A student determined the concentration of copper by ion exchange. He obtained thefollowing results: (4.68x10^1) mL of (9.7770x10^-2) M NAOH solution was requiredto titrate the eluate (HCI solution) from the column. He used a 15.0 mL sample ofcopper chloride solution initially.Calculate the number of moles of Cu*2 that were absorbed by the column.Your answer should be in correct scientific notation (that is what the red text inBrightSpace means.)Note: Your answer is assumed to be reduced to the highest power possible.Your Answer:x10Answer A student determined the concentration of copper by ion exchange. He obtained thefollowing results: (4.2180x10^1) mL of (9.64x10^-2) M NaOH solution was requiredto titrate the eluate (HCI solution) from the column. He used a 15.0 mL sample ofcopper chloride solution initially.Calculate the concentration of Cu*2 in the original solution.Your answer should be in correct scientific notation (that is what the red text inBrightSpace means.)Note: Your answer is assumed to be reduced to the highest power possible.Your Answer:|x10Answer

Answered: Image /qna-images/answer/7c5c7124-8fe0-4c3e-a7f5-e19e3ed3cacc.jpg

A student determined the concentration of copper by ion exchange. He obtained the following results: (4.68x10^1) mL of (9.7770x10^-2) M NaOH solution was required to titrate the eluate (HCI solution) from the column. He used a 15.0 mL sample of copper chloride solution initially. Calculate the number of moles of Cu*2 that were absorbed by the column. Your answer should be in correct scientific notation (that is what the red text in BrightSpace means.) Note: Your answer is assumed to be reduced to the highest power possible. Your Answer:

A student determined the concentration of copper by ion exchange. He obtained the following results: (4.68x10^1) mL of (9.7770x10^-2) M NaOH solution was required to titrate the eluate (HCI solution) from the column. He used a 15.0 mL sample of copper chloride solution initially. Calculate the number of moles of Cu*2 that were absorbed by the column. Your answer should be in correct scientific notation (that is what the red text in BrightSpace means.) Note: Your answer is assumed to be reduced to the highest power possible. Your Answer:

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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Malic acid (C4H6O5) is a dicarboxylic acid that naturally occurs in the production of bignay wine. Maria was tasked to find out the acid content in a 200.0 mL wine sample by titrating it with a standardized solution of KOH. He was able to establish the working concentration of the KOH solution by using 39.12 mL of it to titrate a primary standard of KHP that weighed 3.021 g. The grams and %w/w of Malic acid present in the 200.0 mL wine sample were then determined by titrating a 20.00 mL aliquot using 48.95 mL of the standardized KOH solution. C4H6O5 (aq) + 2KOH (aq) ↔ K2C4H4O5 (aq) + 2H2O (l) Assume the density of the wine sample is 1.000 g/mL MM of KHP = 204.22 g/mol MM of C4H6O5 = 134.0874 g/mol What is the molar concentration of the prepared KOH solution?…
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In a lab, you diluted a sample of bleach to 1/10 concentration in a 250 volumetric flask. Then quantitatively transferred 25 ml of the 1/10 concentration diluted bleach into a beaker and titrated it with a standard sodium thiosulfate solution that has a molarity of 0.1215M. You repeated this 3 times. The data below is the amount of sodium thiosulfate that was titrated in the 3 runs. Calculate the molarity in each run of the diluted bleach and the concentration of undiluted bleach sample. Titration 1: 45.55 ml Titration 2: 45.67 ml Titration 6: 45.58 ml
Standardising a base solution by titration.
A student determined the concentration of copper by ion exchange. He obtained the following results: 28.61 mL of 0.0810 M NaOH solution was required to titrate the eluate (HCl solution) from the column. He used 15.0 mL sample of copper chloride solution initially. Calculate the number of moles of H+ present in the eluate.
The iodine contained in every one mL of the 0.010 M iodine solution in the buret will react with 1.76 mg of vitamin C. (In other words, every mL of iodine solution needed for the titration indicates the presence of 1.76 mg of vitamin C in the juice sample.) If your titration used 5.86 mL of iodine solution, what mass of vitamin C is in your fruit juice sample (in milligrams, mg)?
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