 3 ∗ 0.00044 mol 2 = 0.00066 mol (j) 0.00066 mol + 0.00066 mol 2 = 0.00066 mol

11. The amount of alcohol in a drink is typically reported as the percent alcohol by volume. Volume percent (or volume/volume percent) most often is used when preparing solutions of liquids. Volume percent is defined as: V/v % = [(volume of solute)/ (volume of solution)] x 100% We will assume that all the alcohol in the vodka is ethanol. Complete the following table to determine the percent alcohol by volume for the vodka sample. Be sure to include units and correct number of significant figures on all measurements and calculated results. (a) Calculate the average mass (in grams) of ethanol, C 2 H 5 OH, in the tested sample solution from the calculated average moles of ethanol the table in #9, line (j): 0.0304g (b) Given the density of ethanol, 0.7893g/mL, calculate the volume (mL) of the ethanol (from grams) in each tested samples: 0.385mL (c) Record the volume (mL) of diluted vodka solution used in each test sample (from Step 2 of Part 1 of Experiment 2). 5.0mL (d) Calculate the percent alcohol by volume in the test samples. 0.77% (e ) Recall that the dilute vodka was prepared by diluting 2.00 mL vodka to 100.00 mL. How much more concentrated is the actual vodka than the diluted one? 50 times (f ) Use your answer to (e) to determine the percent alcohol by volume in the original vodka reagent. 38.5%

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Related Questions

Pls help ASAP.

PLEASE HELP ME ANSWER QUESTION 5) A student starts a titration without phenolphthalein in the Erlenmeyer flask. The student realizes the mistake and adds the phenolphthalein during the titration. Once the phenolphthalein is added, the solution in the Erlenmeyer flask remains colorlessCan the results of this titration be used? Concisely explain.

Please answer these three multiple type questions. Thank you very much!

13. What is indicated by the shape of the titration curve? PH a. b. C. d. e. Volume of titrant A diprotic acid was titrated with a strong base. A triprotic acid was titrated with a strong base. A diprotic base was titrated with a strong acid. A triprotic base was titrated with a strong acid. A strong acid was titrated with a strong base.

How does a redox titration differ from an acid base titration in general? How did this titration differ from the acetic acid titration lab specifically?

The answer is not 4.8 x 10^-10 please find the correct answer. Thank you!

1) Why are the titrations in this lab carried out in acidic solution? 2) If a student weighs out 0.565 g of oxalate unknown and it takes 26.8 mL of permanganate solution to titrate it, how much oxalate unknown should the student weigh out in order to use 35.0 mL of permanganate solution?

Scientists and engineers use solutions in their work and investigations. Conduct some research to discover information about two laboratory-based methods that utilize solutions: titration and gravimetric analysis. Use your research to answer these questions. What is titration used to discover? How is it similar to or different from what gravimetric analysis is used to discover? What is the process of titration? What is the process of gravimetric analysis? In what ways have the knowledge and application of solutions benefited scientific advancement? In what ways have the knowledge and application of solutions benefited society?

Compare and contrast the following general methods of argentometric titration. What are the strengths and limitations of each method? Explain. a. Mohr Methodb. Volhard Methodc. Fajans Method

A crucial skill when carrying out an accurate titration is the ability to stop the titration at the very first signs of a lasting color change. Recall the discussion of clarity in descriptions of colors as you compare the six solutions shown in the image below. E9 NB Q1 Homework Unanswered Examine the photo above and write your observations of each of the 4 solutions. H E- B iA X, x N. = E 66

426 Name Haley Doyle Sec.O Exp. # 26 QUESTIONS 1. Why must the Erlenmyer flask and graduated cylinder be dried in an oven before the reaction is run? a. Write an equation showing why the crude aspirin dissolves in the saturated NaHCO3 solution. b. Write an equation showing why the aspirin precipitates from when HCl is added to the saturated NaHCO3 solution.

7) What is the molarity of a 12.46 mL sulfuric acid solution if 18.22 mL of 0.100 M potassium hydroxide is required to reach the endpoint as indicated by a titration .

15. A 0.10 M solution of a strong monoprotic acid will be standardized using anhydrous sodium carbonate. The desired volume of solution to reach the endpoint is 23.0 mL. How many grams of anhydrous sodium carbonate should be weighed out for each standardization titration? 0.09 0.12 0.122 0.1

help please answer in text form with proper workings and explanation for each and every part and steps with concept and introduction no AI no copy paste remember answer must be in proper format with all working!

Please send me the question in 10 minutes it's very urgent plz

please see attached image. Im trying to calulate moles of HCl the volume I drew was 5.0 the volume titrated bas 8.15.

Drag and drop the terms to label this diagram of a titration apparatus accurately. burette stopcock ●NAAAAIANNI titrant Erlenmeyer flask (tube) (solution) 11 (container) (solution) clamp sample solution

Knowing that the unknown acid is monoprotic and the stoic honesty of this reaction is 1:1, we can determine the moles of acid by titration A. true B. false

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