In order to understand how this equation is derived and why it holds true, the product of each side of the equation should be examined. What value and unit do you get when you multiply a concentration of0.514 Mby a volume of 0.100 L? This question can be expressed as0.100 L x 0.514 mol1Express your answer to three significant figures with the appropriate units.• View Available Hint(s)HẢ?M1V1 =ValueUnits%3DSubmitPart BWhen you need to produce a variety of diluted solutions of a solute, you can dilute a series of stock solutions. A stock solution has a significantly higher concentration of the given solute (typically 10' to 104times higher than those of the diluted solutions). The high concentration allows many diluted solutions to be prepared using minimal amounts of the stock solution.What volume of a 6.56 M stock solution do you need to prepare 500. mL of a 0.0842 M solution of KC?Express the volume to three significant figures with the appropriate units.• View Available Hint(s)HẢ?Vi =ValueUnits%3D Part CThe absorbance of a cationic iron(II) sample solution was measured in a spectrophotometer, but the instrument returned an error because the absorbance was too high. The sample was then diluted by usinga pipette to take 100.0 µL of the sample and injecting it into a cuvette already containing 2.00 mL of water (total volume is 2.00 mL + 100.0 µL). The absorbance value of the diluted solution correspondedto a concentration of 9.29x10-6 M. What was the concentration of the original solution?Express the concentration to three significant figures with the appropriate units.• View Available Hint(s)HẢ?original concentration of Fe2+ValueUnits%3DSubmit

Answer :- Part A :- M1V1 = 0.0514 (mol) Part B :- V1 = 6.42 (mL) Part C :- Original Concentration Of…

Part C The absorbance of a cationic iron(II) sample solution was measured in a spectrophotometer, but the instrument returned an error because the absorbance was too high. The sample was then diluted by using a pipette to take 100.0 µL of the sample and injecting it into a cuvette already containing 2.00 mL of water (total volume is 2.00 mL + 100.0 µL). The absorbance value of the diluted solution corresponded to a concentration of 9.29x106 M. What was the concentration of the original solution? Express the concentration to three significant figures with the appropriate units. > View Available Hint(s) ? original concentration of Fe2+ = Value Units Submit

Part C The absorbance of a cationic iron(II) sample solution was measured in a spectrophotometer, but the instrument returned an error because the absorbance was too high. The sample was then diluted by using a pipette to take 100.0 µL of the sample and injecting it into a cuvette already containing 2.00 mL of water (total volume is 2.00 mL + 100.0 µL). The absorbance value of the diluted solution corresponded to a concentration of 9.29x106 M. What was the concentration of the original solution? Express the concentration to three significant figures with the appropriate units. > View Available Hint(s) ? original concentration of Fe2+ = Value Units Submit

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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