A student performed three aqueous layer titrations in Part 1 using a standard sodiumthiosulfate solution with a concentration of 0.01153 M. They reported the followingmeasurements:Final Aqueous LayerBurette ReadingInitial AqueousLayer BuretteReadingFinal ThiosulfateBurette ReadingInitial ThiosulfateBurette ReadingDetermination #114.98 mL5.19 mL30.95 mL0.05 mLDetermination #2 Determination #324.98 mL35.09 mL14.99 mL31.89 mL0.22 mL24.98 mL31.95 mL0.03 mLHow many moles of thiosulfate did they use in their second titration (ie. their seconddetermination)? Report your answer to the correct number of significant figures andonly report the numerical value (no units).

The objective of the question is to find the number of moles of thiosulfate used in the second…

A student performed three aqueous layer titrations in Part 1 using a standard sodium thiosulfate solution with a concentration of 0.01153 M. They reported the following measurements: Final Aqueous Layer Burette Reading Initial Aqueous Layer Burette Reading Final Thiosulfate Burette Reading Initial Thiosulfate Burette Reading Determination #1 Determination #2 14.98 mL 24.98 mL 5.19 mL 30.95 mL 0.05 mL 14.99 mL 31.89 mL 0.22 mL Determination #3 35.09 mL 24.98 mL 31.95 mL 0.03 mL How many moles of thiosulfate did they use in their second titration (ie. their second determination)? Report your answer to the correct number of significant figures and only report the numerical value (no units).

A student performed three aqueous layer titrations in Part 1 using a standard sodium thiosulfate solution with a concentration of 0.01153 M. They reported the following measurements: Final Aqueous Layer Burette Reading Initial Aqueous Layer Burette Reading Final Thiosulfate Burette Reading Initial Thiosulfate Burette Reading Determination #1 Determination #2 14.98 mL 24.98 mL 5.19 mL 30.95 mL 0.05 mL 14.99 mL 31.89 mL 0.22 mL Determination #3 35.09 mL 24.98 mL 31.95 mL 0.03 mL How many moles of thiosulfate did they use in their second titration (ie. their second determination)? Report your answer to the correct number of significant figures and only report the numerical value (no units).

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...

See similar textbooks

Similar questions

Determine the mean value of the solubility product for calcium iodate and the average deviation for your three trials.
• An unknown acid (HA) was titrated with NaOH(aq). •The following titration curve was constructed using the laboratory data. You will use this titration curve to answer the questions related to this problem. • Assume that all laboratory work was completed at 298 K. 14 12 10 6. 4. 4. 9. 8. 10 12 14 16 18 20 22 26 28 30 Volume of Titrant/ mL What is the pK, for the unknown acid in this titration? Round your answer to the nearest whole number. Type your answer.. 24 8. Hd
A student performed three aqueous layer titrations in Part 1 and they reported the following measurements: Final Burette Reading Initial Burette Reading Volume of Aqueous Aliquot Final Burette Reading Initial Burette Reading Volume of Sodium Thiosulfate Determination #1 16.33 mL 6.50 mL 9.83 m 31.98 mL 0.76 mL 31.22 mL Determination #2 Determination #3 26.76 mL 16.33 mL 10.43 mL 33.62 mL 0.88 mL 32.74 mL 36.95 mL 26.76 mL 10.19 mL 32.22 mL 0.41 mL 31.81 mL Which determinations were the student's 'best two'? Calculate the percent difference for the 'best two' and show the complete calculation. Note that the concentration of standard sodium thiosulfate, which the student used, is unknown.
Titrated with 0.3554 M NaOH True molarity of unknown: 0.5018 M Trial 1 Trial 2 trial3 The volume of acid added to flask (mL) 10.00 10.00 10.00 Initial buret reading (mL) 0.00 14.06 28.19 Final buret reading (mL) 14.06 28.19 42.30 Volume of base titrated into flask 14.06 14.13 14.11 calculated molarity of acetic acid in your unknown A) calculate the molarity of acetic acid in your unknown for each trial. b) choose the three trials that have molarities that agree within 1% of one another and use these three molarities to calculate average c)use the true molarity for your acetic acid solution from above. using the average molarity that you calculated above calculate the percent error for your unknown.
A different titration experiment using a 0.122M standardized NaOH solution to titrate a 26.48 mL solution with an unknown Molarity concentration (M) of sulfuric acid (H2SO4) gave the following molarities for 3 trials. Initial Burette Reading (mL) Final Burette Reading (mL) Delivered vol (mL) Acid Concentration (M) Trial 1 0.0345 Trial 2 0.0334 Trial 3 0.0381 From the 3 trials, determine the average Molarity concentration of the H2SO4 to 3 significant digits. Don't include a unit.
To determine the pKa of PNP, a student needs to prepare a solution of 42.0 µM PNP in 30.0 mM acetate pH 5.2, with a total volume of 1,000 µL. Stock solutions of 0.200 mM PNP and 90.0 mM acetate pH 5.2 are available. Calculate the volume of dH2O required to make the solution (in µL).
Hi, I just need to know the correct answer for these. Thank you
11-6. A weak acid HA (pKa = 5.00) with volume 100.0 mL and concentration 0.100 M was titrated with 1.00 M KOH. Find the pH at the following volumes of base added and make a graph of pH versus VB: Vý = 0, 1, 5, 9, 9.9, 10, 10.1, and 12 mL.
In order to adjust the Potassium Permanganate solution, 0.0544g Na2C2O4 was taken and necessary experimental procedures were performed on it and the titrant consumption was found to be 7.9 mL. What is the KMnO4 concentration? A. 0.040B. 0.044C. 0.021D. 0.027
This was what was done before, and it was incorrect. Tried the same method for the next set of numbers just to check and it was also incorrect.
A 25.00 mL unknown water sample is titrated with a standardized 0.0140 M EDTA solution. It is determined that 8.54 mL of EDTA is required to reach the end point. The blank titre was determined to be 1.50 mL. Determine the concentration of Calcium in the water sample in ppm. (mwt. of CaCO3 = 100.0892 g/mol).
In the titration of 25.00 mL of a water sample, it took 19.040 mL of 4.965x 10−3 M EDTA solution to reach the endpoint. The total hardness is always listed in parts-per-million (ppm) of CaCO3 (or mg CaCO3 / Kg H2O). Since the density of water is 1.0 g/mL, one ppm would be the same as the number of mg of CaCO3 per liter of water. Determine the number of moles of CaCO3 present in the titrated sample of water, assuming that all the Ca2+ combines with CO32−. (enter your answer with 3 significant figures)