Exercise 1Data Table 1: NaOH Titration VolumeTrial 1Trial 2Trial 3Initial NaOHVolume (mL)8.789.259.30Final NaOHVolume (mL)????Questions0.300.981.01Average ofTrials 1-3:Total Volume ofNaOH Used (mL)8.48Average Volume of Concentration CH₂COOHNaOH Used (mL) in vinegar (mol/L)0.8358.358.278.29Data Table 2: Concentration of CH₂COOH in Vinegar8.35% CH₂COOHin vinegar4.76%Type your calculations of concentration and percent vinegar here (no photos):8.48 +8.27+8.29=25.04/3=8.346 → 8.35 mL8.35/10=0.835 mol/L1. The manufacturer of the vinegar used in the experiment stated that the vinegar contained 5.0%acetic acid. What is the percent error between your result and the manufacturer statement? Show yourwork.

Percentage error is the accepted value minus experimental value devided by accepted value and…

1. The manufacturer of the vinegar used in the experiment stated that the vinegar contained 5.0% acetic acid. What is the percent error between your result and the manufacturer statement? Show your work.

1. The manufacturer of the vinegar used in the experiment stated that the vinegar contained 5.0% acetic acid. What is the percent error between your result and the manufacturer statement? Show your work.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Q) A student misreads the directions and adds 4.0 g of benzoic acid instead of 0.4 g. What do you expect to happen? Would the experiment still be valid? Explain your reasoning. Pure Lauric Acid Lauric Acid + 0.4 g Benzoic Acid Lauric Acid + 0.5 g Benzoic Acid Mass of Lauric Acid 3.03g 3.00g 3.00g Mass of Benzoic Acid 0 g 0.40g 0.50g Freezing Point 43’C 39’C 38’C Freezing Point Depression * 4’C 5’C Molality of Benzoic Acid in Lauric Acid* 1.026 mol/kg 1.282 mol/kg Moles of Benzoic Acid * 0.003 moles 0.004 moles Experimental Molar Mass of Benzoic Acid * 133.3g/mol 125 g/mol Average Molar Mass * 129.15g/mol Percent Error * 5.75%
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NEED A HELP WITH THIS QUESTION 06
Your 50 mL beaker has a mass of 6.65 g. You add 10.00 mL to the 50 mL beaker and now the total mass is 17.45 g. You originally used 5.14 g of NaCl to make the solution. What is the percent composition of your solution? These calculations are described in the lab procedure in detail.
Explain the results obtained in this experiment
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I have the data, I only need the calculations of the last page.